A) \[{{O}_{2}}\]
B) \[C{{N}^{-}}\]
C) \[CO\]
D) \[N{{O}^{+}}\]
Correct Answer: A
Solution :
Electronic configuration of \[{{O}_{2}}\] is \[{{O}_{2}}=\sigma {{(1s)}^{2}}{{\sigma }^{*}}{{(1s)}^{2}}\sigma {{(2s)}^{2}}{{\sigma }^{*}}{{(2s)}^{2}}\sigma {{(2{{p}_{x}})}^{2}}\pi {{(2{{p}_{y}})}^{2}}\] \[\pi {{(2{{p}_{z}})}^{2}}{{\pi }^{*}}{{(2{{p}_{y}})}^{1}}{{\pi }^{*}}{{(2{{p}_{z}})}^{1}}\] The molecule has two unpaired electrons So, it is paramagnetic
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