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The Antibonding Effect

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Derek W. Smith

Department of Chemistry, University of Waikato, Private Bag 3105, Hamilton, New Zealand

J. Chem. Educ., 2000, 77 (6), p 780

DOI: 10.1021/ed077p780

Publication Date (Web): June 1, 2000

Section:

History, Education, and Documentation

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.

Keywords (Audience):

Upper-Division Undergraduate

Keywords (Domain):

Physical Chemistry

Keywords (Subject):

Covalent Bonding

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