Maximum bond angle at nitrogen is present in | vedclass

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Question

(A) The bond angles are determined by the hybridization and the presence of lone pairs or unpaired electrons on the central nitrogen atom:$1.$ $NO_{2}

Vedclass · Accepted Answer

$NO_{2}^{+}$

Vedclass · Answer

(A) The bond angles are determined by the hybridization and the presence of lone pairs or unpaired electrons on the central nitrogen atom:$1.$ $NO_{2}^{+}$: Nitrogen is $sp$ hybridized,resulting in a linear geometry with a bond angle of $180^{\circ}$.$2.$ $NO_{3}^{-}$: Nitrogen is $sp^{2}$ hybridized,resulting in a trigonal planar geometry with a bond angle of $120^{\circ}$.$3.$ $NO_{2}$: Nitrogen is $sp^{2}$ hybridized with one unpaired electron,resulting in a bent shape with a bond angle of approximately $134^{\circ}$.$4.$ $NO_{2}^{-}$: Nitrogen is $sp^{2}$ hybridized with one lone pair,resulting in a bent shape with a bond angle of approximately $115^{\circ}$.Therefore,the maximum bond angle is in $NO_{2}^{+}$.

Maximum bond angle at nitrogen is present in which of the following?

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