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Hydrogen spectral series
In physics, the spectral lines of hydrogen correspond to particular jumps of the electron between energy levels. The simplest model of the hydrogen atom is given by the Bohr model. When an electron jumps from a higher energy to a lower, a photon of a specific wavelength is emitted according to the Rydberg formula:
Additional recommended knowledge
where n is the initial energy level and n' is the final energy level, and R is the Rydberg constant.
The spectral lines are grouped into series according to n' :
Hydrogen is the element with the simplest-to-analyze emission spectrum. All other atoms possess at least two electrons in their unionized form and the interactions between these electrons makes analysis of the spectrum by such simple methods as described here impractical. The deduction of the Rydberg formula was a major step in physics, but it was long before an extension to the spectra of other elements could be accomplished.
|This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Hydrogen_spectral_series". A list of authors is available in Wikipedia.|