Question

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

• A. $N{O}_2^{+}$
• B. $N{O}_2$
• C. $N{O}_3$
• D. $N_2{O}_3$

Answer 1

The correct option is B $N{O}_2$

1. $\to$ ${NO}_2^{+}$ has $2N=0$ double bonds, and no unpaired electrons; So repulsion between the 2 regions of electron density is minimized by 180degree bond angles.

2. Geometry is linear.

3. $\to$ Neutral ${NO}_2$ has one more electron; which is accommodated by the nitrogen atom. This introduce extra repulsion; but the single electron repulsive power is not as much electron rich as N-O multiple bonds. Thus bond angle is 134degree.

4. $\to$${NO}_3$ (Nitrogen trioxide) has a trigonal planar geometry. They have bond angles of 120degree.

5. $\to$$N_2{O}_3$ (Dinitrogen trioxide) has a O-N-O Bond of 130degree.

6. Hence the maximum bond angle is observed in case of ${NO}_2^{+}$ ion.