Which of the following pairs of species are p | vedclass

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(C) To determine paramagnetism,we look for the presence of unpaired electrons.$1$. $O_2$: According to Molecular Orbital Theory,the electronic configu

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$O_2$ and $KO_3$

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(C) To determine paramagnetism,we look for the presence of unpaired electrons.$1$. $O_2$: According to Molecular Orbital Theory,the electronic configuration is $\sigma 1s^2, \sigma^* 1s^2, \sigma 2s^2, \sigma^* 2s^2, \sigma 2p_z^2, \pi 2p_x^2 = \pi 2p_y^2, \pi^* 2p_x^1 = \pi^* 2p_y^1$. It has $2$ unpaired electrons,so it is paramagnetic.$2$. $Na_2O_2$: Contains the peroxide ion $O_2^{2-}$. The configuration is $\sigma^* 2p_x^2 = \sigma^* 2p_y^2$. All electrons are paired,so it is diamagnetic.$3$. $BaO_2$: Contains the peroxide ion $O_2^{2-}$,which is diamagnetic.$4$. $KO_3$: Contains the ozonide ion $O_3^-$. The $O_3^-$ ion has $19$ valence electrons. Molecular orbital calculations show it has an unpaired electron in the antibonding $\pi^*$ orbital,making it paramagnetic.Therefore,$O_2$ and $KO_3$ are both paramagnetic.

Which of the following pairs of species are paramagnetic?

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