How can a molecule be characterized if it has a permanent dipole?

A molecule with a permanent dipole is characterized as polar. This polarization occurs when there is an uneven distribution of electrons between atoms in the molecule, typically due to differences in electronegativity. When one atom has a stronger attraction for the shared electrons, it becomes more negatively charged while the other atom becomes more positively charged, resulting in a dipole moment. This permanent dipole indicates that the molecule has distinct positive and negative ends, which is a hallmark of polar molecules.

Polar molecules often exhibit unique properties, such as higher boiling and melting points compared to non-polar molecules of similar size, because of the dipole-dipole interactions that arise. In contrast, ionic compounds involve the complete transfer of electrons and the formation of positive and negative ions, but this doesn’t characterize molecular polarity. Non-polar molecules, on the other hand, do not have a permanent dipole due to an even distribution of charge. Radicals refer to molecules with unpaired electrons and are not directly related to the concept of polarity.

Thus, the correct characterization for a molecule exhibiting a permanent dipole is that it is polar.