In which of the following is the O-N-O bond a | vedclass

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(D) To determine the $O-N-O$ bond angle,we look at the hybridization and geometry of the central nitrogen atom in each species:$1$. $NO^{-}_3$: Nitrog

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$NO^{+}_2$

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(D) To determine the $O-N-O$ bond angle,we look at the hybridization and geometry of the central nitrogen atom in each species:$1$. $NO^{-}_3$: Nitrogen is $sp^2$ hybridized with a trigonal planar geometry. The bond angle is approximately $120^{\circ}$.$2$. $NO^{-}_2$: Nitrogen is $sp^2$ hybridized with one lone pair. Due to lone pair-bond pair repulsion,the bond angle is slightly less than $120^{\circ}$ (approx. $115^{\circ}$).$3$. $NO_2$: Nitrogen is $sp^2$ hybridized with one unpaired electron. The bond angle is approximately $134^{\circ}$.$4$. $NO^{+}_2$: Nitrogen is $sp$ hybridized with a linear geometry. The bond angle is $180^{\circ}$.Comparing these,$NO^{+}_2$ has the maximum bond angle of $180^{\circ}$.

In which of the following is the $O-N-O$ bond angle maximum?

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