Information AboutAntibonding |
| CATEGORIES ABOUT ANTIBONDING | |
| chemical bonding | |
| chemistry theories | |
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Antibonding molecular orbits (MOs) are normally ''higher'' in energy than bonding MOs. They are occupied by two electrons at a time and (in the case of Hydrogen ), each Atom can contribute only one electron, therefore only the ''s'' (bonding) MO is occupied and the H2 molecule is more stable than two separate H atoms.
In molecules with several atoms, such as Benzene , a particular MO may be ''bonding with respect to some adjacent pairs of atoms'' and ''antibonding with respect to other pairs''. If the bonding interactions outnumber the antibonding interactions, the MO is said to be "bonding," while if the antibonding interactions outnumber the bonding interactions, the MO is said to be "antibonding". Since each Carbon atom contributes only one electron to the π-system of benzene, there are six π-electrons and therefore only the three lowest-energy MOs (the bonding ones) are filled. Another particular feature of antibonding is that the ''antibonding orbital is more antibonding than the bonding orbital is bonding''. This leads to the conclusion that the energy of both MOs are raised by the presence of nucleus-nucleus repulsion. Antibonding orbitals are also important for explaining Chemical Reaction s in terms of molecular orbital theory. Roald Hoffmann and Kenichi Fukui shared the 1981 Nobel Prize In Chemistry for their work and further development of Qualitative MO explanations for chemical reactions. REFERENCES
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