W2013CHM2311 Part 4a Notes

The effect is inversely proportional to the

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Unformatted text preview: ȹȺ 2 Ⱥȹ in bonding orbitals ȹ ȹ in antibonding orbitals ȹȺ ȹ Ⱥ ȹ Ⱥ H2: Bond order = 0.5(2 – 0) = 1 H2 has a single bond He2: Bond order = 0.5(2 – 2) = 0 He2 has a zero ­order bond Bond order indicates the strength of a bond: Large bond order = stronger bond Bond Type Single bond Bond Order Bond Energy 1 200 – 300 kJ/mol Double bond 2 500 – 600 kJ/mol Triple bond 3 900 – 1000 kJ/mol Bond energy = energy required to break the bond Bond orders do not have to be integers! Bond orders of 0.5, 1.33, 1.5, 2.5, etc. are possible! Molecular Orbital Theory Requirement for Bonding Bonding will only occur if the overall energy of electrons in the molecule is lower than the overall energy of electrons in the isolated atoms – i.e., the molecule must be more stable than the isolated atoms. Rules for MO Diagrams 1)  # of MOs = # AO...
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