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Using their MO diagrams, explain the difference in ionization energy between F2 (1515 kJ/mol) and O2...

Using their MO diagrams, explain the difference in ionization energy between F2 (1515 kJ/mol) and O2 (1165 kJ/mol).

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Answer #1

The MO Diagram for both F2 and O2 is same, as shown:

That is why the energy level from which the electron is to be ionized is same in both the cases which is 2p*. Therefore, the factor which now determines the ionization energy of the molecule is the number and placement (whether pairing is possible or not) of antibonding electrons which is 6 for F2 and 4 for O2.

In case of F2: The HOMO electrons are paired which makes it difficult to get ionized due to their extra stability. Hence higher Ionization Energy.

In case of O2: The HOMO electrons are unpaired and therefore no such higher ionization is required to remove that one electron. Hence it doesn't have the higher ionization energy out of the two.

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