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  Home > JCE Print > Journal of Chemical Education > Issues > 2006  > March  >
Research: Science and Education
The Old Quantum Theory for H2+: Some Chemical Implications
Stephen K. Knudson
Department of Chemistry, College of William and Mary, Williamsburg, VA 23187-8795
Cover
March 2006
Vol. 83 No. 3
p. 464
Abstract
The "old quantum theory" generates eigenvalues dependent entirely on the properties of classical orbits. Application of these old quantum theory ideas to diatomic molecules with one electron, such as H2+, is less successful than the corresponding application to one-electron atoms. Nonetheless, useful insight can be gleaned both from the successes and from the deficiencies of the application. Since obtaining correct values from quantum theory or accurate approximate values from uniform semiclassical theory provides quantitative results, the thrust of any old quantum theory formulation is to aide interpretation of results. The principal goals are then to show (i) the applicability of the method; (ii) the success of the method and its interpretation in terms of bonding in the ground state; and (iii) the fundamental failure of the classical approach and how that failure must influence bonding. The molecular orbits are less useful than their atomic analogues, but still deserve to be more widely known among chemists.
More Information
*  Citation
 Knudson, Stephen K. J. Chem. Educ. 2006 83 464.
*  Keywords
 Covalent Bonding; Graduate Education / Research; Ionic Bonding; Molecular Properties / Structure; Physical Chemistry; Physical Properties; Quantum Chemistry; Textbooks / Reference Books; Theoretical Chemistry; Upper-Division Undergraduate
*  History
 Created:
Last Updated:		 1/31/2006
2/6/2006
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