Multiple Choice
An atom's emission of light with a specific amount of energy confirms that:
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9. Quantum Mechanics
Emission Spectrum
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Which region of the electromagnetic spectrum does the Lyman series for atomic transitions in hydrogen primarily fall into?
A
Visible
B
Microwave
C
Ultraviolet
D
Infrared
Verified step by step guidance1
Understand that the Lyman series corresponds to electronic transitions in the hydrogen atom where electrons fall from higher energy levels (n ≥ 2) down to the ground state (n = 1).
Recall that the energy of a photon emitted during an electronic transition is given by the Rydberg formula: \(E = h \nu = R_H \left( \frac{1}{n_1^2} - \frac{1}{n_2^2} \right)\), where \(n_1 = 1\) for the Lyman series and \(n_2 > 1\).
Recognize that the energy difference for these transitions is relatively large because the electron falls to the lowest energy level, resulting in photons with high energy and thus short wavelengths.
Know that the electromagnetic spectrum regions are categorized by wavelength and energy: ultraviolet light has shorter wavelengths and higher energy than visible light, infrared, and microwaves.
Conclude that since the Lyman series involves high-energy transitions to the ground state, the emitted photons fall in the ultraviolet region of the electromagnetic spectrum.
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