Does NO2− have a dipole?

NO2−, which is the nitrite ion, does have a dipole moment. A dipole moment arises when there is an asymmetry in the distribution of electrons within a molecule, leading to a separation of positive and negative charges. In the case of NO2−, the nitrogen atom (N) is more electronegative than the oxygen atoms (O), which means it attracts electrons more strongly. As a result, there is a partial negative charge on the oxygen atoms and a partial positive charge on the nitrogen atom.

The molecular geometry of NO2− is bent or V-shaped, with a bond angle of approximately 115 degrees. This bent geometry is due to the presence of two lone pairs of electrons on the nitrogen atom, which repel the bonded pairs of electrons, causing the O-N-O bond angle to be less than 180 degrees.

Because of this bent geometry and the unequal sharing of electrons between nitrogen and oxygen atoms, NO2− has a net dipole moment. The dipole moment points from the more positively charged nitrogen atom towards the more negatively charged oxygen atoms, indicating the direction of the overall polarity in the molecule.