The correct pair of species with (A) the high | vedclass

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(B) To determine the bond order and magnetic character,we use Molecular Orbital Theory $(MOT)$. The total number of electrons for each species is:$O_2

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$O_2^{+}, O_2^{2-}$

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(B) To determine the bond order and magnetic character,we use Molecular Orbital Theory $(MOT)$. The total number of electrons for each species is:$O_2$ $(16 \ e^-)$: Bond order = $\frac{10-6}{2} = 2$,Paramagnetic.$O_2^{+}$ $(15 \ e^-)$: Bond order = $\frac{10-5}{2} = 2.5$,Paramagnetic.$O_2^{-}$ $(17 \ e^-)$: Bond order = $\frac{10-7}{2} = 1.5$,Paramagnetic.$O_2^{2-}$ $(18 \ e^-)$: Bond order = $\frac{10-8}{2} = 1$,Diamagnetic.$(A)$ The species with the highest bond order is $O_2^{+}$ (Bond order = $2.5$).$(B)$ The species with diamagnetic character is $O_2^{2-}$ (all electrons are paired).Therefore,the pair is $(O_2^{+}, O_2^{2-})$.

The correct pair of species with $(A)$ the highest bond order and $(B)$ diamagnetic character is

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