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(C) The molecular orbital electronic configuration of $O_2$ ($16$ electrons) is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^

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$5$

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(C) The molecular orbital electronic configuration of $O_2$ ($16$ electrons) is: $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2, \pi 2p_y^2, \pi^* 2p_x^1, \pi^* 2p_y^1$. Bonding molecular orbitals are those without an asterisk $(*)$. The bonding orbitals are $\sigma 1s, \sigma 2s, \sigma 2p_z, \pi 2p_x, \pi 2p_y$. Each of these $5$ orbitals contains $2$ electrons,totaling $10$ bonding electrons. Therefore,the number of bonding electron pairs is $10 / 2 = 5$.

According to molecular orbital theory,the total number of bonding electron pairs in $O_2$ is

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