According to Pearson Higher Education, polar molecules are generally considered permanent dipoles. A polar molecule is present is one end of the molecule has a more positive charge than the other.
Polar molecules sometimes, but not necessarily, have a net charge equivalent to zero. Examples of such molecules, according to Pearson, are carbon monoxide and water. A property of polar molecules that are permanent dipoles is the possession of a permanent dipole moment, but dipole moments are not guaranteed solely by uneven distribution of charge. It is possible to affect permanent dipoles through other permanent dipoles as well as through ionic charges and induced dipoles.