The following sections of this BookRags Literature Study Guide is offprint from Gale's For Students Series: Presenting Analysis, Context, and Criticism on Commonly Studied Works: Introduction, Author Biography, Plot Summary, Characters, Themes, Style, Historical Context, Critical Overview, Criticism and Critical Essays, Media Adaptations, Topics for Further Study, Compare & Contrast, What Do I Read Next?, For Further Study, and Sources.
(c)1998-2002; (c)2002 by Gale. Gale is an imprint of The Gale Group, Inc., a division of Thomson Learning, Inc. Gale and Design and Thomson Learning are trademarks used herein under license.
The following sections, if they exist, are offprint from Beacham's Encyclopedia of Popular Fiction: "Social Concerns", "Thematic Overview", "Techniques", "Literary Precedents", "Key Questions", "Related Titles", "Adaptations", "Related Web Sites". (c)1994-2005, by Walton Beacham.
The following sections, if they exist, are offprint from Beacham's Guide to Literature for Young Adults: "About the Author", "Overview", "Setting", "Literary Qualities", "Social Sensitivity", "Topics for Discussion", "Ideas for Reports and Papers". (c)1994-2005, by Walton Beacham.
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The Rydberg constant, 10,973,731.57 m-1 , is the constant used in the Rydberg equation which describes the Rydberg state energies of a Rydberg series. This equation describes many line series of elements very well and the constant is universal to all elements.
In 1885, Swiss mathematician Johann Balmer showed that the wavelength of the visible spectrum of the hydrogen atom can be described by a formula relating the wavelength to Planck's constant times a function of the principle quantum number. Independently, Johannes Rydberg analyzed the spectra of many elements. He was the first to relate the principal lines of these spectra to a distinct series. To minimize the number of calculations, he introduced the concept of a wave number, which is the reciprocal of the wavelength and is the number of waves per length, more specifically, the number of waves per centimeter. Having made this change he began to see patterns not previously discernable. He found that for a given series when he plotted the difference in wave number versus the principle quantum number he obtained hyperbolic curves that were virtually identical in shape for different series and different elements. From this observation he was able to formulate the Rydberg equation, E = -R /(n-m)[sup2 ] where E is the energy of the line in wave numbers, R is the Rydberg constant, n is the principle quantum number and m is the quantum defect. The quantum defect describes how much the Rydberg series departs from the behavior of the Rydberg states of atomic hydrogen and is directly related to the interaction of the excited electron with the leftover ion core. This equation describes the Rydberg series for the elements. The Rydberg series is a set of bound states of the excited electron for a given set of excited electron angular momentum quantum numbers and ion core state.
In 1913 Niels Bohr showed that the Rydberg constant can be expressed as a combination of the speed of light in a vacuum c, Planck's constant h, the electron's charge e, and its mass m by R = me4 /(8eo[sup2 ]h[sup3 ]c), where eo is the permittivity of vacuum.