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CBSE Sample Paper for Class 11 Chemistry (Solved) – Set E
There is no overall choice in the paper. However, there is n internal choice in one question of 2 marks weight-age, one question of 3 marks weight-age and all t three questions of 5 marks weight age. Please note that the paper given here is only a sample. You can use log table if necessary. Use of calculator is not permitted. Set E of Solved CBSE Sample Paper for Class 11 Chemistry is given below with its solutions.
Sample Question Paper
1. How many spherical nodes do you expect in a 4s-orbital ? 
2. Write resonance structure of sulphur dioxide molecule. [HOTS] 
3. What are the units of coefficient of viscosity ? 
4. Assign the oxidation number to S in H2S2O7. [HOTS] 
5. Name two compounds which retard the decomposition of H2O2 solution. 
6. Express the following in scientific notation : 
7. Dinitrogen and dihydrogen react with each other to produce ammonia according to the chemical equation :
N2(g) + 3H2(g) → 2NH3(g)
(i) Calculate the mass of ammonia produced if 2.00 x 103 g dinitrogen reacts with 1.00 x 103 g dihydrogen.
(ii) Will any of the two reactants remain tutreacted ? 
8. Which of the following are Lewis acids ? 
H2O, BF3, H+, NH4+
9. Name the disease caused by lead and nitrate contamination in drinking water. 
10. Explain why the following systems are not aromatic ? 
An alkene `A’ contains three C—C, eight C—H, σ-bond and one C—C π-bond. ‘A’ on ozonolysis give two moles of an aldehyde of molar mass 44 u write the IUPAC name of ‘A’. 
11. (1) State Heisenberg’s Uncertainty principle. 
(2) Write electronic configuration of Cu metal (Z = 29) and Cr3+ ion. 
(3) Which orbital is represented by n = 4 and 1 = 3? 
12. What are the atomic numbers of elements whose outermost electrons are represented by : (a) 3s1, (b) 3p3, and (c) 3d6‘? 
13. Which out of NH3 and NF3 has higher dipole moment ? Write molecular orbital diagram for o22-. 
14. Calculate the oxidation number of sulphur, chromium and nitrogen in H2SO4, CrO5 and NO3–. 
15. Comment upon the reactions of dihydrogen with (i) chlorine, (ii) sodium, and (iii) copper(H)oxide. 
16. Which is hybridisation ? Write the hybridisation present in PC15 and SF6. 
17. For the reaction PC15 +-> PC13 + C12 at 473K the value of equilibrium constant Kc is 8.3 x 10-3
(1) Write an expression for Kc.
(2) What is the value of Kc for reverse reaction at same temperature ?
(3) What would be effect on Kc if pressure is increased ? [HOTS] 
18. (i) How much time would it take to distribute one Avogadro number of wheat grains if 1010 grains are distributed each second ?
(ii) At constant temperature if the pressure of a fixed mass of gas is doubled what happens to its volume ? Which law governs this behaviour of gases ? [31
19. Do you observe any soil pollution in your neighbourhood ? What efforts will you make for controlling the soil pollution ? 
20. Accounts the following : 
(i) Benzene is extra-ordinarily stable though it contains three double bonds.
(ii) Branching of alkane chain decreases boiling point.
Alkynes show acidic character.
21. Give condensed and bond line structural formulas for :
(a) 2, 2, 4-Trimethylpentane,
(b) 2-Hydroxy-1, 2, 3-propanetricarboxylic acid,
(c) Hexanedial. 
22. Comment on each of the following observations : 
(a) The mobilities of the alkali metal ions in aqueous solution are Li + <Na+ <K+ <Rb+ <Cs+.
(b) Lithium is the only alkali metal which forms nitride directly.
(c) E° for M2+ (aq) + 2e– –> M (s) (where M = Ca, Sr or Ba) is nearly constant.
What happens when : (i) magnesium is burnt in air,
(ii) quick lime is heated with silica,
(iii) chlorine reacts with slaked lime ? 
23. d-block elements are the elements of group 3 to 12 in the centre of the periodic table. These are characterised by the filling of inner d-orbitals by electrons and are therefore referred to as d-block elements. These elements have the general outer electronic configuration (n – 1) d1-10 ns0-2. They are all metals. They generally form coloured ions, exhibit variable valence, paramagnetism and often used as catalyst.
Now answer the following questions :
(i) Explain why d-block elements have higher density than alkaline earth metals. 
(ii) Transition metals are less electropositive than alkaline earth metals. [Value Based Question] 
24. Using the data (all values are in kilocalories per mole at 25°C) given below, calculate the bond energy of C—C and C—H bonds.
ΔH°combustion (ethane) = – 372.0
Delta;H°combustion (Propane) = – 530.0
ΔH° for C (graphite) —> C(g) = 172.0
Bond energy of H—H = 104.0
Δ,f H° of H2O(l) = -68.0
Delta;,f H° for CO2(g) = – 94.0 [HOTS] 
(i) Calculate the work of expansion when 100 g of water is electrolysed at a constant pressure of 1 atn and temperature of 25°C.
(ii) An athlete is given 100 g of glucose (C6H12O6) of energy equivalent to 1560 U. He utilizes 50 percen of this gained energy in the event. In order to avoid storage of energy in the body, calculate the weigh of water he would need to perspire. The enthalpy of evaporation of water is 44 kJ/mol. [HOTS] 
25. (i)Identify the most stable species in the following set of ions giving reasons : 
(ii) Give three points of difference between inductive-heat and resonance effects. 
(a) Give one example each for benzenoid aromatic compound and non-benzenoid compound. 
(b) Explain chain, position and functional group isomerism with examples. 
26. Give reasons for :
(1) [SiF62]– is known whereas [SiCl6]-2 is not known. 
(2) Diamond is a covalent solid, yet it has highest Melting Point. 
(3) Boric acid is considered a weak base. 
(4) BF3 behaves as Levis acid. 
(5) CO2 is a gas while SiO2 is a solid at room temperature. 
(1) What are fullerenes ? 
(2) Why is boric acid monobasic ? 
(3) What is inert pair effect ? 
(4) Why is PbCl2 is a good oxidizing reagent ? 
(5) Write the formula of inorganic benzene.