The relationship between the intermolecular forces present in different substances and their boiling points is that stronger intermolecular forces generally result in higher boiling points. This is because more energy is required to overcome the stronger forces holding the molecules together in the liquid phase, allowing them to transition to the gaseous phase.There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding. The strength of these forces increases in the order of London dispersion < dipole-dipole < hydrogen bonding.Examples of substances with different intermolecular forces and their boiling points:1. Methane CH4 - London dispersion forces: Methane is a nonpolar molecule, so it only experiences weak London dispersion forces. Its boiling point is very low at -161.5C.2. Hydrogen chloride HCl - Dipole-dipole interactions: HCl is a polar molecule, so it experiences stronger dipole-dipole interactions in addition to London dispersion forces. Its boiling point is higher than methane's at -85C.3. Water H2O - Hydrogen bonding: Water is a polar molecule and has hydrogen atoms bonded to highly electronegative oxygen atoms, allowing for strong hydrogen bonding in addition to dipole-dipole interactions and London dispersion forces. Its boiling point is significantly higher than both methane and hydrogen chloride at 100C.In summary, the strength of the intermolecular forces present in a substance directly affects its boiling point. Substances with stronger intermolecular forces require more energy to transition from the liquid to the gaseous phase, resulting in higher boiling points.