Which of the following orders is correct?

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(A) $(1)$ Bond length order: single bond $>$ double bond $>$ triple bond. In $N_2O$,the $N-O$ bond has significant single bond character,whereas in $N

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$NO > N_2O$ : Bond length of $N-O$ bond

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(A) $(1)$ Bond length order: single bond $>$ double bond $>$ triple bond. In $N_2O$,the $N-O$ bond has significant single bond character,whereas in $NO$,it has double bond character. Thus,the bond length in $N_2O > NO$.$(2)$ Acidic character of nitrogen oxides increases with the oxidation state of nitrogen. $N_2O_5$ $(+5)$ is more acidic than $N_2O_3$ $(+3)$.$(3)$ The $O-N-O$ bond angle in $N_2O_4$ is approximately $134^{\circ}$ (planar structure),while in $N_2O_3$ it is approximately $105^{\circ}-117^{\circ}$ depending on the isomer. Comparing the structures,$N_2O_4$ has a larger $O-N-O$ bond angle than $N_2O_3$.

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