Concept: The hydrogen emission spectrum is divided into specific series based on the final energy level (\( p \)) of the electron transition. Each series corresponds to a distinct region of the electromagnetic spectrum.
Formula:$$ \text{Lyman } (p=1) \rightarrow \text{Ultraviolet} $$
$$ \text{Balmer } (p=2) \rightarrow \text{Visible} $$
$$ \text{Paschen } (p=3) \rightarrow \text{Infrared} $$
Solution:- The Lyman series occurs when electrons transition from higher energy levels (\( n \ge 2 \)) down to the ground state (\( p = 1 \)).
- These transitions release the highest amount of energy, corresponding to the shortest wavelengths, which fall strictly in the ultraviolet region.
Why other options are incorrect:Balmer (A) lies in the visible region. Paschen (B) and Brackett (D) both lie in the infrared region.
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