For Hydrogen spectrum of Lyman series falls under ______ region.

Question

Question

Answer 1

CONCEPT:

The spectral lines of the Lyman series fall in the U.V region for the Hydrogen atom.
We can predict this using this equation

\(\frac{1}{\lambda } = {R_H}\left( {\frac{1}{{{2^2}}} - \frac{1}{{{n^2}}}} \right)\)

Where R_H = Rydberg constant

When excited electrons fall from higher energy level to lower energy level, they emit electromagnetic radiations of discrete frequencies and the emission spectrum is formed.
Lyman series – when an electron from higher energy level falls to 1st energy level – UV region.
Balmer series – when an electron from higher energy level falls to 2nd energy level – Visible region.
Paschen series – when an electron from higher energy level falls to the 3rd energy level – Infrared region.
Brackett series – when an electron from higher energy level falls to 4th energy level – Infrared region.
Pfund series – when an electron from higher energy level falls to the 5th energy level – Infrared region.

EXPLANATION:

In a hydrogen atom, the transition of electrons between different energy levels gives spectral lines of different wavelengths. These lines fall into a specific series.
We can predict this using this equation

\(\Rightarrow \frac{1}{\lambda } = {R_H}\left( {\frac{1}{{{2^2}}} - \frac{1}{{{n^2}}}} \right)\)

In the Lyman series, the spectral lines correspond to the transition of an electron from a higher to lower energy level when the quantum number of the final stationary orbit ( n_f) is 1. and it falls under the UV region.