F.sc.Part.2.Chemistry.(Chapter Wise Tests& Their Solution) - Malik Xufyan

2021
CHEMISTRY PART-2: SOLUTION MANUAL BY MALIK XUFYAN
S u p e r W i n g s G r o u p o f C o l l e g e s R a w a l p i n d i Page 1
Name: Class: 12 Portion inorganic
Paper: Chemistry Objective Part Marks: 17
Time: 20 Minutes. Test: 11 Chapter no: 1
Q.1. Each question has FOUR possible answers. Choose the correct answer and encircle it. 17
Sr#. Statement. A B C D
1. Elements of which group form
anions readily?
Oxygen
family
Halogens Alkali
metals
Nitrogen
family
2. Elements on the right side of
periodic table are:
Metals Metaloids Non-
metals
Transition
metals
3. Ionization potential is
maximum for
B Al Ga In
4. Which pair has both members
from same period of periodic
table?
Na-Ca Na-Cl Ca-Cl Cl-Br
5. Which of the following metal
gives an amphoteric oxide?
Ca Fe Cu Zn
6. Elements which exhibit
similarity horizontally and
vertically are:
Coinage
metals
Transition
metals
Alkali
metals
Inert
gases
7. Doberiener arranged elements
in groups called:
Monoad Triad Tetrad Pentad
8. The present periodic table is
given by:
Al-Razi Medeleve Moseley Newland
9. The 6 period contain elements
to anout:
16 18 32 8
10. Hydrogen generaly placed: Above alkali
metals
At the bottom
of alkali metals
In the
middle of
alkaline
earth
metals
Above
the noble
gases
11. 1pm is equal to: 10⁻22
m 10⁻14
m 10⁻12
m 10⁻10
m
12. The atomic radius of oxygen
is:
69pm 66pm 79pm 76pm
13. What type of metals are not
used in our daily life as a
metal:
Zn,K Na,Sr Zn,Na Na,K
14. Ionic halides are strong: Electropositve
elements
Electronagetive
elements
Both None
15. Acidic oxides are: Metals Non-metals Both None
16. Oxidation states of metal effect
by
Acid Basis Both None
17. Which is not an alkali metal? Francium Caesium Rubidium Radium

2021
SECTON –I
Q 2. Give the short answers of the following
EIGHT questions. 16
i. Define periodic table.
ii. What is Newlands’s law of octaves?
iii. Why d and f- block elements are transition
elements?
iv. Why the size of cation is smaller than
parent atom?
v. Why the ionic radii of negative ions are
larger than the size of their parent atom?
vi. Why ionization energy decreases down the
group and increases along the period?
vii. Why the second value of electron affinity
of an element is shown with a positive
sign?
viii.Why the metallic character increases from
top to bottom in a group of metal?
Q 3. Give the answers of the following
EIGHT questions.
16
i. Why the oxidation state of noble gases is
usually zero?
ii. Why diamond is a non-conductor and
graphite is fairly a good conductor?
iii. Differentiate b/w acid oxides basic and
amphoteric oxides.
iv. Define oxidation states and hydration
energy.
v. What is meant by the electrical
conductivity? This property depends upon
different factors also write down.
vi. How blocks help to differentiate the
different elements? Explain.
vii. Give some properties which are similar to
the IVA group elements.
viii.Define atomic radius and ionic radii.
Q 4. Give the answers of the following SIX
questions.
12
i. Why atomic radius increases down the
group? Explain.
ii. What factors effecting on ionization
energy along period and group? Explain.
iii. What is meant by the metallic character?
What do you know about this?
iv. Give the behavior of melting and boiling
points along behavior.
v. Differentiate b/w ionic and covalent
halides.
vi. Differentiate b/w ionic and intermediate
halides.
SECTION-ll
Give the answers of the following THREE
questions.Each question is of FOUR marks.
24
Q 5.A) What type of improvements is made in
Mandeleve’s periodic table?
A) Classify the oxides on the basis of their
acidic and basic character.
Q 6.A) What problems that faced the chemists in
placing the hydrogen atom in the periodic table ?
Explain.
B) Discuss the periodic trends of melting
and boiling points.
Q 7.A) Define and explain hydration energy.
B) Discuss about the position of hydrides
and oxides.
Name: Class: 12 Portion Inorganic
Paper: Chemistry Subjective Part Marks: 68
Time: 2:40 Super Wings College Chapter no: 1

2021
SECTON –I
Q 2. Give the short answers of the following EIGHT questions. 16
i. Define periodic table.
The arrangement of elements in a systematic manner, in order to correlate their properties is
called periodic classification. The resulting table is called periodic table.
ii. What is newland’s law of octates?
In 1864, an English chemist, Newland arranged elements in order of their increasing atomic
masses. He found that
“Every eight elements had properties in common with first one.”
For example: first two octaves of Newland’s are
Li Be B C N O F
Na Mg Al Si P S Cl
Li resembles Na, Be resembles Mg etc.
iii. Why d and f- block elements are transition elements?
d and f block elements have variable oxidation states. They have different chemical and
physical properties. They have different number of electrons in their valance orbit. Therefore,
d and f block elements are also called transition elements.
iv. Why the size of cation is smaller than parent atom?
The size of cation is smaller than parent atom due to these following reasons.
 Many atoms lost their valance or outermost shell due to the removal of one or more
electrons.
 In positive ions number of electrons are reduced but positive charge on nucleus is same.
Therefore, nucleus powerfully attracts outer electrons inward resulting in decrease of
ionic radius.
v. Why the ionic radii of negative ions are larger than the size of their parent atom?
Ionic radii of negative ions are larger due to increase in number of electrons in valance shell.
The size of parent atom is decreased , it is because number of electrons are less in parent
atom than negative ion. When an atom accepts an electron, it takes a negative charge and its
size is increased. Its ionic radius also increased but its positive charge on electron remains
same.
vi. Why ionization energy decreases down the group and increases along the period?
Ionization energy decreases down the group due to increase in the size of atom. Number of
shells increases down the group. Therefore, the size of atom increases and the attraction b/w
the nucleus and valance electrons is decreased. An eletron can easily be removed from the
atom due to increase the atomic radius and small amount of energy is required. Therefore,

2021
ionization energy decreases down the group. Ionization energy is increased along the period
due to the strong attraction of nucleus to their electrons and atomic radius is also decreased.
An electron cannot be removed from the atom due to the strong attraction of nucleus to their
electrons. A large amount of energy is required to remove electron from atom. Therefore,
ionization energy increases along the period.
vii. Why the second value of electron affinity of an element is shown with a positive
sign?
When a second electron is added in a un-negative ion, the incoming electron is repelled by
the negative ion and energy is absorbedin the process indicated by the positive figure.
e.g;
O(g) + eˉ Oˉ E.A1 = -141kJmol-1
O(g) + eˉ O2
ˉ E.A2 = +780kJmol-1
viii. Why the metalic character increases from top to bottom in a group of metal?
Metalic character increases from top to bottom due to increase in atomic size.
e.g;
in halogens, metallic character increases from top to bottom. Thus, the iodine is most
metallic.
Q 3. Give the answers of the following EIGHT questions. 16
i. Why the oxidation state of noble gases is usually zero?
Oxidation state of noble gases is usually zero. It is because no vacancy is present in their
valance shell. No electron will be added in the noble gases. All the shells in noble gass is
completed. Therefore, noble gases are also called zero group elements.
ii. Why diamond is a non-conductor and graphite is fairly a good conductor?
In diamond, C in the form of diamond is non-conductor. It is because all its valance electrons
are used up in making tetrahedral structure and no free electron is present in it.
But C in the form of graphite is a good conductor. It is because it has free valance electrons.
iii. Differentiate b/w acid oxides basic and amphotaric oxides.
Acid Oxides Basic Oxides Amphotaric oxides
i) Oxides of non-metals are i) Oxides of metals are i) Oxides of relatively
less
generally acidic. generally basic. electropositive
elements. E.g; BeO.
ii) These form acids in ii) These form bases in ii) They show
properties of both
water. water. acidic and basic
oxides.
iv. Define oxidation states and hydration energy.

2021
Oxidation state is defined as:
“It is apparent charge with sign, which an atom has in a compound.”
e.g; In ionic compounds, It is usually the number of electrons gain or lost. In NaCl, oxidaion
state of
Na is +1 and that of chlorine is -1.
Hydration energy is defined as:
“it is the amount of heat evolved or absorbed when 1 mole of ions dissolve in
H2O to give infinetly dilute charge.”
e.g; when 1 mole of gaseous hydrogen ions are dissolved in water, 1075 kj energy is
released.
H⁺ + H2O H3O⁺(aq) ∆H h = -1075kmol-1
v. What is meant by the electrical conductivity? This property depends upon
different factors also write down.
Electrical conductivity is a property of elements that causes the electricity. This property is
due to the free electrons in elements. Free electrons are present in metals. Therefore, metals
are the good conductor of electricity. This property depends upon:
 Presence of loose electrons in valance shell of elements.
 Easy removal of loose electrons.
vi. How blocks help to differentiate the different elements? Explain.
Modern periodic table is divided into four blocks on the basis of valance shell electronic
configuration.these blocks are:
i) s-block ii) p-block iii) d-block iv) f-block
These blocks tells about the valance shell of electrons of elements and their properties
especially valancy and oxidation state.
 s-block elements are the elements in which valance electrons are present in s-orbital.
 p-block elements are the elements in which valance electrons are present in p-orbital.
 d-block elements are the elements in which valance electrons are present in d-orbital.
 f-block elements are the elements in which valance electrons are present in f-orbital.
vii. Give some properties if hydrogen which are similar to the IVA group elements.
There are following properties are present in IVA group elements which is similar to
hydrogen atom.
 Valance shell of hydrogen is half filled like group IVA elements.
 Both hydrogen and group IVA members combine with other elements through
covalent bonds.
 Like carbon, hydrogen has strong reducing properties.
e.g. CuO + H2 Cu + H2O
viii. Define atomic radius and ionic radii.

2021
The average distance b/w the nucleus of an atom and the outermost orbit is called atomic
radius, while considering atom as spherical. The atomic radii are usually measured in
picometer (pm).
1 pm = 10-12
m
The radius of ion while considering it spherical is called ionic radius. It is also measured in
picometer (pm).
Q 4. Give the answers of the following SIX questions. 12
i. Why atomic radius increases down the group? Explain.
Atomic radius increases down the group due to three two factors.
i) Increase in number of shell ii) Shielding effect
From up to down number of shell increases and the size of atom is also increased.
Therefore, atomic radius is also increased.
It is the decrease in force of attraction b/w outermost shell and nucleus due to the inner shell
electrons. Shielding effect increases due to increase in size of atom. Therefore, atomic
radius is also increased.
ii. What factors effecting on ionization energy along period and group? Explain.
Following factors effecting on ionization energy along period.
 From left to right in the periodic table magnitude of nuclear charge increases and
I.E is also increased.
Following factors effecting on ionizatin energy along group.
 Along group, atomic radii increased and the I.E decreased.
 Greater the shielding effect of inner shell of electrons lower will be the I.E and
vice verca.
iii. What is meant by the metallic character? What do you know about this?
Elements those have the tendency to give or gain electrons, form positive or negative ions
and also forms basic or acidic oxides which dissolve in water to form bases or acids.
E.g. Na2O + H2O 2NaOH
SO3 + H2O H2SO4
Metals are the good conductors of heat and electricity. While non-metals are the bad
conductors of heat and electricity. Metallic character decreases from left to right due to
decrease in atomic size. Metallic character increases from up to down due to increase in
atomic size.
iv. Give the behavior of melting and boiling points along period.
In short periods, melting points increases up to middle with the increase in valance electrons
and then decreases up to noble gases.
 Group IA elements have lowest melting points because they provide one electron per
atom for binding.

2021
 Group IIA elements have slightly higher melting points because they provide two
electrons for binding.
 Carbon provides maximum number of binding electrons. Thus, it has highest melting
point.
 Melting point decreases from group IVA to noble gases. It is because members of the
last groups, exist as single, small covalent molecules. These have weak
intermolecular forces. Thus, their melting points are low.
v. Define ionic and covalent halides.
1. Strong electropositive elements form ionic halide. it is because they have strong
electronegativity difference with halogens. Halides of group IA elements are purely
ionic. These have 3D crystal lattic. In ionic halides, strong intermolecular forces are
present. They are present high melting solids.
2. Covalent halides:
 In covalent halides, weak intermolecular forces are present.
 These are generally present as gases, liquids or low melting solids.
 Physical properties of covalent halides depend upon the size and polarizability of
halogen atom.
vi. Differentiate b/w ionic and intermediate hydrides.
Ionic hydrides Intermediate hydrides
i) These are ionic in nature. i) These are covalent in nature.
ii) They form basic solution with water. ii) They form acidic or basic
solution with
water.
iii) These are crystalline solids. iii) They may be in the form of
gases
or liquids or low melting
solids.
iv) Elements of group IA and heavier iv) hydrides of Be, Mg etc are
members of IIA form ionic hydrides. Intermediate.
SECTION-ll
Give the answers of the following THREE questions.Each question is of FOUR marks. 24
Q 5.A) What type of improvements is made in Mandeleev’s periodic table?
See the topic of improvements in Mandeleevs’ periodic table.
B) Classify the oxides on the basis of their acidic and basic character.
See the topic of oxides.
Q 6.A) What problems that faced the chemists in placing the hydrogen atom in the periodic
table? Explain.

2021
See the topic of position of hydrogen in the periodic table.
B) Discuss the periodic trends of melting and boiling points.
See the topic of Melting and boiling points.
Q 7.A) Define and explain hydration energy.
See the topic f hydration energy.
C) Discuss about the classification of hydrides and oxides.
See the topic of hydrides and oxides.

2021
Name: Class: 12 Portion inorganic
Paper: Chemistry Objective Part Marks: 17
Time: 20 Minutes. Super Wings College Chapter no: 2
Q 1. Each question has FOUR possible answers. Choose the correct answer and encircle it. 17
Sr#. Statement. A B C D
1. The hydroxide which is most
soluble in water is:
Ba(OH)2 Mg(OH)2 Sr(OH)2 Ca(OH)2
2. Dolomite is an ore of: Strontium Magnesium Barium Potassium
3. Down’s cell is used to prepare: Na2CO3 Na metal NaOH NaHCO3
4. Which metal is resistant to
complete oxidation?
Na K Be None
5. Which metal is not present
abundantly in earth crust?
Si Al Na O
6. Na metal cannot be stored under: Benzene Kerosene Alcohol Toluene
7. NaOH is prepared by the
hydrolysis of:
Molten
NaCl
Aqueous
NaCl
Aqueous
Na2CO3
Molten
Na2CO3
8. In manufacturing of caustic soda
,which is formed as a by-
product?
O2 Cl2 NaCl N2
9. Which one of the following is
most basic?
Al2O3 SiO2 P2O5 MgO
10. Which mineral is used in
isolation of sodium?
Lime stone Natron Halite Barite
11. Which ion will have the
maximum value of heat of
hydrogenation?
Na⁺ Cs⁺ Ba2
⁺ Mg2⁺
12. Which is not alkaline earth
metal?
Be Ra Ba Rn
13. The oxides of baryllium are: Acidic Basic Amphoteric None
14. The mineral CaSO4.2H2O has the
general name:
Gypsum Dolomite Calcite Epsom salt
15. The element Cs bears
resemblance with:
Ca Cr All None
16. Chile saltpeter had chemical
formula:
NaNO3 KNO3 Na2B4O7 Na2CO3.H2O
17. Gypsum is an important source
of
Na,K Na,Cl Ca,S Na,S

2021
SECTON –I
i. Give the occurrence of alkali metals.
ii. Define alkaline earth metals.
iii. What is meant by the peculiar behavior of lithium?
iv. What is meant by solubilities and lactic energies of alkal metals?
v. Give some reaction of oxygen with alkali metals.
vi. How alkali metals react with water?Give some reactions.
vii. How hydrogen and sulphur react with alklain earth metals?
viii. Why the aqueos solution of Na2 CO3 is alkaline in nature?
i. What happened when lithium is heated and lithium hydroxide is heated with water?
ii. Why lime water turns milky with CO2 but become clear with excess CO2?
iii. How gypsum is converted into plaster of paris?
iv. How lime mortar is prepared?
v. How lime and sand are used to make glass?
vi. Give formulas of following ores:
vii. Dolomite ii) Asbestos iii) sylvite iv) Beryl
viii. Describe the role of lime in agricalture.
ix. What is meant by slacked lime?
Q 4. Give the short answers of the following SIX questions. 12
i. What is the function of Ca in plant growth?
ii. What is meant by the setting of plater of paris?
iii. Give the some uses of plaster of paris.
iv. Describe the role of gypsum in agriculture.
v. What is meant by the carbonates of alkaline earth metals?
vi. What do you know about the reactivity of alkaline earth metals?
SECTION-ll
Give the answers of the following three questions.Each question is of FOUR marks. 24
Q 5. Explain in detail about the peculiar behavior of following:
A) Lithium B) Berylium
Q 6. A) Give the commercial preparation of sodium by Down’s cell in detail.
B) Give commercial preparation of NaOH by the diaphragm cell in detail.
Q 7. A) Describe the role of gypsum in industry.
B) Describe the role of lime in industry.

2021
Time: 2:40 Test: 12 Chapter no: 2
SECTON –I
i. Give the occurrence of alkali metals.
Alkali metals are highly reactive. Therefore, they do not occur free in nature. They are found
in combined state. Most of earth crust is made up of insoluble alumino silicates of alkali
metals.
 Na and K are more abundant and constitute to about 2.4% of earth crust.
 Li is found as complex mineral which are widely distributed. An important
commercial source of Li is the mineral spodumene i.e. LiAl(SiO3)2.
 Small amounts of Rb and Cs are found in K salts deposits.
 Fr is not occur in nature. it is radioactive element. It is produced in laboratory by
nuclear reaction. It is very unstable, therefore, its chemistry is not well known.
ii. Define alkaline earth metals.
Elements of group llA elements are called alklaine earth metals. They form ionic compounds.
they show +2 oxidation state. They have two electrons in ‘s’ orbital of their valance shell.
iii. What is meant by the peculiar behavior of lithium?
First member of each main group of periodic table does not follow the regular trends of the
group. Similarly Li shows difference from its family members. This behavior is due to the
following reasons.
 Both Li and Li+
ions have very small size.
 Li+
has high charge density.
 Li has less electropositivity than sodium.
iv. What is meant by solubilities and lattice energies of alkali metals?
Cations of alkali metals have low charge and large radii than the radius of any cations from
the same period. Thus lattice energies of their salts are low. Hence, most of the simple salts
of alkali metals are water-soluble. Most of the salts are ionized completely in aqueous
solution.
v. Give some reaction of oxygen with alkali metals.
Some reactions of oxygen with alkali metals are:
4Li + O2 2Li2O
Li2O + CO2 Li2CO3
4Na + O2 2Na2O
Rb + O2 RbO2
vi. How alkali metals react with water? Give some reactions.

2021
Alkali metals react with water rapidly. A small piece of sodium or potassium or lithium floats
on water and it reacts vigorously with water to liberate hydrogen and form metal hydroxide.
The reaction is highly exothermic. The heat is released may ignite the hydrogen.
2Na + 2H2O 2NaOH + H2
vii. How hydrogen and sulphur react with alklain earth metals?
Reaction with Hydrogen:
Pressure
MgI2
Mg + H2 mgH2
Ca + H2 CaH2
Reaction with sulpher:
Mg + S MgS
viii. Why the aqueos solution of Na2 CO3 is alkaline in nature?
Na2CO3 is hydrolyzed by water to give alkaline solution. In water, Na2CO3 ionized to give
carbonate anions. Na2CO3 2Na⁺ + CO3
2ˉ
Hydrolysis of carbonate anion gives strong alkaline NaOH, which is greatly ionized. While
carbonic acid produced, is a weak acid and is not greatly ionized. Thus, solution of Na2CO3
shows alkaline nature.
CO3
2ˉ
+ 2H2O H2CO3 + 2OHˉ
Overall reaction is
Na2CO3 +2H2O 2NaOH + H2CO3
Strong alkali weaker acid
i. What happened when lithium hydroxide is treated with water?
Lithium hydroxide produced hydrogen when it is treated with water.
LiH + H2O LiOH + H2
ii. Why lime water turns milky with CO2 but become clear with excess CO2?
Lime water is solution of lime CaO in water. When CaO is dissolved in water, it reacts with
water to produced Ca(OH)2. When CO2 is passed through lime water it reacts with Ca(OH)2
and produced CaCO3.
Ca(OH)2 + CO2 CaCO3 + H2O
The milkyness disappears when excess CO2 is passed through it due to the formation of
Ca(HCO3)2, which is soluble in water.
CaCO3 + CO2 + H2O Ca(HCO3)2

2021
iii. How gypsum is converted into plaster of paris?
When gypsum is heated at 100˚C it loses 3/4th
of its water and changes to plaster of paris.
2CaSO4.2H2O CaSO4)2.H2O + 3H2O
Or
CaSO4 .H2O CaSO4.⅟2H2O + H2O
iv. How lime mortar is prepared?
Ordinary mortar is also called lime mortar, is prepared by mixing freshly slaked lime with
sand and water to form a thick paste. Mortar is made by mixing freshly slaked lime (one
volume), sand (three or four volumes) and water to make thick paste. This material is
hardened or sets when placed b/w stones and bricks. Thus, it binds the blocks firmly together.
The reactions for this process are
CaO + H2O Ca(OH)2
Ca(OH)2 + SiO2 CaSiO3 + H2O
v. How lime and sand are used to make glass?
Lime and sand react at high temperature to form calcium silicate (CaSiO3). Calcium silicate
is firther used in the formation of glass.
vi. Give formulas of following ores:
i) Dolomite ii) Asbestos iii) sylvite iv) Natron
The formula of dolomite is MgCO3.CaCO3.
The formula of asbestos is CaMg3(SiO3)4.
The formula of sylvite is KCl.
The formula of natron is Na2CO3.H2O.
vii. Describe the role of lime in agriculture.
The roles of lime in agriculture are:
i) CaO is used for neutralizing acidic soils.
ii) Application of lime to acidic soil increases the amount of readily soluble
phosphorous.
iii) CaO is used for making lime sulpher sprays which have a strong fungicidal action.
viii. What is meant by slacked lime?
When lime is mixed with water it form calcium hydroxide called slaked lime. This process is
called slaking of lime. It is an exothermic process.
CaO + H2O Ca(OH)2
Q 4. Give the short answers of the following SIX questions. 12
I. What is the function of Ca in plant growth?
The functions of Ca in plant growth are:
i) Ca is essential for the normal growth of plant. Different plants required different
amount of Ca.

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