Among KO_2,NO_2^-,BaO_2 and NO_2^+,an unpaire | vedclass

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(C) The electronic configurations are as follows:$1$. $KO_2$ contains the superoxide ion $O_2^-$. The molecular orbital configuration of $O_2^-$ is $\

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$KO_2$ only

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(C) The electronic configurations are as follows:$1$. $KO_2$ contains the superoxide ion $O_2^-$. The molecular orbital configuration of $O_2^-$ is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^1$. It has one unpaired electron.$2$. $NO_2^-$ has $5 + 6(2) + 1 = 18$ valence electrons. All electrons are paired.$3$. $BaO_2$ contains the peroxide ion $O_2^{2-}$. The configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^2 = \pi^* 2p_y^2$. All electrons are paired.$4$. $NO_2^+$ has $5 + 6(2) - 1 = 16$ valence electrons. All electrons are paired.Therefore,only $KO_2$ contains an unpaired electron.

Among $KO_2$,$NO_2^-$,$BaO_2$ and $NO_2^+$,an unpaired electron is present in:

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