Chemistry
Chemistry
Problem
In the optimal Lewis electron-dot structure of nitric oxide (), placement of the single unpaired electron is most consistent with which of the following? a) On the oxygen atom, primarily because the more electronegative oxygen stabilises the radical electron best. b) On the nitrogen atom, primarily because nitrogen is less electronegative than oxygen. c) Delocalised between nitrogen and oxygen owing to resonance that shares the unpaired electron equally over both atoms. d) On the nitrogen atom, because the more electronegative atom should hold additional electron density.Intuitive explanation
Nitric oxide is a rare case where the "optimal" Lewis structure actually leaves an unpaired electron—it's a radical. The key insight is that you need to count valence electrons carefully (5 from N + 6 from O = 11 total, an odd number), then build the most stable structure by maximizing bonds and minimizing formal charges. Once you've drawn the best N–O arrangement, you'll see where that single unpaired electron must live to keep formal charges as close to zero as possible.
Intuitive explanation
Nitric oxide is a rare case where the "optimal" Lewis structure actually leaves an unpaired electron—it's a radical. The key insight is that you need to count valence electrons carefully (5 from N + 6 from O = 11 total, an odd number), then build the most stable structure by maximizing bonds and minimizing formal charges. Once you've drawn the best N–O arrangement, you'll see where that single unpaired electron must live to keep formal charges as close to zero as possible.