Intermolecular Forces Rank from Strongest to Weakest?

Hydrogen bonding, Dipole-dipole forces, London forces

Could you explain how to do this problem step by step please? This entire question is stumping me.

Intermolecular forces are the forces that exist BETWEEN all molecules and atoms. They originate from the interactions between charges and partial charges. Dispersion forces are present in all molecules and atoms and result from the fluctuation in electron distribution within molecules. Since all molecules have electrons, they all exhibit dispersion forces. These are also known as LONDON forces. Dispersion forces increase with molar mass because molecules with a higher molar mass generally have more electrons dispersed over a greater volume.

Dipole-Dipole forces exist in the attraction between 2 polar molecules. Without polar molecules, the nonpolar dipoles will cancel out and no dipole-dipole forces will exist. (Ex: SO2, HI)

Hydrogen bonding is the strongest of the IM forces. These occur when H has the ability to bond to N, F, or O. However, nonpolar molecules cannot form H bonding. (Ex of H-bonding: HF, H2O)

Boiling point is based on the strength of IM forces and molecular mass. The greater the IM forces the greater the boiling point. H2O has a high boiling point (100* C) due to its ability to form TWO hydrogen bonds.

what are three intermolecular forces that are from strongest to weakest?