If 13.6 eV energy is required to ionize the hydrogen atom, then the required energy to remove an electron from n = 2 is:
Correct answer: B. 3.4 eV
- A. 10.2 eV
- B. 3.4 eV
- C. 0 eV
- D. 6.8 eV
Explanation
Ionizing a hydrogen atom from its ground state requires 13.6 eV. For an electron in the second orbit, it's already at a higher energy level, so less energy is needed. Specifically, only one-fourth of 13.6 eV, which is 3.4 eV, is required to remove it.
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Atoms emit or absorb light at specific wavelengths because electrons occupy quantized energy levels and change levels by absorbing or releasing photons. The topic covers emission and absorption spectra, spectral series, hydrogen’s line spectrum, energy-level transitions, and the relation between wavelength, frequency and photon energy.
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