1. Separation of charge: Polar molecules have a separation of charge, meaning that they have a positive end and a negative end. This separation of charge creates a dipole moment, which is a measure of the strength of the molecular polarity.

2. Electronegativity difference: The polarity of a molecule is determined by the difference in electronegativity between the atoms that make up the molecule. Electronegativity is a measure of an atom's ability to attract electrons. When the electronegativity difference between two atoms is large, the molecule will be more polar.

3. Bond polarity: The bonds between atoms in a polar molecule are polar covalent bonds. Polar covalent bonds occur when the electrons in the bond are shared unequally between the atoms. This unequal sharing of electrons creates a partial positive charge on one atom and a partial negative charge on the other atom.

4. Molecular geometry: The molecular geometry of a polar molecule also affects its polarity. Molecules with a symmetrical molecular geometry, such as carbon dioxide (CO2), have no net polarity. However, molecules with an asymmetrical molecular geometry, such as water (H2O), have a net polarity.

5. Dipole moment: The dipole moment of a polar molecule is a measure of the strength of its polarity. The dipole moment is a vector quantity that points from the positive end of the molecule to the negative end. The magnitude of the dipole moment is equal to the product of the charge separation and the distance between the positive and negative ends of the molecule.