K.

RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

Very short answer type questions:

Name of the chapter No. of questions Marks Page
number
States of matter 1 02

Stoichiometry 1 02
Acids-Bases and chemical
1 02
equilibrium
S- block elements
1 02
(Alkali metals)
S- block elements
1 02
(Alkaline earth metals)
14th group elements 2 04

Environmental chemistry 2 04

Organic chemistry 1 02

Total 10 20

Level-2
Thermo dynamics 2 04
13th group elements 2 04

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

4. States of matter
1. State Boyle’s law? Give its mathematical expression? 21(2)
A: Boyle’s law: At constant temperature, the volume of given mass
of a gas is inversely proportional to its pressure. This is called Boyle’s law.
1
V (At constant temperature)
P
2. State Charles law? Give its mathematical expression? ****
A: Charles law: At constant pressure, the volume of given mass of a gas is directly
proportional to its absolute temperature. This is called Charles law.
V  T (At constant pressure)
V=KT
3. What is an ideal gas? [TS 22]
A: The gas which obeys gas laws at all conditions is called an ideal gas.
4. State grahams law of diffusion? 14(1),16(1),18(2), 21(1),22(2)
A: Grahams law of diffusion: At a constant temperature and pressure, the rate of
diffusion of a gas is inversely proportional to square root of its density is called
Grahams law of diffusion.
1
r
d
5. Which of the gas diffuses faster among N2, O2,CH4 ? Why? 17(2)
A: Molecular weight of N2 = 28
Molecular weight of O2 = 32
Molecular weight of CH4 = 16
1
According to Grahams law r 
M
Hence CH4 diffuses faster than N2, O2.
Reason: It has low molecular weight.
6. How many times methane diffuses faster than sulphur dioxide? 22(1)
A:
CH4 SO2
M1=16 M2=64

r M
1  2
r M
2 1
r
1  64
r 16
2
r
1 4
r
2
r
1 2
r
2
r  2 r
1 2
Hence methane diffuses 2 times faster than sulphur dioxide

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7. Find the relative rates of diffusion of CO2 and Cl2 gases? ****
A:

CO2 Cl2
M1=44 M2=71

r M
1  2
r M
2 1
r
1  71
r 44
2
r
1  1.27
r
2
r : r  1.27 : 1
1 2
8. State Dalton’s law of partial pressure? 14(1),16(2)
A: Dalton’s law of partial pressure: At constant temperature and volume, the total
pressure of mixture of non reacting gases is equal to the sum their partial pressures.
This is called Dalton’s law of partial pressure.
Ptotal =P1+ P2
9. What is Boltzmann’s constant? Give its value? ****
R
A: K 
N
The Value of gas constant per molecule is called Boltzmann’s constant.
Its value is 1.38x10-16 erg.molecule-1. k-1
(or)
1.38x10-23 Joul. molecule-1.k-1

10. Define RMS velocity of gas molecules ? 18(2)

A: RMS velocity:
 The square root of mean of squares of velocities of different gas molecules
present in the gas is called RMS velocity.

U  U 2  .................... U n
2 2 2

U rms  1
n
3RT
Urms 
M
11. Define average velocity of gas molecules? 18(2)
A: Average velocity:
 The average of velocities of different gas molecules present in the gas is called
average velocity.
U1  U 2  ................. U n
U av 
n

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

8RT
Uav 
πM
12. Define most probable velocity of gas molecules? 18(2)
A: Most probable speed:
 The velocity possessed by the maximum number of molecules present in the gas
is called most probable velocity
2RT
Ump 
M
13. Give the ratio of RMS, Average and most probable speeds of gas molecules?
A: The order of molecular velocity is Ump < Uav < Urms

2 RT 8RT 3RT
U mp : U av : U rms  : :
M M M
= 0.8166: 0.9213:1
(OR)
= 1: 1.128: 1.224
14. What is compressibility factor? What is its value for a perfect gas? ****
A: Compressibility factor:
 It measures the deviation of real gases from ideal behavior..
 It is denoted by z.
 It is the ratio between PV and nRT
PV
Z
n RT
(OR)
 It is the ratio between molar volume of real gas and molar volume of ideal gas.
V
Z Real
V
Ideal
15. Write the Vander walls equation? 15(2)
A: Vander Waal’s equation is
an 2
(P  ) (V  nb)  nRT
V2
Where a, b are Vander Waal’s constants.
16. Why pressure cooker is used for cooking food on hills? ****
A: Pressure cooker is used for cooking food on hills
Reason: At higher altitudes the atmospheric pressure is low. So the water boils at
low temperature.
17. What is surface tension? 18(1)
A: Surface tension: The force acting per unit length perpendicular to the line drawn
on surface of liquid is known surface tension.
18. Explain the effect of temperature on the Surface tension and Viscosity 17(1)
A: As temperature increases kinetic energy of liquid molecules increases.
Hence inter molecular attraction decreases.
And hence surface tension and viscosity decreases.

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19. Calculate the kinetic energy of 5 moles of N2 at 27oC 13,14,15,18

A: Kinetic energy =?
n= 5 moles
R= 2 calories
T = 270c= 27+ 273= 300K
3
K.E  nRT
2
3
K.E   5  2  300
2
K.E  4500 Calories
20. Calculate the kinetic energy of 3 moles of CO2 at 27oC. 13
A: Kinetic energy =?
n= 3 moles
R= 2 calories
T = 270c= 27+ 273= 300K
3
K.E  nRT
2
3
K.E   3  2  300
2
K.E  2700 Calories
21. Calculate the kinetic energy (in SI units) of 4 g. of methane at -73oC.19
A: Kinetic energy =?
n= w/GMW = 4/16 =1/4 moles
R= 2 calories
T = -730c= -73+ 273= 200K
3
K.E  nRT
2
3 1
K.E    2  200
2 4
K.E  150 Calories
K.E  150  4.18 Joules
K.E= 627 Joules
22. Calculate the ratio of kinetic energies of 3g of Hydrogen and 4g of Oxygen at a
given temperature? 19
A: Weight of H2 =3g
GMW of H2 =2g
Mole number n1= W/GMW = 3/2
3
K.E  n RT
1 2 1
3 3
K.E    RT
1 2 2
Weight of O2 =4g
GMW of O2 =32g
Mole number n2= W/GMW = 4/32 = 1/8
3
K.E  n RT
2 2 2

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3 1
K.E    RT
2 2 8
K.E
1  3 8
K.E 2 1
2
K.E
1  12
K.E 1
2
KE1 : KE2 = 12 : 1
23. On a ship sailing in Pacific Ocean where temperature is 23.40C. A balloon is filled
with 2 litre air. What will be the volume of the balloon when the ship reaches
Indian Ocean where temperature is 26.10C? 20(1)
A:

Pacific Ocean Indian Ocean

P1 =P P2 =P
V1 =2 litres V2 =?
T1 = 23.40C =23.4 + 273 T2 = 26.10C =26.1 + 273
=296.4 =299.1

PV P V
1 1 2 2
T T
1 2
V V
1 2
T T
1 2
2 V
 2
296.4 299.1
2  299.1
V 
2 296.4
V2 = 2Litres
24. 360cm3 of CH4 gas diffused through a porous membrane in 15 minutes, under
similar conditions 120 cm3 of another gas diffused in 10 minutes. Find the molar
mass of the gas? 18(1)
A:
CH4 gas Unknown gas
V V
r  1 r  2
1 t 2 t
1 2
360 120
r  r 
1 15 2 10
r  24 r  12
1 2
M1 = 16 M2 =?
r M2
1
r M1
2
24 M2

12 16

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M2
2
16
M
4 2
16
M  4 16
2
M  64
2
25. Find the RMS speed of N2 at 27oC 14(2)
A: Temperatue T = 270c= 27+ 273= 300K
Molar mass of N2 =28
3RT
RMS velocity =
M
(OR)
T
RMS velocity =1.58  10 4 cm/sec
M
300
=1.58  10 4 cm/sec
28
=1.58 10 4 10.7
=1.58 10 4  3.27
= 5.16 10 4 cm/sec
5. STIOCHIOMETRY
1. Calculate the oxidation number to the under lined elements.

S.No Question Answer Year

1) C 12 H22O11 C 12 H22O11 ****
  
x +1 -2
12(C) + 22(H) +11(O) =0
12(x) + 22(1) +11(-2) =0
12x + 22 -22 =0
12x =0
0
x
12
x=0
2) CO2 CO2 ****

x -2
1(C) +2(O) =0
1(x)+2(-2) =0
x -4 =0
x=0+4
x=+4
3) H2 O 2 H2 O2 ****
 
+1 x

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2(H) +2(O) =0
2(+1)+2(x) =0
2+2x=0
2x=-2
_2
x
2
x=-1
4) OF2 OF2 ****

x -1
1(O) +2(F) =0
1(x)+2(-1) =0
x-2=0
x=0+2
x=+2
5) O2F2 O2F2 ****

x -1
2(O) +2(F) =0
2(x)+2(-1) =0
2x-2=0
2x=0+2
2x=+2
2
x
2
x=1
6) NaHSO4 NaHSO4 ****
 
+1+1x -2
1(Na) + 1(H) +1(S) +4(O) =0
1(1) + 1(1) +1(x) +4(-2) =0
1+ 1+ x -8 =0
x -6 =0
x=0+6
x=+6

7) H2SO5 H2SO5 ****

2(H) +1(S) +3(O) +2(O) =0

2(1) +1(x) +3(-2) +2(-1) =0
2+x -6-2=0
x-6=0
x =0+6
x=+6
8) K2Cr2O7 K2Cr2O7 17(1)
  
+1 x -2
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2(k) +2(Cr) +7(O) =0

2(1) +2(x) +7(-2) =0
2+ 2x -14=0
2x -12 =0
2x=12
12
x
2
x=6
9) Cr2O7-2 Cr2O7-2
 
x -2
2(Cr)+7(O) =-2
2(x) +7(-2) =-2
2x -14=-2
2x =-2+14
2x =12
12
x
2
x=6
10) CrO5 CrO5 ****

1(Cr) +1(O) +4(O) =0

1(x)+1(-2) +4(-1) =0
x-2-4=0
x -6 =0
x=+6
11) KMnO4 KMnO4 15(1)
 
+1 x -2
1(k) +1(Mn) +4(O) =0
1(1) +1(x) +4(-2) =0
1+ x -8=0
x -7 =0
x=+7
12) MnO4- MnO4- ****

x -2
1(Mn)+4(O) =-1
1(x) +4(-2) =-1
x -8=-1
x =-1+8
x=+7
13) MnO4-2 MnO4-2 15(1)
 
x -2
1(Mn)+4(O) =-2
1(x) +4(-2) =-2
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x -8=-2
x =-2+8
x=+6

2. The empirical formula of the compound is CH2O. Its molecular weight is 90.
Calculate the molecular formula of the compound? 13(1),13(2),16(1)
A: The emipirical formula of the compound = CH2O
Emipirical formula weight = 1(C) + 2(H) + 1(O)
= 1(12) + 2(1) + 1(16)
= 12+ 2+ 16
= 30
Molecular weight = 90
Molecular weigtht
n
Empirical formula weight
90
n
30
n=3
Molecular formula = (Empirical formula)n
Molecular formula = (CH2O)3
= C3H6O3
3. What is a redox concept? Give an example. ****
A: Redox reaction: The reaction which contains both reduction and oxidation reactions
is called redox reaction.
Ex: Zn  Cu  2  Zn  2  Cu
4. What are the disproportionation reactions? Give examples. ****
A: Disproportionation reaction: The reaction in which one of the element undergoes
both oxidation and reduction reaction is called Disproportionation reaction.
Ex: 2H2O2  2H2O + O2
5. What are the comproportionation reactions? Give examples. ****
A: Comproportionation reaction: The inverse of dis proportionation reaction is called
comproportionation reaction.
Ex: Ag + Ag+2  2Ag+1
6. How many no. of moles of glucose are present in 540gms of glucose. 14,17,19,22
A: Number of moles n =?
Weight of glucose W= 540grams
Gram molecular weight of glucose C6H12O6 = 6(C)+12(H)+6(O)
= 6(12)+12(1)+6(16)
= 72+12+96
= 180
W
No. of moles 
GMW
540
n
180
n=3

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7. How many no. of moles of CaCO3 present in 200 grams of CaCO3? 14

A: Number of moles n =?
Weight of CaCO3 W= 200grams
Gram molecular weight of CaCO3 = 1(Ca)+1(C)+3(O)
= 1(40)+1(12)+3(16)
= 40+12+48
= 100
W
No. of moles 
GMW
200
n
100
n=2

8. Calculate the weight of 0.1 mole of sodium carbonate. 16,20,21,21

A: Number of moles n =0.1
Weight of Na2CO3 W= ?
Gram molecular weight of Na2CO3 = 2(Na)+1(C)+3(O)
= 2(23)+1(12)+3(16)
= 46+12+48
= 106
W
No. of moles 
GMW
W
0.1
106
W= 0.1  106
W= 10.6 grams

9. Define basicity of acid and acidity of base. 18(2)

A. Basicity: The no. of replaceable hydrogens present in the acid is called its basicity.
Ex:
1) For HCl n=1
2) For H2SO4 n=2
Acidity: The no. of replaceable hydroxyl ions (OH groups) present in the base is
called its acidity.
Ex:
1) For NaOH n=1
2) For Mg(OH)2 n=2
10. A solution is prepared by adding 2 gm of a substance A to 18 gm of water.
Calculate the mass percent of the solute. 15
A: Mass of A =2grams
Mass of water =18grams
Total mass of the solution =2+18=20
Mass of A
Mass % of A = 100
Total mass of the solution
2
= 100
20

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

200
=
20
= 10 %
11. Define Molarity? 13(1)
A: Molarity (M):
The no. of moles of solute present in 1litre of the solution is called molarity.
It is denoted by M
No.of moles of solute
M
volume of the solution in litres
12. Calculate the molarity of NaOH in the solution prepared by dissolving 4 gm in
enough water to form 250 ml of the solution. 18
A: Molarity=?
Weight of the solute (NaOH) =4grams
GMW of the solute (NaOH) = 1(Na) + 1(O) +1(H)
= 1(23) + 1(16) +1(1)
= 23+16+1
= 40
Volume of the solution= 250ml
w 1000
Molarity  
GMW Vml
4 1000
 
40 250
4

10
M=0.4
13. Calculate the molarity of sodium carbonate in a solution prepared by
dissolving 5.3 g in enough water to from 250 ml of solution 13
A: Molarity=?
Weight of the solute (Na2CO3) = 5.3grams
Gram molecular weight of Na2CO3 = 2(Na)+1(C)+3(O)
= 2(23)+1(12)+3(16)
= 46+12+48
= 106
Volume of the solution= 250ml
w 1000
Molarity  
GMW Vml
5.3 1000
 
106 250
53 100
 
106 250
1 100
 
2 250
100

500
1

5
M=0.2

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14. Define Normality? 19(2), 22(1)

A: Normality:
The No. of gram equivalents of the solute present in 1 litre of the solution is
called normality.
It is denoted by N
No.of gram equi valents of solute
N
volume of the solution in litres
n
N
V Litres
15. Calculate the normality oxalic acid solution containing of 6.3gms of H2C2O4.2H2O
present in 500 ml of solution. 20
A: Normality=?
Weight of the solute (H2C2O4.2H2O) = 6.3grams
Gram molecular weight of H2C2O4.2H2O = 6(H)+2(C)+6(O)
= 6(1)+2(12)+6(16)
= 6+24+96
= 126
Volume of the solution= 500ml
Valeny factor n=2
W 1000
Normality   n
GMW Vml
6.3 1000
  2
126 500
63 100
  2
126 500
1 100
  2
2 500
100

500
1

5
N=0.2
16. What volume of CO2 is obtained at STP by heating 4 gms of CaCO3. ****
A: Balanced chemical equation
Δ
CaCO3  CaO + CO2
1mole 1mole
Weight volume problem
100g 22.4lit
4g x

100  x = 4  22.4
100  x = 89.6
x = 89.6/100
x= 0.896 litres
17. Calculate the amount of carbondioxide that could be produced when 1 mole of
carbon is burnt in 16grams of dioxygen. 19(1)
A: Balanced chemical equation
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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

Δ
C + O2  CO2
1mole 1mole
Weight Weight problem
32 44g
16 x

32  x = 16  44
2  x = 44
x = 44/2
x= 22g
18. Calculate the volume of O2 at STP required to completely burn 100 ml of
acetylene. ****
A: Balanced chemical equation
Δ
CxHy + (x + y/4) O2  xCO2 + y/2H2O
Δ
C2H2 + 5/2O2  2CO2 + H2O
Δ
2C2H2 + 5O2  4CO2 + 2H2O
2mole 5mole
Volume Volume problem
2  22,400ml 5  22,400ml
100ml x

2  22,400  x =100  5  22,400

2  x = 100  5
2  x = 500
x = 500/2
x= 250ml

6.Thermodynamics
1. Define a system give an example? ****
A: A small part of the universe is taken for thermodynamic study is called a system.
Ex: Water in beaker.
2. Define the following. 18(2),19(2)
a) Open system
b) Closed system
c) Isolated system.
A: a) Open system: The system which can exchange both heat and matter with its
surroundings is called a open system.
Ex: A liquid in an open vessel
b) Closed system: The system which can exchange only heat but not the matter with its
surroundings is called a closed system.
Ex: A liquid in a closed vessel.
c) Isolated system: The system which cannot exchange both heat and matter with its
surroundings is called an isolated system.
Ex: A liquid in a thermos flask

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3. What are intensive and extensive properties? Give examples?

15(2),17(2),19(1),21(2),22(2)
A: The macroscopic properties are classified
into two types. They are
1) Extensive properties
2) Intensive properties
Extensive properties:
The properties which are depending on the size of the system are called extensive
properties.
Ex:
1) Enthalpy
2) Entropy
Intensive properties:
The properties which are not depending on the size of the system are called intensive
properties.
Ex:
1) Temperature
2) Pressure
4. What are the sign conventions of the work done on the system and work done by
System? ****
A:
1) If the work is done on the system( compression) W=+Ve
2) If the work is done by the system(Expansion) W=-Ve
5. State the 1st law of thermo dynamics? 16(2),21(1)
A: First law of thermo dynamics: It can be defined in different ways.
1) It is also known as law of conservation of energy
2) The energy neither be created nor be destroyed. But it can be converted from one
form to another form.
ΔU  q  W
6. Define enthalpy? 14(2), 22(1)
A: Enthalpy: At constant temperature and pressure the amount of heat is present in the
system is called Enthalpy.
 It is an extensive property.
 It is a state function
 It is denoted by H
H=U+PV
 H=  U+P  V
7. What is standard enthalpy of formation? Explain with one example.
A: The enthalpy change when 1 mole of a compound is formed from its constituent
elements in standard state is called standard enthalpy of formation.
Ex: C + O2  CO2 ΔH  393  5 KJ / Mol
8. What are the Δ H sign conventions for exothermic and endothermic reactions?
****
A: In exothermic reactions ΔH  Ve
In endothermic reactions ΔH  Ve

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9. State and explain Hess law of constant heat summation? 15(2),16(1),18(2),19(2)

22(1)
A: Hess law: The total heat change of a chemical reaction is same whether the reaction
takes place in single step or in several steps. This is called Hess law of constant heat
summation.
 ΔH  ΔH  ΔH 2
1
10. Define Entropy? 14(2),16(1),16(2), 22(1)
A: The thermodynamic property which measures the randomness of the system is
called entropy.
 It is an extensive property.
 It is a state function
 It is denoted by S
 The order of entropy is
Sgaseous > Sliquid > Ssolid
q
 ΔS
T
11. State second law of thermodynamics? ****
A: Second law of thermodynamics: It can be defined in different ways
1) Heat cannot be transferred from cold body to hot body.
2) All the naturally occurring reactions are irreversible reactions.
3) All the irreversible reactions are spontaneous reactions.
4) In most of the spontaneous reactions the entropy increases.
12. State 3rd law of thermodynamics? 17(2),19(1)
A: Third law of thermodynamics: At 0 Kelvin temperature the entropy of pure and
perfectly crystalline substance is taken as’0’ .this is called third law of
thermodynamics.
Lt S0
T0

7.1 ACIDS AND BASES

1. What is a Bronsted acid? Give one example. 16(2)
A: The proton donor is called a Bronsted acid.
Ex: NH3 + H2O ⇌ NH4+ + OH-
BB BA BA BB
2. What is a Bronsted base? Give one example. 21(1)
A: The proton acceptor is called a Bronsted base.
Ex: NH3 + H2O ⇌ NH4+ + OH-
BB BA BA BB
3. What is conjugated acid base pair give example. ****
A: The acid –base pair which differs by one proton is known as conjugate acid-base
pair.
Ex: NH3 + H2O ⇌ NH4+ + OH-
BB BA BA BB
In this reaction, NH4 and NH3 is a coinjugate acid-base pair and H2O and OH- is
+

another conjugate acid base pair.

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4. Write conjugate acid and conjugate base for each of the following:
14(1),16(1), 18(1),19(1), 20(1), 22(1)
(a) OH - (b) H2O (c) HCO3- (d) HSO4- (e) NH3 f) H2O2
A:
Conjugate base Substance Conjugate acid
O -2 OH - H2 O

OH - H2 O H3 O+
CO3-2 HCO3- H2CO3

SO4-2 HSO4- H2SO4

NH2- NH3 NH4+

HO2- H2 O2 H3 O2 +

5. What is Lewis acid? Give one example. 15(1),16(2), 21(2)

A: The elector pair acceptor is called a Lewis acid.
Ex: BF3, BCl3, H+
6. What is a lewis base? Give one example. ****
A: The electron pair donor is called a Lewis base.
Ex: H2O, NH3.
7. All Lewis acids are not bronsted acids .Why? ****
A: Electron pair acceptor is called Lewis acid.
Ex:

LB LA
Proton donor is called Bronsted acid.
BF3 cannot donate a proton.
From the above points it is observed that all Lewis acids are not bronsted acids.
8. All bronsted bases are Lewis bases .Explain. ****
A: Electron pair donor is called Lewis base.
Ex: Br - + AlBr  AlBr -
3 4
LB LA
proton acceptor is called Bronsted base.
Ex: Br- + H+  HBr
BB BA
From the above reactions it is observed that all the Lewis bases are Bronsted bases.
9. What is meant by ionic product of water? 16(2),17(1)
A: At a given temperature the product of molar concentrations of H+ and OH- ions in
water is called ionic product of water.
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It is denoted by Kw
KW=[H+][OH-]
10. What is the value of KW At 250C? What are its units? ****
A: At 250C [H+] = [OH-] = 1107 mol/lit
KW= [H+][OH-]
KW= 1107 mol/lit  1107 mol/lit
KW=1.0  10-14 mol2/lit2
Units: mol2/lit2
11. What is the effect of temperature on ionic product of water? ****
A: The value of KW depends only on temperature.
As the temperature increases, the ionization of water increases.
Hence the value of ionic product of water (KW) also increases.
12. Define PH of a solution. Write its significance. 14(2),17(2)
A: PH: The negative logarithm of the H+ ion concentration in a solution is called the pH
of a solution.

P H   log [H ]
10
Significance:
1) PH is used to distinguish acidic, basic and neutral solutions.
2) When dealing with some biological and cosmetic applications, the
determination of pH of the solution is very essential.
13. What is degree of ionization ? [TS 18]
A: Degree of ionization(  ): The ratio between the number of molecules ionized and
the total number of molecules of an acid or base is called degree of ionization.
No. of molecules ionized
α
Total No. of molecules
14. What is Buffer solution? Give one example. 15(2)
A: A solution which resists the change in its PH value on dilution or on addition of a
small amount of strong acid or a strong base is known as buffer solution.
Buffer solutions are of two types. They are
1) Acidic buffer solution CH3COOH + CH3COONa
2) Basic buffer solution NH4OH + NH4Cl

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7.2 CHEMICAL EQUILIBRIUM

1. Define dynamic equilibrium. [TS 20]
A: At equilibrium both the forward and backward reactions continue to take place with
equal rates. Hence it is called dynamic equilibrium.
2. What is homogenous equilibrium? Write two homogenous reactions. 14(1), 17(1)
A: The equilibrium reaction in which both the reactants and products are in same
phase is called homogeneous equilibrium.
Ex: 1. H2 (g) + I2 (g) ⇌ 2HI (g)
2. N2 (g) + O2 (g) ⇌ 2NO(g)
3. What is heterogeneous equilibrium? Write two heterogeneous reactions.
17(1),18(2),20(2),22(2)
A: The equilibrium reaction in which the reactants and products are in different phases
is called heterogeneous equilibrium.
Ex: 1. CaCO3 (s) ⇌ CaO (s) + CO2 (g)
2. Ni (s) + 4CO(g) ⇌ Ni(CO)4(g)
4. State the law of Mass action. ****
A: Law of mass action: At a given temperature the rate of chemical reaction is directly
proportional to the product of molar concentrations of the reactants. This is called
law of mass action.
xA +yB  Products
y
Rate α [A]x [B]
y
Rate K[A]x [B]
5. Give two chemical equilibrium reactions for which KP > KC. 20(1)
A: If ∆n = +ve then KP > KC
Ex: 1) N2O 4(g) ⇌2NO2 (g)
2) PCl5 (g) ⇌ PCl3 (g) +Cl2 (g)
6. Derive the relation between KP and KC for the reaction PCl5 (g) ⇌ PCl3 (g) +Cl2 (g).
14(2)
A: PCl5 (g) ⇌ PCl3 (g) +Cl2 (g)
P 1P 1
PCl Cl
KP  3 2
P 1
PCl
5
[PCl ] [Cl ]1
1
K  3 2
C
[PCl ]1
5
n  n  n
P R
Δn  (1  1) - 1
= 2-1
=1
K  K (RT) Δn
P C
K  K (RT)1
P C
K K
P C

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7. Define Lechatlier principle. 16(1),19(2)

A: Le-chatliers principle: When a reaction is at equilibrium, if we make any changes in
temperature, pressure or concentration the system will adjust itself to minimize the
change. This is called Le-Chatliers principle.
8. What is the effect of pressure on a gaseous chemical equilibrium? 19(1)
A: If a reaction is at equilibrium
1) If ∆n = 0, No pressure is required.
2) If ∆n = -ve, High pressure is required.
3) If ∆n = +ve, Low pressure is required.

9.1Alkali Metals
1. Write completely the electronic configurations of K and Rb? ****

A:
Element Symbol Atomic number Electronic configuration
Potassium K 19 [Ar] 4s1
Rubidium Rb 37 [Kr] 5s1
2. Why are IA group Elements called as alkali metals? 14(2),18(2)
A: IA group elements are dissolved in water to form strong alkali.
So they are known as alkali metals.
2Na + 2H2O → 2NaOH +H2
3. Why are alkali metals not found in the freestate in nature? 13(1), 17(1)
A: Alkali metals do not found in freestate in nature.
They are found in the combined state.
Reasons:
1) They are highly reactive metals.
2) They have large size.
3) They have low ionization potential.
4) They are readily forms M+ ion by losing electron.
4. Which of the alkali metals shoes abnormal density? What is the order of the
variation of density among the IA group elements? 18(2)
A: The order of density of IA group elements is Li< K< Na <Rb < Cs
Potassium has abnormal density.
The density of potassium is less than sodium.
Reason:
1) It is due to an unusual increase in atomic size of K.
2) It is due to the presence of vacant 3d orbitals.
5. Give any two uses of Lithium metal 21(2)
A: Uses of lithium:
 It is used in electro chemical cells.
 It is used for making alloys.
a) Li + Mg alloy
b) Li + Al alloy
c) Li + Pb

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6. Give an account of the biological importance of Na+ and K+ ions? 18(1)

A: Biological importance of Sodium ions (Na+):
Na+ ions are participate in the
1) Transmission of nerve signals.
2) Transport of sugars and amino acids into cells.
3) Flow of water across the cell membranes.
Biological importance of Potassium ions (K+):
K+ ions are participate in the
1) Transmission of nerve signals.
2) Oxidation of glucose to produce ATP.
3) Activating enzymes.

7. Why is KO2 paramagnetic? 19(2),21(1),22(2)

A: KO2 is a super oxide.
KO2  K+ + O2-
The total number of electrons in O2- = 8+8+1 =17
O2- ion has one unpaired electron in anti bonding molecular orbital.
Hence KO2 is paramagnetic.
8. Lithium reacts with water less vigorously than sodium. Give your reason? ****
A: Lithium reacts with water less vigorously than sodium.
Reasons: It has
1) Low atomic size
2) High hydration energy
9. Lithium salts are mostly hydrated. Why? Give one example. ****
A: Lithium salts are mostly hydrated.
Ex: LiCl.2H2O.
Reasons: It has
1) Low atomic size
2) High hydration energy
10. Describe the important uses of caustic soda. 13(2), 15(1), 16(2)
A: Uses of caustic soda:
1) It is used as a laboratory reagent.
2) It is used for the preparation of soap, paper
11. Potassium carbonate cannot be prepared by Solvay process. Why? 19(1)
A: Potassium carbonate cannot be prepared by Solvay process. Because KHCO3 is
more soluble in water unlike NaHCO3. So it is not isolated.
12. Write the properties of washing soda? 14(1)
A: Properties of washing soda (Na2CO3):
1) It is a white crystalline solid
2) It exists as a hydrated salt Na2CO3. 10H2O
3) On heating it loses the water molecules.
4) It is more soluble in water.
13. Describe the important uses of sodium carbonate? 20(1)
A: Uses of sodium carbonate:
1) It is used as a laboratory reagent
2) It is used in the preparation of soap paper
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14. What is baking soda? ****

A: Sodium bicarbonate is called as baking soda.
Its chemical formula is NaHCO3.
15. Write the uses of baking soda? ****
A: Uses of baking soda:
1) It is used as a laboratory reagent
2) It is used as baking powder
9.2Alkaline Earth Metals
1. What are the characteristic colors imparted by the IIA elements? [TS 22]
A: Alkaline earth metals (except Be and Mg) produce characteristic colour in Bunsen
flame. Due to easily excitation of electrons to higher energy levels.
Calcium – Brick red
Strontium – Crimson red
Barium – Apple green
Radium- Crimson red
2. Mention the important uses of Mg metal?
A: Uses of Mg metal:
1) It is used as a reducing agent.
2) It is used in the preparation of Grignard reagents and Alloys
3. What is milk of magnesia .Give its uses? 15(1)
A: A suspension of Mg(OH)2 in water is called milk of magnesia.
It is used as an antacid.
4. Write about the biological importance of calcium and magnesium. 13(1),13(2)
A: Biological importance of Mg+2:
Mg+2 ions are essential for the
1) Formation of chlorophyll.
2) Formation of animal cells.
3) Formation of phosphohydrolase enzyme.
4) Formation of phosphotransferase enzyme.
5) Carbohydrate metabolism.
Biological importance of Ca+2 :
Ca+2 ions are essential for the
1) Formation of bones and teeth.
2) Muscle contraction.
3) Maintaining of heart beat.
4) Blood clotting.
5. What happens when magnesium metal is burnt in air? 17(2)
A: When magnesium metal is burnt in air magnesium oxide and magnesium nitrides
are formed with drazzling brilliant white light.
2Mg+ O2  Δ 2MgO
Δ Mg3N2
3Mg+ N2 

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6. Why does the solubility of alkaline earth metal hydroxides in water increase
down the group? 20(1)
A: Alkaline earth metals form hydroxides
Be(OH)2 ,Mg(OH)2 ,Ca(OH)2 ,Sr(OH)2 ,Ba(OH)2
   
SS SS LS SS
Same Different
Less soluble More soluble
Less More
Hence the solubility increases from Be(OH)2 to Ba(OH)2
Reason:
1) Hydration energy increases
2) Lattice energy decreases
7. Why does the solubility of alkaline earth metal carbonates and sulphates in
water decrease down the group? [TS 20]
A: Alkaline earth metals form carbonates and sulphates
BeCO3 , MgCO3 , CaCO3 , SrCO3 , BaCO3
BeSO4 , MgSO4 , CaSO4 , SrSO4 , BaSO4
   
SS LS LS LS
Different Same
More soluble Less soluble
More Less
 The solubility decreases from BeCO3 to BaCO3 and BeSO4 to BaSO4
Reason:
1) Hydration energy decreases
2) Lattice energy increases
8. Show that Be (OH)2 is amphoteric in nature? 21(2)
A: Be(OH)2 is amphoteric in nature.
Reason: It reacts with both acid and base.
Be(OH)2 +2HCl → BeCl2 + 2HOH
Be(OH)2 +2NaOH → Na2[Be(OH)4]
The maximum co-ordination number of Be = 4
9. What happens when hydrated Mg(NO3)2 is strongly heated ?Give the balanced
equation? 22(1)
A: When hydrated Mg(NO3)2 is strongly heated MgO is formed.
2Mg(NO3)2  Δ 2MgO + 4NO2 + O2
10. Describe the important uses of quick lime? 14(1),19(2)
A: Uses of Quick lime (CaO):
1) It is used as a drying agent for alcohol
2) It is used for the preparation of cement
11. What is Plaster of Paris? 14(2),15(2),16(2),17(1),17(2),18(1),19(1), 22(1)
A: Calcium sulphate semi hydrate(or) hemi hydrate is called plaster of Paris.
12. Write the formula of Plaster of Paris? 14(2),15(2)
1
A: Formula of Plaster Paris is CaSO4 H2O (or) 2CaSO4.H2O
2

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13. Write the preparation of plaster of Paris. 15(2)

A: Plaster of Paris is prepared by heating gypsum at 1200C.
0C 1 3
CaSO4 2H2O 120    CaSO4 H2O + H2 O
2 2
Gypsum Plaster of Paris
14. Describe the importance of Plaster of Paris.
14(2),15(2),17(2),18(1),19(1),21(1), 22(1),22
A: Uses of plaster of paris: It is used in the
1) Setting of fractured bones.
2) Dentistry.
3) Preparation of chalks.
4) Manufacture of crucibles, models, toys, statues etc.
5) Building industry as well as plasters.
15. Why is gypsum added to cement? ****
A: Gypsum is added to cement to slow down the process of setting of the cement and
to get sufficiently hardened cement.
16. Write the average composition of Portland cement? ****
A: The average composition of Portland cement is
CaO: 60%
SiO2: 25%
Al2O3: 10%
MgO: 3%
Fe2O3: 1%
SO3: 1%
13th Group elements.
1. Explain why atomic radius of Ga less than that of Al 22(1)
A: Generally atomic size increases in a IIIA group from top to bottom.
But Gallium has less atomic size than Aluminium.
Reasons:
1) It has d10 electronic configuration in the penultimate shell.
2) It has less shielding effect.
3) It has high nuclear charge.
2. How do you explain higher stability of TlCl than TlCl3? ****
A: The oxidation state of Tl in TlCl = +1
The oxidation state of Tl in TlCl3 = +3
Thallium is more stable in +1 oxidation state due to inert pair effect.
Hence TlCl is more stable than TlCl3

3. Explain inert pair effect. Give the stable oxidation state of thallium. 21(2),22(2)
A: The reluctance of ns2 electrons to take part in the bond formation is called inert pair
effect.
Ex: Thallium has 3 valence electrons (ns2np1) but it shows +1 oxidation state.
4. Write the names of two important boron compounds? 21(2)
A: Important compounds of boron:
1) Borax (or) Tyncol
2) Colemanite
3) Ortho boric acid

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4) Diborane
5. Write the names of two important boron compounds?
(OR)
6. Give the formula of ****
a) Borax (or) Tyncol
b) Colemanite
c) Ortho boric acid
d) Diborane
A: a) The formula of borax(or) Tyncol is Na2B4O7.10H2O
b) The formula of colemanite is Ca2B6O11.5H2O
c) The formula of ortho boric acid is H3BO3 (or)B(OH)3
d) The formula of diborane is B2H6
7. Give the formula of borazine. What is its common name? ****
A: The formula of borazine is B3N3H6
Its common name is inorganic benzene. Because it has benzene like structure.
8. What is the hybridization of B in diborane and borazine? ****
A: In diborane boron atom undergoes SP3 hybridization.
In borazine boron atom undergoes SP2 hybridization.
9. What is banana bond? ****
A: The BHB bond of diborane is called banana bond.
It is an anomalous bond because it contains 3 atoms and 2 electrons.
10. Boron is unstable to form BF6-3 ion. Why? 21(1),22(2)
A: Boron exhibits a maximum covalency of 4.
Boron is unstable to form BF6-3 ion.
Reason: Due to the absence of d orbitals
11. Why doesBF3 behaves as a Lewis acid? 22(1)
A: BF3 is an electron deficient compound.so it accepts a pair of electrons to get octet
configuration.Hence it behaves as a Lewis acid
12. Give the uses of aluminium? 21(1)
A: Uses of aluminium:
1) Aluminium foils are used as wrappers for chocolates.
2) Aluminium wires are used as electrical conductors.
3) It is used for the preparation of alloys.
14th Group elements
1. What is inert pair effect? 19(1)
A: The reluctance of ns2 electrons to take part in the bond formation is called inert pair
effect.
Ex: Lead has 4 valence electrons (ns2np2) but it shows +2 oxidation state.
2. What is the effect of water on tin? ****
A: Tin decomposes steam and liberates hydrogen gas.
Sn + 2H2O  SnO2 + 2H2

3. [SiF6]-2 is known while [SiCl6]-2 not. Give possible reasons. 16(1), 19(2)
A: [SiF6]-2 is known while [SiCl6]-2 not known.
Reasons:
1) Six large chloride ions cannot be accommodated around small size Si+4 ion.

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2) Interaction between lone pair of chloride ion and Si+4 ion is weak.
4. CCl4 is not dissolved in water, but SiCl4 dissolves why? give reasons? 14(2)
A: CCl4 does not dissolved(hydrolysed) in water
Reason: Due to the absence of empty d- orbitals in carbon atom.
SiCl4 dissolved in water.
SiCl4 + 4H2O  Si(OH)4 + 4HCl
Reason: Due to the presence of empty d- orbitals in silicon atom.
Water molecules form dative bonds with empty d orbitals of silicon atom.
5. What is allotropy? Give the crystalline allotropes of carbon? 13(1), 16(2), 19(1),
20(1)
A: The existance of an element in different physical forms with similar
chemical properties is known as allotropy.
The crystalline allotropes of carbon are diamond, graphite and fullerene.
6. Write the crystalline allotropes of carbon and mention any hybridization
involved in them? 13(2), 16(1)
A: The crystalline allotropes of carbon are diamond, graphite and fullerenes.
a) Diamond-sp3
b) Graphite-sp2
c) Fullerenes- sp2
7. Mention the hybridization of carbon in 14(2)
a) CO3-2
b) diamond
c) graphite
d) fullerene
e) CO2
A:
a) CO3-2 __________ sp2
b) Diamond ______ sp3
c) Graphite _______ sp2
d) Fullerene _______ sp2
e) CO2 _____________ sp

8. Why is diamond hard? 13(2)

(OR)
9. Diamond has high melting point Explain? 18(2), 19(2), 22(1)
(OR)
10. Diamond is used as an abrasive. Explain? ****
A:
 Diamond has 3D structure.
 Diamond has polymeric structure.
 Each carbon atom is surrounded by four other carbon atoms by strong covalent
bonds.
 These covalent bonds are very difficult to break.
 So it is very hard
 So it has high melting point.
 So it is used as an abrasive for the sharpening of hard tools.

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11. How does graphite function as a lubricant? ****

A:
 It has 2D structure.
 It has hexagonal layered structure.
 The layers are held by weak Vander Waals forces.
 One layer can be slide over the other.
 Hence it has slippery nature and it is soft.
 Hence graphite function as a lubricant
12. Graphite is a good conductor. Explain? 15(2), 17(1), 18(2), 22(1)
A:
 In graphite, each carbon atom undergoes sp2 hybridization.
 Each carbon forms three covalent bonds with other three carbon atoms to form
hexagonal rings.
 Each carbon has one free electron.
 Due to the presence of free electrons graphite acts as a good conductor of
electricity.
13. Why is CO poisonous? 13(1), 16(2), 18(1)
A:
 When CO is inhaled, it combines with haemoglobin of the blood to form carboxy
haemoglobin.
 It is more stable than oxy haemoglobin.
 It prevents haemoglobin from carrying oxygen, which causes dizziness or coma.
14. What is water gas (or) blue gas (or) synthesis gas (or) syn gas? 20(1)
A: The mixture of carbon monoxide and hydrogen (CO + H2) is known as water gas or
blue gas or synthesis gas or syn gas.
15. What is producer gas? ****
A: The mixture of carbon monoxide and nitrogen (CO + N2) is called producer gas.
16. How is water gas prepared? 18(1), 20(1)
A: Water gas is prepared by passing steam over hot coke.
473  1273K
C(s)+ H2O(g)  CO(g)+ H2(g).
17. How is producer gas prepared? ****
A: Producer gas is prepared by passing air over hot coke.
1273K
2C(s) + O2 (g)+ 4N2(g)  2CO(g)+4N2(g).
18. What is meant by dry ice? Give its use? 15(1)
A: solid carbon dioxide is called dry ice.
Uses: It is used as a refrigerant for ice cream and frozen food.
19. Mention any four uses of carbon dioxide gas? 17(1)
A: Uses of carbon dioxide gas:
1) It is used in photo synthesis
2) It is used in soft drinks.
3) It is used in the manufacture of urea.
4) It is used in the manufacture of white lead and sodium carbonate.
5) It is used as fire extinguisher.
20. Give the use of CO2 in photosynthesis? 14(1)
A: In photosynthesis plant cells absorb water from soil and CO2 from air for the
formation of carbohydrates and oxygen.

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h , Chlorophyl
6CO2+ 12H2O   C6H12O6+ 6O2+ 6H2O
21. What are silicones? Give examples. 15(1)
A: Silicones :
 The organo silicon polymers containing Si –O– Si bonds are called Silicones.
 Silicones contain R2SiO as repeating unit.
 The structure of R2SiO is similar to that of ketone.
 Ex: R3SiCl, R2SiCl2, RSiCl3.
22. Write any two uses of silicones? ****
A: Uses of silicones: silicones are used
1) In the preparation of silicone rubber.
2) In the preparation of water proof cloth and paper.
3) In the preparation greases which are used as lubricants in aeroplanes.
4) In paints and enamels.
5) In surgical and cosmetic plants as they are bio-compatible.
23. Name any two manmade silicates? 14(1) 15(2)
A: Glass and cement.
24. Write the use of ZSM-5? ****
A: ZSM -5 is a type of zeolite which is used to convert alcohol directly in to gasoline
(group of hydro carbons).
25. Wite the uses of zeolites? [TS 16]
A: Uses of zeolites:
1) Zeolites are used in softening of hard water.
2) Zeolites act as cation exchangers and molecular sieves.
3) ZSM -5 is used to convert alcohols directly in to gasoline.

Environmental Chemistry
1. What is pollutant, contaminant ****
A: Pollutant: A substance which is present in the environment whose quantity is
increased due to natural or human activity and has an adverse effect on
environment is called pollutant.
Ex: CO2, NO2, SO2
Contaminant: A substance which is not present in the environment, but released
into environment due to human activity and has an adverse effect on environment
is called contaminant.
Ex: Industrial effluents, pesticides, MIC (Methyl iso cyanate CH3-N-C=O)
2. Define the terms receptor, sink? 13(1),15(1), 17(1) , 18(1)
A: Receptor: The medium which is affected by the pollutant is called receptor.
Ex: Human eyes in traffic
Sink: The medium which reacts with pollutant and decrease the concentration of the
pollutant in the environment is called sink.
Ex: Sea water, Trees are the sinks for CO2.
3. Name two important sinks for CO2. ****
A: Sea water, Trees are the sinks for CO2..
4. Define the TLV. ****
A: Threshold limit value (TLV): The minimum level of toxic pollutants present in the
atmosphere which effects a person adversely when he is exposed to this for 6-8 hours

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in a day is called threshold limit value (TLV)

Ex: TLV of a zinc is 1.00mg/m3
5. What is chemical oxygen demand (COD)? 14(1),14(2)15(2),16(1), 16(2) , 18(2)
A: Chemical oxygen demand (COD): The amount of oxygen required to oxidise organic
substances present in polluted water is called chemical oxygen demand (COD).
6. What is Bio chemical oxygen demand (BOD)?
14(1),15(2), 16(1),16(2), 17(2) ), 18(2), 20(1)
A: Bio chemical oxygen demand (BOD): The amount of oxygen used by the suitable
micro organisms present in polluted water during five days at 200C is called BOD.
7. Give the possible BOD values of clean water and polluted water. [TS14,20]
A:
 BOD value of clean water is 1ppm.
 BOD value of polluted water is 17ppm or more.
8. Name the major particulate pollutants present in troposphere. 19(2)
A: Particulate pollutants are of two types. They are
1) Viable particulate pollutants:
Ex: Bacteria, Fungi, Algae,Virus.
2) Non -viable particulate pollutants:
Ex: Dust, smoke, mist, smog.

9. What are the smoke and mist? ****

A: Smoke: Very small sooty particles are produced by burning and combustion of
organic matter is called smoke.
Mist: The particles which are produced by spray liquids and formed by condensation
of vapours in air are called mist.
10. Name the common components of photochemical smog. 16(2) , 19(1)
A: common components of photochemical smog are ozone, nitric oxide, formaldehyde,
acrolein and PAN (peroxy acetyl nitrate)
11. What is PAN? What effect is caused by it? 19(2)
A: PAN means Peroxy acetyl nitrate.
It is a component of photo chemical smog.
Effects:
 It has toxic effect.
 It is a powerful eye irritant.
 It causes corrosion of metals, rubber and building materials.
12. List out four gaseous pollutants present in the polluted air? ****
A: List out four gaseous pollutants:
1) CO2
2) NO2
3) SO2
4) O3
13. What happens when CO concentration is increased in atmosphere? ****
A: When CO is inhaled, it combines with haemoglobin of the blood to form carboxy
haemoglobin, which is more stable than oxy haemoglobin. This prevents haemo
globin from carrying oxygen, which causes dizziness or coma.
14. Which oxides cause acid rain? What is its PH value. 13(1)
A: Oxides of Nitrogen, Sulphur are caused to acid rain.

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

The pH value of Acid rain is less than 5.6.

15. Name two adverse effects caused by acid rains. 13(2),15(2),16(1), 18(1)
A: Adverse effects caused by acid rains:Acid rains decrease the
1) Life of buildings and historical monuments.
2) Fertility of soil.
3) PH value of the soil.
4) Agricultural productivity.
16. What is greenhouse effect (or) Global warming? 13(2), 14(1), 18(2)
A: Greenhouse effect: The Earth’s surface is heated due to blanketing effect of
CO2 and water vapour in the atmosphere is called greenhouse effect.
17. Greenhouse effect is caused by---------------and------------------ gases.
14(1), 14(2), 20(1) (OR)
18. What are Greenhouse gases? Give examples? ****
A: The gases which are caused to greenhouse effect are called greenhouse gases.
Ex: CO2, CH4, CFC'S (chloro fluoro Carbons) , O3 and water vapour in the atmosphere

19. Write the harmful effects of global warming. 17(1)

A: Harmful effects of global warming:
1) Melting of polar ice caps
2) Flooding of low lying areas all over the earth.
3) Increases infectious diseases like Dengue, Malaria, Yellow fever, sleeping sickness.
20. Mention the harmful effects caused due to the ozone depletion of ozone layer.
(or) 15(1)
21. What happens when holes are formed in ozone layer?
A: When holes are formed in ozone layer, then UV rays will pass through these holes
and reach the earth.
1) They are caused to skin cancer, cataract of eyes.
2) They can decrease moisture content of the soil.
3) They can decrease the efficiency of photosynthesis in plants
22. What is the harm caused by CFC’S?
A:
1) CFCs cause the depletion of ozone layer.
2) Then, the U.V rays from the sun fall directly on the earth.
3) This causes skin cancer and cataract.
23. How do CFC’S break down the ozone layer?
A:
 CFCs from different sources reach the stratosphere.
 Powerful UV rays break down CFCs to free radicals.
 Chlorine radical reacts with ozone to form O2 and chlorine monoxide radical.
 Chlorine monoxide radical produces more chlorine radicals by reacting with
oxygen atoms.
 Process gets repeated leading to more break down of ozone.
 This causes to depletion of ozone layer.
24. What agrochemicals are responsible for water pollution? 19(1)
A: Agro chemicals such as fertilizers containing phosphates, Pesticides, insecticides,
herbicides, fungicides are responsible for water pollution.
25. What happens when fluorides are present in water? ****

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

A:
 The fluorides react with calcium present in the body to form CaF2
Ca + F2  CaF2
 If concentration of fluorides more than 3ppm in drinking water, it becomes harmful.
 Excess of fluorides in water causes fluorosis disease.
 Due to fluorosis the colour of the teeth turns yellow and bones become weak.
26. Write one strategic adopted in green chemistry to avoid environmental pollution.
17(2)
A: Strategic adopted in green chemistry:
In earlier days Chlorine solution was used for bleaching clothes and paper.
Nowadays, it is replaced by H2O2.
13. Organic chemistry
Topic-1 (IUPAC Names)
Type-1 Write the structural formula of the given compounds

S. Name of the Structure of the compound Year

No compound
Two carbon compounds
1. Ethylene glycol (or) 2 1 ****
Ethane 1,2-diol CH2 - CH2

OH OH
2. Trichloro ethanoic 2 1 13(1),21(1)
acid CCl3-COOH
3. Ethanal 2 1
CH3-CHO
Three carbon compounds
Four carbon compounds
4. 2- methyl But-1-ene 1 2 3 4 14(1)
CH2 =C- CH2-CH3

CH3
5. 2,3 -dimethyl butane 1 2 3 4 BP
CH3 –CH - CH - CH3

CH3 CH3
Five carbon compounds
6. 2-methyl pent 1- 1 2 3 4 5 17(2)
ene CH2 =C- CH2-CH2-CH3

CH3
7. Neopentane CH3 13(1),21(1)
(2,2-dimethyl 1 2 3
propane) CH3 –C – CH3

CH3

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8. 2,5 dimethyl 1 2 3 4 5 6 22(2)

hexane CH3 –CH– CH2– CH2 –CH-CH3

CH3 CH3
Seven carbon compounds
9. 3,4,4,5 -tetra CH3 14(1),22(2)
methyl heptane 1 2 3 4 5 6 7
CH3 –CH2– CH– C –CH-CH2-CH3

CH3 CH3 CH3

10. 3,3,4,5- tetra CH3 17(2)
methyl heptane 1 2 3 4 5 6 7
CH3 –CH2– C – CH –CH-CH2-CH3

CH3 CH3 CH3

Aromatic copounds
11. P- Nitro ****
benzaldehyde

Type-2 Write the IUPAC names of the following compounds:

S. Structure of the compound Name of the Year

No compound
Type-1
1. CH3CH=C(CH3)2 2-methyl but 2-ene 18(2)
,
4 3 2 1 21(2)
CH3 –CH= C-CH3

CH3
2. (CH3)2C(C2H5)2 3,3- dimethyl pentane 19(1)
CH3 ,
1 2 3 4 5
CH3 –CH2 - C – CH2- CH3

CH3

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3. (CH3)3CCH2C(CH3)3 2,2,4,4- tetra methyl 19(2)

CH3 CH3 pentane
1 2 3 4 5
CH3 –C – CH2-C- CH3

CH3 CH3
Type-2
4. 1 2 3 2-Methyl propene-1 19(2)
CH2=C-CH3

CH3
5. Butanone-2
O

CH3 –CH2 –C-CH3

4 3 2 1
6. CH3 3,3 -di methyl 13(2)
4 3 2 1 pentanoic acid-1
CH3 –C-CH2-COOH

CH3
7. 1 2 3 4 5 Pent 1-ene 3- yne
CH2 =CH-C  C- CH3

8. 1 2 3 4 5 Pentene-1
CH2 =CH- CH2-CH2-CH3

9. 1 2 3 4 5 Pentan 2-ol
CH3 – CH- CH2 –CH2-CH3

OH
10. CH3 2,2,3-tri methyl pentane 13(2)
1 2 3 4 5
CH3 –C - CH–CH2-CH3

CH3CH3

11. CH3 CH3 2,2,4,4-tetra methyl

1 2 3 4 5 pentane
CH3 –C-CH2 -C-CH3

CH3 CH3
12. CH3 3,3,5- trimethyl heptane 19(1)
3 4 5 6 7
CH3 –C-CH2 CH–CH2-CH3
2 1
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CH2-CH3 CH3

Type-3
13. But 1,3 diene 16(1)
,
18(1)
,
21(2)

14. Petanone-2 18

15. Pentanone-3 16(1)

,
18(1)
,
20(1)

16. 4,5-dimethyl hexanol-1 18(2)

17. Oct 1,3,5,7 tetraene 20(1)

18. 3- ethyl 2-methyl

pentane

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

19. 3-ethyl 4-methyl hexane

Topic-2 (Benzene)
S.No
1. An alkyne A undergoes cyclic polymerization by passing 15(1)
through a red hot iron tube to give B. Find A&B
A: When acetylene is passed through a red hot metal tube, it
undergoes cyclic polymerisation to form benzene.
Red hot metal tube
3C2H2  C6H6
Where A= acetylene
B= Benzene
2. How is nitro benzene prepared from benzene? 15(2)
A: Nitration: Benzene reacts with nitration mixture (Conc. HNO3
+ Conc. H2SO4) to form nitro benzene.
Conc.H SO
C6H6 + Conc.HNO3 2
4  C6H5NO2+ H2O

3. Write the reagents and equation required for the conversion ****
of benzene to methyl benzene.
A: Friedel craft’s alkylation: Benzene reacts with methyl chloride
in the presence of anhydrous AlCl3 to form methyl benzene
(or) toluene. This reaction is known as Friedel craft’s
alkylation.
Anhydrous AlCl
C6H6 + CH3Cl 
3
 C6H5CH3 + HCl

4. What is friedel crafts alkylation reaction? ****

A: Friedel craft’s alkylation: Benzene reacts with methyl chloride
in the presence of anhydrous AlCl3 to form methyl benzene
(or) toluene. This reaction is known as Friedel craft’s
alkylation.
Anhydrous AlCl
C6H6 + CH3Cl 
3
 C6H5CH3 + HCl

5. What is friedel crafts acetylation reaction? ****

A: Friedel craft’s acetylation: Benzene reacts with acetyl chloride
in the presence of anhydrous AlCl3 to form acetophenone. This
reaction is known as Friedel craft’s acetylation.
Anhydrous AlCl
C6H6 + CH3COCl 
3
 C6H5COCH3 + HCl

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

Topic-3(Ethane)
S.No
1. What is wurtz reaction? 22(1)
A: Wurtz reaction:
2 moles of methyl chloride reacts with sodium metal in the
presence of dry ether to form ethane. This reaction is known
as Wurtz reaction.
dry ether
2CH3Cl + 2Na  C2H6 + 2NaCl

Topic-4(Isomerism)
S.No
1. What is position isomerism? Give one example. ****
A: Position isomerism: The compounds having same molecular
formula but differ in the position of substituent are called position
isomers and this phenomenon is called position isomerism.
Ex: CH3-CH2-CH2Br - 1Bromo propane
CH3-CHBr-CH3 - 2Bromo propane

2. Write the chain isomer structures of the carbon compound C4H10 [TS 20]
A: 1) n –Butane

2) 2-methyl propane

3. What is functional isomerism? Give one example. 16(2)

A: Functional isomerism: The compounds having same molecular
formula but differ in the functional group are called functional
isomers and this phenomenon is called functional isomerism.
Ex: CH3-CH2-CN - Ethyl cyanide
CH3-CH2-NC - Ethyl isocyanide
4. Name the functional group isomers of the molecular formula [TS
C3 H 6 O 17,20]
A: CH3-CH2-CHO ( Propanal)
CH3-CO-CH3 (propanone)
5. Draw Cis and Trans isomers of the following compounds. Also 14(2),
write their IUPAC Names 22(1)
a) CHCl = CHCl
b) C2H5C CH3= C CH3 C2H5

A:

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K.RAAMUDU SL IN CHEMISTRY NARAYANA JUNIOR COLLEGE CELL: 8247748589

Topic- 5
1. What is the type of hybridization of each carbon atoms in the following
compounds? 17(1)
a) CH3-CH=CH2
b) CH3-C  CH
c) HC  C-CH=CH2
A:
a) CH3-CH=CH2
4σ 3σ 3σ
SP3, SP2, SP2
b) CH3-C  CH
4σ 2σ 2σ
SP3, SP, SP
c) HC  C-CH=CH2
2σ 2σ 3σ 3σ
SP, SP, SP2, SP2
2. What is polymerization reaction? Give one example. [TS 17]
A: Polymerization: The process of formation of a large molecule (polymer) by the
combination of simple molecules is known as polymerization.
Ex: Ethylene undergoes polymerization reaction to form poly ethylene
(polythene)

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