The O-N-O bond angle is maximum in: | vedclass

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(D) The bond angles for the given species are as follows:$NO_2^+$: The nitrogen atom is $sp$ hybridized,resulting in a linear geometry with a bond ang

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$NO_2^+$

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(D) The bond angles for the given species are as follows:$NO_2^+$: The nitrogen atom is $sp$ hybridized,resulting in a linear geometry with a bond angle of $180^\circ$.$NO_2$: The nitrogen atom is $sp^2$ hybridized with one unpaired electron,resulting in a bent geometry with a bond angle of approximately $134^\circ$.$NO_2^-$: The nitrogen atom is $sp^2$ hybridized with one lone pair,resulting in a bent geometry with a bond angle of approximately $115^\circ$.$NO_3^-$: The nitrogen atom is $sp^2$ hybridized,resulting in a trigonal planar geometry with a bond angle of $120^\circ$.Comparing these values,the $O-N-O$ bond angle is maximum in $NO_2^+$.Therefore,the correct option is $(D)$.

The $O-N-O$ bond angle is maximum in:

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