Why is KO_{2} paramagnetic? | vedclass

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(B) The compound $KO_{2}$ consists of $K^{+}$ and $O_{2}^{-}$ ions. The superoxide ion $O_{2}^{-}$ has $13$ valence electrons. According to molecular

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Due to the presence of one unpaired electron in the $\pi^{*} 2p$ molecular orbital.

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(B) The compound $KO_{2}$ consists of $K^{+}$ and $O_{2}^{-}$ ions. The superoxide ion $O_{2}^{-}$ has $13$ valence electrons. According to molecular orbital theory,the electronic configuration of $O_{2}^{-}$ is $\sigma 1s^{2}, \sigma^{*} 1s^{2}, \sigma 2s^{2}, \sigma^{*} 2s^{2}, \sigma 2p_{z}^{2}, \pi 2p_{x}^{2} = \pi 2p_{y}^{2}, \pi^{*} 2p_{x}^{2} = \pi^{*} 2p_{y}^{1}$. The presence of one unpaired electron in the $\pi^{*} 2p$ molecular orbital makes $O_{2}^{-}$ paramagnetic.

Why is $KO_{2}$ paramagnetic?

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