The correct order of increasing bond angles i | vedclass

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(D) As the number of lone pairs of electrons increases,the bond angle decreases.$NO_2^+$ is isoelectronic with $CO_2$. It is a linear ion with $sp$-hy

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$NO_2^- < NO_2 < NO_2^+$

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(D) As the number of lone pairs of electrons increases,the bond angle decreases.$NO_2^+$ is isoelectronic with $CO_2$. It is a linear ion with $sp$-hybridization at the central $N$ atom,resulting in a bond angle of $180^{\circ}$.In $NO_2^-$,the $N$ atom undergoes $sp^2$-hybridization. Due to the presence of one lone pair,the bond angle is reduced from the ideal $120^{\circ}$ to approximately $115^{\circ}$.In $NO_2$,the $N$ atom has one unpaired electron in an $sp^2$-hybrid orbital. The bond angle is approximately $134^{\circ}$ (often cited as $132^{\circ}-134^{\circ}$),which is greater than $120^{\circ}$ due to the repulsion of the unpaired electron.Therefore,the increasing order of bond angles is $NO_2^- < NO_2 < NO_2^+$ $(115^{\circ} < 134^{\circ} < 180^{\circ})$.

The correct order of increasing bond angles in the following triatomic species is

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