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Revision Model Question Paper 2

11th Standard

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Chemistry

Time : 03:00:00 Hrs
Total Marks : 70

    Part I

    Answer all the questions.

    Choose the most suitable answer from the given four alternatives and write the option code with the corresponding answer.

    15 x 1 = 15
  1. The oxidation number of fluorine in all its compounds is equal to

    (a)

    -1

    (b)

    +1

    (c)

    -2

    (d)

    +2

  2. Which of the following does not represent the mathematical expression for the Heisenberg uncertainty principle?

    (a)

    \(\triangle x.\triangle p\ge \frac { h }{ 4\pi } \)

    (b)

    \(\triangle x.\triangle v\ge \frac { h }{ 4\pi m } \)

    (c)

    \(\triangle E.\triangle t\ge \frac { h }{ 4\pi } \)

    (d)

    \(\triangle E.\triangle x\ge \frac { h }{ 4\pi } \)

  3. Match the list-I and list-II using the correct code given below the list.

      List-I   List -II
    A. Jewels 1. 1.Sodium chloride
    B. Bolts and cot 2. Copper
    C. Table salt 3. Gold
    D. Utensils 4. Iron
    (a)
    A B C D
    3 4 1 2
    (b)
    A B C D
    4 1 3 2
    (c)
    A B C D
    1 4 2 3
    (d)
    A B C D
    2 3 4 1
  4. Non-stoichiometric hydrides are formed by

    (a)

    palladium, vanadium

    (b)

    carbon, nickel

    (c)

    manganese, lithium

    (d)

    nitrogen, chlorine

  5. Consider the following statements.
    (i) Alkali metals exhibit high chemical reactivity due to their low ionization energy.
    (ii) Lithium is a very soft metal and even it can be cut with a knife.
    (iii) Francium is a radioactive element in group 1 elements
    Which of the above statements is/are not correct?

    (a)

    (i) only

    (b)

    (ii) only

    (c)

    (i) and (iii)

    (d)

    (i), (ii) and (iii)

  6. Pressure of a gas is equal to __________.

    (a)

    \(\frac{F}{a}\)

    (b)

    F x a

    (c)

    \(\frac{a}{F}\)

    (d)

    F - a

  7. The enthalpies of formation of Al2O3 and Cr2Oare -1596 kJ and -1134 kJ, respectively. ΔH for the reaction 2AI + Cr2O3 ⟶ 2Cr + Al2O3 is

    (a)

    - 1365 kJ

    (b)

    2730 kJ

    (c)

    - 2730 kJ

    (d)

    - 462 kJ

  8. [Co(H2O)6]2+ (aq) (pink) + 4Cl (aq) ⇌ [CoCl4]2– (aq) (blue)+ 6 H2O (l)
    In the above reaction at equilibrium, the reaction mixture is blue in colour at room temperature. On cooling this mixture, it becomes pink in colour. On the basis of this information, which one of the following is true?

    (a)

    ΔH > 0 for the forward reaction

    (b)

    ΔH = 0 for the reverse reaction

    (c)

    ΔH < 0 for the forward reaction

    (d)

    Sign of the ΔH cannot be predicted based on this information

  9. The KH for the solution of oxygen dissolved in water is 4 × 104 atm at a given temperature. If the partial pressure of oxygen in air is 0.4 atm, the mole fraction of oxygen in solution is

    (a)

    4.6 x 103

    (b)

    1.6 x 104

    (c)

    1 x 10-5

    (d)

    1 x 105

  10. Which of the following has see saw shape?

    (a)

    PCI5

    (b)

    IO2F-2

    (c)

    SOF4

    (d)

    ClO-3

  11. The isomer of ethanol is

    (a)

    acetaldehyde

    (b)

    dimethylether

    (c)

    acetone

    (d)

    methyl carbinol

  12. Which one of the following has least acidic character?

    (a)

    HCOOH

    (b)

    CH3COOH

    (c)

    CH2CICOOH

    (d)

    CCl3COOH

  13. Molecular formula of benzene is ________.

    (a)

    C6H6

    (b)

    C6H5

    (c)

    C7H8

    (d)

    CH4

  14. ​​​​​​​Identify the correct order of boiling point of halo alkanes?

    (a)

    CH3-CH2-CH2-CH2CI>(CH3)3C-CI > CH3-CH2-\(\underset { \overset { | }{ Cl } }{ CH } \)-CH3

    (b)

    CH3-CH2-CH2-CH2CI>CH3-CH2-\(\underset { \overset { | }{ Cl } }{ CH } \)-CH3< (CH3)3C-CI

    (c)

    (d)

  15. Assertion (A): Excessive use of chlorinated pesticide causes soil and water pollution.
    Reason (R) : Such pesticides are non-biodegradable.

    (a)

    Both (A) and R are correct and (R) is the correct explanation of (A)

    (b)

    Both (A) and R are correct and (R) is not the correct explanation of (A)

    (c)

    Both (A) and R are not correct

    (d)

    (A) is correct but( R) is not correct

  16. Part II

    Answer any 6 questions. Question no. 24 is compulsory.

    6 x 2 = 12
  17. Calculate the equivalent mass of the following - Sodium Hydroxide

  18. The stabilisation of a half filled d - orbital is more pronounced than that of the p-orbital why?

  19. Explain what is meant by efflerescence.

  20. Why are the airplane cabins artificially pressurized?

  21. The bond dissociation energies of gaseous chlorine, hydrogen, and hydrogen chloride are 104, 58, and 103 k.cal mol-1 respectively. Calculate the enthalpy of formation of HCI(g). Predict in which of the following, entropy increases/decreases. - 2NaHCO3(s) \(\rightarrow\)Na2CO3(s) + CO2(g) + H2O(s)

  22. For a given reaction at a particular temperature, the equilibrium constant has constant value. Is the value of Q also constant? Explain.

  23. Indicate the \(\sigma\) and \(\pi\) bonds in the following molecules.
    C6H6, CH2CI2, CH3NO2, CH2=C=CH2

  24. 0.24g of an organic compound gave 0.287 g of silver chloride in the carius method. Calculate the percentage of chlorine in the compound.

  25. Discuss the aromatic nucleophilic substitutions reaction of chlorobenzene.

  26. Part III

    Answer any 6 questions. Question no.33 is compulsory.

    6 x 3 = 18
  27. Balance the following reaction:
    S2O32- + I2\(\rightarrow\)S2O62- + I-

  28. State and explain pauli's exclusion principle

  29. Justify that the fifth period of the periodic table should have 18 elements on the basis of quantum numbers.

  30. Give a brief account of covalent hydrides.

  31. Why sodium hydroxide is much more water soluble than chloride?

  32. Explain graphical representation of Gay Lussac's law.

  33. The equilibrium constant of a reaction is 10, what will be the sign of ΔG? Will this reaction be spontaneous?

  34. 0.24 g of a gas dissolves in 1 L of water at 1.5 atm pressure. Calculate the amount of dissolved gas when the pressure is raised to 6.0 atm at constant temperature.

  35. Carry over the following reaction mechanisms.
    (i) Bromination of alkene
    (ii) Addition of HCN to CH3CHO
    (iii) Formation of alkyl bromide with benzoyl peroxide as radical initiator.

  36. Part IV

    Answer all the questions.

    5 x 5 = 25
    1. Explain about sp hybridisation with suitable example.

    2. Mention the standards prescribed by BIS for quality of drinking water

    1. An isotope of hydrogen (A) reacts with diatomic molecule of element which occupies group number 16 and period number 2 to give compound (B) is used as a moderator in nuclear reaction. (A) adds on to a compound ( C), which has the molecular formula C3H6 to give (D). Identify A, B, C and D.

    2. Starting from methyl magnesium iodide, how would you prepare
      (i) Ethyl methyl ether
      (ii) methyl cyanide
      (iii) methane

    1. Calculate the heat of glucose and its calorific value from following data:
      (i) C(graphite)+O2(g) ➝ CO2(g); ΔH= -395 KJ
      (ii) H2(g)+\(\frac{1}{2}\)O2 ➝ H2O(l);  ΔH= -269.4 KJ
      (iii) C+6H2(g)+3O2(g) ➝ C6H12O6(s);  ΔH= -1169.8 KJ

    2. Give IUPAC names for the following compounds
      1) CH3 – CH = CH – CH = CH – C ≡ C – CH3
      2) 
      3) (CH3)3 C – C ≡ C – CH (CH3)2
      4) ethyl isopropyl acetylene
      5) CH ≡ C – C ≡ C – C ≡ CH

    1. If an electron is moving with a velocity 600 ms-1 which is accurate upto 0.005%, then calculate the uncertainty in its position. (h = 6.63 x 10-34 Js. mass of electron = 9.1 x 10-31 kg)

    2. An alkali metal (A) belongs to period number II and group number I react with oxygen to form (B). (A) reacts with water to form (C) with liberation of hydrogen compound (D).Identify A, B, C and D.

    1. Balance the following equations by oxidation number method.
      K2Cr2O7 + HI ⟶ KI + Crl3 + H2O + I2

    2. Calculate the effective nuclear charge experienced by the 4s electron in potassium atom.

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