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During change of $O^2$ to $O_2^-$ ion, the electron adds on which one of the following orbitals?
$\sigma^*$ orbital
$\sigma$ orbital
$\pi^*$ orbital
$\pi$ 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.
Similar Questions
Match List$-I$ with List$-II.$
| List$-I$ | List$-II$ |
| $(a)$ $Ne _{2}$ | $(i)$ $1$ |
| $(b)$ $N _{2}$ | $(ii)$ $2$ |
| $(c)$ $F _{2}$ | $(iii)$ $0$ |
| $(d)$ $O _{2}$ | $(iv)$ $3$ |
Choose the correct answer from the options given below:
