A pair of isoelectronic species having bond o | vedclass

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(C) To determine the bond order,we calculate the number of electrons and use the molecular orbital theory formula: $B.O. = \frac{N_b - N_a}{2}$.For $O

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$O_2^{2-}, F_2$

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(C) To determine the bond order,we calculate the number of electrons and use the molecular orbital theory formula: $B.O. = \frac{N_b - N_a}{2}$.For $O_2^{2-}$,the total number of electrons is $8 + 8 + 2 = 18 \ e^{-}$. The bond order is $\frac{10 - 8}{2} = 1$.For $F_2$,the total number of electrons is $9 + 9 = 18 \ e^{-}$. The bond order is $\frac{10 - 8}{2} = 1$.Both species are isoelectronic $(18 \ e^{-})$ and have a bond order of $1$.

$A$ pair of isoelectronic species having bond order of $1$ is

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