The number of antibonding electron pairs in O | vedclass

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(B) The total number of electrons in $O_{2}^{2-}$ is $8 + 8 + 2 = 18$. The molecular orbital configuration is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^

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$4$

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(B) The total number of electrons in $O_{2}^{2-}$ is $8 + 8 + 2 = 18$. The molecular orbital configuration is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^2$. The antibonding orbitals are $\sigma^* 1s$,$\sigma^* 2s$,$\pi^* 2p_x$,and $\pi^* 2p_y$. Each of these contains $2$ electrons,forming $4$ antibonding electron pairs.

The number of antibonding electron pairs in $O_{2}^{2-}$ molecular ion on the basis of molecular orbital theory is (Atomic number of $O$ is $8$)

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