Atomic line spectra and energy levels Quiz
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5 questions, one answer each
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1. An electron in an atom falls from a level of −2.0 eV to −5.0 eV. What is the energy of the photon emitted?
- A. 7.0 eV
- B. 2.5 eV
- C. 3.0 eV
- D. −3.0 eV
2. What does a line emission spectrum show about the energy of electrons in atoms?
- A. Electron energy can take any value
- B. Electron energy is restricted to discrete values
- C. Electrons have no energy
- D. Electron energy is the same in all elements
3. A photon of energy 6.0 eV meets atoms whose gaps from the ground state are 4.9 eV, 6.7 eV and 8.8 eV. What happens?
- A. It is absorbed and the extra energy kept as kinetic energy
- B. It excites an electron to the 4.9 eV level and 1.1 eV is lost
- C. It passes through without being absorbed
- D. It is absorbed to the 6.7 eV level
4. Which frequency is emitted for an energy change of 2.0 eV? (h = 6.63 × 10⁻³⁴ J s, e = 1.60 × 10⁻¹⁹ C)
- A. 4.8 × 10¹⁴ Hz
- B. 3.0 × 10¹⁴ Hz
- C. 2.1 × 10⁻¹⁵ Hz
- D. 4.8 × 10¹⁵ Hz
5. Why are dark lines seen when white light passes through cool hydrogen gas?
- A. Hydrogen atoms absorb all photons equally
- B. The photons are converted into heat that is not detected
- C. Hydrogen atoms emit dark photons
- D. Hydrogen atoms absorb photons whose energies match transitions and re-emit them in random directions