Smallest wavelength occurs for:
A. Lyman series
B. Balmer series
C. Paschen series
D. Brackett series

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Detailed Solution

According to Bohr’s model, an electron absorbs energy when it moves from its lowest stationary state (ground state) to a higher energy level. Conversely, it emits energy in the form of radiation when it returns from a higher energy level to a lower stationary state. The emitted radiations have specific wavelengths, which correspond to the regions of the electromagnetic spectrum.

Different spectral series are observed depending on the electron transitions:

Series	Transition (n₁ → n₂, n₃, …)	Spectral Region
Lyman series	1 → 2, 3, 4…	Ultraviolet (UV)
Balmer series	2 → 3, 4, 5…	Visible light
Paschen series	3 → 4, 5, 6…	Infrared (IR)
Brackett series	4 → 5, 6, 7…	Infrared (IR)
Pfund series	5 → 6, 7, 8…	Infrared (IR)