Final answer:
London dispersion forces are the weakest intermolecular force, followed by dipole-dipole interactions, with hydrogen bonds being the strongest among the three types of intermolecular forces.
Step-by-step explanation:
Intermolecular forces are vital in dictating the physical properties of substances. When ordered from weakest to strongest, these forces are: London dispersion forces, dipole-dipole forces, and hydrogen bonds. London dispersion forces are present in all molecules due to instantaneous fluctuations in electron density, leading to temporary dipoles. They are the weakest and their strength increases with molecular size due to increased polarizability of electrons.
Dipole-dipole interactions occur when molecules with permanent dipoles interact, and their strength is proportional to the product of the charges and inversely proportional to the cube of the separation distance between the dipoles. Hydrogen bonding is a particularly strong type of dipole-dipole interaction that occurs between a hydrogen atom bonded to a highly electronegative atom like nitrogen, oxygen, or fluorine and a lone pair of electrons on another electronegative atom. This type of bonding is responsible for many unique properties of compounds such as water’s high boiling point.