Rank these intermolecular forces in terms of their typical relative strengths: hydrogen bonding; dipole-dipole; induced dipole-induced dipole.

Intermolecular forces are forces of attraction between molecules, and they are weaker than the intramolecular forces that hold atoms together within a molecule. They can largely affect the physical properties of substances such as boiling point, melting point, and vapor pressure. There are three types to understand: 1. Hydrogen Bonding: This is a special type of dipole-dipole attraction between molecules where hydrogen is bound to a highly electronegative atom (such as nitrogen, oxygen or fluorine), and this hydrogen is attracted to another electronegative atom in another molecule. 2. Dipole-dipole forces: These occur when the positive end of a polar molecule is attracted to the negative end of another polar molecule. They are stronger than induced dipole-induced dipole forces but weaker than hydrogen bonding. 3. Induced dipole-induced dipole forces: These are also known as London dispersion forces and they are the weakest intermolecular forces. They occur in all molecules, polar and nonpolar, due to the shifting electron cloud which can create a temporary partial charge.

The types of intermolecular forces can be ranked according to their strength as follows: hydrogen bonding > dipole-dipole > induced dipole-induced dipole. Hydrogen bonding is generally the strongest of the three because it involves a hydrogen atom which is very strongly attracted to an electronegative atom, creating a strong polar bond. Dipole-dipole forces are the next strongest. These forces occur between polar molecules where there is an electronegativity difference greater than 0.5 but the molecules do not involve hydrogen. Induced dipole-induced dipole forces are the weakest intermolecular forces. These interactions become more significant as the size and shape of the molecules increase.