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

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(B) To determine the $O-N-O$ bond angle,we look at the hybridization and geometry of the molecules:$1$. $NO_2^+$: The nitrogen atom is $sp$-hybridized

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$NO_2^+$

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(B) To determine the $O-N-O$ bond angle,we look at the hybridization and geometry of the molecules:$1$. $NO_2^+$: The nitrogen atom is $sp$-hybridized with a linear geometry. The bond angle is $180^{\circ}$.$2$. $NO_2$: The nitrogen atom is $sp^2$-hybridized with one unpaired electron. The bond angle is approximately $134^{\circ}$.$3$. $NO_2^-$: The nitrogen atom is $sp^2$-hybridized with one lone pair. The bond angle is approximately $115^{\circ}$.$4$. $NO_3^-$: The nitrogen atom is $sp^2$-hybridized with no lone pairs,resulting in a trigonal planar geometry. The bond angle is $120^{\circ}$.Comparing these values,the $O-N-O$ bond angle is highest in $NO_2^+$.

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

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