A) \[O_{2}^{2-}\]
B) \[{{B}_{2}}\]
C) \[N_{2}^{+}\]
D) \[O_{2}^{{}}\]
Correct Answer: A
Solution :
Molecular orbital electronic configuration of \[O_{2}^{2-}\]is \[\sigma 1{{s}^{2}}{{\sigma }^{*}}1{{s}^{2}}{{\sigma }^{*}}2{{s}^{2}}{{\sigma }^{*}}2{{s}^{2}}\sigma 2{{p}^{2}}_{z}\equiv \pi 2{{p}^{2}}_{y}{{\pi }^{*}}2{{p}^{2}}_{x}\equiv {{\pi }^{*}}2{{p}^{2}}_{y}\] \[\operatorname{Unpaired} electrons = 0\,\,i.e.,diamagnetic.\]
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