The energy level of hydrogen is quantized, and the electrons in a hydrogen atom transition between these quantized energy levels. Each series of spectral lines corresponds to transitions that end at a specific level.
The energy levels
(n) for a hydrogen atom are given by the formula:
En=−‌When a hydrogen atom is bombarded with 13.6 eV electrons, the electrons are excited from the ground state
(n=1) to higher energy levels. When these electrons return to lower energy levels, they emit photons corresponding to specific spectral series:
Lyman Series: Transitions to
n=1 (ultraviolet region).
Balmer Series: Transitions to
n=2 (visible region).
Paschen Series: Transitions to
n=3 (infrared region).
Brackett Series: Transitions to
n=4 (infrared region).
Pfund Series: Transitions to
n=5 (infrared region).
Since the excited electrons started from the ground state with an energy of 13.6 eV , they returned to the ground state by releasing energy, corresponding to the Lyman series.
Thus, the emitted spectral line belongs to the Lyman series. Therefore, the correct option is:
Option A: Lyman series.
