Sample Question Paper 2: Chemistry, Class 11 | Sample Papers for Class 11 Medical and Non-Medical - JEE PDF Download

 Page 1


  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
CBSE 
CLASS – XI 
CHEMISTRY 
SAMPLE PAPER 2 
Time: 3 Hours  Marks: 70 
 
General Instructions 
? All questions are compulsory. 
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each. 
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each. 
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each. 
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each. 
? There is no overall choice. However an internal choice has been provided in two 
questions of one mark, two questions of two marks, four questions of three marks 
and all the three questions of five marks weightage. You have to attempt only one of 
the choices in such questions. 
? Use of log tables if necessary, use of calculators is not allowed. 
 
 
Section A 
 
1. Arrange the isomers of pentane in increasing order of their boiling point.   [1] 
 
2. Predict the shape of ClF3 and BF3 on the basis of VSEPR theory.                                         [1] 
 
OR 
 
     What is meant by bond pairs of electrons? 
 
3. Although benzene is highly unsaturated it does not undergo addition reactions.      [1] 
 
4. What is the composition of London smog?   [1] 
OR 
 
List the gases which are responsible for greenhouse effect. 
 
5. Why do alkali metals give characteristic flame colouration?  [1] 
 
 
 
  
Page 2


  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
CBSE 
CLASS – XI 
CHEMISTRY 
SAMPLE PAPER 2 
Time: 3 Hours  Marks: 70 
 
General Instructions 
? All questions are compulsory. 
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each. 
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each. 
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each. 
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each. 
? There is no overall choice. However an internal choice has been provided in two 
questions of one mark, two questions of two marks, four questions of three marks 
and all the three questions of five marks weightage. You have to attempt only one of 
the choices in such questions. 
? Use of log tables if necessary, use of calculators is not allowed. 
 
 
Section A 
 
1. Arrange the isomers of pentane in increasing order of their boiling point.   [1] 
 
2. Predict the shape of ClF3 and BF3 on the basis of VSEPR theory.                                         [1] 
 
OR 
 
     What is meant by bond pairs of electrons? 
 
3. Although benzene is highly unsaturated it does not undergo addition reactions.      [1] 
 
4. What is the composition of London smog?   [1] 
OR 
 
List the gases which are responsible for greenhouse effect. 
 
5. Why do alkali metals give characteristic flame colouration?  [1] 
 
 
 
  
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
Section B 
 
6. What is mean by iso-electronic species? Name the species that will be iso-electronic with 
each of the F
-
, Ar atoms/ ions?  [2] 
  
7. Considering the atomic number and position in the periodic table, arrange the following 
elements in increasing order of metallic character: Si, Be, Mg, Na, P.     [2] 
 
8. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm.     [2] 
 
9.  Calculate the root mean square speed of methane molecules at 27
0
C.                                 [2] 
 
10. Calculate the oxidation number of Mn in K2MnO4 and N in HNO3 [2] 
  
  OR 
Explain which one is oxidised and which one is reduced in the given equation 
          3MnO2 + 4Al ? 3Mn + 2Al2O3 
 
11. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm. Calculate 
frequency ( ?) and wave number of the yellow light?                    [2] 
 
12. Calculate the volume of oxygen at N.T.P that would be required to convert 5.2 L of 
carbon monoxide to carbon dioxide.                      [2] 
OR 
  
What will be the mass of one 
12
C atom in g? 
 
 
Section C 
 
13. An element with atomic number 7 has following given configurations        [3] 
           (a) 1s
2
 2s
2
2px
2
2py
1
 2pz
0
 
           (b) 1s
2
 2s
2
2px
1
2py
1
 2pz
1
 
  Which of the two is correct and why? 
 
OR 
 
How would you justify the presence of 18 elements in the 5
th
 period of the Periodic 
table?    
 
 
Page 3


  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
CBSE 
CLASS – XI 
CHEMISTRY 
SAMPLE PAPER 2 
Time: 3 Hours  Marks: 70 
 
General Instructions 
? All questions are compulsory. 
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each. 
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each. 
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each. 
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each. 
? There is no overall choice. However an internal choice has been provided in two 
questions of one mark, two questions of two marks, four questions of three marks 
and all the three questions of five marks weightage. You have to attempt only one of 
the choices in such questions. 
? Use of log tables if necessary, use of calculators is not allowed. 
 
 
Section A 
 
1. Arrange the isomers of pentane in increasing order of their boiling point.   [1] 
 
2. Predict the shape of ClF3 and BF3 on the basis of VSEPR theory.                                         [1] 
 
OR 
 
     What is meant by bond pairs of electrons? 
 
3. Although benzene is highly unsaturated it does not undergo addition reactions.      [1] 
 
4. What is the composition of London smog?   [1] 
OR 
 
List the gases which are responsible for greenhouse effect. 
 
5. Why do alkali metals give characteristic flame colouration?  [1] 
 
 
 
  
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
Section B 
 
6. What is mean by iso-electronic species? Name the species that will be iso-electronic with 
each of the F
-
, Ar atoms/ ions?  [2] 
  
7. Considering the atomic number and position in the periodic table, arrange the following 
elements in increasing order of metallic character: Si, Be, Mg, Na, P.     [2] 
 
8. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm.     [2] 
 
9.  Calculate the root mean square speed of methane molecules at 27
0
C.                                 [2] 
 
10. Calculate the oxidation number of Mn in K2MnO4 and N in HNO3 [2] 
  
  OR 
Explain which one is oxidised and which one is reduced in the given equation 
          3MnO2 + 4Al ? 3Mn + 2Al2O3 
 
11. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm. Calculate 
frequency ( ?) and wave number of the yellow light?                    [2] 
 
12. Calculate the volume of oxygen at N.T.P that would be required to convert 5.2 L of 
carbon monoxide to carbon dioxide.                      [2] 
OR 
  
What will be the mass of one 
12
C atom in g? 
 
 
Section C 
 
13. An element with atomic number 7 has following given configurations        [3] 
           (a) 1s
2
 2s
2
2px
2
2py
1
 2pz
0
 
           (b) 1s
2
 2s
2
2px
1
2py
1
 2pz
1
 
  Which of the two is correct and why? 
 
OR 
 
How would you justify the presence of 18 elements in the 5
th
 period of the Periodic 
table?    
 
 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
14.                      [3] 
(a) What is the hybridization of central atom in following?  NH3 , C2H2  
(b)  Define dipole moment. 
What is the dipole moment of CCl4 molecule? Account for your answer. 
 
OR 
 
Describe the hybridization in case of PCl5. Why are axial bonds longer as compared to 
the equatorial bonds? ?              
 
15. Dinitrogen and dihydrogen react with each other to produce ammonia according to the 
following chemical equation:                            [3] 
              N2(g) + 3H2(g) ? 2NH3(g)   
(i) Calculate the mass of ammonia produced if 2.00 ×10
3
 g dinitrogen reacts with  
1. 00×10
3
 g diydrogen. 
(ii) Will any of the two reactants remain unreacted? 
(iii) If yes, which one and what would be its mass? 
 
16.  
(a) Define:                       [3] 
(i) Intensive properties  
(ii) Adiabatic process 
(b) Starting with thermodynamic relationship G = H- TS derive the following 
relationship ?G= -T?S total 
 
17.                      [3] 
(a) Define Le chatelier’s principle.
 
(b) Following reactions occurs in a blast furnace.
 
 
? ? ? ? ? ?
? ? g
2 3 2 s g s
F O  3CO 2Fe 3CO ?? 
Use Le chatelier’s principle to predict the direction of reaction when equilibrium 
mixture is distributed by 
(i)  Adding Fe2O3 
(ii) Removing CO2 
(iii) Removing CO 
OR  
 
18. Depict the galvanic cell in which reaction, Zn(s) +  2Ag
+
(aq) ? Zn
2+
(aq) + 2Ag(s) takes place   
Further show,  [3] 
(i) Which of the electrode is negatively charged? 
(ii) The carrier of the current in the cell  
(iii) Individual reaction at each electrode 
Page 4


  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
CBSE 
CLASS – XI 
CHEMISTRY 
SAMPLE PAPER 2 
Time: 3 Hours  Marks: 70 
 
General Instructions 
? All questions are compulsory. 
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each. 
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each. 
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each. 
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each. 
? There is no overall choice. However an internal choice has been provided in two 
questions of one mark, two questions of two marks, four questions of three marks 
and all the three questions of five marks weightage. You have to attempt only one of 
the choices in such questions. 
? Use of log tables if necessary, use of calculators is not allowed. 
 
 
Section A 
 
1. Arrange the isomers of pentane in increasing order of their boiling point.   [1] 
 
2. Predict the shape of ClF3 and BF3 on the basis of VSEPR theory.                                         [1] 
 
OR 
 
     What is meant by bond pairs of electrons? 
 
3. Although benzene is highly unsaturated it does not undergo addition reactions.      [1] 
 
4. What is the composition of London smog?   [1] 
OR 
 
List the gases which are responsible for greenhouse effect. 
 
5. Why do alkali metals give characteristic flame colouration?  [1] 
 
 
 
  
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
Section B 
 
6. What is mean by iso-electronic species? Name the species that will be iso-electronic with 
each of the F
-
, Ar atoms/ ions?  [2] 
  
7. Considering the atomic number and position in the periodic table, arrange the following 
elements in increasing order of metallic character: Si, Be, Mg, Na, P.     [2] 
 
8. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm.     [2] 
 
9.  Calculate the root mean square speed of methane molecules at 27
0
C.                                 [2] 
 
10. Calculate the oxidation number of Mn in K2MnO4 and N in HNO3 [2] 
  
  OR 
Explain which one is oxidised and which one is reduced in the given equation 
          3MnO2 + 4Al ? 3Mn + 2Al2O3 
 
11. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm. Calculate 
frequency ( ?) and wave number of the yellow light?                    [2] 
 
12. Calculate the volume of oxygen at N.T.P that would be required to convert 5.2 L of 
carbon monoxide to carbon dioxide.                      [2] 
OR 
  
What will be the mass of one 
12
C atom in g? 
 
 
Section C 
 
13. An element with atomic number 7 has following given configurations        [3] 
           (a) 1s
2
 2s
2
2px
2
2py
1
 2pz
0
 
           (b) 1s
2
 2s
2
2px
1
2py
1
 2pz
1
 
  Which of the two is correct and why? 
 
OR 
 
How would you justify the presence of 18 elements in the 5
th
 period of the Periodic 
table?    
 
 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
14.                      [3] 
(a) What is the hybridization of central atom in following?  NH3 , C2H2  
(b)  Define dipole moment. 
What is the dipole moment of CCl4 molecule? Account for your answer. 
 
OR 
 
Describe the hybridization in case of PCl5. Why are axial bonds longer as compared to 
the equatorial bonds? ?              
 
15. Dinitrogen and dihydrogen react with each other to produce ammonia according to the 
following chemical equation:                            [3] 
              N2(g) + 3H2(g) ? 2NH3(g)   
(i) Calculate the mass of ammonia produced if 2.00 ×10
3
 g dinitrogen reacts with  
1. 00×10
3
 g diydrogen. 
(ii) Will any of the two reactants remain unreacted? 
(iii) If yes, which one and what would be its mass? 
 
16.  
(a) Define:                       [3] 
(i) Intensive properties  
(ii) Adiabatic process 
(b) Starting with thermodynamic relationship G = H- TS derive the following 
relationship ?G= -T?S total 
 
17.                      [3] 
(a) Define Le chatelier’s principle.
 
(b) Following reactions occurs in a blast furnace.
 
 
? ? ? ? ? ?
? ? g
2 3 2 s g s
F O  3CO 2Fe 3CO ?? 
Use Le chatelier’s principle to predict the direction of reaction when equilibrium 
mixture is distributed by 
(i)  Adding Fe2O3 
(ii) Removing CO2 
(iii) Removing CO 
OR  
 
18. Depict the galvanic cell in which reaction, Zn(s) +  2Ag
+
(aq) ? Zn
2+
(aq) + 2Ag(s) takes place   
Further show,  [3] 
(i) Which of the electrode is negatively charged? 
(ii) The carrier of the current in the cell  
(iii) Individual reaction at each electrode 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
   
OR 
 
Identify the substance oxidised, reduced, oxidising agent and reducing agent for each 
of the following reactions: 
    
? ?
? ? ? ?
? ?
? ? ? ? ? ? ? ?
? ? ? ?
? ? ? ?
ll
s 6 6 2 aq s aq 6 4 2 aq
l 3 s aq 3 aq
2
( ) ( ) ( ) ( ) ( )
( ) ( ) 2 aq l
aq
2 4 2 2 2 2 gl
i     2AgBr C H O 2Ag 2HBr C H O
ii   HCHO 2 Ag NH 2 3OH H O
(iii) N H 2H O N
Ag HCOO 4NH
4H O
?
? ?
?? ? ? ?
??
? ? ?
? ? ? ?
? ? ?
 
 
19. Write balanced equations or reactions between:     [3] 
(i) Na2O2   and water 
(ii) KO2 and water 
(iii) Na2O and CO2 
 
20. Give IUPAC names of following:                    [3] 
(a) 
6 5 2
C H CH COOH 
  
(b)  
2
2
 CH -OH
 |
 CH-OH
 |
 CH -OH
                                
(c)   
32
       Br        O
       |        || 
CH -CH-CH -C-Cl 
 
21.                        [3]                    
(a) What conclusion would you draw if the Lassaigne’s extract gives a blood red 
colouration with FeCl3?     
(b)   
                     
Which of the given free radicals is most stable and why? 
(c)  Why is an organic compound fused with metallic sodium for testing for N, S and 
halogens? 
 
22. Define:                  [3] 
(i) Biochemical Oxygen Demand (BOD) 
(ii) Ozone Hole 
(iii) Green Chemistry 
Page 5


  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
CBSE 
CLASS – XI 
CHEMISTRY 
SAMPLE PAPER 2 
Time: 3 Hours  Marks: 70 
 
General Instructions 
? All questions are compulsory. 
? Section A: Q.no. 1 to 5 are very short answer questions and carry 1 mark each. 
? Section B: Q.no. 6 to 12 are short answer questions and carry 2 marks each. 
? Section C: Q.no. 13 to 24 are also short answer questions and carry 3 marks each. 
? Section D: Q.no. 25 to 27 are long answer questions and carry 5 marks each. 
? There is no overall choice. However an internal choice has been provided in two 
questions of one mark, two questions of two marks, four questions of three marks 
and all the three questions of five marks weightage. You have to attempt only one of 
the choices in such questions. 
? Use of log tables if necessary, use of calculators is not allowed. 
 
 
Section A 
 
1. Arrange the isomers of pentane in increasing order of their boiling point.   [1] 
 
2. Predict the shape of ClF3 and BF3 on the basis of VSEPR theory.                                         [1] 
 
OR 
 
     What is meant by bond pairs of electrons? 
 
3. Although benzene is highly unsaturated it does not undergo addition reactions.      [1] 
 
4. What is the composition of London smog?   [1] 
OR 
 
List the gases which are responsible for greenhouse effect. 
 
5. Why do alkali metals give characteristic flame colouration?  [1] 
 
 
 
  
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
Section B 
 
6. What is mean by iso-electronic species? Name the species that will be iso-electronic with 
each of the F
-
, Ar atoms/ ions?  [2] 
  
7. Considering the atomic number and position in the periodic table, arrange the following 
elements in increasing order of metallic character: Si, Be, Mg, Na, P.     [2] 
 
8. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm.     [2] 
 
9.  Calculate the root mean square speed of methane molecules at 27
0
C.                                 [2] 
 
10. Calculate the oxidation number of Mn in K2MnO4 and N in HNO3 [2] 
  
  OR 
Explain which one is oxidised and which one is reduced in the given equation 
          3MnO2 + 4Al ? 3Mn + 2Al2O3 
 
11. Yellow light emitted from a sodium lamp has a wavelength ( ?) of 580 nm. Calculate 
frequency ( ?) and wave number of the yellow light?                    [2] 
 
12. Calculate the volume of oxygen at N.T.P that would be required to convert 5.2 L of 
carbon monoxide to carbon dioxide.                      [2] 
OR 
  
What will be the mass of one 
12
C atom in g? 
 
 
Section C 
 
13. An element with atomic number 7 has following given configurations        [3] 
           (a) 1s
2
 2s
2
2px
2
2py
1
 2pz
0
 
           (b) 1s
2
 2s
2
2px
1
2py
1
 2pz
1
 
  Which of the two is correct and why? 
 
OR 
 
How would you justify the presence of 18 elements in the 5
th
 period of the Periodic 
table?    
 
 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
14.                      [3] 
(a) What is the hybridization of central atom in following?  NH3 , C2H2  
(b)  Define dipole moment. 
What is the dipole moment of CCl4 molecule? Account for your answer. 
 
OR 
 
Describe the hybridization in case of PCl5. Why are axial bonds longer as compared to 
the equatorial bonds? ?              
 
15. Dinitrogen and dihydrogen react with each other to produce ammonia according to the 
following chemical equation:                            [3] 
              N2(g) + 3H2(g) ? 2NH3(g)   
(i) Calculate the mass of ammonia produced if 2.00 ×10
3
 g dinitrogen reacts with  
1. 00×10
3
 g diydrogen. 
(ii) Will any of the two reactants remain unreacted? 
(iii) If yes, which one and what would be its mass? 
 
16.  
(a) Define:                       [3] 
(i) Intensive properties  
(ii) Adiabatic process 
(b) Starting with thermodynamic relationship G = H- TS derive the following 
relationship ?G= -T?S total 
 
17.                      [3] 
(a) Define Le chatelier’s principle.
 
(b) Following reactions occurs in a blast furnace.
 
 
? ? ? ? ? ?
? ? g
2 3 2 s g s
F O  3CO 2Fe 3CO ?? 
Use Le chatelier’s principle to predict the direction of reaction when equilibrium 
mixture is distributed by 
(i)  Adding Fe2O3 
(ii) Removing CO2 
(iii) Removing CO 
OR  
 
18. Depict the galvanic cell in which reaction, Zn(s) +  2Ag
+
(aq) ? Zn
2+
(aq) + 2Ag(s) takes place   
Further show,  [3] 
(i) Which of the electrode is negatively charged? 
(ii) The carrier of the current in the cell  
(iii) Individual reaction at each electrode 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
   
OR 
 
Identify the substance oxidised, reduced, oxidising agent and reducing agent for each 
of the following reactions: 
    
? ?
? ? ? ?
? ?
? ? ? ? ? ? ? ?
? ? ? ?
? ? ? ?
ll
s 6 6 2 aq s aq 6 4 2 aq
l 3 s aq 3 aq
2
( ) ( ) ( ) ( ) ( )
( ) ( ) 2 aq l
aq
2 4 2 2 2 2 gl
i     2AgBr C H O 2Ag 2HBr C H O
ii   HCHO 2 Ag NH 2 3OH H O
(iii) N H 2H O N
Ag HCOO 4NH
4H O
?
? ?
?? ? ? ?
??
? ? ?
? ? ? ?
? ? ?
 
 
19. Write balanced equations or reactions between:     [3] 
(i) Na2O2   and water 
(ii) KO2 and water 
(iii) Na2O and CO2 
 
20. Give IUPAC names of following:                    [3] 
(a) 
6 5 2
C H CH COOH 
  
(b)  
2
2
 CH -OH
 |
 CH-OH
 |
 CH -OH
                                
(c)   
32
       Br        O
       |        || 
CH -CH-CH -C-Cl 
 
21.                        [3]                    
(a) What conclusion would you draw if the Lassaigne’s extract gives a blood red 
colouration with FeCl3?     
(b)   
                     
Which of the given free radicals is most stable and why? 
(c)  Why is an organic compound fused with metallic sodium for testing for N, S and 
halogens? 
 
22. Define:                  [3] 
(i) Biochemical Oxygen Demand (BOD) 
(ii) Ozone Hole 
(iii) Green Chemistry 
  
 
CBSE XI | Chemistry 
Sample Paper – 2 
 
    
 
 
23. Write a short note on the following:               [3] 
(a) Wurtz  Reaction     
(b) Friedel-crafts alkylation 
 
24. Write the balanced equations:                [3] 
       
?
33
3 2 6
(a) H BO
(c) NH B H
? ? ?
? ? ? ?
  
 
Section D 
25.                     [5] 
 
(a) For the reaction 2A(g)  + B(g) ?2D(g) 
     ?u
0
 = -10.5 kJ and ?S
0
 = -44 J/K 
    Calculate ?G
0
 for the reaction and predict whether the reaction may occur            
spontaneously. 
(Given: R= 8.314 JK
-1
mol
-1
, T = 298 K) 
 
(b) Calculate the number of kJ of heat necessary to raise the temperature of 60 g of 
aluminium from 35 to 55 
°
C. Molar heat capacity of Al is 24 JK
-1
mol
-1
. 
 
OR 
 
(a) What is bond energy? Why is it called enthalpy of atomisation? 
(b) Calculate the bond energy of C-H bond, given that the heat of formation of CH4, heat 
of sublimation of carbon and heat of dissociation of H2 are -74.8, +719.6, 435.4 
kJmol
-1
 respectively. 
                                      
26. Give reasons for the following:             [5] 
(a) [SiF6]
2-
 is known whereas [SiCl6]
 2-
 is not known. 
(b) Diamond is covalent, yet has high melting point. 
(c) PbX2 is more stable than PbX4 (X= Cl, Br) 
(d) Boron is unable to form BF6
3-
 ion. 
(e) BF3 behaves as Lewis acid. 
OR 
(a) Give one method for industrial preparation and one for laboratory preparation of 
CO and CO2 each. 
(b) Select the member(s) of group 14 that (i) forms the most acidic dioxide (ii) used 
as semiconductors. 
(c) Explain structure of Diborane.