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  Home > JCE Print > Journal of Chemical Education > Issues > 2000  > June  >
Research: Science and Education
The Antibonding Effect
Derek W. Smith
Department of Chemistry, University of Waikato, Private Bag 3105, Hamilton, New Zealand
Cover
June 2000
Vol. 77 No. 6
p. 780
Abstract
It is shown that the consequence of filling both a bonding molecular orbital (MO) and its antibonding counterpart leads to a total orbital energy greater than that of the separated atoms. The resulting antibonding effect can be buffered if the antibonding MO mixes with higher empty MOs of the same symmetry. These considerations explain why Be2 has a weak covalent bond, much stronger than in He2. The antibonding effect also helps to explain the weakness of the F-F, O-O, and N-N single bonds. It is also useful in dealing with the stereochemistry of dn transition metal ions (n > 7); the favored coordination geometries are those that minimize the antibonding effect, or which allow its effective buffering.
More Information
*  Citation
 Smith, Derek W. J. Chem. Educ. 2000 77 780.
*  Keywords
 Bonding Theory; MO Theory; Theoretical Chemistry
*  History
 Created:
Last Updated:		 April 25, 2000
April 15, 2005
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