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11th Standard Chemistry English Medium Public Exam Model Question Paper June 2020 Question Bank Software May-26 , 2020

11th Standard Chemistry English Medium Public Exam Model Question Paper June 2020

11th Standard Chemistry English Medium Public Exam Model Question Paper June 2020

Public Exam Model Question Paper June 2020

11th Standard

    Reg.No. :
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Chemistry

Time : 02:30:00 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. Identify the incorrect statement about a compound.

    (a)

    A molecule cannot be separated into its constituent elements by physical methods of separation

    (b)

    A molecule of a compound has atoms of different elements

    (c)

    A compound retains the physical properties of its constituent element

    (d)

    The ratio of atoms of different elements in a compound is fixed

  2. The ratio of de Broglie wavelengths of a deuterium atom to that of an \(\alpha\) - particle, when the velocity of the former is five times greater than that of later, is ____________

    (a)

     4

    (b)

    0.2

    (c)

    2.5

    (d)

    0.4

  3. Which of the following N3-, O2-, F- is largest in size?

    (a)

    N3-

    (b)

    O2-

    (c)

    F-

    (d)

    All of these

  4. Non-stoichiometric hydrides are formed by _____________

    (a)

    palladium, vanadium

    (b)

    carbon, nickel

    (c)

    manganese, lithium

    (d)

    nitrogen, chlorine

  5. Half life of francium is _______

    (a)

    12.3 years

    (b)

    12.3 mins

    (c)

    21 years

    (d)

    21 mins

  6. The SI unit of pressure is __________.

    (a)

    Nm-2 Kg-1

    (b)

    Pascal

    (c)

    bar

    (d)

    atmosphere

  7. An ideal gas expands from the volume of 1 x 10-3 m3 to 1 x 10-2 m3 at 300 K against a constant pressure at 1 x 105 Nm-2. The work done is ______________

    (a)

    - 900 J

    (b)

    900 kJ

    (c)

    270 kJ

    (d)

    -900 kJ

  8. The equilibrium constant for a reaction at room temperature is K1 and that at 700 K is K2. If K1 > K2, then _____________

    (a)

    The forward reaction is exothermic

    (b)

    The forward reaction is endothermic

    (c)

    The reaction does not attain equilibrium

    (d)

    The reverse reaction is exothermic

  9. Phenol dimerises in benzene having van't Hoff factor 0.54. What is the degree of association ?

    (a)

    0.46

    (b)

    92

    (c)

    46

    (d)

    0.92

  10. During the formation of a chemical bond ________.

    (a)

    energy decreases

    (b)

    energy increases

    (c)

    energy remains zero

    (d)

    energy remains constant

  11. The IUPAC name of the compound \({ H }_{ 3 }C-\overset { \underset { | }{ { CH }_{ 3 } } }{ \underset { \overset { | }{ { CH }_{ 3 } } }{ C } } -CH=C{ \left( { CH }_{ 3 } \right) }_{ 2 }\) is _____________

    (a)

    2,4,4 – Trimethylpent -2-ene

    (b)

    2,4,4 – Trimethylpent -3-ene

    (c)

    2,2,4 – Trimethylpent -3-ene

    (d)

    2,2,4 – Trimethylpent -2-ene

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

    (a)

    HCOOH

    (b)

    CH3COOH

    (c)

    CH2CICOOH

    (d)

    CCl3COOH

  13. The most stable conformation of Butane is

    (a)

    Gauche-form

    (b)

    Partially eclipsed form

    (c)

    Anti-form

    (d)

    Eclipsed form

  14. Which one of the following is used as an insecticide and as a soil sterilising agent?

    (a)

    Chloroform

    (b)

    Chloral

    (c)

    Chloropicrin

    (d)

    Tetrachloromethane

  15. Assertion (A) : Excessive use of chlorinated pesticide causes soil and water pollution.
    Reason (R) : Such pesticides are non-biodegradable.
    i) Both (A) and R are correct and (R) is the correct explanation of (A)
    ii) Both (A) and R are correct and (R) is not the correct explanation of (A)
    iii) Both (A) and R are not correct
    iv) (A) is correct but( R) is not correct

    (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

  16. Define - Empirical formula of a compound

  17. For each of the following, give the sub level designation, the allowable m values and the number of orbitals
    (i) n = 4, l = 2
    (ii) n = 5, l = 3
    (iii) n = 7, l = 0

  18. Substantiate lithium fluoride has the lowest solubility among group one metal fluorides.

  19. Describe an experiment to show that V \(\alpha \) T

  20. What are spontaneous reaction? Give three examples for spontaneous reaction.

  21. Deduce the Vant Hoff equation.

  22. Calculate the formal charge on the carbon atom and oxygen atom in the structure:\(\overset { .. }{ \underset { .. }{ O } } =C=\overset { .. }{ \underset { .. }{ O } } \)\(\)

  23. Describe the reactions involved in the detection of nitrogen in an organic compound by Lassaigne method.

  24. Give reasons for polarity of C-X bond in halo alkane.

    25. Part III

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

    6 x 3 = 18

  25. Identify the type of redox reaction taking place in the following
    \(\overset { 0 }{ { Ca }_{ (s) } } +\overset { +1 }{ 2 } \overset { -2 }{ { H }_{ 2 }O_{ (l) } } \longrightarrow \overset { +2 }{ Ca } \overset { -2+1 }{ { (0H) }_{ 2(aq) } } +\overset { 0 }{ H } _{ 2(g) }\)

  26. State and explain pauli exclusion principle.

  27. Energy of an electron in the ground state of the hydrogen atom is -2.8 x 10-18 J. Calculate the ionisation enthalpy of atomic hydrogen in terms of kJ mol-1.

  28. Give a brief account of metallic (interstitial) hydrides.

  29. Write balanced chemical equation for each of the following chemical reactions.
    Lithium metal with nitrogen gas.

  30. What is meant by Boyle temperature (or) Boyle point? How is it related with compression point?

  31. What are state and path functions? Give two examples

  32. 2.82 g of glucose is dissolved in 30 g of water. Calculate the mole fraction of glucose and water.

  33. Illustrate with examples, the three types of electron movement in organic reaction.

    34. Part IV

    Answer all the questions.

    5 x 5 = 25

  34. Balance the following equation by ion electron method.
    Zn + NO3- ⟶ Zn + NH4+2

  35. A neutral atom of an element has 2K, 8L and 5M electrons. Find out the following.
    (i) Atomic number of the element 
    (ii) Total number of s-electrons 
    (iii) Total number of p-electrons
    (iv) Number of protons in the nucleus 
    (v) Valency of the element

  36. Give the characteristics of p-block elements.

  37. Explain preparation of hydrogen using electrolysis.

  38. Distinguish between alkali metals and alkaline earth metals.

  39. What are thermochemical equation? What are the conventions adopted in writing thermochemical equation?

  40. Explain about metallic bonding

  41. Give IUPAC names for the following compounds
    CH3 – CH = CH – CH = CH – C ≡ C – CH3

  42. Explain the mechanism involved in bimolecular nucleophilic substitution reaction.

  43. What are particulate pollutants ? Explain any three.

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