Worksheet: Atomic Models

In this worksheet, we will practice describing the historical development of atomic models and the rationales, strengths, and limitations of each model.

Q1:

Which of the following accurately defines the quantization of electron energies within an atom?

  • AThe energies of two electrons cannot be equal.
  • BAn electron can possess any energy within a certain range.
  • CThe total electron energy is fixed.
  • DAn electron can possess only certain discrete energy values.
  • EOnly one electron can undergo a change in energy.

Q2:

Which of the following statements is true?

  • AIn the Bohr model of the atom, it is possible for electrons to have zero angular momentum.
  • BIn the quantum mechanical model of the atom, the distance of an electron from the atomic nucleus is quantized.
  • CThe electron in a hydrogen atom has different energies in the Bohr and quantum mechanical models of the atom.
  • DThe electron orbits of the Bohr model of the atom violate the Heisenberg uncertainty principle.
  • EOnly the quantum mechanical model of the atom can account for the discrete lines of an atomic emission spectrum.

Q3:

Which of the following statements is false?

  • AElectrons in the quantum mechanical model of the atom can exist in any finite volume of space.
  • BThe non-quantized electron orbits of the Rutherford model of the atom would not be stable.
  • CIn both the Bohr and quantum mechanical models of the atom, the energy of an electron is described by quantum numbers with discrete values.
  • DIn both the Bohr and quantum mechanical models of the atom, the position of an electron is described by quantum numbers with discrete values.
  • EIn the Rutherford, Bohr and quantum mechanical models of the atom, most of the volume of an atom contains infinitesimal mass.

Q4:

Rutherford investigated the properties of the atomic nucleus by firing 𝛼 particles at atoms of gold and measuring their deflection. How would the results of this experiment differ if neutrons were used instead of 𝛼 particles?

  • ANeutrons would not be deflected because they have no charge, so they are not attracted electrostatically to the electrons of the gold atoms.
  • BNeutrons would be deflected less because they are smaller than 𝛼 particles and, therefore, less likely to collide with the nuclei of the gold atoms.
  • CNeutrons would be deflected more because they are smaller than 𝛼 particles and therefore less likely to bind with the nuclei of the gold atoms.
  • DNeutrons would not be deflected because they have no charge, so they are not repelled electrostatically by the nuclei of the gold atoms.
  • ENeutrons would appear to be deflected more, as collisions with the gold nuclei would cause neutrons to be emitted over a wide range of angles.

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