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4.Chemical Bonding and Molecular Structure
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During change of $O^2$ to $O_2^-$ ion, the electron adds on which one of the following orbitals?
A
$\sigma^*$ orbital
B
$\sigma$ orbital
C
$\pi^*$ orbital
D
$\pi$ orbital
Solution
Molecular orbital configuration of $\mathrm{O}_{2}$ (total $\mathrm{e}^{-}=16$ )
The electronic confiugration of oxygen is given as:
$\begin{array}{l}=1 \mathrm{s}^{2}, \sigma^{*} 1 \mathrm{s}^{2}, \sigma 2 \mathrm{s}^{2}, \sigma^{*} 2 \mathrm{s}^{2}, \sigma 2 \mathrm{p}_{z}^{2}, \pi 2 \mathrm{p}_{\mathrm{x}}^{2}=\pi 2 \mathrm{p}_{\mathrm{y}}^{2}, \pi^{*} 2 \mathrm{p}_{\mathrm{x}}^{1}=\pi^{*} 2 \mathrm{p}_{\mathrm{y}}^{1} \\ \mathrm{O}_{2}^{-}=8+8+1=17\end{array}$
Thus, during the change of $\mathrm{O}_{2}$ to $\mathrm{O}_{2}^{-}$ the electron is added into $\pi^{*}$ orbital.
Standard 11
Chemistry
