REVIEW QUESTIONS

Chapter 7

  1. Calculate the wavelength and energy of a photon of radiation with frequency of .
  2. What is the wavelength of radiation with energy of ? In what region of the electromagnetic spectrum would this radiation be found?
  3. For each of the following transitions in the hydrogen atom, calculate the energy, wavelength and frequency of the associated radiation and determine whether radiation is absorbed or emitted during the transition.
    a) from to
    b) from to
  4. Use the diagrams below to determine the wavelength and frequency of each wave shown. (Assume the same time and distance scale for both waves)
  5. The energy needed to remove an electron completely from an atom is called its ionization energy. In terms of Bohr's model, ionization can be considered a process in which the electron moves to an "orbit" of infinite radius. The ionization of a ground-state hydrogen atom can therefore be calculated by assuming that the electron undergoes a transition from state to state. Calculate this energy in .
  6. The energy required to ionize sodium atom is . What minimum frequency of light is required to ionize sodium?
  7. The binding energy of electrons in a metal is . Determine the threshold frequency for this metal.
  8. Determine the velocity of an electron emitted by a metal whose threshold frequency is when it is exposed to visible light of .
    (mass of electron )
  9. Determine if each set of quantum numbers below is permissible or not. If yes, write the orbital designation for each.
    a)
    b)
    c)
    d)
  10. Write the quantum numbers associated with each of the following orbitals:
    a) 4p
    b) 3d
    c) 7s n= l=
    d) 5f
  11. The quantum numbers listed below are for four different orbitals. List them in order of increasing energy. Indicate whether any two have the same energy.
    a)
    b)
    c)
    d)
  12. When a compound containing cesium is heated in a Bunsen burner flame, photons with energy of are emitted. What color is the cesium flame?
  13. The ion contains one electron and is therefore a hydrogen-like ion. Calculate the wavelength of the first four electron transitions ( and ) for this ion and compare with the same transitions in the H atom. Comment on the differences. ( R for )