Intermolecular attractive forces, collectively referred to as van der Waals forces, are responsible for the behavior of liquids and solids and are electrostatic in nature. Dipole-dipole attractions result from the electrostatic attraction of the partial negative end of one polar molecule for the partial positive end of another.

The temporary dipole that results from the motion of the electrons in an atom can induce a dipole in an adjacent atom and give rise to the London dispersion force. Hydrogen bonds are a special type of dipole-dipole attraction that results when hydrogen is bonded to one of the three most electronegative elements: F, O, or N

dispersion force — (also, London dispersion force) attraction between two rapidly fluctuating, temporary dipoles; significant only when particles are very close together. van der Waals force — attractive or repulsive force between molecules, including dipole-dipole, dipole-induced dipole, and London dispersion forces; does not include forces due to covalent or ionic…. intermolecular force — noncovalent attractive force between atoms, molecules, and/or ions. dipole-dipole attraction — intermolecular attraction between two permanent dipoles.