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

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(B) To determine the bond angle,we analyze the hybridization and geometry of the species:$1$. $NO_2^+$: The nitrogen atom is $sp$-hybridized with a li

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$NO_2^+$

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(B) To determine the bond angle,we analyze the hybridization and geometry of the species:$1$. $NO_2^+$: The nitrogen atom is $sp$-hybridized with a linear geometry,resulting in a bond angle of $180^{\circ}$.$2$. $NO_3^-$: The nitrogen atom is $sp^2$-hybridized with a trigonal planar geometry,resulting in a bond angle of $120^{\circ}$.$3$. $NO_2^-$: The nitrogen atom is $sp^2$-hybridized with one lone pair,resulting in a bent geometry with a bond angle of approximately $115^{\circ}$.$4$. $N_2O$: The structure is $N \equiv N^+-O^-$,where the central nitrogen is $sp$-hybridized,but the $O-N-O$ angle is not applicable as it is a linear $N-N-O$ molecule.Comparing these,the $O-N-O$ bond angle is maximum in $NO_2^+$ $(180^{\circ})$.

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

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