key term - Hydrogen spectrum wavelength

Definition

The hydrogen spectrum wavelength corresponds to the specific wavelengths of light emitted or absorbed by hydrogen atoms when electrons transition between energy levels. These wavelengths form a series of spectral lines that are fundamental to understanding atomic structure.

5 Must Know Facts For Your Next Test

1. The hydrogen spectrum is divided into several series: Lyman, Balmer, Paschen, Brackett, and Pfund.
2. The Balmer series corresponds to transitions where the electron falls to the second energy level and is visible in the optical spectrum.
3. Each spectral line in the hydrogen spectrum can be calculated using the Rydberg formula: $\frac{1}{\lambda} = R_H \left(\frac{1}{n_1^2} - \frac{1}{n_2^2}\right)$ where $R_H$ is the Rydberg constant.
4. The Lyman series involves transitions to the ground state (n=1) and emits ultraviolet light.
5. Bohr's model explains that these discrete wavelengths result from quantized electron energy levels.

Review Questions

Related terms

Rydberg Constant:

A physical constant associated with atomic spectra, denoted as $R_H$, used in calculating wavelengths of spectral lines.

Balmer Series: A set of spectral lines for hydrogen that appear when an electron transitions to n=2 from higher energy levels; visible in optical light.

$Bohr\\textquotesingle{}s Theory$: $A model proposing that electrons exist in quantized energy levels around an atom\\textquotesingle{}s nucleus and emit or absorb specific wavelengths of light during transitions.$