Draw the energy level diagram for hydrogen atom. Show the transitions of Lyman, Balmer, Paschen, Brackett and Pfund series in the diagram. In which region do these spectrum lie?
Show Hint
The energy of emitted light depends on the difference in energy levels. Smaller transitions (e.g., Balmer) lie in the visible range, while larger ones (e.g., Lyman) lie in the UV region.
Energy Level Diagram:
The hydrogen atom has discrete energy levels given by the formula:
\[
E_n = -13.6 \, \frac{1}{n^2} \, \text{eV} \quad \text{where} \quad n = 1, 2, 3, \ldots
\]
The electron transitions from a higher energy level \(n_i\) to a lower level \(n_f\) result in the emission of photons of specific wavelengths. Different spectral series correspond to transitions ending at specific lower energy levels:
Lyman series: Transitions to \(n = 1\)
Balmer series: Transitions to \(n = 2\)
Paschen series: Transitions to \(n = 3\)
Brackett series: Transitions to \(n = 4\)
Pfund series: Transitions to \(n = 5\)
Regions of the Electromagnetic Spectrum:
Lyman series – Ultraviolet region Balmer series – Visible region Paschen, Brackett, Pfund – Infrared region
