The increasing order (lowest first) for the values of e/m (charge/mass) for
  • e, p, n, α
  • n, p, e, α
  • n, p, α, e
  • n, α, p, e
The ionization enthalpy of hydrogen atom is312 × 10J mol. The energy required to excite the electron in the atom from n = 1 to n = 2 is
  • 8. 51 × 10J mol
  • 6. 56 × 10J mol
  • 7. 56 × 10J mol
  • 9. 84 × 10J mol
or a given principal level n = 4, the energy of its subshells is in the order
  • s < p < d < f
  • s > p > d > f
  • s < p < f < d
  • f < p < d < s
A gas absorbs a photon of 355 nm and emits at two wavelengths. If one of the emissions is at 680 nm, the other is at:
  • 518 nm
  • 1035 nm
  • 325 nm
  • 743 nm
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
The magnetic quantum number specifies
  • Size of orbitals
  • Shape of orbitals
  • Orientation of orbitals
  • Nuclear Stability
The electronic configuration of silver atom in ground state is
  • [Kr]3d4s
  • [Xe]4f5d6s
  • [Kr]4d5s
  • None of the above
Which of the following element has least number of electrons in its M-shell?
  • K
  • Mn
  • Ni
  • Sc
Which one of the following sets of ions represents a collection of isoelectronic species? (Atomic nos. : F = 9, Cl = 17, Na = 11, Mg = 12, Al = 13, K = 19, Ca = 20, Sc = 21)
  • K, Ca, Sc, Cl
  • Na, Ca, Sc, F
  • K, Cl, Mg, Sc
  • Na, Mg, Al, Cl
In the ground state, an element has 13 electrons in its M-shell. The element is_____.
  • Copper
  • Chromium
  • Nickel
  • Iron
The electrons of the same orbitals can be distinguished by
  • Principal quantum number
  • Azimuthal quantum number
  • Spin quantum number
  • Magnetic quantum number
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
In Hydrogen atom, energy of first excited state is –4 eV. Then find out KE of same orbit of Hydrogen atom
  • 3. 4 eV
  • 6. 8 eV
  • -13. 6 eV
  • +13. 6 eV
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 = + \(\frac {1}{2}\)
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
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
A sub-shell with n = 6 , l = 2 can accommodate a maximum of
  • 12 electrons
  • 36 electrons
  • 10 electrons
  • 72 electrons
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 =63 × 10Js)
  • 6. 63 × 10 m
  • 6. 64 × 10 m
  • (i) and (ii)
  • None of the above
0 h : 0 m : 1 s

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