Bond Polarity & Intermolecular Forces

When two atoms in a covalent bond have different electronegativities, the shared electrons are pulled toward the more electronegative atom, producing an unequal distribution of charge. This is a polar covalent bond, in which the more electronegative atom carries a partial negative charge, $\delta-$, and the other a partial positive charge, $\delta+$. The separation of charge across the bond creates a bond dipole. When the two atoms are identical, as in $\text{H}_2$ or $\text{Cl}_2$, the bond is pure or nonpolar covalent. As the electronegativity difference grows, the bond becomes increasingly polar, and beyond a difference of roughly 1.8 the bonding is better described as ionic. Bonding therefore forms a continuum from nonpolar covalent through polar covalent to ionic.

Whether a whole mole