Discussion
The correct order of ONO bond angle in the given species is
Answer: B
The correct order is \(\mathrm{NO_2^- \lt NO_3^- \lt NO_2 \lt NO_2^+}\).
The angles follow from the electron domains around nitrogen:
- \(\mathrm{NO_{2}^{+}}\): two bonding domains and no lone pair on N, so it is linear, 180°.
- \(\mathrm{NO_{2}}\): one unpaired electron on N. A single electron repels the bonds less than a lone pair, so the angle opens to about 134°.
- \(\mathrm{NO_{3}^{-}}\): three equivalent bonding domains, trigonal planar, 120°.
- \(\mathrm{NO_{2}^{-}}\): a full lone pair on N compresses the angle below 120°, to about 115°.
The first option is this order reversed. The third puts nitrate below nitrite, though nitrite's lone pair makes it the smaller. The last puts \(\mathrm{NO_{2}^{+}}\) below \(\mathrm{NO_{2}}\), but a linear ion has the largest possible angle.
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