In which of the following molecules would you | vedclass

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(B) Bond length is inversely proportional to bond order. Higher bond order results in a shorter bond length.In $N_2H_4$ $(H_2N-NH_2)$,the $N-N$ bond i

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$N_2$

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(B) Bond length is inversely proportional to bond order. Higher bond order results in a shorter bond length.In $N_2H_4$ $(H_2N-NH_2)$,the $N-N$ bond is a single bond (bond order = $1$).In $N_2O_4$ $(O_2N-NO_2)$,the $N-N$ bond is a single bond (bond order = $1$).In $N_2O$ $(N \equiv N^+-O^-)$,the $N-N$ bond is a triple bond (bond order = $3$).In $N_2$ $(N \equiv N)$,the $N-N$ bond is a triple bond (bond order = $3$).Comparing $N_2$ and $N_2O$,the $N-N$ bond in $N_2$ is a pure triple bond,whereas in $N_2O$,the resonance structures result in a bond order slightly less than $3$. Therefore,$N_2$ has the shortest $N-N$ bond length.

In which of the following molecules would you expect the nitrogen-to-nitrogen bond length to be the shortest?

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