Important 1mark -chapter 1,2

11th Standard

    Reg.No. :
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Chemistry

Use blue pen Only

Time : 00:20:00 Hrs
Total Marks : 50

    Part A

    Answer all the questions

    50 x 1 = 50
  1. Assertion: Two mole of glucose contains 12.044 x 1023 molecules of glucose
    Reason: Total number of entities present in one mole of any substance is equal to 6.02 x 1022

    (a)

    both assertion and reason are true and the reason is the correct explanation of assertion

    (b)

    both assertion and reason are true but the reason is not the correct explanation of assertion

    (c)

    an assertion is true but reason is false

    (d)

    both assertion and reason are false

  2. 1 g of an impure sample of magnesium carbonate (containing no thermally decomposable impurities) on complete thermal decomposition gave 0.44 g of carbon dioxide gas. The percentage of impurity in the sample is ______________

    (a)

    0%

    (b)

    4.4%

    (c)

    16%

    (d)

    8.4%

  3. When 22.4 litres of H2(g) is mixed with 11.2 litres of Cl2(g), each at 273 K at 1 atm the moles of HCl (g), formed is equal to

    (a)

    2 moles of HCI (g)

    (b)

    0.5 moles of HCI (g)

    (c)

    1.5 moles of HCI (g)

    (d)

    1 moles of HCI (g)

  4. Hot concentrated sulphuric acid is a moderately strong oxidizing agent. Which of the following reactions does not show oxidising behaviour?

    (a)

    Cu + 2H2 SO4 \(\longrightarrow \) CuSO4 +SO2 + 2H2O

    (b)

    C + 2H2 + SO4 \(\longrightarrow \) CO2 + 2SO2 + 2H2O

    (c)

    BaCl2 + H2SO4 \(\longrightarrow \) BaSO4 + 2HCl

    (d)

    None of the above

  5. Fe2 + \(\longrightarrow\) Fe3+ + e- is a ________ reaction.

    (a)

    redox

    (b)

    reduction

    (c)

    oxidation

    (d)

    decomposition

  6. The oxidation number of oxygen in O2 is _______________

    (a)

    0

    (b)

    +1

    (c)

    +2

    (d)

    -2

  7. Which one of the following represents 180g of water?

    (a)

    5 Moles of water

    (b)

    90 moles of water

    (c)

    \(\frac { 6.022\times { 10 }^{ 23 } }{ 180 } \) molecules of water 

    (d)

    6.022 x 1024molecules of water

  8. Among the three metals, zinc, copper and silver, the electron releasing tendency decreases in the following order.

    (a)

    zinc >silver >copper

    (b)

    zinc >copper >silver

    (c)

    silver > copper >zinc

    (d)

    copper > silver > zinc

  9. Match the list-I with list-II and select the correct answer using the code given below the lists.

    List-I List-II
    A Cr2O72- 1 +5
    B MnO4- 2 +6
    C VO3- 3 +3
    D FeF63+ 4 +7
    (a)
    A B C D
    3 1 4 2
    (b)
    A B C D
    4 3 2 1
    (c)
    A B C D
    2 4 1 3
    (d)
    A B C D
    3 2 1 4
  10. The correct increasing order of the oxidation state of sulphur in the anions \({ SO }_{ 3 }^{ 2- },{ SO }_{ 3 }^{ 2- }{ , }{ { S }_{ 2 }{ O } }_{ 4 }^{ 2- },{ S }_{ 2 }{ O }_{ 6 }^{ 2- }\)

    (a)

    \({ SO }_{ 3 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ { S }_{ 2 }{ O } }_{ 4 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }\)

    (b)

    \({ SO }_{ 4 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 3 }^{ 2- }\)

    (c)

    \({ { S }_{ 2 }{ O } }_{ 4 }^{ 2- }<{ SO }_{ 3 }^{ 2- }<{ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 4 }^{ 2- }\)

    (d)

    \({ S }_{ 2 }{ O }_{ 6 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ SO }_{ 4 }^{ 2- }<{ SO }_{ 3 }^{ 2- }\)

  11. Two 22.4 litre containers A and B contains 8 g of O2 and 8 g of SO2 respectively at 273 K and 1 atm pressure, then

    (a)

    Number of molecules inA and B are same

    (b)

    Number of molecules in B is more than that in A.

    (c)

    The ratio between the number of molecules in A= to number of molecules in B is 2:1

    (d)

    Number of molecules in B is three times greater than the number of molecules in A

  12. Which of the following compound(s) has /have a percentage of carbon same as that in ethylene (C2H4)

    (a)

    propene

    (b)

    ethyne

    (c)

    benzene

    (d)

    ethane

  13. 1 amu (or) 1 u \(\approx \) 

    (a)

    1.6605 x 10-25 kg

    (b)

    1.6605 x 10-26 kg

    (c)

    1.6605 x 10-27 kg

    (d)

    1.6605 x 10-28 kg

  14. If a beaker holds 576g of water, what will be the gram molecules of water in that beaker?

    (a)

    23 gram molecule

    (b)

    23%

    (c)

    32%

    (d)

    32 gram molecule

  15. How many moles of magnesium phosphate Mg3(PO4)2 Will Contain 0.25 moles of oxygen atoms?

    (a)

    0.02

    (b)

    3.125 x 10-2

    (c)

    1.25 x 10-2

    (d)

    2.5 x 10-2

  16. Assertion: Equal volumes of all the gases do not contain equal number of atoms
    Reason: Atom is the smallest particle which takes part in chemical reactions.

    (a)

    Both assertion and reason are correct and reason is the correct explantion for assertion

    (b)

    Both assertion and reason are correct but reason  is not the correct explantion for assertion

    (c)

    Assertion is true but reason are false

    (d)

    Both assertion and reason are false

  17. How many equivalents of sodium sulphate is formed when sulphuric acid is completely neutralized by a base NaOH:

    (a)

    0.2

    (b)

    2

    (c)

    0.1

    (d)

    1

  18. Which of the following is a mono-atomic molecule?

    (a)

    Hydrogen

    (b)

    Oxygen

    (c)

    Sodium

    (d)

    Ozone

  19. How much volume of CO2 is produced when 50 g of CaCO3 is heated strongly?

    (a)

    2.24 x 10-2m3

    (b)

    22.4 L

    (c)

    11.2L

    (d)

    22400 Cm3

  20. In the reaction 2AuCl3 + 3SnCl2 \(\rightarrow\) 2Au + 3SnCl4 which is an oxidising agent?

    (a)

    AuCl3

    (b)

    Au

    (c)

    SnCl2

    (d)

    Both AuCl3 and SnCl2

  21. The number of moles of H, in 2.24 litre of hydrogen gas at STP is _______________

    (a)

    1

    (b)

    0.1

    (c)

    0.01

    (d)

    0.001

  22. The mass of an atom of nitrogen is _______________.

    (a)

    \(\frac { 14 }{ 6.023\times { 10 }^{ 23 } } \)

    (b)

    \(\frac { 28 }{ 6.023\times { 10 }^{ 23 } } \)

    (c)

    \(\frac { 1 }{ 6.023\times { 10 }^{ 23 } } \)

    (d)

    14 amu

  23. The oxidation number of carbon in CH3 - CH2OH is _______________.

    (a)

    +2

    (b)

    -2

    (c)

    0

    (d)

    +4

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

      List-I (acids   List-II (Basicity)
    A HCl 1 3
    B H2SO4 2 4
    C H4P2O7 3 2
    D H3PO4 4 1
    (a)
    A B C D
    4 3 2 1
    (b)
    A B C D
    3 4 1 2
    (c)
    A B C D
    4 1 3 2
    (d)
    A B C D
    4 1 3 2
  25. Match the List-I and List-II using the correct code given below the list.

      List-I (Empirical Formula)   List-II (Molecular formula)
    A Benzene - CH 1 H2O2
    B Fructose - CH2O 2 C2H2
    C Acetylene - CH 3 C6H6
    D Hydrogen peroxide-OH 4 C6H12O6
    (a)
    A B C D
    4 2 3 1
    (b)
    A B C D
    3 4 2 1
    (c)
    A B C D
    4 1 2 3
    (d)
    A B C D
    1 4 3 2
  26. Splitting of spectral lines in an electric field is called

    (a)

    Zeeman effect

    (b)

    Shielding effect

    (c)

    Compton effect

    (d)

    Stark effect

  27. According to the Bohr Theory, which of the following transitions in the hydrogen atom will give rise to the least energetic photon?

    (a)

    n = 6 to n = 1

    (b)

    n = S to n = 4

    (c)

    n = S to n = 3

    (d)

    n = 6 to n = S

  28. Which of the following pairs of d-orbitals will have electron density along the axes ?

    (a)

    dz2, dxz

    (b)

    dxz, dyZ

    (c)

     dz2, dx2-y2

    (d)

    dxy ,dx2-y2

  29. For d-electron, the orbital angular momentum is

    (a)

    \(\frac { \sqrt { 2 } h }{ 2\pi } \)

    (b)

    \(\\ \frac { \sqrt { 2h } }{ 2\pi } \)

    (c)

    \(\frac { \sqrt { 2\times 4 } h }{ 2\pi } \)

    (d)

    \(\frac { \sqrt { 2\times 4 } h }{ 2\pi } \)

  30. As per Aufbau principle, arrange the orbitals in increasing order of energy

    (a)

    4p > 4d > 5s > 5p

    (b)

    4p < 4d < 5s < 5p

    (c)

    4d < 4p < 5s < 5p

    (d)

    4p < 5s < 4d < 5p

  31. Which one of the following orbitals is spherical in shape?

    (a)

    4s

    (b)

    3p

    (c)

    3d

    (d)

    4f

  32. The total number of orbitals associated with the principal quantum number n = 3 is

    (a)

    9

    (b)

    8

    (c)

    5

    (d)

    7

  33. How many electrons in an atom with atomic number 105 can have (n + I) = 8 ? 

    (a)

    30

    (b)

    17

    (c)

    15

    (d)

    unpredictable

  34. If uncertainty in position and momentum are equal, then minimum uncertainty in velocity is

    (a)

    \(\frac { 1 }{ m } \sqrt { \frac { h }{ \pi } } \)

    (b)

    \( \sqrt { \frac { h }{ \pi } } \)

    (c)

    \(\frac { 1 }{ 2m } \sqrt { \frac { h }{ \pi } } \)

    (d)

    \( { \frac { h }{4\pi } } \)

  35. 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)

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

  36. Consider the following statements
    1.\(\lambda\) .= h / mv is valid only when the particle travels at speed much less than the speed of light.
    2. Einstein's mass-energy relationship is E=mc2
    3. The angular momentum (mvr) ofthe electron must be equal to an integral multiple of h/4\(\pi\) . Which of the following statementts) given above is/ are correct?

    (a)

    1&3 

    (b)

    Only 1

    (c)

    1 & 2

    (d)

    1, 2 & 3

  37. How many neutrons and protons respectively are present  in the 6C13 nuclei?

    (a)

    6, 13

    (b)

    6, 7

    (c)

    13,6

    (d)

    7,6

  38. Almost the entire mass of an atom is concentrated in the ----

    (a)

    proton

    (b)

    electrons

    (c)

    neutrons

    (d)

    nucleus

  39. The value of Bohr radius for hydrogen atom is

    (a)

    0.529 \(\times\) 10-8 cm

    (b)

    0.529 \(\times\) 10-10 cm

    (c)

    0.529 \(\times\) 10-12 cm

    (d)

    0.529 \(\times\) 10-12 cm

  40. What is the maximum number of orbitals that can be identified with the following quantum numbers? n=3,l=1,m1=0

    (a)

    1

    (b)

    2

    (c)

    3

    (d)

    4

  41. The de-Broglie wavelength of a particle with mass 19and velocity 100 m/s is

    (a)

    6.63 \(\times\) 10-35 m

    (b)

    6.63 \(\times\) 10-34 m

    (c)

    6.63 \(\times\) 10-33 m

    (d)

    6.65 \(\times\) 10-35 m

  42. The wavelength associated with an electron moving with velocity 1010 ms-1 is

    (a)

    6.62 \(\times\) 10-10 m

    (b)

    7.28  \(\times\) 10-14 m

    (c)

    3.69 \(\times\) 10-12 m

    (d)

    4.92 \(\times\) 10-11 m

  43. Assertion: The spectrum of Heis expected to be similar to that of hydrogen
    Reason: He is also one electron system.

    (a)

    If both assertion and reason are true and reason is the correct explanation of correct explanation of assertion.

    (b)

    If both assertion and reason are reason are true but reason is not the correct explanation of assertion

    (c)

    If assertion is true but reason is false

    (d)

    If both assertion and reason are false

  44. Assertion: Number of radial and angular nodes for 3p orbital are 1, 1 respectively.
    Reason: Number of radial and angular nodes depends only on principal quantum number.

    (a)

    both assertion and reason are true and reason is the correct explanation of assertion.

    (b)

    both assertion and reason are true but reason is not the correct explanation of assertion.

    (c)

    assertion is true but reason is false

    (d)

    both assertion and reason are false

  45. For a principle quantum number n = 4, the total number of orbitals having l = 3 is:

    (a)

    3

    (b)

    7

    (c)

    5

    (d)

    9

  46. How many orbitals are possible in 3rd energy level?

    (a)

    16

    (b)

    9

    (c)

    3

    (d)

    27

  47. The value of n, I, m and s of 8th electron in an oxygen atom are respectively____________.

    (a)

    \(1,0,0,+\frac{1}{2}\)

    (b)

    \(2,1,+1,-\frac{1}{2}\)

    (c)

    \(2,1,-1,-\frac{1}{2}\)

    (d)

    \(2,1,0,+\frac{1}{2}\)

  48. Who proposed the dual nature of light to all forms of matter?

    (a)

    John Dalton

    (b)

    Neils Bohr

    (c)

    Albert Einstein

    (d)

    J. J. Thomson

  49. The crystal used in Davison and Germer experiment is____________________

    (a)

    nickel

    (b)

    zinc sulphide

    (c)

    gold foil

    (d)

    NaCI

  50. When l= 0, the number of electrons that can be accommodated in the subshell is_______________

    (a)

    0

    (b)

    2

    (c)

    6

    (d)

    8

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