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Publication# Observation of the Rydberg states of nitric oxide trapped in an argon matrix

Abstract

Three new progressions consisting of broad bands (full width at half max. .simeq. 130 meV) were obsd. in the absorption spectrum of NO trapped in an Ar matrix. A Wannier model fails to describe these transitions; they are identified as the mol. Rydberg transitions A2S+, C2P, and D2S+-X2P(v',0), blue shifted with respect to their gas-phase positions by .apprx.0.85 eV. [on SciFinder (R)]

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Related concepts (21)

Rydberg formula

In atomic physics, the Rydberg formula calculates the wavelengths of a spectral line in many chemical elements. The formula was primarily presented as a generalization of the Balmer series for all atomic electron transitions of hydrogen. It was first empirically stated in 1888 by the Swedish physicist Johannes Rydberg, then theoretically by Niels Bohr in 1913, who used a primitive form of quantum mechanics. The formula directly generalizes the equations used to calculate the wavelengths of the hydrogen spectral series.

Rydberg constant

In spectroscopy, the Rydberg constant, symbol for heavy atoms or for hydrogen, named after the Swedish physicist Johannes Rydberg, is a physical constant relating to the electromagnetic spectra of an atom. The constant first arose as an empirical fitting parameter in the Rydberg formula for the hydrogen spectral series, but Niels Bohr later showed that its value could be calculated from more fundamental constants according to his model of the atom.

Hydrogen spectral series

The emission spectrum of atomic hydrogen has been divided into a number of spectral series, with wavelengths given by the Rydberg formula. These observed spectral lines are due to the electron making transitions between two energy levels in an atom. The classification of the series by the Rydberg formula was important in the development of quantum mechanics. The spectral series are important in astronomical spectroscopy for detecting the presence of hydrogen and calculating red shifts.

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