Concept: Spectral lines are grouped by the lowest energy state involved in the transition. The larger the atomic drop, the higher the energy and the shorter the wavelength.
Formula:$$ \text{Lyman} \implies p = 1 $$
Solution:- The Lyman series is defined by transitions down to the ground state (\( n=1 \)).
- Because the energy gap between \( n=1 \) and any higher state is the largest in the hydrogen atom, these transitions yield the highest energy photons.
- High energy correlates with short wavelengths, placing these emissions entirely within the Ultraviolet (UV) light band.
Why other options are incorrect:Brackett (spelled 'Brachett' in the original exam), Pfund, and Paschen all involve transitions to much higher orbits (\( n=4, 5, 3 \) respectively). These smaller drops emit low-energy Infrared radiation.
Quality & Fidelity Assurance:
Every question on BeambePrep is rigorously curated against the official PMDC syllabus with zero filler, zero out-of-syllabus content, and zero typos. When an authentic past paper originally contained a historical mistake or ambiguity from the examining board (such as UHS or NUMS), BeambePrep faithfully reflects the original paper while detailing the nuance and scientific consensus in the autopsy above.