Periodic Table
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Periodic Table
Mandeleev's Periodic Table
Introduction
In 1969 a Russian chemist studied the properties of elements, on the
basis of experimental results, Mendeleev put forwarded a law which is
known as periodic law. The periodic law can be stated as
The properties of the elements are the periodic function of their atomic masses.
If the elements are arranged in order to increase atomic masses then
similar properties reoccur with definite intervals. Mandeleev arrange
the known elements in order to increase atomic masses in the form of
table, which is known as Mandeleev's Table. In this table, the
elements with similar properties appear in the same vertical column
known as groups, the horizontal rows of the elements are called
periods.
Advantages of Mandeleev's Periodic Table
Mandeleev's periodic table had a number of advantages over the classification developed till that time.
1. Prediction of New Elements
While arranging the elements in order to increase atomic masses in the
table, Mandeleev come across certain positions where no known element
was seen fit to him. He left those spaces between vacant and predicted
that new elements would be discovered which could be fit in those
spaces.
2. Correction of Atomic Masses
At the time of Mandeleev the atomic masses of some elements were not
correctly known. Mandeleev's classification of elements help to correct
the atomic masses of these elements.
3. Prediction About Properties
Mandeleev also made prediction about the properties of the unknown
elements. Many of these predictions were later found correct. He was
able to make these prediction because the elements falling in the same
group have similar properties.
4. Unication of Elements
Mandeleev's classification co-relates all the elements. The discovery
of periodic classification showed that all the elements despite their
apparent diversity are co-related with one another and make one
systematic whole. Thus, all the elements are unified through a
classification.
Periods
There are seven periods (horizontal rows) in the periodic table. The
first table period contains two elements that are hydrogen and helium.
The second and third periods have eight elements andeach are called short periods. The fourth and fifth periods have eighteen elements each and are called long term. The sixth period contains thirty two elements and is called very long period. The seventh period is incomplete. The properties change gradually within the period or across the table from left to right.
Groups
The vertical columns in the periodic table are called groups or
families. There are thirty-two groups or vertical columns in the modern
periodic table. There are light groups, which consist of five or six
elements and are called main groups, represented by 'A' group, to distinguish them from remaining smaller groups by Transition Elements. The elements of main groups are called Representative Elements or Typical Elements.
The remaining groups that are the short groups of the periodic table
are known as transition group. The elements of these groups are
collectively called transition elements. These elements are further
classified into outer transition elements and inner transition elements.
The elements of outer transition elements (d-block) are usually known
as 'B' group. The transition elements of 'B' group consist of eight
groups and three periods, which are known as a Series. The first series
of outer transition elements started from Sc (Scandium) to Zn (Zinc).
The inner transition elements (f-block) consist of two series of
elements having fourteen elements each. The first series of inner
transition elements is called Lanthanide series and the elements are
called Lanthanide's. The second series of inner transition elements is
called Actinide series and the elements are called Actinides. The
Lanthanide and Actinide are also known as Rear Earth Elements and Heavy Rear Earth Elements respectively.
Blocks of Periodic Table
On the basis of the kind of orbital of elements occupied by the last
electron, the periodic table is classified into four blocks.
1. s - Block Elements
Those elements in which the last electron occupies 's' orbital are
called s - block of the periodic table. The elements of IA and IIA
including hydrogen and helium are called s - Block Elements.
2. p - Block Elements
Those elements in which the last electron occupies 'p' orbital are
called p - Block Elements of periodic table. The elements of IIIA to
VIIIA (six groups) are p - block elements.
3. d - Block Elements
Those elements in which last electron occupies 'd' orbital are called d
- Block Elements. The outer transition elements that is B group (10
groups) belongs to d - block of Periodic Table.
4. f - Block Elements
Those elements in which last electron occupies 'f' orbital are called f
- Block Elements. The elements of inner transition (14 groups) that is
Lanthanide Series and Actinide Series belongs to f - block elements
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Copper (Extraction)
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Copper (Extraction)
Extraction Of Copper
Copper is widely distributed in nature. It occurs in free as well as
combined state. Blister copper is mainly extracted from sulphide ores
(copper pyrite). The extraction of Blister Copper proceeds through
following four steps.
Step I - Concentration
The sulphide ores are concentrated by any of the following methods.
a. Gravity Separation
The powdered ore is passed over a wheel so that it falls in two section due to difference in specific gravity.
b. Forth Floatation Process
The finely powdered copper pyrite ore is introduced into water
containing Rine oil. The suspension is vigorously agitated with air. The
stony matter settles to the bottom and the ore is carried to the top
in the forth. The object of this process is to increase the
concentration of copper in the ore.
Step II - Heating / Roasting
The concentrated ore is heated strongly (roasted) in a multiple heater
roaster (Reverberatory Furnace) in excess of air in order to achieve
the following.
1. To remove sulphur as sulphur dioxide.
2. To remove arsenic and antimony as their volatile oxides.
3. To convert the copper pyrite into a mixture of cuprous sulphide and ferrous sulphide.
4. To partially oxidize cuprous sulphide and ferrous sulphide to copper oxide and ferrous oxides respectively.
5. To remove fusible impurities and moisture.
6. To change the ore into porous form.
Step III - Smelting
The roasted ore is mixed with Silica (SiO2) and smelted in a water
jacketed blast furnace about 5ft to 6ft high and 1.6 m in diameter. It
is a tower like structure made of steel sheet and lined inside with
firebricks. A blast of air is necessary for the combustion of ore. This
ore is blown through the pipes provided at the base. Since, most of the
heat is produced by the combustion of ore itself, therefore, small
amount of fuel is required. The cuprous oxide formed during roasting
react with unoxidized ferrous sulphide to form cuprous sulphide and
ferrous oxide.
CuO + FeS ----> Cu2S + FeO
Silica act as flux, it reacts with ferrous oxide to form fusible slag
(Ferrous Silicate) because iron has more affinity for oxygen than
copper.
FeO + SiO2 ----> FeSiO3 (Slag)
Slag is removed from the slag hole while a molten mass containing
mostly cuprous sulphide, with a very little ferrous sulphide is taken
out from the bottom and is called Matte.
Step IV - Bessemerization
The molten is now transferred into Bessemer converter. It is a pear
shaped furnace made of steel plates and provides with a basic lining
like that of lime or Magnesium Oxide.
Diagram Coming Soon
The main features of this process is that air is blasted through the
molten matte. As a result, ferrous sulphide still present gets oxidized
to ferrous oxide and is removed as slag. Cuprous sulphide is partially
oxidized to oxide, which reacts with remaining cuprous sulphide to form
metallic copper.
Cu2S + 2Cu2O ----> 6Cu + SO2↑
The molten copper is run into sand moulds and allowed to solidify. When
it gives out absorbed SO2, it leaves blister type appearance at the
surface of the metal. The metal thus obtained is known as Blister Copper. It is about 98% pure.
Refining
The crude copper obtained by the above methods contain about 2% of
impurities consisting of Fe, Ni, Zn and Ag. It is refined by
electrolysis. The process is carried out in a large tank lined with
lead. Thick plates of crude copper served as anode and thin plates of
pure copper act as cathode. The cathode is coated with oil which helps
in easy scraping of pure copper. These electrodes are dipped into
electrolytic copper sulphate solution. The electrolysis is then carried
out by a current of 1.3 volts. The pure copper is deposited at the
cathode while impurities like Fe, Ni, Zn passes into solution and other
like Ag and Au fall down as anode mud. During electrolysis following
reactions occur.
Cu0 ----> Cu11 + 2e- (At Anode)
Cu11 + 2e- ----> Cu0 (At Cathode)
Copper thus obtained is 99.99% pure and is known as Electrolytic Copper
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Sulphuric Acid (Contact Process)
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Sulphuric Acid (Contact Process)
Introduction
On industrial scale two methods are employed for the manufacture of
sulphuric acid, the Lead Chamber Process and the Contact Process.
The Contact Process
When a mixture of pure and dry sulphur dioxide and air is passed over a
heated catalyst such as Platinum Asbestos, then Sulphur dioxide is
oxidized into sulphur trioxide. This gas gives sulphuric acid when
treated with water.
The plant used in Contact in Contact Process is composed of following parts.
1. Sulphur and Pyrite Burner
In this part, SO2 is produced by either burning sulphur in air or roasting ores. Like ZnS, PbS, FeS2 in air.
S + O2 ----> SO2
4FeS2 + 11O2 ----> 2Fe2O3 + 8S2
2. Dust Chamber
The SO2 obtained from pyrite burner contains impurities such as
unreacted coal, dust, moisture, arsenic compounds etc. These impurities
are removed from the gas in dust chamber. In this chamber hot air is
blown as a result the heavy particles are removed and unreacted sulphur
convert into SO2. Now the gases are passed through a cooling pipe into
water chamber.
3. Water Chamber
In this chamber a stream of water is showed on the gas to remove the
dust particles. The SO2 gas is now proceed into another chamber, which
is known as drying tower.
4. Drying Tower
In drying tower moist SO2 gas is mixed with concentrated H2SO4. As a
result the gas become dry and dilute H2SO4 is sink at the bottom.
5. Oxidation Tower
Before oxidation the dry gas is allowed to pass through arsenic
purifier containing ferric hydroxide here the arsenic compounds are
absorbed. The purified gases are then passed through a strong beam of
light to remove any remained dust particle.
The purified and dry SO2 gas is passed through the oxidation tower.
This tower consist of iron pipes packed with plantanized asbestos
coated with Vanadium Penta Oxide (V2O5), which act as catalyst. In this
tower the temperature is kept constant at about 480ºC, under high
pressure and high concentration of sulphur dioxide and oxygen, oxidation
of SO2 takes place in a favourable condition to yield maximum amount
of SO3.
2SO2 + O2 <----> 2SO3 (45000 cal)
6. Absorption Tower
Sulphur trioxide formed in Oxidation Tower is passed up to Absorption
tower, where it meets a stream of concentrated sulphuric acid and hence
absorbed to form OLEUM. The maximum absorption of sulphur trioxide is
60% at which oleum has maximum density.
SO3 + H2SO4 ----> H2S2O7
Oleum can be diluted to obtain any desired concentration of sulphuric acid.
H2S2O7 + H2O ----> 2H2SO4
Sulphuric acid is obtained from this process is nearly 99.99% pure
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Aluminium (Extraction)
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Aluminium (Extraction)
Extraction of Aluminium
Aluminium does not occur free in nature, but it widely distributed in
combine state. Aluminium is mainly extracted from Bauxite ore
(Al2O3.nH2O). The extraction of Aluminium from Bauxite proceeds through
following two steps.
1. Purification of Bauxite to Alumina.
2. Electrolysis of Pure Bauxite (Alumina)
1. Purification of Bauxite
Bauxite contains iron oxide (Fe2O3) and Silica (SiO2) as chief
impurites. These impurities must be removed from Bauxite, because they
make the aluminium brittle and liable to corrosion. Bauxite ore may be
purified by the following methods.
a. Hall's Method
This method is used for the purification of Bauxite containing Fe2O3
and SiO2 as impurities. The finely divided Bauxite is fused with sodium
carbonate (Na2CO3), as a result sodium aluminate is formed while the
impurities are left unaffected.
Al2O3.nH2O + Na2CO3 ----> 2NaAlO2 + CO2 + nH2O
The fused mass is rapidly extracted with water leaving behind both the
impurites Sodium aluminate is heated up to 50ºC - 60ºC in the presence
of CO2. As a result while glatinous precipitates of aluminium hydroxide
are formed.
The precipitates of Al(OH)3 are separated, washed to remove Na2CO3,
dried and ignited about 1500ºC to get pure bauxite (alumina)
b. Bayer's Method
This method is used for the purification of Bauxite containing excess
of Fe2O3 as impurity. The finely divided Bauxite is treated with
concentrated solution of Sodium Hydroxide. As a result soluble sodium
Aluminate is formed, while the impurities are removed by filtering the
solution.
Al2O3.nH2O + NaOH ----> 2NaAlO2 + 2(n)H2O
Soluble sodium Aluminate is treated with excess water to form white gatinous precipitates of Aluminium Hydroxide.
2NaAlO2 + 4H2O ----> 2Al(OH)3 + 2NaOH
The precipitates of Al(OH)3 are separated, washed to remove NaOH, dried and ignited about 1500ºC to get pure bauxite (alumina)
c. Serpek's Method
This method is used for the impurities of Bauxite ore containing excess
of SiO2 as impurity. The finely divided Bauxite is mixed with carbon
and heated up to 1800ºC in the current of Nitrogen. As a result
Aluminium Nitride is formed.
2. Electrolysis of Pure Bauxite (Alumina)
The electrolysis of pure bauxite is carried out in a steel tank lined
with carbon (graphite). The carbon lining serve as cathode. The anode
consist of carbon rods hanging in the molten mass.
In fused state pure alumina is bad conductor of electricity and its
melting point is about 2050ºC. So flourspar and cryolite is added in
alumina to increase the fluidity of the melt and lower the melting
point respectively. When electric current is passed through this
mixture, the aluminium is obtained at cathode in liquid state. It sink
to bottom from where it drawn, periodically through the tapping hole.
Aluminium produced by this method is 98% and contains traces of Fe, Si and Al2O3 etc.
Refining of Aluminium
The molten aluminium so obtained contains 2% impurities which is further purified by electrolysis in hoop's cell.
Construction
The Hoop's cell consist of an iron box lined with carbon (graphite),
the carbon lining served as anode. This iron box consist of three
layers, the upper most layer is of pure aluminium the middle layer
molten flourides (AlF3, BaF2 and NaF) act as electrolyte, where as the
lower layer consist of impure aluminium. The cathode consist of carbon
rods hanging in pure aluminium.
Working
When electric current is passed through the impure aluminium goes into
the middle layer as all leaving impurities and the pure aluminium is
deposited at the top of molten flourides at cathode. The aluminium
layer grows and drawn off time to time from tapping hole. The refined
Aluminium so obtained is 99.99% pure
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Nitric Acid (Ostwald's Process)
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Nitric Acid (Ostwald's Process)
Introduction
On industrial process three methods are employed for the manufacture of
nitric acid. Ostwald's Process uses Ammonia as raw material.
Ostwald's Process
When a mixture of ammonia and air is passed through a catalytic chamber
containing electrically heated Platinum Gauze, (NO) nitric oxide is
formed. This nitric oxide combines with more oxygen to form nitrogen
dioxide (NO2). This gas is then absorbed by water to form nitric acid.
The plant used in Ostwald's Process consist of following parts.
1. Catalytic Chamber
A mixture of pure and dry ammonia is passed through a catalytic chamber
containing heated (800ºC) platinum, which serves as catalyst. Here
ammonia is completely oxidized to nitric oxide.
2. Oxidation Tower
The nitric oxide is passed into oxidation tower where the temperature of
gases falls to 200ºC - 250ºC. At this temperature nitric is oxidized to
nitrogen dioxide.
2NO + O2 ----> 2NO2
3. Absorption Tower
Now the gases containing NO2 and oxygen are than sent to a series of
absorption tower, which is filled with broken quartz and water is
showered from top of the tower. Then NO2 reacts with H2O in the presence
of oxygen to form HNO3.
4NO2 + 2H2O + O2 ----> $HNO3
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Sodium Carbonate (Ammonia-Solvay Process)
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Sodium (Down's Process)
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Sodium (Down's Process)
Introduction
On large scale, sodium is manufactured by electrolysis of fused sodium
chloride. The process was given by scientist Dawn, therefore, it is
called Dawn's Process.
Construction of Down's Cell
A special electrolytic cell known as Dawn's cell is used for the
electrolysis of sodium carbonate. The cell consists of a cylindrical
shape iron basin lined inside by firebricks. The iron cathode is
separated from anode by iron gauze diaphragm. Anode consists of a carbon
rod, which is present between two iron cathodes. The electrolytic
solution consists of a mixture of sodium chloride (NaCl) and calsium
chloride (CaCl2). Calsium Chloride (CaCl2) is added to decrease the
melting point of sodium chloride from 801ºC to 600ºC.
Working of Dawn's Cell
When electric current is passed through molten NaCl, the sodium ion
migrates towards cathode. It gains and electron and converts into molten
sodium metal, which floats inside the cathode compartment. This molten
sodium metal is allowed to pass through pipe 'p' which collects it in a
vessel 'V' outside the cell.
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Caustic Soda Or NaOH (Castner Kellner's Process)
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Chlorine (Castner-Kellner's)
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Chlorine (Castner-Kellner's)
Introduction
Chlorine plays an important role in industries. Therefore to fulfill
the demands, chlorine is manufactured on large scale. It is prepared by
the electrolysis of aqueous solution sodium chloride, this process is
known as Castner-Kellner's Process and it is carried out in
Castner-Kellner's Cell.
Construction of Castner-Kellner's Cell
The Castner-Kellner's cell consist of a steel tank which contain Hg
flows from right to left in the cell and is connected with the negative
terminal of the battery therefore it acts as cathode. The cell is
filled with saturated aqueous solution of NaCl, which also flows in the
same direction as Hg. Some graphite rods are dipped into the solution
of NaCl. These rods connected with positive terminal of the battery
therefore act as anode.
Working Of Castner-Kellner's Cell
When the electric current is passed through the cell. The sodium ion
and chloride ion migrates towards their respective electrodes. Chlorine
ion moves towards anode, loses its electron and converts into chlorine
gas. The free chlorine gas comes out of the tube at the top of the
cell. The sodium ion migrates towards cathode gains electrons and
converts into sodium metal. The sodium is dissolved in Hg to form
sodium amalgum which comes out with the flow of Hg from the cell.
NaCl <----> Na+ + Cl-
Na+ + e- ----> Na0 (At Cathode)
2Cl ----> Cl2↑ + 2e (At anode)
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Chemistry XII Viva Notes
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Chemistry XII Viva Notes
Friendsmania.net
Qs.1 What is salt? What are its two parts?
Ans. Salt is the neutralized product of acid and base. The two essential
parts are acidic radical (Anion) and Basic radical (cation).
Qs.2 What is meant by “ion”?
Ans. Ion is an atom with positive or negative change or charges.
Qs.3 What is meant by radical?
Ans. Charged atom or group of atoms. Which exists as a single unit in crystal or in solution form is known as a radical.
Qs.4 What is Acid radical?
Ans. The radical which is contributed by an acid during salt formation
and having a negative charge is called acid radical (Anion).
Qs.5 What is basic radical?
Ans. The radical which is contributed by a base during salt formation
and having a positive charge is called basic radical (cation).
Qs.6 Why positive radical is called cation?
Ans. On passing the current through a solution it moves towards cathode
Qs.7 Why negative radical is called Anion?
Ans. Negative ions moves towards anode during electrolysis hence they are called Anion.
Qs.8 How the formation of cation and Anion takes place fron an atom?
Ans. When an electron is removed from an atom cation is formed on the other hand when atom gains an electron Anion is formed.
X→ X+ + e- and X + e- X-
Cation Anion
Qs.9 What is meant by group reagent?
Ans. It is the reagent or chemical, used to find out a particular group of cations or Anions.
Qs.10 How many groups are there for Anion?
Ans. There are three main group for Anion.
Qs.11 How many groups are there for cation?
Ans. There are six group for cation.
Qs.12 What are the group reagents for I, II & III group of cation?
Ans. The group reagent for I group is Hcl, Hcl + H2S for II group and NH4Cl +NH4OH are the group reagent for III group.
Qs.13 What are the group reagent for I, II and III of Anion?
Ans. For I group H2SO4 or HCl (dilute) is a group reagent for II groups
H2SO4 while III group gives precipitation by Bacl2 or Ammonium molyblate
(NH4)2 MoO4.
Qs.14 How the cations of group I, II & III group of Anion?
Ans. The cations of group 1st are precipitated as chlorides, cations of
the group at once, hence they are analysised individually e.g.BaCl2 for
SO4 2-.
Qs.15 How the cations of group VI are precipitated?
Ans. There is no any specific reagent to precipitate all the cations of
the group at once, hence they are analysised individually e.g. BaCl2 for
SO4 2-.
Qs.16 What is difference between an “atom” “molecule” and “ion”?
Ans. Atom is the smallest part of an element which can take part in
ordinary types of chemical changes. It is electrically neutral because
it carries equal number of electrons & protons i.e. two particles of
apposite charges. Symbol “Cl” represents a chlorine atom. Molecule is
the smallest unit quantity of matter which can exist by itself and
contain all the properties of the original substance. A molecule may
consists of two similar atoms or two dissimilar atoms. Formula of
chlorine “Cl2” represents a chlorine molecule of similar atoms and
“NaCl” molecules with two dissimilar atom. Ion It is a charged form of
an atom or group of atoms. It carries either a negative or a positive
charge according as the number of electrons is greater or lesser than
the number of protons present in it. Symbol of chlorine “Cl” represents a
negatively charged chlorine atom (Anion) “Cl” while symbol of Ammonium
NH4 represents an ammonium ion (cation) “(NH4+)”.
Qs.17 What is the group reagent for cation in group II?
Ans. Hydrogen Sulphate (H2S) in presence of Hydrochloric acid (HCl)
Qs.18 What is Nessler’s reagent and what for its used?
Ans. It is alkaline solution of potassium mercuric iodide K2 (Hgl4). It gives brown precipitation with ammonium salts.
Qs.19 What is chromyl chloride test?
Ans. When solid chloride is heated with potassium dichromate and Conc.
Sulphate acid it gives red vapours of chromyl chloride CrO2Cl2.
Qs.20 Which chlorides are in soluble in water?
Ans. AgCl, PbCL2 and Hg2Cl2 salts are in soluble in waters.
Qs.21 What is solubility product?
Ans. It is the product of ionic conc, of the saturated solution of a
salt. The Conc, is expressed in moles per liter of the ions.
Qs.22 What do you mean by qualitative analysis?
Ans. It is the process by which the components of a substance or a mixture can be detected
Qs.23 What do you mean by qualitative inorganic analysis?
Ans. It is the process by which the constituent ions of an inorganic Salt can be detected.
Qs.24 What are double salts?
Ans. Those salts whose crystals contain two salts are commonly known as double salts e.g. FeSO4 (NH4)2 SO4. 6H2O
Qs.25 What are complex salts?
Ans. The salts contains a complex cation or Anion in which a transition
metal ion has coordinated with a number of electron pair donor e.g. [Fe
(CN)6].
Qs.26 What is precipitate (ppt.)?
Ans. It is a compound which separates out in the solid phase from the solution phase on adding a reagent.
Qs.27 Is it possible to use “NaCl” instead of dilute HCl?
Ans. Yes, any soluble chloride can precipitate the radicals of the first
group as chloride in cation. The advantage with Hcl is that it does not
allow to introduce another basic radical in the solution.
Q.28 Why water and HCl are preferred for the preparation of the original solution (O.S) in the detection of basic radical?
Ans. Because no interference is caused by H2O and HCl while other acids
like HNO3 and H2SO4 interfere e.g. Cation like pb2+ , Ca2+ , Sr2+ and
Ba2+ form in soluble sulphates with H2SO4 and HNO3 being oxidizing agent
interferes in the second groups by oxidizing H2S to S.
Qs.29 What fruity smell indicates?
Ans. The fruity smell is generally due to the formation of an ester.
Which indicates the presence of CH3COO ion due to the formation of ethyl
acetate CH3COO2H5 or mixed ester fruity smell obtained.
Qs.30 What is meant by water of crystallization give few examples of some compounds?
Ans. The water of crystallization is the molecule of water present in a
compound e.g. Copper Sulphate CuSo4 . 5H2O. Magnesium sulphate MgSO4 .
7H2O Barium Chloride Bacl2 . 2H2O etc.
Qs.31 What is functional group?
Ans. It is a group of atoms responsible for their specific properties to the compound possessing it e.g.
i) Carbonyl group > C=O ii) Carboxylic acid group―COOH
iii) Hydroxyl group – OH iv) Amino group – NH2 etc.
Qs.32 What is vinegar?
Ans. Vinegar is a dilute solution of acetic acid. By the smell of which CH2COO- (acetate) ion is confirmed.
Qs.33 Why is testing Cl- radical, When a rod dipped in NH4OH is held
over the mouth of test tube, a dense white fumes are produced?
Ans. Because chloride with conc. H2SO4 produce HCl gas which forms white fumes of NH4Cl with NH4OH.
2Cl- + H2SO4 → 2HCl + SO42-
HCl + NH4OH → NH4Cl + H2O
Qs.34 During testing of 2nd group of acidic radicals a brown gas may
evolve, which may be due to Br radical or due to NO3 –radical, how will
you distinguish them?
Ans. If evolved gas becomes denser on adding MnO2 then it is Br2 gas if
it increased by adding copper turnings then it is NO2 gas.
Qs.35 Why in the ring test for Nitrate, a brown ring is formed at the junction of two liquid layers?
Ans. The H2SO4 decompose NO3- radical and evolves “NO” which makes a
complex nitro ferrous compound with FeSo4 at the junction which appears
as a brown ring.
Qs.36 Why it is necessary to prepare the original solution (O.S) of the
salt for the detection of basic radicals except NH4+ radical?
Ans. All the basic radicals are metallic ions except NH4+ therefore they
cannot form a volatile substance which can be detected by evolution of a
gas by a particular smell. Hence they are detected only by
precipitation method from their solution.
Qs.37 Why NH4+ radical can be detected, directly from its salt?
Ans. On testing with an alkali, like NaOH it evolves NH3 gas the smell of which confirms the NH4 radical.
NH4+ + NaOH → NH3 + H2O + Na+
Qs.38 Why the basic radicals are divided into six groups?
Ans. Actually they are divided on the basis of solubility product of their corresponding compounds.
Qs.39 If original solution is prepared in HCl, Why it is concluded that 1st group of basic radicals is absent?
Ans. The first group radicals from in soluble chlorides with HCl, Hence
if the solution is clear in HCl it means that 1st group radicals are
absent.
Qs.40 Why the ppt of AgCl is soluble in NH4OH?
Ans. Because AgCl is insoluble in water but in the presence of NH4OH it
forms a complex diamine compound which can be dissolved easily in water.
Qs.41 What are brisk effervescence?
Ans. Brisk effervescence is due to the evolution of CO2 gas.
Qs.42 How does lime water turn milky on passing CO2 gas through it?
Ans. Lime water turns milky due to the formation of in soluble CaCo3.
Qs.43 What is lime water?
Ans. It is a solution of Ca(OH)2-.
Qs.44 What is slaked lime?
Ans. It is Ca(OH)2-.
Qs.45 What is lime?
Ans. It is calcium oxide CaO.
Qs.46 What is red gas?
Ans. Chromyl chloride is called red gas CrO2Cl2.
Qs.47 What violet vapours indicate?
Ans. They indicate the presence of Iodine.
Qs.48 Mention some cations with their characteristics flames?
Ans. Cations Colour of the flame
Ca2+ Brick red
Sr2+ Deep red
Ba2+ Grassy green
Cu2+ Bluish green
Qs.49 What are crystalline and amorphous salt?
Ans. The salt containing crystals are known as crystalline while powder like salts are called amorphous.
Qs.50 If the salt is coloured what cations may be present?
Ans. If the salt is coloured the following cations may be present
e.g. Cu2+, CO2+, Fe2+, Nl2+, Mn2+ and Fe3+ etc
Qs.51 Give the name of a non-metallic basic radical?
Ans. The non-metallic basic radical is Ammonium NH4+ radical.
Qs.52 In the preparation of original solution for cation. Why H2SO4 is never used?
Ans. Because it is oxidizing agent and precipitate various cation In
different groups e.g. Ba2+, Sr2+ and pb2+ are precipitate as sulphate in
group II. In this way the whole scheme of cation will disturbe.
Qs.53 Lead may be precipitated in group I as well in group II of cation why?
Ans. In first group PbCl2 is sparingly soluble and hence not all the
lead ions Pb2+ are precipitated. Thus the remaining Pb2+ are separated
out in group II as Pbs.
Qs.54 What are Alums?
Ans. Alums are the Isomorphous compound.
Qs.55 What are Isomorphous?
Ans. Compounds having the same crystal structures are known as Isomorphous compounds
Qs.56 What is potash alum?
Ans. The hydrated double sulphates salt of potassium and aluminum is known as potash alum e.g. K2SO4Al2 (SO4)3. 24H2O
Qs.57 What are the common uses of potash alum?
Ans. It is used as mordant in dyeing of fabrics sizing of paper as
coagulating agent and also for cleaning of water on small scale.
Qs.58 Give the formula for some other Alums?
Ans. Ammonium iron alum (NH4)2 SO4,Fe(SO4)3 . 24H2O
Lithium chromium alum Li2SO4 .Cr2(SO4)3 . 24H2O
Soda alum Na2 SO4 . Al2(SO4)3 . 24H2O
Qs.59 What is the formula of Iodoform give its I.U.P.A.C. name?
Ans. Formula of Iodoform is CHl3 and in IUPAC its name is Tri-Iodomethane.
Qs.60 Give the formula and name of other Haloforms?
Ans. Chloroform CHCl3 and Bromoform CHBr3.
Qs.61 During the preparation of Iodoform temperature should not be higher than 80ºC Why?
Ans. Iodoform may be hydrolyzed above 80ºC.
Qs.62 What is mean by haloform reactions?
Ans. The reaction by which chloroform, bromoform and Iodoform may be prepared .
Qs.63 What is the melting point of Iodoform?
Ans. Its melting point is 119ºC.
Qs.64 What types of compounds gives haloform reactions?
Ans. The compounds like methyl ketone, acetaldehyde and ethyl alcohol can give haloform reactions.
Qs.65 What are plastics?
Ans. Plastics are the polymerized products of simple organic molecule or
when two or than two simple molecules (Monomer) combine to form a big
groups of polymer, it is known as plastic e.g. polythene from ethane.
This is a plastic commonly known as polythene i.e.
(C2H4)n = (C2H4)n
Qs.66 What are monomers, polymers and polymerization?
Ans. A large number of simple molecules which may be combine and form a
large molecule of high molecular mass are known as “Monomers”, the
resulting heavy product is known as the “polymer” and the process of
formation of a polymer is known as “polymerization”.
Qs.67 What is P.V.C and P.V.A?
Ans. P.V.C is only poly vinyl chloride plastic and P.V.A is poly vinyl acetate plastic.
Qs.68 What is Bakelite?
Ans. It is a plastic, which is condensation polymer of phenol and formaldehyde.
Qs.69 What is the difference between thermo-plastic & thermo-setting plastics?
Ans. “Thermo-plastics” are those which may be moulded several times by
liquefaction without any chemical change e.g. poly vinyl plastic. Where
as “Thermo-setting plastic” are those which may be molded once at a time
of preparation and become decomposed on heating e.g. Bakelite.
Qs.70 What is the formula of phenol and formaldehyde?
Ans. Phenol is C6H5OH while formaldehyde is HCHO.
Qs.71 What is the formula of Aniline and Iodoform?
Ans. Aniline is C6H5NH2 while Iodoform is CHl3.
Qs.72 What are carbohydrates?
Ans. Carbohydrates are either polyhydroxy aldehydes or ketones or
substances which on hydrolysis yield these compounds i.e. polyhydroxy
aldehydes or ketones.
Qs.73 Why carbohydrates are also known as hydrates of carbon?
Ans. The general formula of carbohydrates may be Cx(H2O)y i.e. the ratio
between hydrogen and oxygen is same as that in water e.g. C6H12O16
Hence they are also known as hydrates of carbon.
Qs.74 Why carbohydrates are also known as saccharides?
Ans. They are also known as saccharides because various carbohydrates gives sweet taste.
Qs.75 What are mono-saccharides?
Ans. Monosaccharides are those carbohydrates which cannot be broken into
simpler substances on hydrolysis due to the reason that they consists
of single unit of polyhydroxy aldehyde or ketones e.g. glucose and
fructose.
Qs.76 What are disaccharides?
Ans. These carbohydrates gives two molecule of monosaccharides on hydrolysis e.g. Maltose, Lactose, and sucrose etc.
Qs.77 What are polysaccharides?
Ans. Those carbohydrates which consists of very large number of
monosaccharides units are known as polysaccharides units are known as
polysaccharides e.g. starch and cellulose etc.
Qs.78 What is the importance of carbohydrates in living beings?
Ans. Carbohydrates are of major importance to both plants & animals.
Human beings use it for many purposes only 65 percent of carbohydrates
are used in our diet. It is the chlorophyll in leaves and grass that
makes them green, plants gives carbohydrates during the process of
photosynthesis. Where plant take CO2 from the air and H2O from the soil
and the process occur.
Friendsmania.net
i.e. 6CO2 + 6H2O = C6H12O6 + 6O2
It may also used in for clothing (Cotton, Rayon, linon) and wood for building burning and making paper.
Qs.79 What are reducing sugars?
Ans. Those carbohydrates which are oxidized by Fehling’s solution and
contain free aldehydic group are known as reducing sugar e.g. maltose
and glucose etc.
Qs.80 What are non-reducing sugars?
Ans. Those carbohydrates which do not reduce Fehling’s solution by
forming red ppt and contain no free aldehydic group are called
non-reducing sugars e.g. fructose and sucrose etc.
Qs.81 What is Fehling’s solution?
Ans. It is a mixture of two solution i.e. A & B the solution “A”
contains copper sulphate solution while solution “B” contain a solution
of sodium potassium tatrate (alkaline medium) along with NoOH.
Qs.82 What is starch?
Ans. Starch is not a single molecule but a mixture of “Amylose” (water
soluble, blue colour with iodine) and “Amylopectin” (insoluble in water,
violet colour with iodine). The composition of the two is, amylose
10-20% and amylopectin 80-90%.
Qs.83 What is Benedict’s reagent?
Ans. An aqueous solution of cupric sulphate, sodium citrate and sodium carbonate is called Benedict’s reagent.
Qs.84 What is Tollen’s reagent?
Ans. Ammonical silver nitrate solution is known as Tollen’s reagent.
Qs.85 What is Roschell’s salt?
Ans. Sodium potassium tartarate is also known as Roschell’s salt. Which is used in the preparation of Fehling’s soluton.
Qs.86 What are Amino Acids?
Ans. The amino acids that occur in protein all have the – NH2 group and –
COOH group attached to the same carbon atom. They are thus alpha amino
acids, the carbon atom being the alpha carbon simplest formula by which
it can be represent is
H
│
R ― C ― COOH
│
NH2
Qs.87 What are proteins?
Ans. The complex nitrogenous organic compound found in living cell are
called proteins which on hydrolysis yield amino acids and these amino
acids linked together by a peptide bond.
OR
The polymers of amino acids containing large no of amino acids joined by peptide bond is called protein
Qs.88 What is peptide bond?
O
║
Ans. The acid amide ( - C – NH - ) or the linkage through which amino acids are linked in protein is known as peptide bond.
H O H
│ ║ │
H2N ─── C ── C ─── NH ── C ── COO
│ │
R R
Pipette Bond
Qs.89 What are simple protein?
Ans. The protein on hydrolysis give only simple amino acids are simple proteins e.g. Albumin, glubuiline etc.
Qs.90 What are conjugated proteins?
Ans. Those proteins which on hydrolysis give some other compounds along
with amino acids are commonly known as conjugated proteins e.g.
phospholecithine
Qs.91 What is meant by derived protein?
Ans. Derived proteins are the products obtained by the action of heat, enzyme or bychemical reaction.
Qs.92 What is the effect of heat on protein and what is the effect of HNO3?
Ans. By heating it coagulates (as in egg) while it becomes yellow by the action of HNO3.
Qs.93 What are fats?
Ans. They are esters of higher fatty acids (palmatic acid, stearic acid,
and oleic acid,) with glycerol and the esters are made up of an alcohol
part and an acid part.
R – C – OR , C2H6O3
║
O
Acid part Alcohol part
(Mainly glycerol)
Qs.94 Why oils are formed in liquid state at ordinary temperature?
Ans. Oils are in liquid state due to the presence of unsaturated fatty acids in which one OH group of glycerol is esterified.
Qs.95 Why fats are solid at room tempertature?
Ans. Fats are solid because they contain saturated acids with glycerol.
Qs.96 What is the general formula of fats and oils?
Ans. The general formula of fat and oil is as follows.
CH2 ───── OOCR1
│
CH ───── OOCR2
│
CH2 ───── OOCR3
Facts or oil (Here R-may be same or different)
Qs.97 What is the difference between a fat and an oil?
Ans. Fat is a solid at room temperature and contains saturated fatty
acids while oil is liquid and contains unsaturated fatty acids.
Qs.98 Write down the name and formula of saturated and unsaturated fatty acids found in fat & oil?
Ans. Palmatic acid C15H31 COOH saturated fattu acid.
Stearic acid C17H35 COOH saturated fatty acid.
Oleic acid C17H33 COOH saturated fatty acid.
.Qs.99 What is the formula of glycerol?
Ans. The formula is
CH2OH
│
CHOH Glycerol
│
CH2OH
Qs.100 What is Saponoifications?
Ans. Hydrolysis of fats or oil by mean of alkali is commonly known as Saponoification.
CH2 – OOC – R1 CH2 – OH ROONa
│ │ │
CH – OOC – R2 + 3NAOH → CH – OH + RCOONa
│ │ │
CH2 – OOC – R3 CH2 – OH RCOONa
Glycerine SOAP
Qs.101 What is soap?
Ans. The sodium or potassium salt of a fatty acid is called a soap e.g.
RCOONa
│
RCOONa Soap
│
RCOONa
Chemistry XII Viva Notes 2nd Year Chemistry Notes http://karachiboardnotes.blogspot.com/ Chemistry XII Viva Notes Friendsmania.net Qs.1 Wh...
Chemistry XII Fill in the Blanks
2nd Year Chemistry Notes
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Chemistry XII Fill in the Blanks
Five Year Papers
1. Plastics are polymers of __________.
2. From crude oil, additional quantity of petrol is obtained by __________ process.
3. Tertiary alkyl halides react by __________ reaction mechanism.
4. __________ period is incomplete.
5. Elements, which follow actinium, are called __________ elements.
6. Ionic hydrides are also called __________.
7. Compounds with the general formula CnH2n + 2O are called __________.
8. Resorcinol is not an alcohol but a __________.
9. A ketone contianing different alkyl radicals is called __________ ketone.
10. The hydrolysis of fats and oils with a strong alkali is called __________.
11. __________ is active in the stomach of young children.
12. The chemical name of Lunar caustic is __________.
13. Aluminium resists corrosion due to the formation of __________.
14. EDTA is a __________ ligand.
15. The chemical formula of rust is __________.
16. Sub-Group B elements are called __________ elements.
17. The hybridization of carbon in graphite is __________.
18. The chemical name of vitamin B2 is __________.
19. The reactions between metallic sodium and alkyl halides are called __________ reaction.
20. The fractional distillation of crude petroleum yields only __________% petrol.
21. Starch and Cellulose are the examples of __________ carbohydrates.
22. AgCl dissolves in ammonia to form __________.
Chapter 1
Periodic Classification of Elements
1. In 1913 Moseley, A British physicist, found that a __________ is the fundamental property of an atom.
2. In the modern Periodic table recommended by the International Union
of Pure and Applied Chemistry (IUPAC) in 1982, the elements are arranged
in the ascending order of __________.
3. Horizontal rows of elements in the periodic table are called __________.
4. The vertical columns of elements arranged in the Periodic table are called __________.
5. In the Modern Periodic Table there are __________ periods.
6. The first period of Modern Periodic Table contains __________elements.
7. Hydrogen lies in __________ Period.
8. Helium lies in __________ Period.
9. All the elements belonging to the second period are __________.
10. Second period contains __________ elements.
11. The elements of the second period of the modern Periodic table are __________.
12. Third period of periodic table contains __________ elements.
13. The elements of the fourth period of the modern periodic table are __________.
14. Fourth period of Modern Periodic Table contains __________ elements.
15. Fifth period of Modern Periodic Table contains __________ elements.
16. Those elements, which have ‘d’ orbitals in the process of completion in the form of ions or atoms, are called __________.
17. Elements in IB group are called __________.
18. Those elements, which involve ‘s’ orbital filling in their valence shells, are called __________.
19. The sixth period of Modern Periodic Table contains __________ elements.
20. The longest period of modern Periodic Table is __________.
21. The eight ‘s’ and ‘p’ block elements in the 4th and 5th periods are known as __________.
22. The elements of group IA and IIA are classified as __________ elements.
23. The seventh period of modern Periodic table contains __________ elements.
24. The elements on the right hand side of the Periodic table are called __________.
25. The outer most shell involved in chemical bonding are called __________.
26. The number of electrons in the outermost or valence shells is called __________.
27. Na2O is strongly __________ in nature.
28. Cl2O7 is strongly __________ in nature.
29. Greater the electronegativity of an element, stronger is the __________ character of its oxide.
30. In case of transition elements, the last electrons are received by __________.
31. Elements in group IB, IIB through VIIB are known as __________.
32. Elements in group IB, IIB through VIIB are known as __________.
33. Elements in the group VI A and __________ are the most active non-metals.
34. The correct order of second ionization potential of carbon, nitrogen, oxygen and fluorine is __________.
35. The elements having seven valence electrons are known as __________.
36. The elements of group IIIA to VIIA are called __________.
37. Maximum number of electrons present in sixth period is __________.
38. The elements of group VIIIA are called __________.
39. In case of inner transition elements the last electrons are received by __________.
40. In case of outer transition elements the last electron are received by __________.
Chapter 2
Hydrogen
1. Hydrogen was first prepared by Cavendish in 1766 by the action of __________.
2. Hydrogen is evolved by the action of cold diluted HNO3 on __________.
3. Hydrogen is found in nature in combined state. The most abundant compound of hydrogen is __________.
4. The electronic configuration of hydrogen atom is __________.
5. Hydrogen forms slat like hydrides with the elements of __________.
6. Hydrogen forms interstitial hydrides with the elements of __________.
7. An example of covalent hydride is __________.
8. Alkali metals need __________ electron to complete their outermost shells.
9. The number of isotopes of hydrogen is __________.
10. 1H1 is symbol of __________.
11. 1H2 is the symbol of __________.
12. 1H3 is the symbol of __________.
13. The number of neutrons in the nuclei of tritium atom is __________.
14. The number of neutrons in the nucleus of protium is __________.
15. The mass number of deutrium is __________.
16. Tritium is present to the extent of one atom in __________ atoms.
17. Chemical formula of heavy water is __________.
18. Hydrogen is obtained industrially as a by-product during electrolysis of __________.
19. Hydrogen is commercially prepared by the thermal decomposition of
20. Hydrogen burns in air with __________ flame.
21. Density of hydrogen is about of 1/14th of that of __________.
22. The electronegativity of hydrogen is __________.
23. The bond energy of hydrogen is __________.
24. Hydrogen liquefies at __________.
25. Hydrogen freezes at __________.
26. The symbol of hydride ion is __________.
27. Hydrogen burns on ignition in the presence of oxygen to produce __________.
28. Hydrogen reacts on heating with P directly to form __________.
29. The hydrides formed by the combination of non-metals of groups IVA, VA, VIA and VIIA with hydrogen are called __________.
30. LiAlH4 is an example of __________.
31. The atomic weight of heavy hydrogen is __________.
32. __________ is the commonest gas in the atmosphere.
33. The element, which does not make salt like hydride is __________.
Chapter 3
S-Block Elements
1. In s-block elements the outermost orbitals are filled with __________ electrons at the outer most.
2. S-block elements consist of __________.
3. The colour of the flame of potassium is __________.
4. On bunsen flame sodium gives __________.
5. On bunsen flame Potassium gives __________.
6. On bunsen flame Cesium gives __________.
7. On bunsen flame Calsium gives __________.
8. On bunsen flame Strontium gives __________.
9. On bunsen flame Barium gives __________.
10. Alkaline earth metals are relatively __________ reactive than alkali metals.
11. An apparatus used for commercial preparation of sodium is named as __________.
12. Baking soda is also called __________.
13. The radius of K-atom is 2.31A°. The radius of K+ will be __________.
14. Bicarbonate of alkali metals and alkaline earth metals are formed by
passing __________ through a solution of the carbonates of alkali
metals or a suspension of carbonates of alkaline earth metals in water.
15. Metallic sodium was first obtained by Sir H. Davy in 1807 by the electrolysis of fused __________.
16. Gay Lussac and Thenard in 1811 prepared sodium by reducing sodium hydroxide with __________.
17. The process in which sodium was prepared by distilling sodium
carbonate with carbon and a small amount of chalk as a catalyst was
introduced by __________.
18. Down’s cell is used for the production of __________.
19. The density of sodium metal is __________.
20. Melting point of sodium is __________.
21. Boiling point of sodium is __________.
22. The annual consumption of NaCl is about __________.
23. __________ percentage of NaCl is present in sea water.
24. __________ percentage of NaCl or Common salt is present in rock salt.
25. Sodium carbonate is generally called __________.
26. Sodium carbonate is prepared by __________.
27. Aqueous solution of sodium carbonate on heating gives sodium carbonate and __________.
28. __________ is medically used for the treatment of hyperacidity in the stomach.
29. In firge extinguishers __________ is used as a source of carbon dioxide.
30. Mixture of sodium bicarbonate and crystals of vegetable acids, e.g. tartaric acid or citric acid is known as __________.
31. Anhydrous sodium carbonate is called __________.
32. Industrial use of sodium carbonate is in the manufacture of __________.
33. __________ is used in the smelting of iron ores of high sulphur content.
34. Sodium Hydroxide is manufactured on large scale by electrolysis of aqueous solution of __________.
35. Nelson’s cells is used for the manufacture of __________.
36. Castner-Kellner Process is used for the production of __________ on industrial scale.
37. The melting point of NaOH is __________.
38. NaOH decomposes into its elements at about __________.
39. Bleaching powder is manufactured by treating lime with chlorine in __________.
40. The colour of bleaching powder is __________.
41. Bleaching powder smells strongly like __________.
42. When bleaching powder is treated with strong solution of ammonia, __________ gas is evolved.
43. Calsium sulphate occurs in nature as dihydrate salt called __________.
44. Gypsum can be prepared by the action of dilute sulphuric acid on __________.
45. At __________ temperature gypsum loses its three fourth of water.
46. Gypsum is sparingly soluble in water. Its solubility increases with rising temperature up to __________.
47. Magnesium sulphate is usually sold as hydrated salt called __________.
48. Epsom salt is prepared from magnesite MgCO3 on boiling with dilute __________.
49. Epsom salt loses six molecules of water at __________.
50. Epsom salt becomes anhydous at __________.
51. Epsom salt is converted into magnesium oxide by heating it with carbon at about __________.
52. __________ is used in medicine as purgative.
Chapter 4
P-Block Elements
1. The elements, which belong to III-A group to VIII-A group, are called __________.
2. In p-block elements the metallic character __________ down the group.
3. In p-block elements the orbital in the process of completion is __________.
4. Crystalline boron is a hard substance which is __________ in colour.
5. Out of all the elements of group IIIA, the highest Ionization potential is for __________.
6. Boron possesses close resemblance with __________.
7. Orthoboric acid is prepared by the acidification of hot concentrated
solution of borax with calculated quantity of __________.
8. In the Hall-Berou.t process for producing aluminium the substance produced at the cathode is __________.
9. Hydrogen gas many be produced by the reaction of aluminium with a concentrated solution of __________.
10. The most widely distributed element in the earth’s crust after oxygen and silicon is __________.
11. Aluminium resists corrosion due to the formation of a coat of __________.
12. Hall’s Process is used for the production of __________.
13. Duralum is an alloy which contains Mg + Cu + __________ + Mn.
14. The group IV-A of the periodic table consists of __________.
15. Diamond has a high refractive index of __________.
16. At 700°C graphite burns in air to form __________.
17. Red lead is commonly known as __________.
18. __________ is the product of thermal decomposition of sodium bicarbonate.
19. Lead Monoxide is a yellow powder and also called __________.
20. Nitrogen, phosphorus, arsenic, antimony and bismuth are the members of the group __________.
21. All members of group VA exhibit maximum oxidation state of __________.
22. The shape of diamond is __________.
23. On an industrial scale nitric acid is prepared by __________.
24. Poisonous gas present in the exhaust fumes of car is __________.
25. The boiling point of nitric acid is __________.
26. The freezing point of nitric acid is __________.
27. Oxygen, sulphur, selenium, tellurium and polonium are the members of group __________.
28. The first four members of the group VI-A are collectively called __________.
29. There are __________ electrons in the valence shell of elements of group VI-A.
30. The maximum valency of oxygen is __________.
31. Oxygen has __________ allotropic forms.
32. The transition temperature of sulphur is __________.
33. X-rays analysis shows that __________ sulphur consists of chains of sulphur atoms.
34. The purest H2S is obtained by passing vapours of sulphur and hydrogen over finely divided __________ at 450°C.
35. __________ was first prepared in the laboratory by Jabir Bin Hayyan.
36. __________ is called king of chemicals.
37. Lead Chamber process is used for the preparation of __________.
38. Contact Process is used for the production of __________.
39. __________ is called Oleum.
40. Freezing point of pure sulphuric acid is __________.
41. Dilute sulphuric acid dissolves many metals with the evolution of __________ and the corresponding sulphates are formed.
42. Formic acid is converted into carbon monoxide by the action of concentrated __________ and heating.
43. Gases such as oxygen, hydrogen, carbon dioxide, chlorine and sulphur
dioxide are often dried by bubbling them through __________.
44. Concentrated sulphuric acid absorbs sulphur trioxide forming __________.
45. Carbon is oxidized to __________ in the presence of sulphuric acid.
46. In a process called pickling the metal sheets are soaked in __________ to remove rust or by chemical action.
47. Phosphine may be produced by the action of water on __________.
48. In the refining of petroleum, __________ is employed to remove tarry materials and sulphur compound.
49. In the Ostwald process, the substance which is used to oxidize NH3 is __________.
50. In the periodic table, halogens, namely fluorine, chlorine, bromine, iodine and astatine are placed in group __________.
51. The brown gas formed when metals reduce HNO3 is __________.
52. __________ is used as catalyst in the Contact Process.
Chapter 5
Transition Elements
1. Annual production of antimony being mined in Pakistan is __________.
2. Annual production of Orchro being mined in Pakistan is __________.
3. Annual production of Chromite being mined in Pakistan is __________.
4. Annual production of manganese being mined in Pakistan is __________.
5. Transition elements other than Sc, Y and Ti have density above __________.
6. Due to d-d transition of electrons, Cu2+ ion appears __________ in colour.
7. The colour of Fe3+ ion is __________.
8. The colour of Fe2+ ion is __________.
9. The colour of Cr3+ ion is __________.
10. The colour of Mn3+ ion is __________.
11. The colour of Mn2+ ion is __________.
12. The colour of the fmale of potassium is __________.
13. The magnetic moment is related to the number of unpaired electron ‘n’ by the equation __________.
14. All the 3-d series elements show an oxidation state of __________ in addition to higher oxidation states except Sc.
15. The majority of transition metal’s ion complexes contain __________ ligands surrounding the central octrahedrally.
16. Copper is known since __________.
17. In Pakistan copper mines at Saindak in __________ were first discovered in 1962.
18. It is estimated that the Saindak mines will yield an annual
production of __________ tones of copper from its sulphide ore for a
period of 16 years on the commencement of production.
19. __________ percentage of total copper metal is obtained from sulphide ore.
20. The colour of copper is __________.
21. Copper becomes __________ when it is heated.
22. Copper melts at __________ °C.
23. Cu2O is __________ in colour.
24. The colour of CuO oxide is __________.
25. When copper is heated in air, then CuO + __________ are formed.
26. Bronze contains __________% Cu and 10% Sn.
27. __________ is prepared in the laboratory by the action of dilute sulphuric acid on cupric oxide or cupric carbonate.
28. __________ is prepared by dissolving metallic silver in warm dilute nitric acid.
29. The highest common oxidation state of chromium is __________.
30. __________ is prepared in the laboratory by the addition of
potassium chloride to hot concentrated solution of sodium dichromate.
31. __________ is used an an indicator in silver nitrate titration for the estimation of halide ions.
32. Potassium permanganate oxidizes acid in presence of dilute __________.
33. __________ is used as a disinfectant for purification of water.
34. __________ is used in bleaching paper pulp.
35. The rusting of iron is catalyzed by __________.
36. Conversion of any metal into its oxide by the action of environment is called __________.
37. Rusting of iron is an example of __________.
38. Aluminium resists the process of corrosion due to the formation of __________.
39. An alloy of iron, which contains chromium 18%, nickel 8% and carbon 0.18% is __________.
40. The black image on an exposed and developed photographic film is composed of __________.
41. In photography printing is accomplished by using an emulsion of __________.
42. All transition elements are __________.
43. Iron rust has the composition of __________.
44. When hydrated, Fe2+ ions are __________.
Chapter 6
Organic Chemistry
1. The main component of coal is __________.
2. When coal is heated in the absence of air, temperature ranging from
__________, it is converted into coke, coal gas and coal tar.
3. The octane number of gasoline may also be increased by ading __________ as knoc inhibitor.
4. In Houdry process the breaking down of long-chain hydrocarbons is
accelerated in the presence of a catalyst, made up of a mixture of
__________.
5. The process of cracking takes place between temperature __________.
6. Molecular formula of ethers is __________.
7. Alkanes have general formula __________.
8. How many isomers can be obtained from the alkane C6H14.
9. Each alkane differs from its neighbours by __________.
10. The structural formula of ethane is __________.
11. Alkenes have general formula __________.
12. Alkyl halides have general formula __________.
13. On destructive distillation of 1000 kg of coal amount of coal tar formed is __________.
14. Natural gas consist of methane __________.
15. An alkane forms isomers if the number of least carbon atoms is __________.
16. The functional group of alkyle halids is __________.
17. The formula of alkane is __________.
18. The functional group o primary amines is __________.
19. The functional group of ether is __________.
20. The functional group of primary alcohol is __________.
21. The formula of methanol is __________.
22. The formula of ethanol is __________.
23. The formula of propanal is __________.
24. The formula of butanal is __________.
25. Formula of formic acid is __________.
26. The formula of acetic acid is __________.
27. The formula of propnoic acid is __________.
28. The formula of butyric acid is __________.
29. The formula of valeric acid is __________.
30. The formula of capric acid is __________.
31. Phenyl group is represented by __________.
32. The molecular formula of ethane is __________.
Chapter 7
Hydrocarbons
1. An example of alkane is __________.
2. __________ is the smallest hydrocarbon.
3. Natural gas consists of about __________% of methane.
4. A reaction catalyzed by the presence of __________ is called a photochemical reaction.
5. C2H2 reacts with HCl to produce __________.
6. __________ is used as catalyst in the oxidation of methane.
7. Methane reacts with superheated steam, on passing through hot tubes
containing a __________ catalyst to yield carbon monoxide and hydrogen.
8. In methane H – C – H bond angles are __________.
9. The structural formula of ethylene is __________.
10. __________ is called ozone.
11. When ethene is passed through a dilute alkaline solution of KMnO4, the pink colour of the solution __________.
12. __________ reagent distinguishes ethylene from acetylene.
13. __________ polymerizes at 100 atmosphere pressure and 400°C to give polyethylene.
14. The polyethene produced in the presence of __________ and titanium
tetrachloride as catalyst, shows improvement in its properties such as
higher softening temperature, low permeability and greater rigidity.
15. __________ is called Dutch Liquid.
16. General formula of alkynes is __________.
17. __________ is called Acetylene.
18. Carboxylic acids combine with acetylene in the presence of
__________ as catalyst, forming vinyl esters and the reaction is termed
as Vinylation.
19. When a mixture of acetylene and nitrogen is submitted to an electric discharge, it forms __________.
friendsmania.net
20. When acetylene is passed through a copper tube at about 300°C it polymerizes to __________.
21. The brand of synthetic rubber is made by Polymerization of __________.
22. The process in which orbitals of different energies and shapes mix
with each other to give equivalent hybrid orbital is called __________.
23. The sp3 signifies that each sp3 orbital is made up of s and p orbitals in the ratio of __________.
24. A molecule of methane has __________sigma bond(s).
25. A molecule of ethane has __________ sigma bond(s).
26. The sp3 hybridization occurs when carbon is bonded to __________ other atoms.
27. Sp2 hybrid orbitals are composed of s and p orbitals in the ratio of __________.
28. __________ bond is weaker.
Chapter 9
Organic Compounds
1. The general formula of alcohol is __________.
2. The general formula of aldehyde is __________.
3. Alcoholic fermentation is brought out by the action of __________.
4. The general formula of carboxylic acid is __________.
5. The general formula of esters is __________.
6. The general formula of ketone is __________.
7. The general formula of ether is __________.
8. The general formula of phenol is __________.
9. Methyl alcohol is used as the starting matrial in the manufacture of __________.
10. The formula of ethyl alcohol is __________.
11. To start the reversibility Estrification we use concentrated
__________ used as absorbent of water produced during the reaction.
12. Dehydration means removal of __________.
13. The compound formed when silver powder is ehated with chloform is __________.
14. __________ is used as a fuel for internal combustion engines in many European countries and Brazil.
15. The formula of formaldehyde is __________.
16. The derivatives of carboxylic acids are obtained by replacing the –OH group of the carboxylic group with –OH and __________.
17. The formula of Fehling’s solution is __________.
18. The formula of Iodoform is __________.
19. Melting point of Phenol is __________.
20. Boiling point of Phenol is __________.
21. Phenol when treated with __________, yields both ortho and para sulphonic acids.
22. General formula of Grignard’s Reagent is __________.
23. The formula of Cyanogen chloride is __________.
24. The formula of Chloramine is __________.
Chemistry XII Fill in the Blanks 2nd Year Chemistry Notes http://karachiboardnotes.blogspot.com/ Chemistry XII Fill in the Blanks Five Yea...
Chemistry True and False 2nd year 2010
2nd Year Chemistry Notes
http://karachiboardnotes.blogspot.com/
Chemistry True and False 2nd year 2010
1. PVC is a polymer of benzene.
2. Fructose is a reducing sugar.
3. The deficiency of vitamin C causes scurvy.
4. Methanol causes blindness.
5. Diamond is the hardest known substance in the world.
6. The properties of boronoxide are acidic.
7. Graphite is a good conductor of electricity.
8. The deficiency of vitamin A causes night-blindness.
9. Wurtz reaction can be used to prepare Methane.
10. Bakelite is polymer of phenol and alkyl halide.
11. The heat of hydration of Li+ ion is equal to that of Cs+ ion.
12. The molecule of H2S is non-linear.
13. CuSO4 in excess of NH3 forms Cu(OH)2.
14. Compounds have benzene ring are called aeromatic.
15. Polyethenes are the most common plastics.
16. Lead-containing paints are banned because of the high cost.
17. Na2CO3 decomposes on heating.
18. The atomic weights of isotopes are different because of the difference in the number of protons.
19. Gastric juice is pale yellow in colour.
20. Ascorbic acid is enzyme.
21. The main function of carbohydrates is to circulate blood.
22. The preparation of vegetable ghee is a dehydrohalogenation process.
23. There are eight periods and seven groups in the Periodic table.
24. Hydrated copper sulphate is a white crystalline solid.
25. Pure diamond is colourless.
26. The first transition series starts from scandium and ends at zinc.
27. Markownikoff’s rule is not applicable to alkynes.
28. Methylated spirit is ethanol containing some methanol.
29. A functional group is the most reactive part of the molecule.
30. Vitamins A.D.K are water-soluble vitamins.
31. Kerosene oil is a petroleum product.
Answers to True and False
Five Year Papers
1. False
2. True
3. True
4. True
5. False
6. True
7. True
8. False
9. False
10. False
11. True
12. False
13. True
14. True
15. False
16. True
17. False
18. False
19. False
20. False
21. False
22. False
23. False
24. False
25. True
26. True
27. False
28. True
29. True
30. False
31. True
Chemistry True and False 2nd year 2010 2nd Year Chemistry Notes http://karachiboardnotes.blogspot.com/ Chemistry True and False 2nd year...
Chemistry MCQs 2nd year
2nd Year Chemistry Notes
http://karachiboardnotes.blogspot.com/
Chemistry MCQs 2nd year
Five Year Papers
1. On passing steam over red-hot coal we get __________.
(Water gas, Ethane, Carbonmonoxide)
2. ‘d’ and ‘f’ block elements are called __________.
(Heavy metals, Rare elements, Transition elements)
3. The correct formula of pyrosulphuric acid is __________.
(H2SO4, H2S2O7, H3S2O5)
4. Aqua regia is mixture of one part of __________ by volume and three parts of __________.
(H2SO4, H3PO4, HNO3, HCl)
5. Heavy hydrogen is also called __________.
(Proteum, Deuterium, Hydronium)
6. When boric acid (H3BO3) is heated of 140°C, it forms __________.
(Boric Acid, Pyroboric acid, Metaboric acid)
7. Photographic film is made of sheets of __________.
(Cellulose Acetate, P.V.A, Nylon)
8. C4H8 is a saturated hydrocarbon because it is __________.
(Cyclic, Open chain, Polymer)
9. n-Octane is __________ at room temperature.
(Gas, Liquid, Semi-solid)
10. The compound formed between an element A of group IIIA and an element B of group VIA has the formula __________.
(AB, A2, B3, A2B3)
11. The oxide formed by AI is __________.
(Acidic, Amphoteric, Basic)
12. Bakelite is a polymer of __________ and form aldehyde.
(Ethane, Methanol, Phenol)
13. The plastics, which can be heated only once, are known as __________ plastics.
(Perspex, Thermoplastic, Thermosetting)
14. The deficiency of __________ in the human body is the cause of diabetes.
(Insulin, Alamin, Ptyalin)
15. If the level of cholesterol increases in the blood serum, it causes __________.
(Diabetes,Heart attact, High blood pressure)
16. The formula of baking soda is __________.
(NaHCO3, Na2CO3, Na2CO310H2O)
17. The formula of Plaster of Paris is __________.
(CaSO4.2H2O, 2CaSO4.H2O, (CaSO4)2H2O)
18. The atoms of the elements belonging to the same period of the Periodic table have __________.
(Same number of protons, same number of neutrons, same number of valence shells)
19. Sodium thiosulphate is used in photography because of its __________.
(Reducing power, Complex formation, Oxidizing behaviour)
20. The outer electronic configuration of copper is __________.
(4s14d10, 4s23d10, 4s13d10)
21. H2S solution in water is __________.
(Neutral, Acidic, Basic)
22. __________ is isomer of ethanol.
(CH3OH, CH3OCH3, C6H5OH)
23. Petroleum is a mixture of __________.
(Alkanes and alkenes, aromatic hydrocarbons, all of these)
24. Glucose is __________.
(Reducing sugar, oxidizing sugar, none of these)
25. Pentane shows __________.
(Two isomers, three isomers, four isomers)
Chapter 1
Periodic Classification of Elements
1. __________ elements have been discovered so far.
(100, 110, 120, 150)
2. so far 110 elements have been discovered. Out of these __________ elements are naturally occurring.
(100, 96, 92, 94)
3. __________ classified the then known elements into metals, non metals and their derivatives.
(Dobreiner, Al-Razi, Newlands, Mendeleeve)
4. In 1817, a German chemist, __________ made use of the idea of
relationship between atomic weights and properties of elements for the
classification of elements.
(Dobreiner, Al-Razi, Newlands, Mendeleeve)
5. __________ presented the law of triads.
(Dobreiner, Al-Razi, Newlands, Mendeleeve)
6. Dobreiner’s work led to the law of triads which states that __________.
(Atomic weight of any one lement was found to be approximately the mean
of the other two elements of triad, Atomic weight of the middle element
was found to be approximately the mean of the other two elements of a
triad, Atomic number of any one element was found to be approximately
the mean of the other two elements of a triad, Atomic number of the
middle element was found to be approximately the mean of the other two
elements of triad)
7. The law of octaves was given by __________.
(Dobreiner, Al- Razi, Newlands, None of these)
8. Law of octaves states that __________.
(The properties of every 6th element from the given one were similar to
the first, the properties of every 9th element from the given one were
similar to the first, the properties of every 8th element from the given
one were similar to the first, the properties of every 7th element from
the given one were similar to the second)
9. “Physical and chemical properties of elements are periodic functions of their atomic weight.” This is called __________.
(Dobereiner’s Law of Triads, Newlands’ Law of Octaves, Mendeleev’s Periodic Law, None of these)
10. Lother Meyer arranged the elements in order of their increasing atomic weights and found that __________.
(Physical propertis of the elements were the periodic function of their
atomic weights, chemical properties of the elements were the periodic
function of their atomic number, physical properties of the elements
were the periodic function of their atomic number, chemical properties
of the elements were periodic function of their atomic weights)
11. Mendeleev’s Periodic table was based on __________.
(Atomic number, Atomic mass, Atomic volume, Electronic Configuration)
12. Mandeleev formulated a rule for the classification of elements and concluded that __________.
(Physical and chemical properties of the elements are periodic functions
of their atomic numbers, physical and chemical properties of the
elements are periodic functions of their atomic weights, physical
properties of the elements are periodic function of their atomic
weights, Chemical properties of the elements are periodic functions of
their atomic numbers)
13. Modern Classification of elements is based on __________.
(Doberiner’s law of Triads, Newlands’ law of Octaves, Mendeleev’s Periodic Table, None of these)
14. Excluding H and He, the smallest element in the periodic table is __________.
(Lithium, Fluorine, Cesium, Iodine)
15. “Physical and chemical properties of elements are the periodic
functions of their atomic numbers.” This is called __________.
(Law of Triads, Law of Octaves, Periodic Law, None of these)
16. Moseley’s work led to the periodic law, which states that __________.
(the number of the electrons in the 1s energy level increases as the
atomic number increases, The properties of the elements are a periodic
function of their atomic masses, The x-rays spectra of the elements are
more complex than the optical spectra, The properties of elements are
the periodic function of their atomic number)
17. A pair of elements in the same family in the periodic table classification is __________.
(Chlorine and carbon, calcium and aluminium, nitrogen and neon, sodium and potassium)
18. In the period, the elements are arranged in strict sequence in order of __________.
(Increasing charges in the nucleus, increasing atomic weight, increasing
number of electrons in valence shell, increasing valency)
19. Most of the known elements are metals of __________ of periodic table.
(d-block, p-block, III-group, Zero block)
20. __________ reflects combining capacity of an element.
(Valency, atomic number, ionization energy, ionization potential)
21. As we move from left to right in second period of the periodic table, the gram atomic volume of the elements __________.
(Increases at a constant rate, remains unchanged, decreases, will change indefinitely)
22. The volume in cubic centimeters occupied by one gram atom of the element is called __________.
(Atomic Volume, Atomic weight, Mass number, None of these)
23. In a __________, atomic volume increases with atomic number, from
top to bottom, as new shells are added up with increase in atomic
number.
(Group, Period, Sub-group, None of these)
24. __________ of the following is a transition element.
(Ni, Rb, Al, As)
25. On moving from left to right across a period in the periodic table, the size of atom generally __________.
(decreases, increases, remains constant, decreases up to IV A group and then increases)
26. The amount of energy required to remove an electron from an atom of an element in the gaseous state I called __________.
(Ionization Potential, Ionization energy, Electron volt, both a and b)
27. Each vertical row of the periodic table includes elements with chemical characteristics that are in general __________.
(identical, similar, different, sometimes identical and sometimes differents)
28. The ionization energy __________ in a group from top to bottom with the increase in atomic size.
(Increases, decreases, remains constant, none of these)
29. The lowest ionization energies are found in the __________.
(inert gases, alkali metals, Transition elements, Halogens)
30. Ionization energy is lowest for __________.
(Inert gases, alkali metals, halogens, alkaline earth metals)
31. In the periodic table, the highest ionization energies are for __________.
(Halogens, Noble gases, Alkali metals, Chalcogens)
32. The atomic weight of an element divided by its density is called __________.
(Atomic mass, Atomic volume, Atomic density, Atomic number)
33. Elements in the same family __________.
(have same atomic number, have the same molecular weight, have similar
chemical properties, constitute a group of elements with the same
electronic configuration)
34. In a given period, the alkali metals have __________.
(smallest atomic size, lowest ionization energy, lowest density, highest electron affinity)
35. Of the following given elements __________ atom has the highest ionization energy.
(Be, F, N, Ne)
36. The value of ionization energy __________ in a period from left to right due to the decrease in atomic size.
(increases, decreases, remains constant, None of these)
37. __________ is the most electronegative element.
(Fluorine, Iodine, Oxygen, Sodium)
38. The unit of ionization energy is __________.
(Joule, Calorie, electron volt, none of these)
39. Of the following elements, __________ element has the highest first ionization potential.
(Boron, carbon, nitrogen, oxygen)
40. The unit of ionization potential is __________.
(Joule, joule per mole, calorie per mole, none of these)
41. In a period, the ensity of normal elements first __________ and then
__________ after reaching a maximum value somewhere in the middle.
(Increases, decreases, remains constant, none of these)
42. Most of the known elements are __________.
(Rrystalloids, Metals, Metalloids, Non metals)
43. Melting and boiling points gradually __________ in a periodic table from left to right up to the middle.
(increases, decreases, remains constnt, none of these)
44. The electropositive elements form __________.
(acidic oxides, basic oxides, neutral oxides, none of these)
45. __________ of the following elements has the lowest first ionization energy.
(Na, F, I, Cs)
46. The electronegative elements form __________.
(Acidic oxides, Basic oxides, Neutral oxides, none of these)
47. __________ is the most volatile compound.
(HI, HCl, HBr, HF)
48. The ionization energy of nitrogen is more than oxygen because of __________.
(more attraction of electrons by the nucleus, more peneration effect,
the extra stability of half filled p-orbitals, the size of nitrogen atom
is smaller)
49. The elements of group IIA are called __________.
(Metals, Non-metals, Alkaline earth metals, Transition elements)
50. __________ ion has the largest radius.
(Al+3, Cl-, F-, O-2)
51. __________ atom has the smallest size.
(C, F, Li, Rb)
52. __________ of the following has highest first ionization energy.
(Br, Cl, F, I)
53. The most electropositive among the following elements is __________.
(Fe, Na, Cs, Pb)
Chapter 2
Hydrogen
1. Large amounts of atomic hydrogen are present in the atmosphere of __________.
(Earth, Sun, Moon, none of these)
2. Hydrogen atom contains __________ electrons.
(1, 2, 3, 4)
3. During the electrolysis of water hydrogen is liberated at the __________.
(Anode, Cathode, Diode, none of these)
4. The atomic weight of hydrogen is __________.
(1.00, 1.008, 1.08, 1.800)
5. In nature hydrogen exists in __________.
(Gaseous state, Solid state, Liquid state, Plasma state)
6. __________ is the lightest gas.
(Nitrogen, Helium, Oxygen, Hydrogen)
7. Alkali metals do not exist in __________.
(Monoatomic, Diatomic, Triatomic, none of these)
8. Hydrogen generally combines with other elements to form __________.
(Ionic bond, Covalent bond, Polar bond, none of these)
9. Hydrogen may be readily prepared by the action of water on __________.
(Fe, HCl, Zn, Na)
10. In organic compounds, __________ element is found in close association with hydrogen.
(C, N, O, none of these)
11. Ionic hydrides are usually __________.
(liquids at room temperature, good reducing agents, good electrical conductors in solid state, Easily reduced)
12. The atoms of the same element, which have the same atomic number but different mass numbers, are called __________.
(Isotopes, Actanides, Isobars, none of these)
13. The difference in atomic weights or mass numbers of the atoms of the same element is due to __________.
(Different number of electrons in them, different number of protons in
them, different number of neutrons in them, none of these)
14. A tritium nucleus has __________.
(one proton and two electrons, one proton and two neutrons, one neutrons and two protons, one proton and three neutrons)
15. Physical properties of elements depend upon the number of __________.
(Protons in the nucleus, neutrons in the nucleus, electrons in the valence shell, both protons and neutrons in the nucleus)
16. Chemical properties of elements depend upon the number of __________.
(electrons in the valence shell, protons in the nucleus, neutrons in the nucleus, protons and neutrons in the nucleus)
17. Chemical properties of elements depend upon their __________.
(Atomic number, Atomic weight, volume, none of these)
18. The hydronium ion is a/an __________.
(ion with formula H2O+, ion with the formula H3O+, free radical rather
than an ion, ion formed by removal of H- form a water molecules)
19. Hydrogen is an important constituent of __________.
(Water, Petroleum, Natural gas, all of these)
20. When steam is passed over red hot coke at 1000°C, a mixture of
carbon monoxide and hydrogen gas is produced. It is known as __________.
(Heavy water, Water gas, Phosgen gas, none of these)
21. The most suitable process for the separation of CO from water gas is __________.
(Bosch Proces, Lane’s Process, Electrolysis of water, None of these)
22. When steam is passed over iron at 500°C, magnetic oxide and hydrogen gas is produced. This is called __________.
(Bosch Process, Lane’s Process, Electrolysis, All of these)
23. The presence of an acid or base renders water __________.
(good conductor of electricity, poor conductor of electricity, very bad conductor of electricity, all of these)
24. The process of loss of oxygen from a substance or addition of hydrogen is called __________.
(Oxidation, Reduction, Hydrogenation, None of these)
25. Hydrogen is a very good __________.
(Reducing agent, Oxidizing agent, Reducing agent as well as oxidizing agent, none of these)
26. Lowering of oxidation state of a metal is termed s __________.
(Oxidation, Reduction, Hydrogenation, All of these)
27. The process of addition of hydrogen (H2) to a molecule is called __________.
(Oxidation, Reduction, Hydrogenation, all of these)
28. Formation of vegetable ghee from vegetable oil is an example of __________.
(Oxidation, Reduction, Hydrogenation, all of these)
29. Ethylene can be hydrogenated to __________ under pressure at about 300°C, when double bond is changed to single compounds.
(Methane, Ethane, Ethyne, None of these)
30. Hydrogen reacts with halogens to give __________.
(Hydrogen halides, hydrogen hydrides, hydrogen sulphides, All of these)
31. Hydrogen is used in the manufacture of __________.
(Fertilizers, CO2, O2, None of these)
32. Hydrogen at the time of its generation during chemical reaction is in the form of atomic state and is called __________.
(Ionic Hydrogen, Nascent hydrogen, atomic hydrogen, none of these)
33. Hydrogen molecule consists of two atoms linked together by a strong __________.
(Ionic bond, Covalent bond, Hydrogen bonding, None of these)
34. Nascent hydrogen is used in the reduction of __________.
(Ionic compounds, Organic compounds, Inorganic compounds, none of these)
35. The compounds formed between two elements are called __________.
(Hydrides compounds, Binary compounds, Tertiary compounds, None of these)
36. Hydrogen reacts with some elements to form binary compounds called __________.
(Halides, Hydrides, Oxides, all of these)
37. The hydrides formed by the transfer of electrons from electropositive metals to hydrogen are called __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)
38. NaH is an example of __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)
39. Ionic hydrides ionize to produce __________.
(H-ion, OH-ion, H+ion, all of these)
40. The hydrides, which are good conductors of electricity in the fused state, are called __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides)
41. Covalent hydrides generally exist in __________.
(Solid state, Liquid state, Gaseous state, all of these)
42. Covalent hydrides are prepared by the direct action of __________.
(metals with hydrogen, non-metals with hydrogen, transition elements with hydroge, none of these)
43. Hydrides, which are non-stoichimetric in nature, are called __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides
44. The law of chemical combination is not obeyed by __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides
45. Electron deficient hydrides are called __________.
(Ionic hydrides, covalent hydrides, Complex hydrides, Interstitial hydrides
46. Hydrogen occurs in __________.
(One isotopic forms, two isotopic forms, three isotopic forms, four isotopic forms)
47. Atomic hydrogen is __________.
(More reactive than molecular hydrogen, less reactive than molecular
hydrogen, very less reactive than molecular hydrogen, all of these)
48. The process of addition of hydrogen to a molecule is called __________.
(Halogenation, Hydrogention, Sulphonation, Reduction)
Chapter 3
S - Block Elements
1. Out of all the elements of group IA, the highest atomic number is for __________.
(Na, Cs, Rb, K)
2. Out of all the elements of group IA, the highest melting and boiling point is for __________.
(Li, Na, Rb, K)
3. __________ of the following elements has highest ionization potential.
(K, Rb, Cs, Li)
4. Out of all the elements of group IA, the highest heat of hydration is for __________.
(Li, Na, K, Rb)
5. __________ of the elements has highest melting and boiling point.
(Be, Ca, Mg, Ba)
6. __________ of the following elements have highest oxidation potential.
(Na, Li, Rb, K)
7. Out of all the elements of group IIA, the highest density at 20°C is for __________.
8. Out of all the following elements of group IIA, the highest atomic number is for __________.
(Be, Ba, ca, Sr)
9. The alkali metals possesses __________ electrons in their outermost orbitals.
(1, 2, 3, 4)
10. Out of all the elements of group IIA, the highest heat of hydration is for __________.
(Be, Ba, Ca, Mg)
11. __________ of the elements has highest ionic radius.
(Be, Ba, Sr, Ca)
12. Out of all the elements of group IA, the highest heat of hydration is for __________.
(Li, Na, K, Cs)
13. Of all the group II elements, the highest oxidation potential is for __________.
(Li, Be, Ba, Ra)
14. Sodium is not observed in +2 Oxidation State because of its __________.
(high first ionization potential, high second oxidation potential, high ionic radius, high electronegativity)
15. The metallic lustre of sodium is explained by the presence of __________.
(Na+ ions, conduction electrons, free protons, a body centred cubic lattice)
16. __________ of the following substances is manufactured by electrolysis of NaCl solution.
(NaOH, Na2ClO3, NaClO3, Na)
17. When NaCl is dissolved in water, the sodium ions become __________.
(Oxidized, Reduced, Hydrolyzed, Hydrated)
18. NaCl imparts a golden yellow colour to the Bunsen flame. This can be interpreted due to __________.
(Low ionization potential of sodium, Photosensitivity of sodium,
Sublimation of metallic sodium to give yellow colour, Emission of excess
energy absorbed as a radiation in the visible region)
19. The alkaline earth metals possess __________ electron or electrons in their outermost orbitals.
20. Alkali metals form __________.
(Ionic bond, covalent bond, non-polar, Vander waal’s forces)
21. Sodium salts constitute __________% of earth’s crust.
(2.40, 2.35, 2.30, 2.25)
22. Potassium salts constitute __________% of the earth’s crust.
(2.40, 2.35, 2.30, 2.25)
23. Alkaline earth metals occur in nature in __________.
(free state, combined state, both free and combined state, none of these)
24. In general alkali metals act as __________.
(Reducing agents, Oxidizing agents, Both reducing and oxidizing agents, none of these)
25. All alkaline metals except __________ are white in colour.
(Be, Mg, Ca, None of these)
26. In the alkali metal series __________ of the following is most reactive.
(Li, Na, K, Rb)
27. In the alkali metal series, Cesium is the most reactive metal because __________.
(its incomplete shell is nearest to nucleus, the valence electron has a
larger orbit than the orbit of the valence electron of any of the
others, it exerts considerable Beautiful force on the valence electrons,
it is a heavier metal)
28. Alkali metals are __________.
(lighter than water, heavier than water, enlarged than water , all of these)
29. __________ does not belong to alkali metals.
(Li, Na, Rb, K)
30. A graphite anode is used in Down’s cell for the production of sodium because __________.
(It does not react with sodium, it does not react with chorine, it is
easy to fashion in circular form, it floats on the fused sodium
chloride)
31. __________ is a reducing agent and a constituent of a gun powder.
(KNO3, C, CaCO3, Na)
32. Alkaline earth metals form __________ carbides on heating with carbon.
(Stable, Unstable, soluble, none of these)
33. Except lithium, all alkali metal hydroxides are strongly __________.
(acidic in nature, basic in nature, neutral in nature, none of these)
34. Alkaline earth metal carbonates, sulphates and phosphates are __________.
(soluble in water, insoluble in water, sometimes soluble and sometimes insoluble in water, none of these)
35. Alkali metal carbonates, sulphates and phosphates are __________ in water with the exception of Li2CO3 and Li3PO4.
(soluble, insoluble, Both soluble and insoluble, none of these)
36. LiCl is soluble in organic solvents while NaCl is not. This is because __________.
(Lattice energy of NaCl is less than LiCl, Li+ has higher value of
hydration energy than that of Na+, LiCl is more covalent in nature than
NaCl, Li+ has lower value of hydration energy than Na+)
37. When burnt in air, Lithium forms __________.
(Normal oxide, Peroxide, Super oxide, none of these)
38. The chlorides of alkali metals and alkaline earth metals are generally __________.
(Ionic, Covalent, non polar, vander waal’s forces)
39. Sodium is a __________.
(good conductor of electricity, poor conductor of electricity, bad conductor of electricity, none of these)
40. Sodium reacts vigorously with oxygen on heating to form __________.
(Sodium oxide, Sodium peroxide, sodium superoxide, all of these)
41. Sodium is very reactive with water. Hence due to its high reactivity with water, it is stored in __________.
(Alcohol, Kerosine oil, Benzene, all of these)
42. Sodium reacts vigorously with water, liberating __________.
(Oxygen, hydrogen, Carbonoxide, Neon)
43. Sodium is a powerful __________.
(Reducing agent, oxidizing agent, bleaching agent, all of these)
44. __________ is used s a reducing agent in the preparation of such
metals as titanium and zicronium from their chlorides or oxides.
(Mg, Na, Cu, Ag)
45. __________ is used in the synthesis of rubber.
(Mg, Cu, Na, Fe)
46. __________ reducing action is used in the manufacture of certain dyes and drugs.
(Na, Mg, Cu, Ca)
47. __________ is used often in highway lamps as filaments to produce yellow light.
(Na, Tungston, Mg, Fe)
48. Purification of sodium chloride is accomplished by __________.
(Sublimation, Crystallization, Hydrogenation, Melting)
49. Ice and sodium chloride form a freezing mixture, which is used in __________.
(Refregeration, Preserving fish, Sublimation, None of these)
50. Sodium bicarbonate is commonly called __________.
(Soda Ash, Baking soda, Caustic soda, none of these)
51. Soap is often composed of __________.
(sodium carbonate, calcium carbonate, rubidium carbonate, sodium stearate)
52. Solvay’s process is also called __________.
(Haber’s Proess, Ammonia Soda Process, Washing Soda Process, Down’s Process)
53. __________ is a stronger base.
(NaOH, KOH, LiOH, HCl)
54. Na2CO3 is marketed as __________.
(Soda ash, baking soda, caustic soda, none of these)
55. When a solution of sodium carbonate is evaporated, Na2CO3.10H2O
crystallizes out t room temperature and marketed as __________.
(Soda ash, baking soda, caustic soda, washing soda)
56. By the action of aqueous NaOH on aluminium, __________ is produced.
(H2, CO2, H2O, O2)
57. __________ is used for weighing cotton cloth.
(Gypsum, Soda ash, Magnesium Sulphate, Washing soda)
Chapter 4
P - Block Elements
1. __________ of the following is non-metal.
(Boron, Aluminium, Indium, Thallium)
2. __________ of the following was isolated by Davy in 1807 by electrolysis of moist boric acid.
(Boron, Indium, Aluminium, Gallium)
3. __________ of the following is chemically inert.
(Boron, Indium, Aluminium, Gallium)
4. __________ is not the member of group IIIA.
(B, In, C, Al)
5. The oxides of Boron are __________ in nature.
(Acidic, Basic, Neutral, None of these)
6. __________ forms the most acidic oxide.
(B, Al, Ga, In)
7. Boron bursts into flame at __________.
(600°C, 700°C, 800°C, None of these)
8. B3+ cannot exist in aqueous solution because of its __________.
(Strong reducing ability, large size and small charge, small size and large charge, strong oxidizing ability)
9. Orthoboric acid on heating to about 100°C looses a water molecule to form __________.
(Metaboric acid, Pyroboric Acid, Metaboric and Pyroboric acid, none of these)
10. The reduction of metal oxides is sometimes accomplished by using aluminium in the __________.
(Goldshmidt’s reaction, Silberchmdit’s reaction, Baeyer’s reaction, Zilch’s reaction)
11. Baeyer’s Process is used for the purification of __________.
(Alum stone, Cryolite, Bauxite, none of these)
12. Hall’s Process is based on electrolysis of __________.
(Alumina, Gypsum, Borax, none of these)
13. __________ is a better conductor of heat.
(Fe, Sn, Al, none of these)
14. Al2O3 formation involves evolution of a larger quantity of heat, which makes its use in __________.
(Deoxidizer, confectionary, indoor photography, thermite welding)
15. A mixture of iron oxide and aluminium is called __________.
(Thermite, Bauxite, Alum, none of these)
16. Aluminium is used in __________.
(X-ray welding, Spot welding, Thermite welding, none of these)
17. __________ metal is used in photo-flash bulbs.
(Ca, Na, W, Al)
18. The alloy of aluminium, which contains small quantities of manganese, copper and magnesium, is called __________.
(duralumin, Magnalium, Alnico, none of these)
19. The alloy of aluminium with small percentage of magnesium is called __________.
(Duralumin, Magnalium, Alnico, none of these)
20. The aluminium which contains 20% nickel, 20% aluminium, 50% iron and 10% cobalt is called __________.
(Duralumin, Magnalium, Alnico, none of these)
21. A magnet made of __________ will lift approximately 4000 times of its own weight of iron.
(Duralumin, Magnalium, Alnico, none of these)
22. An alloy of aluminium made by alloying 5-15% aluminium and has a golden lustre is called __________.
(duralumin, Magnalium, Aluminium Bronze, none of these)
23. All the alums crystallize to yield __________.
(Octahedral crystal, Tetrahedral crystal, Trigonal crystal, Linear crystal)
24. The process of permanent dyeing is called __________.
(Mordanting, Painting, Calination, none of these)
25. The solvent used in the extraction of aluminium from its ore is __________.
(Cryolite, Bauxite, Molten sodium chloride, Water)
26. The group IV-A of the periodic table consists of __________ elements.
(three, four, five, six)
27. In group IV-A the metallic character down the group __________.
(Increases, Decreases, remains constant, none of these)
28. __________ does not contain aluminium.
(Felsper, Cryolite, Kaoline, Anhydrite)
29. Carbon differs from other members of its group due to the absence of __________ electrons.
(s, p, d, none of these)
30. Elements, which exist in two or more physical or molecular forms, are called __________.
(Isotopes, Allotropes, Isobars, none of these)
31. Out of the following elements of group IV A of the periodic table the higher density is for the element __________.
(C, Si, Ge, Pb)
32. Diamond is a __________ conductor of electricity and heat.
(Poor, Good, None, none of these)
33. Out of all the elements of group IV the higher density is for __________.
(C, Si, Ge, Pb)
34. __________ is used as a lubricant for machinery and also as a moderator in nuclear reactors.
(Diamond, Graphite, Epsom, Gypsum)
35. Highest melting and boiling point is for __________.
(C, Ge, Si, Pb)
36. PbO behaves as a/an __________.
(Amphoteric oxide, basic oxide, super oxide, sub oxide)
37. White lead is prepared by __________.
(Dutch process, Solvay’s Process, Down’s Process, none of these)
38. __________ member of the group V-A show several oxidation states such as –1, +2, +3, +4 and +5.
(P, As, Sb, N)
39. __________ member of the group V-A forms multiple bonds.
(P, Bi, As, N)
40. __________ member of group V-A does not show allotropy.
(P, Sb, N, As)
41. In __________ solution glass is soluble.
(HNO3, HCl, HF, H2CO3)
42. On industrial scale Nitric acid is prepared by __________.
(Dutch Process, Birkland-Eyde’s Process, Solvay’s Process, Down’s Process)
43. In Ostwald’s Process the substance used to oxide ammonia is __________.
(Zn, Pt, CO, none of these)
44. Copper reacts with dilute nitric acid to form __________.
(Nitric oxide, nitrogen peroxide, nitrous oxide, none of these)
45. Nitric acid is a strong __________.
(reducing agent, bleaching agent, oxidizing agent, none of these)
46. A mixture consisting of one volume of concentrated HNO3 and three volumes of concentrated HCl is called __________.
(Aqua regia, Meta stannic acid, Alum, Sandhur)
47. Lead tertraethyle is used as __________.
(Fire extinguisher, Pain Killer, Mosquito repellent, Petroleum Additive)
48. Nitric acid is used in the manufacture of __________.
(Cellulose, Varnishes, T.N.T, all of these)
49. __________ allotropic form of coal is hard.
(Peat, Lignite, Anthracite, Graphite)
50. __________ molecule is paramagnetic nature.
(O, S, Se, Po)
51. __________ element edhibits the largest number of allotropic forms amongst the elements.
52. __________ element is the most abundant element in earth’s crust.
(Ca, Si, C, O)
53. There are __________ rings in unit cell of Rhombic sulphur.
(12, 16, 20, 24)
54. Graphite is used in nuclear reactor as __________.
(A Lurbicant, A fuel, for lining the inside of reactor as an insulator, for reducing the velocity of neutrons)
55. In its unit cell, monoclinic sulphur possesses how many S8 rings.
(12, 6, 3, 0)
56. H2S is a good __________.
(reducing agent, oxidizing agent, bleaching agent, none of these)
57. In the aqueous solution H2S ionizes to produce __________ ions and behaves as a weak acid.
(H+, H-, OH-, none of these)
58. H2S reduces halogens to __________.
(hidrides, halides, halogens, none of these)
59. By __________ process the H2SO4 produced is pure and can be produced of any desired strength.
(Lead Chamber Process, Contact Process, Down’s Cell, none of these)
60. __________ gas is responsible for rising of bread.
(CO, CO2, NH3, O2)
61. At what temperature H2SO4 completely dissociates into sulphur trioxide and water.
(416°C, 516°C, 616°C, 716°C)
62. Concentrated sulphuric acid acts as a __________.
(Reducing agent, Oxidizing agent, Dehydrating agent, None of these)
63. __________ charcoal is used to decolourise brown sugar solution.
(Wood, Coconut, Animal, Sugar)
64. In the sale of diamonds the unit of weight is carat. One cart is equal to __________.
(100mg, 200mg, 300mg, 400mg)
65. Hot concentrated sulphuric acid acts as an __________ usually itself reduced to sulphur dioxide.
(Dehyrating, Oxidizing, Reducing, none of these)
66. __________ are the two elements that find wide application in transistor industry.
(Silicon and Germinium, Carbon and Platinium, Iridium and Germanium, Tungsten and Platinium)
67. In the manufactur of certain explosives such as nitroglycerine,
trinitrotoluene and gun-cotton etc. Sulphuric acid is used as a
__________.
(Oxidizing agent, Reducing agent, Dehydrating agent, none of these)
68. __________ prepared chlorine in 1774, by the action of hydrochloric acid on manganese dioxide.
(Cavendish, C.W. Scheele, Sir Humphry Davy, Lane)
69. __________ suggested the name chlorine for the gas produced by the action of hydrochloric acid on manganese dioxide.
(Sir Humphry Davy, C.W. Scheele, Cavendish, none of these)
70. Chlorine is obtained by reacting concentrated HCl with __________ agent, such as MnO2, KClO3, KMnO4.
(Reducing, oxidizing, dehydrating, none of these)
71. Electrolysis of Brine produces __________.
(Chlorine, Hydrogen, H2S, Nitrogen)
72. The process based on the oxidation of hydrochloric acid with oxygen is __________.
(Nelson’s Cell, Contact Process, Down’s Process, Deacon’s Process)
73. __________ process is used for the production of chlorine gas.
(Deacon’s, Contact, Solvay’s, Electrolysis of water)
74. Chlorine gas is __________ in colour.
(Yellow, Greenish Yellow, Violet, Blue)
75. __________ produces inflammation of the nose and throat when breathed in considerable quantities.
(Nitrogen, Carbon dioxide, Chlorine, Hydrogen Sulphide)
76. To kill bacterial, molst of the drinking water is treated with __________.
(Nitrogen, Carbon dioxide, Chlorine, Hydrogen Sulphide)
77. Chlorine is used in the preparation of poisonous gases of warfare, such as __________.
(COCl2, H2S, HCl, none of these)
78. In phosphorus oxide the number of oxygen atoms bonded to each phosphorus atom is __________.
(1, 2, 3, 4)
79. Of the following elements the only one which does not exhibit allotropy is __________.
(P, As, Sb, Bi)
80. Phosgene is the common name of __________.
(Carbon dioxide and Phosphine, Phosphoryle chloride, Carbonyle Chloride, Carbon Tetrachloride)
81. Out of all the elements of group VI A, the highest melting and boiling point is for __________.
(Te, Se, S, Pb)
82. In group VIA highest electronegativity is for __________.
(S, O, Pb, Se)
83. Large deposits of sulphur in nature are found as __________.
(Sulphuric acid, hydrochloric acid, free sulphur, none of these)
84. On the basis of available data of the structure of monoclinic sulphur, it probably consists of __________ chains.
(S6, S2, S4, S8)
85. Rhombic sulphur consists of __________.
(S8 chains, S2 chains, S4 rings, S8 rings)
86. Pure sulphuric acid is a solid compound which __________.
(Is always colloidal, slowly decomposes to form SO2, Seves as a useful source for H2S, has never been observed)
87. The form of sulphur, which is stable at room temperature and normal atmospheric pressure, is __________.
(orthorhombic, hexagonal, mono clinic, amorphous)
88. When H2S gas is dissolved in aqua regia, the function of HCl in the mixture is to __________.
(oxidize the sulphur, oxidize the mercury, complex the sulphur, complex the mercury)
89. When liquid sulphur at one atmosphere pressure is very slowly
cooled, unless super cooling occurs, the first solid to appear is
__________.
(monoclinic sulphur, Rhombic sulphur, Hexagonal sulphur, metallic sulphur)
90. The synthesis of ethers from alcohol depends on the fact that sulphuric acid is a good __________.
(oxidizing agent, reducing agent, complexing agent, dehydrating agent)
91. __________ of the following has the highest catenation capability.
(Oxygen, Sulphur, Selenium, Tellurium)
92. the halogen with the highest ionization potential is __________.
(F, Cl, I, At)
93. The halide ion with the highest hydration energy is __________.
(F-, Cl-, I-, At-)
94. Hydrofluoride acid is __________.
(a powerful oxidizing agent, a weak acid, a strong acid, a good reducing agent)
95. __________ of the following is most powerful oxidizing agent.
(F2, Cl2, Br2, I2)
96. __________ of the following exhibits the largest electrical conductivity in the liquid state.
(F2, Cl2, Br2, I2)
97. __________ of the following exhibits the highest bond energy.
(F2, Cl2, Br2, I2)
98. __________ does not form its oxy acids.
(F2, Cl2, Br2, I2)
99. The colour of I2 solution can be discharged by shaking a aqueous solution of __________.
(Sulphur dioxide, sodium thiosulphate, sodium sulphite, sodium sulphate)
100. Bleaching powder is obtained by the interaction of Cl2 and __________.
(a dilute solution of Ca(OH)2, conc. Solution of Ca(OH)2, dry CaO, dry slaked lime)
Chapter 5
Transition Elements
1. Transition elements are those in which __________ orbitals are in the process of completion.
(d, f, s, d or f)
2. Transition elements are located between __________ elements in the periodic table.
(s and p block, s and f block, d and p block, none of these)
3. Out of total 110 elements known, there are more than __________ transition elements.
(40, 50, 60, 70)
4. Elements in which d-orbitals are in the process of completion are called __________ elements.
(outer transtion, inner transition, non-transition, none of these)
5. __________ of the following is transition element.
(Sr, Sn, Cr, B)
6. __________ of the following elements is not included in the list of transition elements.
(Ca, Cu, Cr, CO)
7. Due to the addition of electrons in inner f-robitals atomic and ionic
radii or f-block elements have a regular trend. This is called
__________.
(Contraction, Lanthanide contraction, actanide, contraction, none of these)
8. The transition elements usually have very __________ melting and boiling points.
(low, high, intermediate, none of these)
9. Transition elements show a tendency of __________.
(high reactivity, less reactivity, very high reactivity, none of these)
10. Finely divided iron is used in __________.
(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Contact Process)
11. __________ reagent can be used to identify Cu2+ ion.
(Nitric acid, Sulphuric acid, Sodium hydroxide, Potassium chromate)
12. Vanadium pentaoxide is used in __________.
(Haber Process, Oxidation of sulphur dioxide to sulphur trioxide, oxidation of ammonia to nitric oxide, Contact Process)
13. __________ is the important ore of copper.
(Malachite, Bauxite, Blue Vitriol, Alumina)
14. Copper is used in __________.
(Haber Process, Oxidation of ethyl alcohol to acetaldehyde, oxidation of ammonia to nitric oxide, Contact Process)
15. Bessemer converters are used to get __________.
(Aluminium, Copper, Steel, Sodium)
16. Titanium is used as catalyst in __________.
(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Polymerization of ethyle into polyethylene)
17. Platinium or Palladium is used as catalyst in __________.
(Haber Process, Catalytic Hydrogenation, Oxidation of ammonia to nitric oxide, Contact Process)
18. __________ of the following does not belong to d-block elements.
(Chromium, Cobalt, Silicon, Copper)
19. Compounds attracted into a magnetic field are called __________.
(Magnets, Paramagnets, Dimagnets, none of these)
20. Transition metal compounds, which show paramagnetism, have __________.
(unpaired electrons, paird electrons, unpaired protons, paired protons)
21. A substance, which have even number of electrons and have paired spin is called __________.
(Ferromagnetic, Paramagnetic, Dimagnetic, none of these)
22. Magnetic movement is measured with help of __________.
(Guoy’s balance, Spring balance, Physical balance, Cavendish Appratus)
23. __________ property provides information about the presence of unpaired electrons in an atom or ion.
(Dipole moment, Magnetic moment, torque, none of these)
24. By measuring the magnetic moment values we can measure __________.
(Nature of the transition metal compound, oxidation state of the
transition metal, both nature and oxidation state of transition metal
compound, none of these)
25. Transition elements show variable valencies because of the involvement of the d-electrons in addition to __________.
(p-electrons, f-electrons, d-electrons, e-electrons)
26. The empty spaces between atoms of transition metals in their crystal lattices are called __________.
(Vacant spaces, valence spaces, interstices, none of these)
27. The formation of non-stoichiometric compounds is due to the defects in solid structure and __________.
(Variabel valency of transition elemennts, even number of electrons, even number of protons, unpaired electrons)
28. Interstitial compounds have __________ formula.
(definite, half, indefinite, no)
29. Strong paramegnetism is called __________.
(dimagnetism, ferromagnetism, both dimagnetism and ferromagnetism, none of these)
30. When a number of molecules or negatively charged ions combine with a
central d-block atom or ion to form complex ion or molecule, __________
is formed.
(a co-ordinate compound, interstitial compound, di-atomic compound, none of these)
31. In coordinate bonding the molecules or ions, which bond onto the central metal ion or atom, are called __________.
(actanides, Lanthanides, Ligands, none of these)
32. Ligands are __________.
(electron pair donors, electron pair acceptros, neutral, none of these)
33. [Ni(CN)4]2- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
34. [Cu(NH3)4]2+ is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
35. MnO4- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
36. CrO42- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
37. [Cu(CN)4]3- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
38. [Zn(NH3)4]3- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
39. [Fe(CN)6]3- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
40. [Fe(CN)6]4- is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
41. [Ni(NH3)6]2+ is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
42. [Co(NH3)6]3+ is an example of __________.
(Squre planar, tetrahedral complexes, octahedral complexes, none of these)
43. In the system of naming complex coordinate compounds cations are named __________ anions.
(after, beforem, inbetween, none of these)
44. The names of __________ are usually unchanged.
(anionic ligands, cationic ligands, neutral ligands, none of these)
45. NH3 is an example of __________ ligand.
(anionic, cationic, neutral, none of these)
46. H2O is an example of __________ ligand.
(anionic, cationic, neutral, none of these)
47. The suffix “ate” at the end of the name of the coordinate complex ion represents a/an __________.
(cation, anion, cathode, anode)
48. A mixture of iron sulphide and copper sulphide is called __________.
(gangue, matte, matter, residue)
49. Sulphide ore is concentrated by __________.
(Froth floatation Process, Dutch Process, Bessemerization, none of these)
50. __________ does not copper.
(Carborundum, Azurite, Blue Vitriol, Malachite)
51. Utensils used to carry out fermentation are made of __________.
(Cu, Fe, Al, Ca)
52. An alloy of copper, which contains 80% copper and 20% zinc, is called __________.
(Brass, Bronze, Bell metal, none of these)
53. Copper sulphate reacts with solution of potassium iodide giving __________.
(sulphur dioxide, iodine, copper oxide, potassium oxide)
54. An alloy of copper, which contains 90% Cu and 10% Sn is called __________.
(Bronze, Brass, Bell Metal, all of these)
55. An alloy of copper, which contains 80% Cu and 20% Sn is called __________.
(Bronze, Brass, Bell metal, all of these)
56. The substance attracted by magnetic field is known as __________.
(diamagnetic, paramagnetic, antimagnetic, all of these)
57. Copper sulphate is commonly called __________.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
58. Silver nitrate is commonly called __________.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
59. Stainless steel is __________.
(a mixture, a compound, an element, all of these)
60. Potassium dichromate is commonly called __________.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
61. Manganese differs from most other transition elements because it reacts with __________.
(oxygen, water, sulphur, iodine)
62. __________ of the following elements can be included in the category of transition elements.
(Cu, Al, Ar, At)
63. Potassium ferrocyanide is a __________.
(normal salt, mixed salt, double salt, complex salt)
64. __________ of the following combination is included in the Iron triad of elements.
(Pd and Pt, Mn and Hg, Co and Ni, V and Ti)
65. __________ is a blue crystalline solid which is freely soluble in water.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
66. __________ is an orange crystalline solid which is freely soluble in water.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
67. __________ is a yellow crystalline solid which is freely soluble in water.
(Nila Thotha, K2CrO4, Surkh Kahi, none of these)
68. __________ is a colourless crystalline solid.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
69. __________ is used as fungicide and germicide.
(Nila Thotha, Lunar Caustic, Surkh Kahi, none of these)
70. Ferric oxide is __________.
(a basic anhydride, an acid anhydride, an amphoteric anhydride, green in colour)
71. Potassium dichromate is a strong __________.
(reducing agent, oxidizing agent, dehydrating agent, all of these)
72. The densest element is __________.
(Pb, Hg, Pt, Os)
73. The most strongly ferromagnetic element is __________.
(Fe, Co, Ni, Os)
74. Alloying of metals serves to inhibit __________.
(Corrosion, Froth Floatation, Erossion, None of these)
75. Mechanical strains can be removed by __________.
(heat treatment, polishing the metal surface, both heat treatment and polishing the metals surface, none of these)
76. __________ has the lowest density.
(Cu, Ni, Sc, Zn)
77. Galvanizing is done by dipping clean iron sheet in a zinc chloride bath and __________.
(heating, rusting, froth floatation, alloying)
78. There are two well known theories to explain the phenomenon of corrosion namely __________.
(Acid theory, Electromechanical theory, electrochemical theory, acid and electromechanical theory)
79. __________ one of the following metals exists in liquid form.
(Sc, Y, La, Hg)
80. The process of depositing a thin layer of tin on base metals to protect them from corrosion is called __________.
(Exposure, tin plating, Fixing, none of these)
81. The most strongly ferromagnetic element is __________.
(Fe, Ni, S, C)
82. The property of a substance which permits it being drawn into wire is called __________.
(softness, Ductility, Brittleness, Hardness)
83. One of the constituent of German silver is __________.
(Ag, Cu, Mg, Al)
84. When potassium permanganate is added to a saturated aqueous solution of potassium hydroxide, __________ gas is evolved.
(Hydrogen, Oxygen, Carbon dioxide, none of these)
85. __________ reagent can be used to identify nickle ion.
(Resorcinol, Dimethyl glyoxime, Dimethyl Benzidine, Potassium Ferrocyanide)
86. __________ of the following is the transition element.
(Sr, Sn, Cr, Fe)
87. Bessemer converters are used to get __________.
(Aluminium, copper, steel, none of these)
88. __________ is not the ore of copper.
(Blue vitriol, Cuprite, Chalcocite, Steel)
89. __________ of the following elements is not included in the list of transition elements.
(Ca, Cu, Cr, Co)
90. __________ one of the following does not belong to d-block elements.
(Chromium, Silicon, Cobalt, Nickel)
Chapter 6
Organic Chemistry
1. The branch of chemistry which deals with the study of compounds
containing carbon as a essential element is called __________.
(Organic chemistry, In organic chemistry, Physical chemistry, all of these)
2. The first organic compound synthesized in the laboratory is __________.
(Methane, Urea, Acetic Acid, Glucose)
3. __________ of the following is not an organic compound.
(CH4, CO2, CH2-CH2, CH3OH)
4. __________ of the following is not an organic compound.
(Penicillin, Urea, Oxalic acid, Plaster of Paris)
5. __________ is the important sources of naturally occurring compounds of carbon.
(Animals, Plants, Rock salts, Sea water)
6. __________ is not a component of coal.
(H, O2, N, Si)
7. Hard black form of coal containing 92 – 98% carbon is called __________.
(Anthracite, Sub-bituminous coal, Bituminous coal, Lignite)
8. The most abundant form of coal and is used as energy souce and
carbonization for coke, coal tar and coke-oven is called __________.
(Anthracite, sub-bituminous coal, Bituminous coal, Lignite)
9. Form of coal used at power generating stations is called __________.
(Antracite, Sub-bituminous coal, Bituminous coal, Lignite)
10. A soft and brown form of coal which contains 50 to 60% carbon is called __________.
(Anthracite, Sub-bituminous coal, Bituminous coal, Lignite)
11. In Pakistan deposits of lignite are found at __________.
(Dandot, Saindak, Khewra, none of these)
12. __________ is a pure carbon.
(Coke, Coal gas, Coal tar, none of these)
13. Its major constituents are hydrogen (50%), methane (35%) and carbon monoxide (8%).
(Coke, coal gas, coal tar, none of these)
14. Number of organic compounds present in coal tar is __________.
(115, 215, 315, 415)
15. Residue left after fractional distillation of coal tar is called __________.
(Pitch, Dutch, Gangue, Matte)
16. Petroleum in the unrefined form is called __________.
(Coke, Coal gas, Crude oil, Rock oil, both crude oil and rock oil)
17. Natural gas mainly consists of __________.
(Methane, Ethane, propane, Butanes)
18. In Pakistan there are vast reserves of natural gas at __________ in Baluchistan.
(Bandot, Khewra, Saindak, Sui)
19. __________ is a mixture of methane, ethane, propane and butane, used as a fuel and for making other organic chemicals.
(Refinary gas, Gasoline, Kerosene oil, gas oil)
20. __________ is a mixture of hydrocarbons containing 5-8 carbon atoms and boiling in the range of 40-180°C.
(Refinary gas, Gasoline, Kerosene oil, gas oil)
21. __________ is a mixture of hydrocarbons having 11-12 carbon atoms and boiling point in the range of 250°C.
(Refinary gas, Gasoline, Kerosene oil, gas oil)
22. A mixture of hydrocarbons having 13-25 carbon atoms is called __________.
(Refinary gas, Gasoline, Kerosene oil, gas oil)
23. On strong heating the fractions containing the larger hydrocarbon
molecules are broken up into smaller and more volatile molecules, this
is called __________.
(Sublimation, Cracking, Roasting, Refining)
24. Cracking is also termed as __________.
(Pyrolysis, Refining, Polymerization, Hydrohalogenation)
25. A large number of organic compounds, especially the unsaturated
ones, show a great tendency to unite. This process is termed as
__________.
(Pyrolysis, Cracking, Polymerization, none of these)
26. An isomer of ethanol is __________.
(Dimethyl ether, Diethyl ether, Ethylene glycol, Methanol)
27. Organic compounds made up of carbon and hydrogen are called __________.
(Polymers, Hydrocarbons, Butanes, none of these)
28. Organic compounds other than the hydrocarbons may be considered to
be derived from the hydrocarbons by the replacement of one or more of
their __________ atoms with atoms or groups of atoms of other element.
(Carbon, Hydrogen, Nitrogen, none of these)
29. When ethylene is heated under pressure, a transparent solid polymer, __________ is obtained.
(Polyethene, Ethane, Methane, None of these)
30. An atom or group of atoms, which confers characteristic properties to an organic molecule, is called __________.
(Radical, Functional group, Polymer, none of these)
31. Compounds having same molecular formula but different structures are said to be __________.
(Polymers, Isomers, Radical, Functional group)
32. The quality of petroleum is determined by __________.
(Decane number, octane number, hexane number, none of these)
33. __________ of the following obey isomerism.
(CO2, C2H6O, CuSO4, none of these)
34. Two or more than two different compounds having the same molecular
formula but different carbon chains or skeletons are said to be
__________.
(Chain isomers, position isomers, functional group isomers, metamers)
35. The kind of isomerism which depends upon the relative position of
the group, or the position of double or single bond in case of
unsaturated compounds in termed as __________.
(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)
36. Isomerism, which involves compounds having the same molecular
formula, but different functional groups are called __________.
(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)
37. __________ is exhibited by compounds having the same functional
group but different alkyl attached to the same multivalent atom.
(Chain isomerism, Position isomerism, Functional Group isomerism, Metamerism)
38. In cracking usually catalyst used is __________.
(Pt, Aluminosilicate, Ni, Tetra-ethyl lead)
39. Iso-butane exhibited __________.
(Chain Isomerism, Position Isomerism, Functional group Isomerism, Metamerism)
40. In CCl4 molecule the four valencies of carbon atom are directed towards the corners of a __________.
(Cube, Hexagon, Prism, Tetrahedron)
41. Tetrahedral nature of bonding in carbon atom was first shown by __________.
(Wohler, Vant Hoff and LeBel, Lewis, Kekule)
42. The general formula (RCO)2O represents __________.
(An ether, ketone, an ester, an acid anhydride)
43. Formation of alkane by the action of zinc on alkyl halide is called __________.
(Frankland reaction, Wurtz reaction, Cannizzaro’s reaction, Kolbe’s reaction)
44. __________ of the following are isomers.
(Methyl alcohol and dimethyl ether, Ethyl alcohol and dimethyl ether, Acetone and Acetaldehyde, Proponoic acid and proponanone)
45. The isomers must have the same __________.
(Structural formula, molecular formula, chemical properties, physical properties)
46. __________ has the longest bond length.
(C = C, C º C, C – C, all of these)
47. In alkanes all C – C bonds have __________.
(single bond, double bond, triple bond, none of these)
48. Removal of one of the hydrogen atoms of an alkane produces a __________.
(alkyl group, ethyl group, methyl group, none of these)
49. Compounds in which two alkyl groups are attached to an oxygen atom are called __________.
(alkanes, ethers, alcohals, isomers0
50. Many hydrocarbons contain more than one OH groups in a molecule. Molecules of this type are called __________.
(Ethers, Polyhydroxy alcohols, aldehydes, none of these)
51. __________ is the common name of methanol.
(formaldehyde, acetaldehyde, propionaldehyde, none of these)
52. Compounds which contain carbonyl group but differ from aldehydes in
that two alkyl groups are attached to the carbon of carbonyl group are
called __________.
(Ethers, Ketons, Alcohols, none of these)
53. __________ is the common name of propanone.
(Acetone , ketone, Diethyl Ketone, none of these)
54. Benzene is a __________.
(Heterocyclic compound, Alicyclic compound, Aromatic compound, Acyclic)
55. Common name of formic acid is __________.
(Methanoic acid, Ethanoic acid, Propanoic acid, none of these)
56. The properties of organic compounds are due to __________.
(Covalent bonds, Functional groups, Ionic bonds, None of these)
Chapter 7
Hydrocarbons
1. Organic compounds, which contain element carbon and hydrogen only are called __________.
(Hyrocarbons, Ethers, Ketones, none of these)
2. The number of hydrocarbons is very large because of the property of
hydrogen to __________, with it self in the form of chains and rings.
(Cmbine, Catenate, Sulphonation, none o these)
3. Carbon usually exhibits a covalency of __________.
(Two in most of its compounds, three in most of its compounds, four in most of its compounds, none of these)
4. Hydrocarbons, which contain single bonds, are called __________.
(alkanes, alkenes, alkynes, none of these)
5. Hydrocarbons, which contain double bonds, are called __________.
(alkanes, alkenes, alkynes, none of these)
6. Hydrocarbons, which contain triple bonds, are called __________.
(alkanes, alkenes, alkynes, none of these)
7. The alkanes have __________.
(tetrahedral frame work, planar molecules, linear structure, none of these)
8. The alkynes have __________.
(tetrahedral frame work, planar molecules, linear structure, none of these)
9. The alkenes have __________.
(tetrahedral frame work, planar molecules, linear structure, none of these)
10. Saturated Hydrocarbons are also called __________.
(Alkanes, Olefins, Alkenes, Alkanes and Olefins)
11. Unsaturated hydrocarbons are also called __________.
(Alkenes, Paraffins, alkanes, none of these)
12. Alkenes are characterized by the presence of __________ bond between two carbon atoms.
(single, double, triple, none of these)
13. Alkanes or paraffins are characterized by the presence of __________ bond between two carbon atoms.
(Single, double, triple, none of these)
14. Alkynes are characterized by the presence of __________ bond between two carbon atoms.
(single, double, triple, none of these)
15. Alkanes are also called __________.
(Paraffins, Olefins, Aldehydes, none of these)
16. Alkenes are also called __________.
(Paraffins, Olefins, Carbonyl, none of these)
17. An alkane hydrocarbon chain on cyclization would result in the formation of __________.
(Alicyclic compound, aromatic compound, ethers, none of these)
18. Benzene is the simplest example of hydrocarbon called __________.
(Alicyclic, aromatic, open chain, none of these)
19. Solid CH4 is __________.
(molecular solid, covalent solid, ionic solid, does not exist)
20. Methane is also known as __________.
(oil gas, marsh gas, gasoline, none of these)
21. A liquid hydrocarbon is converted into a mixture of gaseous hydrocarbon by __________.
(Cracking, Hydrolysis, Oxidation, Reduction)
22. __________ is obtained in the laboratory by heating a mixture of sodium acetate and soda lime.
(Alcohol, Ethene, Methane, none of these)
23. Alkenes undergo __________.
(addition reaction, substitution reaction, both addition and substitution reaction)
24. __________ does not react with aqueous solution of acids, alkalies,
or potassium permanganate or other oxidizing agents and most of the
usual laboratory reagents.
(Benzene, Ether, Methane, Acetic acid)
25. Bromine reacts with methane when the reaction is catalyzed by __________.
(Sunlight, high frequency radiation, diffused sunlight, nickel)
26. In methane the replacement of hydrogen by _ NO2 is called __________.
(Pyrolysis, Nitration, Halogenation, none of these)
27. Methane when heated to extreme temperature in the absence of air undergoes thermal decomposition, called __________.
(Nitration, Catalytic oxidation, Pyrolysis, none of these)
28. Urea, a useful fertilizer, is prepared on industrial scale from __________.
(Natural gas, Coal, Coke, Petroleum)
29. Carbon black is a raw material for paints and automobile tyres and is prepared from __________.
(Ethane, Ethene, Methane, none of these)
30. C2H6 is called __________.
(Methane, Ethane, Methanol, none of these)
31. __________ is obtained in the laboratory by heating sodium proponoate and soda lime.
(Methane, Ethane, Ethene, none of these)
32. In the laboratory ethane is prepared by the reaction called __________.
(Sabatier-Senderens Reaction, Pyrolysis, Catenation, Hydrohalogenation)
33. When an aqueous solution of sodium or potassium salt of
mono-carboxylic acid is subjected to electrolytic, corresponding alkane
is formed. This reaction is called __________.
(Sabatier-Senderens Reaction, Kolbe’s Electrolysis, Polymerization, chlorination)
34. On burning __________ produces a considerable amount of heat energy which may be used for welding process.
(Ethane, Benzene, Ethene, none of these)
35. __________ is found to be present in wood gas and coal gas.
(Methane, Ethene, Ethane, Benzene)
36. __________ is prepared on a small scale in the laboratory by heating together ethyl alcohol and sulphuric acid.
(Methane, Ethane, Ethylene, none of these)
37. The elimination of hydrogen halide (HX) from adjacent carbon atoms is called __________.
(Pyrolysis, Chlorination, Dehydrohalogenation, none of these)
38. __________ process is important in the hardening of vegetable and
animals oils to produce solid fats which are used to make margarine.
(Pyrolysis, Catenation, Hydrogenation, Dehydrohalogenation)
39. When a mixture of ethene and air is passed over heated silver under pressure, we get __________.
(Epoxide, Superoxide, Suboxide, none of these)
40. The negative part of the addendum adds on to the carbon atom joined
to the least number of hydrogen atoms. The statement is called
__________.
(Markownikoff’s rule, Peroxide effect, Theile’s theory, Baeyer’s strain theory)
41. Baeyer’s test is the basis for detection of a __________ bond in an organic molecule.
(single, double, triple, none of these)
42. __________ was used in first world war.
(Phosgene gas, Mustard gas, Oil gas, Coal gas)
43. When a mixture of CO, C2H4 and C2H2 is passed through ammonical cuprous chloride solution then __________.
(Acetylene and CO are absorbed, CO is absorbed, C2H4 is absorbed, Nothing happens)
44. Ethylene dichloride is also called __________.
(Mustard gas, Dutch liquid, Polyethene, none of these)
45. __________ is used to manufacture mustard gas which is poisonous gas used as war gas.
(Ethane, Methane, Ethylene, none of these)
46. __________ is most found in alkenes.
(Chain isomerism, Geometrical isomerism, Mesomerism, Position Isomerism)
47. __________ poisonous gas is present in the exhaust fumes of car.
(Methane, Acetylene, HCl, Carbon dioxide)
48. __________ is used to import colour to stile green citrus fruit form ripening.
(Ethylene, Methane, Ethane, none of these)
49. The number of xylene isomers is __________.
(2, 3, 4, 5)
50. Ethylene dichloride and ethylene chloride are isomeric compounds.
The statement which is not applicable to both of them is __________.
(react with alcoholic potash, react with aqueous potash and give the same product, are dihalides, answer Beilstein’s test)
51. Structure of benzene is __________.
(Diagonal, Planner, Pyramidal, Tetrahedral)
52. __________ is used in the manufacture of plastic and synthetic rubber.
(Styrene, Mustard gas, Polythene, none of these)
53. The polythene is a polymer of __________.
(Ethylene, Aceton, Propylene, Butadiene)
54. Acetylene or ethyne was discovered accidentally in 1899 by the American chemist __________.
(Wilsson, Lane, Nelson, none of these)
55. Acetylene is present in small proportions (about 0.06% by volume) in __________.
(Natural gas, Coal gas, Gasoline, Petroleum)
56. __________ is prepared in the laboratory by dropping water on calcium carbide.
(Ethylene, Acetylene, Methane, none of these)
57. The process used for the preparation of acetylene is __________.
(Berthelot Process, Sabatier-Senderns Reaction, Kolbe’s Process, none of these)
58. Acetylene has a characteristic ethereal smell resembling that of __________.
(Rotten egg, Garlic, Benzene, none of these)
59. Acetylene burns with __________ flame.
(Greenish, Bluish, Smoky, none of these)
60. Benzene was found by __________ in 1825 in the gas produced by the destructive distillation of vegetable oils.
(Hofmann, Michael Faraday, Solvay, none of these)
61. __________ found benzene in coal-tar.
(Hofmann, Michael Faraday, Solvay, none of these)
62. When n-hexane obtained from petroleum is heated in the presence of
platinum at 500°C under 10 – 20 atmosphere pressure, it cyclises to give
__________.
(Ether, Benzene, Mustard Gas, none of these)
63. Phenol is reduced to __________, when its vapours are passed over red hot zinc dust.
(Ether, Benzene, Ethane, Acetylene)
64. Replacement of hydrogen atom by – SO2 OH is called __________.
(Nitration, Sulphonation, Alkylation, Hydrogenation)
65. _ SO2OH is called __________.
(Sulphonic Group, Carbonyl group, Methyl group, none of these)
66. Under the influence of anhydrous aluminium chloride as a catalyst,
benzene reacts with alkyl and acyl halides giving alkylated and acylated
benzens. The reaction is called __________.
(Friedel-Cracts Reactions, Berthelot’s Reaction, Sabatier-Senderens Reaction, none of these)
Chapter 8
Alkyl Halides
1. Monohalo derivatives of alkanes are called __________.
(Acyl halides, Aryl Halides, Alkyl Halides, none of these)
2. The general formula of alkyl halides is __________.
(CnH2n+1 X, CnHn+1 X, C2nH2n+1 X, none of these)
3. When an alkene is treated with halogen acids, __________ is formed.
(Alkyl halide, Acyl halide, Carbonyl chloride, all of these)
4. Formula of Thionyl Chloride is __________.
(SOCl2, ZnCl2, CH3Cl, none of these)
5. If ethane is treated with HBr then __________.
(Ethyl bromide is formed, Methyl bromide is formed, Bromine is evolved, Hydrogen is obtained)
6. When metallic sodium in ether is heated with an alkyl halide, a higher alkane is formed. It is called __________.
(Sulphonation, Wurtz’s Reaction, Friedel-Crafts Reaction, none of these)
7. If sodium lead alloy is treated with methyl chloride then __________.
(Tetra ethyl lead is formed, Tetra methyl lead is formed, Tri methyl lead is formed, Di methyl lead is formed)
8. Dehydrohalogenation of alkyl halide is carried in the presence of alcoholic __________.
(NaOH, KOH, Ca(OH)2, none of these)
9. Grignard’s reagent when reacts with ammonia then __________.
(Methane is formed, Ethane is formed, Nitrogen is evolved, Magnesium is separated)
10. Grignard’s reagent reacts with alkyl halide to form __________.
(Alkanes, Alkynes, Alkenes, Alcohols)
11. Grignard’s reagents are __________.
(Alkyl halide, Alkyl magnesium halide, Alkyl sodium halide, none of these)
12. On passing CO2 through Grignard reagent __________ is formed.
(Methanoic acid, Ethanoic acid, Propanoic acid, No reaction occurs)
13. Alkyl halides (methyl chloride or ethyl chloride) when treated with
__________, react to produce the important anti-knock gasoline
additives.
(Sodium, Lead, Sodium-lead Alloy, none of these)
14. On adding formaldehyde to Grignard’s reagent __________ is formed.
(Primary alcohol, Secondary alcohol, Aldehyde, Acetone)
15. Action of zinc with alkyl halide in the presence of an inert solvent
forms a corresponding higher alkane. This is called __________.
(Wurtz’s Reaction, Frankland Reaction, Hoffman’s Reaction, none of these)
16. The hydrolysis of alkyl halides by heating with aqueous alkali is a __________ substitution reaction.
(Electrophilic, Nucleophilic, Electrophile and Nucleophile, none of these)
17. __________ of the following compounds does not react with bromine.
(Ethylamine, Propene, Phenol, Chloroform)
18. A reaction in which an atom or group of atoms replaces an atom or
group of atoms already present in the molecule of a substance is called
__________.
(Nitration, Halogenation, Substitution, Sulphonation)
19. __________ is a Neucliphile.
(OH-, CN-, NH3, all of these)
20. General formula of Grignard’s reagent is __________.
(R – Mg – X, R – Al – X, R – Na – X, R – Cl – X)
21. __________ is prepared by heating methyl iodide with fresh magnesium turnings in anhydrous ether.
(Grignard’s reagent, Mustard gas, Benzene, none of these)
22. When Grignard’s reagent is hydrolyzed with water, it is converted into __________.
(Alkynes, Alkenes, Alkanes, Acetons)
23. __________ of the following alkyl halides is used as a methylating agent.
(C2H5Cl, C2H5Br, C2H5I, CH3I)
24. Ethyl chloride reacts with alcoholic KOH to give __________.
(C2H5OH, C2H6, C2H2, C2H4)
25. Dry carbon dioxide is passed through Grignard’s Reagent in the presence of __________ as a solvent.
(Acetone, Benzene, Ether, none of these)
26. Grignard’s reagent reacts with CO2 to form __________.
(HCl, Carboxylic acid, Acetic acid, Carbonic acid)
27. Grignard’s reagent reacts with acetaldehyde to form __________.
(Primary alcohol, Secondary alcohol, Tertiary alcohol, all of these)
28. Alkyl halides reacts with Zn to form __________.
(Alkynes, Alkanes, Alkenes, none of these)
Chapter 9
Organic Compounds
1. The action of nitrous acid on ethyl amine gives __________.
(Ethane, Ammonia, Ethyl alcohol, Nitroethane)
2. Isopropyl alcohol on oxidation gives __________.
(Ether, Acetone, Ethylene, Acetaldehyde)
3. Rectified spirit contains __________ % alcohol.
(95.6, 75.0, 100.0, 85.4)
4. __________ is the end product in the process of fermentation.
(Methyl alcohol, Ethanol, CH3OH, Ethylene)
5. __________ is not the characteristic of the alcohols.
(Their boiling points rise fairly uniformly with a rise in molecular
weight, Lower members have a pleasant smell but burning taste and the
higher ones are odourless and tasteless, these are lighter than water,
Lower members are soluble in water and organic solvents but solubility
decreases with increase in molecular weight)
6. In the dehydration of ethyl alcohol to ethylene with concentrated sulphuric acid __________.
(Carbonium ions are involved, carbonium are evolved, sulphuric acid acts as an electrophile, none of these)
7. A compound is an/a __________ if the “R-” group is derived from aliphatic or alicyclic hydrocarbons.
(Ether, Ketone, Alcohol, Phenol)
8. A compound which has –OH group attached to an aromatic hydrocarbon is called __________.
(Alcohol, Phenol, Ether, none of these)
9. A product formed by the reaction of sodium with ethanol is __________.
(H2O, NaOH, NaH, H2)
10. An alcohol, which contains on –OH group is called __________.
(Monohydric, Dihydric, Trihydric, none of these)
11. An alcohol, which contains on –OH group is called __________.
(Monohydric, Dihydric, Trihydric, none of these)
12. Primary, secondary and tertiary alcohols may be distinguished by using __________.
(Fehling’s solution, Victor Meyer test, Hofmann set, Beilstein test)
13. The number of structural isomers for C4H9OH is __________.
(3, 4, 5, 6)
14. In cold countries glycerol is added to water in car radiators as it helps to __________.
(bring down the specific heat of water, lower the freezing point, reduce the viscosity, make water a better lubricant)
15. Aldehydes and Ketons are commonly referred to as __________.
(Ethers, Carbonyl compounds, phenols, none of these)
16. Aldehyde may be distinguished from ketons by the use of __________.
(Concentrated Sulphyric acid, Grignard’s Reagent, Pyrogallol, Fehlings solution)
17. In aldehydes one bond of carbonyl group is always attached to __________.
(Carbon atom, Hydrogen atom, Nitrogen atom, none of these)
18. An aldehyde on oxidation gives __________.
(an alcohol, a ketone, an acid, an amine)
19. Acid anhydrides are calls of carboxylic acid derivatives, which may be formed by the elimation of __________.
(Carbon, Hydrogen, Water, none of these)
20. Formaline is an aqueous solution of __________.
(Formic acid, Formaldehyde, Flurescein, Furfuraldehyde)
21. Methyl alcohol is known commercially as __________.
(Wood-spirit, Wood Naphtha, Mustard gas, both Wood spirit and Wood- Naphtha)
22. __________ discovered Methyl alcohol.
(Boyle, Salvay, Jabber Bin Hayyan, none of these)
23. When wood is heated with an insufficient supply of air, organic
materials are driven off as gases, and the cellulose is decomposed to
almost pure carbon is called __________.
(Coal, Charcoal, Oil gas, Natural gas)
24. Now a days a large quantity of methyl alcohol is obtained by passing
__________ over heated zinc and chromium oxides at 400 - 450°C under
200 atmospheric pressure.
(Natural gas, Water gas, Ethylene, none of these)
25. Methyl alcohol can cause __________.
(Cancer, Blindness, Aneimia, none of these)
26. The reaction of alcohol with thionyl chloride (SOCl2) in the presence of solvent called __________.
(Pyridine yields, Adenine yields, Guanine yields, none of these)
27. Ethyl alcohol often called __________.
(Alcohol, Spirit, Ether, Lacquer)
28. Ethyl alcohol is also called __________.
(Methyalted spirit, Spirit of wine, Wood spirit, none of these)
29. __________ is also present in the urine of diabetic patients.
(Spirit of wine, Wood spirit, Methane, none of these)
30. In 1808, __________ discovered ethyl alcohol in urine of diabetic patients.
(Boyl, Suassure, Mendleeve, none of these)
31. Ethyl alcohol is produced on commercial scale by the biological break down of __________,
(Starch, Minerals, Cellulase, None of these)
32. The 14 enzymes present in the living cells of the yeast are collectively called __________.
(Substrate, Zymase, Amylase, none of these)
33. The force of attraction of the electrons of one atom for the protons
of another atom in close proximity is called __________.
(Ionic bond, Hydrogen bond, Covalent bond, all of these)
34. __________ of the following compounds can form a hydrogen bond.
(CH4, H2O, NaCl, CHCl3)
35. When two ice cubes are pressed over each other, they unite to form
one cube. __________ of the following forces is responsible to hold them
together.
(Hydrogen bond formation, Vander Waal’s forces, Covalent bond, Dopole Interaction)
36. CH3OH and C2H5OH are highly miscible with water because they exhbits __________.
(Ionic bonding, Covalent bonding, Hydrogen bonding, none of these)
37. Alcohols may be converted to the corresponding __________ by actions of halogen acids in the presence of ZnCl2.
(Aldehydes, Alkyl halides, acyl halides, none of these)
38. Compounds obtained by the elimination of a molecule of water between
an alcohol and hydroxyl group of the acid are called __________.
(Ethers, Esters, Ketons, Phenols)
39. During the dehydration of alcohols, relatively high temperature and
moderate alcohol concentration yield the corresponding __________.
(Ether, Olefin, Paraffin, none of these)
40. Ethyl alcohol may be identified by the __________.
(Bayer’s Test, Flame Test, Idoform Test, Chloroform Test)
41. Industrially, formaldehyde is made from methyl alcohol by __________.
(Dehydrogenation, Dehydrohalogenation, Oxidation, Reduction)
42. Dry distillation of calcium formate yields __________.
(Ether, formaldehyde, Acetic acid, none of these)
43. An aldehyde is converted to carboxylic acid on __________ with K2Cr2O7 and H2SO4.
(Reduction, Oxidation, Dehydrogenation, all of these)
44. When aldehydes are warmed with __________, red precipitates of cuprous oxide are precipitated.
(Grignard’s Reagent, Fehlings solution, KMnO4, none of these)
45. Aldehydes can be distinguished from Ketons by using __________.
(Schiff’s reagent, Concentrated sulphruric acid, Anhydrous Zinc chloride, Resorcinol)
46. In ketons the two bonds of the carbonyl are attached to two __________.
(alkyl group, aryl group, hydrogen group, alkyl group and aryl group)
47. Formation of acetaldehyde from ethanol is called __________.
(Addition, Reduction, Oxidation, Substitution)
48. Aldehydes can be distinguished from ketons by __________.
(AgNO3, CH3COOH, conc. H2SO4, Fehlings solution)
49. Acetaldehyde reacts with __________.
(nucleophiles only, electrophiles only, free radicals only, both with nucleophiles and electrophiles)
50. When aldehydes are warmed with a ammonical solution of silver
nitrate, they precipitated metallic silver which often form a mirror.
This reaction is called __________.
(Tollen’s Test, Fehlings Test, Idoform Test, none of these)
51. Acetaldehyde reacts with ammonia to form __________.
(Condensation products, substitution products, addition product, resin like product)
52. __________ prepared the first synthetic plastic, by combing formaldehyde with phenol under heat and pressure.
(Newlands, Blackeland, Russel, Charles)
53. __________ is used medically as a urinary antiseptic.
(Formaldehyde, Benzene, Sulphuric acid, Methanamine)
54. Aldol condensation can occur between __________.
(an aldehyde and ketone, an aldehyde and ester, an aldehyde and benzene, none of these)
55. Aldol condensation between __________ of the following compounds, followed by dehydration gives methyl vinyl ketone.
(HCHO and CH3COCH3, HCHO and CH3CHO, Two molecules of CH3CHO, Two molecules of CH3COCH3)
56. Aldol condensation can occur between __________.
(two aldehydes (identical or different), an aldehyde and ester, an aldehyde and benzene, none of these)
57. Aldol condensation can occur between __________.
(two aldehydes and phenols, two ketons(identical or different), an aldehyde and benzene, none of these)
58. A nucleophilic addition of carbonion, generated by the loss of
proton from a-position of an aldehyde or a ketone by a base, to the
carbonyl group, is called __________.
(Nitration, Aldol Condensation, Esterification, none of these)
59. The aldehydes having no hydrogen attached to a-carbon atom when
treated with concentrated solution of an alkali, undergo self-oxidation
and reduction, forming a mixture of an alcohol and a salt of
corresponding carboxylic acid. The reaction is known as __________.
(Fehlings reaction, Cannizzaro reaction, Formalin reaction, none of these)
60. An aqueous solution containing about 40% of formaldehyde and a little alcohol is sold under the name of __________.
(Formalin, Malt-sugar, Pyridine, Starch)
61. Gelatine, a substance readily soluble in water, becomes insoluble when it is treated with __________.
(Formalin, Malt sugar, Benzene, Resins)
62. __________ is used as preservative for biological specimens.
(Benzene, Ketone, Alcohol, Formaline)
63. Alive polio virus in the culture fluid is made harmless by addition of __________ in the processing of anti-virus vaccine.
(Benzene, Acetic acid, formaldehyde, Carboxylic acid)
64. Acetic acid is manufactured from the brown aqueous distillate known
as __________ which is obtained by the destructive distillation of wood
and contains a mixture of acetic acid, acetone and methyl alcohol.
(Formalin, Pyroligenous acid, Pyridine, Acetylene)
65. The most general method of preparing __________ is by oxidation of corresponding aldehydes or primary alcohols.
(Phenols, Carboxylic acids, ketones, none of these)
66. The chemical properties of the carboxylic acids depend chiefly on the __________.
(Hydroxyl group, Carbonyl group, Methyl group, none of these)
67. __________ is used for coagulating rubber and latex and curing fish as well.
(Alcohol, Acetic acid, Wood spirit, none of these)
68. Ethyl acetate is an example of a important class of substance known as __________.
(Ketones, Esters, Alcohols, none of these)
69. Ethyl acetate (an ester) can be prepared by the action of __________ on carboxylic acid, in the presence of acidic media.
(Phenols, Formalin, Pyradine, Alcohol)
70. Molecular hydrogen in presence of suitable catalysts reduces carbonyl compounds to __________.
(aCetones, Ethers, Esters, Alcohols)
71. __________ is used as a nail-polish remover.
(acetone, Benzene, Idoform, none of these)
72. Acetone may be converted into propane by heating with __________.
(conc HCl and 24/Hg, Mg + H2O, conc HI and red P, Zn/Cu couple and ethanol)
73. __________ is the solvent used in the preparation of Grignard’s reagent and in Wurtz reaction.
(Ethers, Phenoles, Ketons, Alcohols)
74. The hydroxyl group derivatives of aromatic hydrocarbons, which have
the –OH group directly bonded to the ring carbon atoms are called
__________.
(Esters, Acetons, Alcohols, Phenols)
75. Carbolic acid is prepard from __________.
(Dow’s Process, Down’s Process, Nelson’s Process, none of these)
76. Phenol is colourless, poisonous __________.
(Liquid, Gas, Solid, none of these)
77. Above __________ °C phenol is miscible with water in all
proportions, but below this temperature, it is only partially miscible.
(78.5, 68.5, 58.5, none of these)
78. Phenol is reduced to __________ when its vapours are passed over red
hot zinc dust or distilled in the presence of zinc dust.
(Alcohol, Benzene, acetone, none of these)
79. Action of zinc with alkyl halide in the presence of an inert solvent
forms a corresponding higher alkane. This is called __________.
(Wurtz’s reaction, Frankland’s reaction, Hoffman’s reaction, none of these)
80. The hydrolysis of alkyl halides by heating with aqueous alkali is a __________ substitution reaction.
(Electricphilic, Nucleophilic, Electrophilic and Nucleophilic, none of these)
81. __________ is prepared by heating methyl iodide with fresh magnesium turnings in anhydrous ether.
(Grignard’s reagent, Mustards gas, Benzene, none of these)
82. Dry carbon dioxide is passed through Grignard’s reagent in the presence of __________.
(Acetone as a solvent, Benzene as a solvent, Ether as a solvent, none of these)
Chapter 10
Chemistry of Life
1. Starch is a polymer of __________.
(Glucose, Fructose, Lactose, Maltose)
2. A material cannot be termed as food unless it contains at least one __________.
(Vitamine, Mineral, Nutrient, Amino acid)
3. On heating glucose with Fehling’s solution we get a precipitate of colour __________.
(Yellow, Red, Black, Green)
4. It is the best to carry out reactions with sugars in neutral or acid
medium and not in alkaline medium. This is because in alkaline medium
sugars undergo __________ of the following changes.
(Racemisation, Decomposition, Inversion, Rearrangement)
5. __________ food component regulates body processes.
(Minerals, Fats, Proteins, Carbohydrates)
6. The process by which large non-diffusuble organic molecules are
converted into smaller diffusible molecules is known as __________.
(Ingestion, Fermentation, Decomposition, Digestion)
7. The solution of sugar in water contains __________.
(Free atoms, Free ions, Free molecules, Free atoms, and free molecules)
8. During digestion carbohydrates are broken down to __________.
(Glucose, Amino acids, Fatty acids, None of these)
9. During digestion proteins are broken down to __________.
(Glucose, Amino acids, Fatty acids, none of these)
10. __________ of the following gives a deep blue colour with a drop of dilute solution of iodine.
(Cellulose, Glucose, Starch, Sugar)
11. During digestion fats are broken down to __________.
(Glucose, Amino acids, Fatty acids, none of these)
12. The use of the products of digestion in synthesis of cellular structure is known as __________.
(Metabolism, Assimilation, Homeostasis, None of the above)
13. The percentage of glucose in human blood is __________.
(0.1, 0.2, 9.3, 0.4)
14. Carbohydrates supply about __________ of energy per gram.
(4 kcal, 2 kcal, 2 kcal, 1 kcal)
15. The main source of cellulose is __________.
(cotton, wood, both cotton and wood, none of these)
16. Fats provide about __________ of energy per gram.
(4kcal, 2 kcal, 9kcal, 5kcal)
17. Of the following, __________ is a high-energy food.
(Proteins, Fats, Carbohydrates, none of these)
18. Glucose and fructose are __________.
(Geometrical Isomers, Metamers, Optical Isomers, none of these)
19. __________ isomers of glucose are known.
(4, 8, 16, 32)
20. The digestion of carbohydrates begins with the mastication in the
mouth, where enzyme __________ of the saliva hydrolyses some of the
starch to maltose.
(Ptyalin, Amylase)
21. Human body tissue contains __________% carbohydrates.
(1, 2, 3, 4)
22. Carbohydrates are ultimately converted into glucose and other simpler products in the __________.
(Mouth, Stomach, Small intestine, Large intestine)
23. The use of products of digestion in synthesis of cellular structures is called __________.
(Assimilation, Metabolism, Excretion, Digestion)
24. The products of oxidation of glucose are __________.
(Carbon dioxide and water, Oxygen and Hydrogen, Carbon dioxide and hydrogen, none of these)
25. Glucose is termed as __________.
(Single nutrient food, double nutrient food, multi nutrient food, none of these)
26. Deficiency of all nutrients leads to __________.
(Nutrition, Malnutrition, Under Nutrition, none of these)
27. The recommended daily intake of protein per kilogram of the body weight is __________.
(0.8 gm, 0.9 gm, 0.6 gm, 1.0 gm)
28. Lipids and Proteins are made of __________.
(Macromolecule, Micromolecule, Microatom, None of these)
29. The digestion of proteins begins in the __________.
(Mouth, Stomach, Small intestine, Large intestine)
30. The enzyme __________ of gastric juice, catalyses the hydrolysis of peptide linkage in protein molecules.
(Renin, Trypsin, Pepsin, Amylase)
31. In the mouth of some of the starch is hydrolyzed to maltose by the action of enzyme __________.
(Ptylin, Lipase, Renin, Amylase)
32. In the body dietary proteins are the source of __________,
(Amino acids, Fatty acids, Lipids, none of these)
33. A large class of compounds that are polyhydroxy aldehydes or
ketones, or substances that yield such compounds upon acid hydrolysis
are called __________.
(Fats, Carbohydrates, Proteins, vitamins)
34. Plants are able to synthesis their own carbohydrates from CO2 of the
air and water taken from the soil in the presence of sunlight and
chlorophyll. This process is called __________.
(Nutrition, Assimilation, Photosynthesis, Homeostasis)
35. Human diet consist of 60 – 65% by mass of the average diet on __________.
(Fats, Carbohydrates, Proteins, vitamins)
36. Carbohydrates, which have three to nine carbon atoms and are not hydrolysable are called __________.
(Monosacchrides, Ddi-saccharides, Poly-saccharides, None of these)
37. The carbohydrates, which have three to nine carbon atoms and are not hydrolysable are called __________.
((Monosacchrides, Ddi-saccharides, Poly-saccharides, None of these)
38. The balanced diet contains amount __________ per day.
(60 gm, 70 gm, 80 gm, 90 gm)
39. Glucose is __________.
(a monosacchride carbohydrate, a di-saccharide carbohydrate, a poly-saccharide carbohydrate, none of these)
40. A class of carbohydrates which are formed by the condensation of two
or more monosaccharide units with the loss of water molecules are
called __________.
(Disaccharides, Poly saccharides, Pentoses, none of these)
41. Sucrose is an example of __________.
(a monosacchride carbohydrate, a di-saccharide carbohydrate, a poly-saccharide carbohydrate, none of these)
42. On hydrolysis __________ is broken down into two simpler sugars glucose and fructose.
(Glucose, Sucrose, Maltose, none of these)
43. Glucose is also called __________.
(Dextrose, Maltose, Fructose, Mannose)
44. Corn syrup contains __________.
(Glucose, Fructose, Mannose, Maltose)
45. Fructose occurs in many __________.
(Cereals, Fruits, Vegetables, none of these)
46. Honey is a mixture of __________.
(Glucose and Fructose, Glucose and Maltose, Fructose and Mannose, Glucose and Fructose with vitamins and minerals)
47. The carbohydrates, which contain hundreds to thousands of monosacchride units are called __________.
(Polysacchrides, Oligosaccharides, Hexoses, None of these)
48. Cellulose is an example of __________.
(Monosaccharides, Di-saccharides, Polysaccharides, None of these)
49. The main difference between starch and cellulose is the type of links between __________.
(Mannose units, Glucose units, Fructose, units, none of these)
50. Vitamin was discovered by __________.
(Casimir Funk, Blackeland, Hopkins, Elmer)
51. Vitamin A was discovered by __________.
(Elmer McCollum, Casimir funk, Hopkins, none of these)
52. Vitamin D was discovered by __________.
((Elmer McCollum, Casimir funk, Hopkins, none of these)
53. Fat-soluble vitamins are found associated with __________ in natural foods.
(Renin, Lipids, Peptides, Maltose)
54. Fat soluble vitamins include __________.
(Vitamin A, B, C, D, Vitamin A, B, C, Vitamin A, D, E, K, Vitamin K)
55. Water-soluble vitamins include __________.
(Vitamin A, B, Vitamin A, B, C, vitamin B, C, Vitamin A, C)
56. Vitamin B1 is called __________.
(Thiamin, Riboflavin, Niacin, Pyridoxine)
57. Vitamin B2 is called __________.
(Thiamin, Riboflavin, Niacin, Pyridoxine)
58. Vitamin B5 is called __________.
(Thiamin, Riboflavin, Niacin, Pyridoxine)
59. Vitamin B6 is called __________.
(Thiamin, Riboflavin, Niacin, Pyridoxine)
60. Vitamin B12 is called __________.
(Cyanocoalamine, Riboflavin, Niacin, Pyridoxine)
61. Most water-soluble vitamins act as __________.
(Enzymes, Coenzymes, Coenzymes or are required for the synthesis of coenzymes, none of these))
62. People who consume too much vitamin __________, may develop bone
pain, bone like deposits in the kidneys, and mental retardation.
(A, B, C, D)
63. Edible lipids constitute approximately __________ % of the diet of an average person.
(25-28, 25-30, 25-32, 25-35)
64. The most important energy storage compounds in the animal kingdom are __________.
(Peptides, Lipids, Amino acids, none of these)
65. Plants store most of the energy in the form of carbohydrates primarily as __________.
(Amino acids, Starch, Cellulose, Maltose)
66. The nutrients of our food which provide insulation for the vital
organs, protecting them from electrical shocks and maintaining optimum
body temperature are called __________.
(Amino acids, Steroids, Lipids, Fatty acids)
67. Lipids that contain both polar and non polar groups are integral components of __________.
(Cell wall, Cell membrane, Cytoplasm, Mitochondria)
68. Steroids is an important type of __________.
(Proteins, Vitamins, Lipids, Carbohydrates)
69. The most abundant and the most important steroid in the human body is __________.
(Riboflavin, Cholestrol, Folic acid, Inositol)
70. __________ is an important precursor in the biosynthesis of sex-hormones, synthesis of adrenal hormones and vitamin D.
(Insitol, Cholestrol, Lipoic Acid, Biotin)
71. On the average, more than 50% of the total dry weight of the cells is composed of __________.
(Carbohydrates, Proteins, Fats, Water)
72. The Dutch chemist, GJ Mulder (1883), is credited as being one of the
first scientists to recognize the importance of __________.
(Vitamins, Carbohyrates, Proteins, Fats)
73. __________ organic compound is a major structural component of an animal tissue.
(Carbohydrates, Proteins, Cellulose, Lipids)
74. Hormones are made of __________.
(Proteins, Fats, Carbohydrates, Lipids)
75. Antibodies are __________.
(fats in nature, carbohydrates in nature, protein in nature, vitamins in nature)
76. Enzymes are __________.
(carbohydrates in nature, proteins in nature, fats in nature, none of these)
77. Haemoglobin is a __________.
(Protein, Carbohydrate, Fat, Mineral)
78. The primary function of proteins is __________.
(Energy supply, body building, body building and maintenance, protection of body)
79. __________ nutrients of food are stored by the body as energy reserves.
(Carbohydrates and lipids, proteins and lipids, proteins and carbohydrates, none of these)
80. for a normal adult with a constant weight, the recommended daily
intake of protein is approximately __________ gram per kg of body
weight.
(0.2, 0.4, 0.6, 0.8)
81. 33% - 43% protein is present in __________.
(Food yeast, Soya bean, Rice, Cheese)
82. The percentage of protein in chicken food is __________%.
(28, 21, 33, 12)
83. The protein in milk is __________%.
(2, 3, 12, 19)
84. Fats are esters of glycerol and __________.
(Faty acids, Lipids, Steroids, none of these)
85. The percentage of protein in egg is __________%.
(12-18 , 12-24, 12-36, 12-48)
86. The percentage of protein in flour is __________%.
(18, 12, 6, 3)
87. The percentage of protein in fish is __________%.
(18-21, 12-18, 6-36, 3-9)
88. The percentage of protein in rice is __________%.
(6-7, 2-3, 5-11, 11-19)
89. The percentage of protein in fresh vegetables is __________%.
(5-6, 7-17, 4-7, Rarely contains 2-3)
90. Amino acids are the building blocks of __________.
(Carbohydrates, Proteins, Lipids, Fats)
91. Proline amino acids have __________ group and –COOH group attached to the same carbon atom.
(-NH3, -NH2, -NH, -OH)
92. Amino acids are widely classified __________.
(according to the number of –NH2 group, according to the number of –COOH
group, according to polarity of their side chain, all of these)
93. The first amino acid was isolated in 1806 and was given the name __________.
(Asparangine, Glycine, Renin, Maltose)
94. The major amino acid found in gelatin is __________.
(Glycine, Asparangine, Renin, none of these)
95. Esters of Glycerol and Fatty acids are called __________.
(Acids, F, Proteins, Carbohydrates)
96. Among the most important of the natural __________ are the cotton seed oil, corn oil, butter, tallow and olive oil.
(Fats, Proteins, Carbohydrates, Vitamins)
97. Unsaturated vegetable oils, such as cotton seed oil are converted into fast on __________.
(Oxidation, Dehydration, Hydrogenation, Sulphonation)
98. The hydrogenation of oils is accomplished easily by bubbling hydrogen into the oil in the presence of catalyst __________.
(Pt, Ni, Zn, ZnO)
99. Naturally occurring fatty acid nearly always have an/a __________ number of carbon atoms.
(Even, Odd, Even and odd, none of these)
100. Liquid fats are called __________.
(Fatty acids, Oils, Ketones, Lipids)
101. The degree of undaturation of a fat or oil is usually measured by the __________.
(number of carbon atoms, number of hydrogen atoms, iodine number, none of these)
102. The number of grams of iodine that will be consumed by 100 grams of fat or oil is called __________.
(Iodine complex, Iodine number, Iodoform, None of these)
103. Brain cells are made of __________.
(Proteins, Fats, Carbohydrates, Lipids)
104. Nerve tissues are made of __________.
(Fats, Proteins, Carbohydrates, Steroids)
105. Fat-soluble vitamins are obtained from __________.
(Carbohydrates, proteins, fats, lipids)
106. Vegetable oils such as peanut oil contain vitamin __________.
(A, B, C, E)
107. Milk fat, butter, cream, and fish liver oil contain vitamin __________.
(A, B, C, A and D)
108. Our balanced diet contains 70 grams per day of __________.
(Carbohydrates, Proteins, Fats, None of these)
109. About 35% of our daily caloric requirements are obtained from __________,
(Carbohydrates, Proteins, Fats, Vitamins)
110. __________ is the term used to reflect the development of any disagreeable odour in the fat or oil.
(Acidity, Basicity, Rancidity, none of these)
111. Two principal chemical reactions responsible for causing rancidity are __________.
(Oxidation and Hydrogenation, Oxidation and Hydrolysis, Hydrolysis and fermentation, Oxidation and Pyrolysis)
112. The reaction of fat with a strong base such as NaOH to produce
glycerol and the salt of a fatty acid is used to produce __________.
(Soap, Glucose, Vegetable oil, Gastric Juice)
113. The word enzyme has a __________.
(Greek origin, Latin origin, Roman origin, Arabic origin)
114. In living systems enzymes catalyze reactions at __________°C.
(0, 25, 100, 37)
115. The substance upon which an enzyme acts is known as its __________.
(base, substrate, nutrient, pair)
116. The amount of enzyme, which will catalyze the transformation of one
micro-mole of a substrate per minute is termed as __________.
(Substrate, potency, activity, specific activity)
117. Units of enzyme per milligram of proteins are termed as __________.
(activity, potency, turn over, none of these)
118. The number of moles of substrate transformed per mole of enzyme per minute at a definite temperature is called __________.
(Potency, Turn over, Activity, none of these)
119. Enzymes are most commonly named by adding the suffix to the root of the name of the substrate __________.
(ose, ase, ane, ene)
120. Urease acts upon __________.
(Sucrose, Urea, Ammonia, Starch)
121. Sucrose is also called __________.
(invertase, Urea, Renin, Amylase)
122. __________ is an enzyme.
(Sucrose, Sucrase, Maltose, Urea)
123. __________ enzyme was first obtained by grinding pancreatic tissue with glycerol.
(Amylase, Urea, Ascorbic Acid Oxidase, Trypsin)
124. The site of the enzyme, which combines with the substrate, and at
which transformation from substrate to products occurs, is called he
__________.
(Cellular site, Active site, Vacant site, Complex)
125. The main factors, which effect enzyme activity, are __________.
(concentration, temperture and pH, concentration, temperature, pH and
co-enzymes, concentration, temperature, pH, co-enzymes (activators and
inhibitors) and radiation, co-enzymes, activators and inhibitors)
126. The majority of enzymes are most active at about __________ °C.
(35, 45, 55, all of these)
127. Many enzymes contain a protein part and a non-protein part. The protein part is called the __________.
(Apoenzyme, Coenzyme, Enzyme, none of these)
128. The non-protein part in enzyme is termed as __________.
(Apoenzyme, coenzyme, substrate, all of these)
129. Examples of co-enzymes are __________.
(Vitamins, Compounds derived from vitamins, Vitamins or compounds derived from vitamins, all of these)
130. In organic substances that tend to increase the activity of an enzyme are called __________.
(activators, Inhibitors, Apoenzymes, coenzymes)
131. Magnesium ion is an inorganic activator for the enzyme __________.
(Trypsin, Carbonic anhydrate, Sucrase, Phosphatase)
132. Zinc ion is an activator for the enzyme __________.
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(Amulase, Carbonic anhydrase, Renin, Phosphatase)
133. Substances, which tend to decrease the activity of enzyme are called __________.
(Activators, Accelerators, Inhibitors, Retarders)
134. Enzymes are generally inactivated rapidly by exposure to __________.
(Ultraviolet light, b-rays, g-rays, X-rays, all of these)
Chapter 11
Chemical Industries in Pakistan
1. The substances added to the soil to provide one or more nutrient elements essential for plants growth are called __________.
(Growth hormones, Minerals, Fertilizers, Salts)
2. The substances added to the soil in very small amounts (about 6 grams to 200 grams per acre) are called __________.
(Macronutrients, Micronutrients, Fertilizers, none of these)
3. Fertilizers are classified into __________.
(two major categories, three major categories, four major categories, none of these)
4. Natural fertilizers are materials derived from __________.
(plants, animals, algae, all of these)
5. A natural fertilizer provide about __________ kg of nitrogen.
(4.5, 3.2, 2.2, 1.5)
6. A natural fertilizer provides __________ kg of P2O5.
(4.5, 3.2, 2.2, 1.5) A
7. A natural fertilizer provides __________ kg of potash (K2O).
(4.5, 3.2, 2.2, 1.5)
8. The percentage of nitrogen in ammonia is __________%.
(32, 55, 82, 25)
9. The percentage of nitrogen in ammonium Nitrate is __________%.
(32-33.5, 50-55, 80-82, 20-25)
10. The percentage of nitrogen in ammonium sulphate is __________%.
(27, 21, 23, 19)
11. The percentage of sulphur in ammonium sulphate is __________%.
(25, 21, 23, 19)
12. The percentage of nitrogen in Urea is __________%.
(37, 50, 46, 82)
13. Ammonia when used directly as a fertilizer is to be injected about __________ under the surface to keep it from seeping out.
(2 inches, 4 inches, 6 inches, 8 inches)
14. Ammonium nitrate is sold as a mixture with __________.
(Soda Ash, Limestone, Zinc, None of these)
15. The percentage of nitrogen in Diammonium hydrogen phosphate is __________%.
(16, 48, 32, 64)
16. The percentage of P2O5 in diammonium hydrogen phosphate is __________%.
(16, 32, 48, 64)
17. A fertilizer; potassium chloride is sold as __________.
(Muriate of potash, Mixture of potash, Potency of potash, none of these)
18. The percentage of K2O in potassium chloride is __________%.
(60-63, 50-70, 40-80, 30-90)
19. Potassium sulphate with 48% to 52% potash, is made from __________.
(Potassium Phosphate, Potassium Chloride, Potassium Nitrate, none of these)
20. __________ is preferred for horticultural crops and for tobacco and potatoes.
(Potassium chloride, Potassium sulphate, Potassium Nitrate None of these)
21. __________ is used for fruits, vegetables and tobacco.
(Potassium chloride, Potassium sulphate, Potassium Nitrate None of these)
22. Any material, which changes the cleaning effect of water, is called __________.
(Fertilizers, Detergent, Acid none of these)
23. __________ are sodium and potassium salt of long chain fatty acids.
(Soaps, Detergents, Fertilizers, None of these)
24. __________ contain sodium or potassium salts of aryl or alkly sulphonated acids as one of their constituents.
(Soaps, Detergents, Fertilizers, none of these)
25. Soap is a surfactant of the type __________.
(anionic, cationic, nonionic, none of these)
26. __________ is best in its cleaning action.
(Soap, Detergents, Surfactant, None of these)
27. Hydrolytic reaction of fat with caustic soda is known as __________.
(Esterification, Saponification, Acetylation, Carboxylation)
28. Turpentine is obtained from __________.
(Oak tree, Pine tree, Birch tree, Lemon tree)
29. __________ surfactants perform well over a wide range of water hardness and pH.
(Anionic, Cationic, Nonionic, none of these)
30. Fats and oils are __________.
(Acids, alcohols, salts, none of these)
31. Washing soap can be prepared by saponification with alkali of __________ of the following oil.
(Rose oil, Paraffin oil, Groundnut oil, Kerosene oil)
32. Commercial detergents contain mainly __________.
(RCOON, RONa, RSNa, ROSO3Na)
33. Sodium tripolyphosphate is __________.
(a surfactant, a builder, a auxiliary agent, none of these)
34. In glass or vitreous state solid the atoms are arranged in __________.
(Regular fashion, Random fashion, Linear fashion, none of these)
35. Glass was first made by about __________.
(40BC, 400BC, 4000BC, none of these)
36. The number of glass products now manufactured is __________.
(25,000, 50,000, 75,000, none of these)
37. The substance that can form the glassy, non-crystalline structure is called __________.
(Formers, Fluxes or modifiers, Stabilizers, none of these)
38. The principle former of almost all glasses is __________.
((SiO2)n, (SiO3)n, (SiO2)X, none of these)
39. Chemical compounds, which are added to reduce the reactivity of glass, are called __________.
(Formers, Modifiers, Stabilizers, none of these)
40. __________ is used as stabilizer.
(Ca2O, SiO2, Na2O, none of these)
41. In glass making the whole combination of ingredients is called a __________.
(Gangue, Batch, Mixture, none of these)
42. The melting of nearly all glass is done in a continuous tank
furnace, which operates steadily over periods of up to __________.
(a day, a month, a year, none of these)
43. __________ is a heat-treatment cycle that prevents glass from harmful stress.
(Forming, Annealing, Batching, none of these)
44. __________ is used for Annealing.
(Klin, Batch, Converter, Oven)
45. The main constituents of __________ are boron oxide and silica.
(Pyrex glass, Soda-lime glass, Low silica glass, Fibrous glass)
46. In Pakistan how many units are involved in the production of glass __________.
(20, 25, >25, none of these)
47. In Pakistan the total production of glass is over __________ tons per year.
(800, 8000, 80,000, none of these)
48. Asbestos is a __________.
(Mineral fibre, Animal fibre, Vegetable fibre, none of these)
49. __________ is the fibre in which the basic polymer (fibre forming
substance) is a long chain composed of least 85% by weight of
Acrylonitrile units.
(Acrylic Fibre, Modacrylic fibre, Polyster fibre, Rayon Fibre)
50. The fibre, which has less than 85% but more than 35% proportion by weight, of acrylonitrile units is called __________.
(Acrylic fibre, Modacrylic fibre, Polyster fibre, Rayon fibre)
51. __________ is the fibre in which the fibre-forming substance is a
long chain synthetic polymer composed of at least 85% by weight of an
ester of a dihydric alcohol and terephthalic acid.
(Acrylic fibre, Modacrylic fibre, Polyster fibre, Rayon fibre)
52. __________ is a fibre composed of regenerated cellulose in which
substituents have replaced nor more than 15% of the hydrogen of the
hydroxyl group.
(Acrylic fibre, Modacrylic fibre, Polyster fibre, Rayon fibre)
53. __________ compound contains cellulose acetate as fibre forming substance.
(Acrylic fibre, Modacrylic fibre, Acetate fibre, Rayon fibre)
Chemistry MCQs 2nd year 2nd Year Chemistry Notes http://karachiboardnotes.blogspot.com/ Chemistry MCQs 2nd year Five Year Papers 1. On p...