The line spectrum of the hydrogen atom is a fundamental concept in atomic physics, revealing the discrete energy levels within the atom. When electrons transition between these specific energy levels, they emit or absorb photons, resulting in distinct groups of spectral lines known as spectral series. There are several well-identified spectral series for hydrogen, each characterized by the principal energy level to which the electron falls.
The prominent spectral series observed in the hydrogen atom's emission spectrum, along with their respective regions in the electromagnetic spectrum, are listed below:
| Spectral Series | Electromagnetic Region |
|---|---|
| Lyman series | Ultraviolet |
| Balmer series | Visible |
| Paschen series | Near Infrared |
| Brackett series | Far Infrared |
| Pfund series | Far Infrared |
| Humphreys series | Far Infrared |
Each series is named after its discoverer and represents transitions of an electron from higher energy states down to a specific lower energy level. For instance, the Lyman series involves transitions to the first energy level, the Balmer series to the second, and so on. The energy of the emitted photons determines the wavelength of the spectral lines, thus placing each series in a specific part of the electromagnetic spectrum.
