dipolar attraction

In chemistry, a dipole refers to the unequal distribution of electrical charge across atoms within a bond, creating partial positive and negative charges. This occurs when atoms with different electronegativities bond, as the more electronegative atom attracts electrons more strongly. For example, in hydrogen chloride (HCl), chlorine is more electronegative than hydrogen, resulting in a partial negative charge on chlorine and a partial positive charge on hydrogen.1

This polarity leads to dipolar attraction, where the positive end of one molecule is attracted to the negative end of another. This intermolecular force is responsible for phenomena like the condensation of gases into liquids. A related interaction is the dipole-induced-dipole interaction, where a polar molecule can distort the electron distribution of a nonpolar molecule, inducing a temporary dipole and causing attraction between them. This polarity significantly impacts physical properties like boiling points and solubility.23