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  Home > JCE Print > Journal of Chemical Education > Issues > 2005  > August  >
In the Classroom
Some Observations on Molecular Orbital Theory
James F. Harrison
Department of Chemistry, Michigan State University, East Lansing, MI 48824-1322

Daniel B. Lawson
Department of Natural Science, University of Michigan-Dearborn, Dearborn, MI 48128-1491

Cover
August 2005
Vol. 82 No. 8
p. 1205
Abstract
The authors show, according to molecular orbital theory, why molecular orbital energies are not equally spaced above and below their constituent atomic orbital energies. Also, comments are made describing MO theory's ability to predict experimental properties such as bond length, dissociation energy, and the theory's incorrect ordering of the low-lying electronic states of C2.
More Information
*  Citation
 Harrison, James F.; Lawson, Daniel B. J. Chem. Educ. 2005 82 1205.
*  Keywords
 Computational Chemistry; Covalent Bonding; Graduate Education / Research; Mathematics / Symbolic Mathematics; Misconceptions / Discrepant Events; MO Theory; Molecular Modeling; Physical Chemistry; Quantum Chemistry; Textbooks / Reference Books; Theoretical Chemistry; Upper-Division Undergraduate
*  History
 Created:
Last Updated:		 July 5, 2005
July 8, 2005
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