the atoms a full outer shell of electrons (or other stable formation).
Polar bonds are covalent bonds with a large electronegativity difference but not large enough for the formation of an ionic bond. Since the electronegativity difference is unequal, the electrons spend more time around the more electronegative atom. As a result, the molecule has a slight polarity. This polarity causes polar bonds to resemble weak ionic bonds.
Dipole interactions occur between molecules with polar bonds. Since molecules with polar bonds are slightly charged, having both a positive and a negative end, the positive end of one molecule is attracted to the negative end of a nearby molecule.A special case of the dipole interaction is
hydrogen bonding. Since a hydrogen atom is
essentially a positively charged proton, it is
attracted to the negative electrons of the
highly electronegative atoms O, N, F or Cl.
(i.e., electrons of atoms the hydrogen
is not bonded to).
Van der Waals forces occur between the molecules made up of atoms with no major electronegativity imbalances called non-polar molecules. Slight imbalances in the charge distribution in the electron cloud of one non-polar molecule can induce distortions in the electron clouds of other nearby non-polar molecules.
