However, if the orientation of the bond dipoles is such that they do not cancel out, the molecules
will have a net dipole moment and therefore be polar. For instance, H 2 O has two polar O–H bonds.
According to the VSEPR model, its shape is angular. The two dipoles add together to give a net
dipole moment to the molecule, making the H 2 O molecule polar.
A molecule of two atoms bound by a polar bond must have a net dipole moment and therefore be
polar. The two equal and opposite partial charges are localized at the ends of the molecule on the
two atoms.