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The total number of electrons in O2²⁻ is 16 + 2 = 18. The molecular orbital configuration is σ1s², σ*1s², σ2s², σ*2s², σ2p²x, π2p²y, π2p²z, π*2p²y, π*2p²z. The antibonding electrons are 8 (4 pairs).

1. The total number of electrons in O2²⁻ is 16 + 2 = 18.
2. It is known that the bond order in O2 is 2, while in O2²⁻ it is 1.5. Hence, this statement is incorrect.
3. The bond length of N-O decreases in a specific order.
4. This configuration includes four fully occupied bonding molecular orbitals and one fully occupied antibonding molecular orbital.

Correct answer: It is known that the bond order in O2 is 2, while in O2²⁻ it is 1.5. Hence, this statement is incorrect.

Solution

Statement B is incorrect because the bond order of O2²⁻ is 1, not 1.5. Bond order is calculated as (Nb - Na)/2, where Nb and Na are the number of bonding and antibonding electrons, respectively.

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