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Molecular Orbital Energy Diagrams

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Question

Explain on the basis of molecular orbital theory why bond order decreases when N₂changes to N₂⁺ while it increases when O₂changes to O₂⁺.

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Solution

Hi,

it is so because in N₂⁺, there is one electron less in bonding orbital as compared to electrons in N₂, and we know that bond order is (bonding electron-anti bonding electrons)/2, thus reducing the bond order.

In case of O₂, there are 2 electrons in anti bonding orbital but when it forms O₂⁺, it has one electron less in anti bonding electron, thus bond order is increased as the number of electrons in antibonding orbital has reduced from 2 to 1 in O₂⁺.

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N - N

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N_{2}^{+}

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when $O_{2}$ goes to $O_{2}^{+}$ , the o - o bond distance....

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