CBSE  /  Class 11  /  Chemistry  /  Structures of Atom

  • 1. 
    The electrons of the same orbitals can be distinguished by

  • Principal quantum number
  • Azimuthal quantum number
  • Spin quantum number
  • Magnetic quantum number

  • 2. 
    Consider the ground state of Cr atom (Z = 24). The numbers of electrons with the azimuthal quantum numbers, l = 1 and 2 are, respectively:

  • 12 and 4
  • 12 and 5
  • 16 and 4
  • 16 and 5

  • 3. 
    A body of mass 10 mg is moving with a velocity of 100 ms. The wavelength of de-Broglie wave associated with it would be (Note: h = 6. 63 × 10Js)

  • 6. 63 × 10 m
  • 6. 63 × 10 m
  • 6. 63 × 10 m
  • 6. 63 × 10 m

  • 4. 
    In Hydrogen atom, energy of first excited state is – 3. 4 eV. Then find out KE of same orbit of Hydrogen atom

  • 3. 4 eV
  • 6. 8 eV
  • -13. 6 eV
  • +13. 6 eV

  • 5. 
    Which of the following sets of quantum numbers represents the highest energy of an atom?

  • n = 3, l = 0, m = 0, s = + \(\frac {1}{2}\)
  • n = 3, l = 1, m = 1, s = + \(\frac {1}{2}\)
  • n = 3, l = 2, m = 1, s = + \(\frac {1}{2}\)
  • n = 4, l = 0, m = 0, s = + \(\frac {1}{2}\)

  • 6. 
    In the Bohrs model of the hydrogen atom, the ratio of the kinetic energy to the total energy of the electron in a quantum state n is:

  • 1
  • 2
  • -1
  • -2

  • 7. 
    Which of the following statements does not form a part of Bohrs model of hydrogen atom?

  • Energy of the electrons in the orbit is quantised
  • The electron in the orbit nearest the nucleus has the lowest energy
  • Electrons revolve in different orbits around the nucleus
  • The position and velocity of the electrons in the orbit cannot be determined simultaneously

  • 8. 
    Which of the following statements in relation to the hydrogen atom is correct?

  • 3s orbital is lower in energy than 3p orbital
  • 3p orbital is lower in energy than 3d orbital
  • 3s and 3p orbitals are of lower energy than 3d orbital
  • 3s, 3p and 3d orbitals all have the same energy

  • 9. 
    A sub-shell with n = 6 , l = 2 can accommodate a maximum of

  • 12 electrons
  • 36 electrons
  • 10 electrons
  • 72 electrons
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