Is N{O^ - } paramagnetic or diamagnetic?

To determine if a molecule or ion is paramagnetic or diamagnetic, we need to consider its electron configuration and whether it has unpaired electrons.

The notation N{O^-} indicates that it is the nitric oxide molecule with a negative charge, which means it has gained an extra electron.

Nitric oxide (NO) normally has 15 electrons. If we add one more electron due to the negative charge, we have 16 electrons to distribute. The electron configuration of nitrogen (N) is 1s² 2s² 2p³. Oxygen (O) has 1s² 2s² 2p⁴. When these atoms combine to form NO, they share an electron to form a sigma bond, and one electron from nitrogen and one from oxygen form a pi bond.

The nitrogen atom in NO has one unpaired electron, making it paramagnetic. So, N{O^-} is paramagnetic.