The strength of intermolecular forces has a direct relationship with the boiling point of a substance. A substance with stronger intermolecular forces requires more energy to overcome these forces and transition from the liquid phase to the gas phase, resulting in a higher boiling point. Conversely, a substance with weaker intermolecular forces requires less energy to overcome these forces, resulting in a lower boiling point.Two examples of substances with different types of intermolecular forces are water H2O and methane CH4 .Water has hydrogen bonding, which is a type of dipole-dipole interaction that occurs between molecules containing a hydrogen atom bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine . In the case of water, hydrogen bonding occurs between the hydrogen atoms of one water molecule and the oxygen atoms of another water molecule. Hydrogen bonding is a relatively strong intermolecular force, which results in water having a high boiling point of 100C 212F .Methane, on the other hand, has London dispersion forces also known as van der Waals forces , which are the weakest type of intermolecular forces. These forces arise from temporary fluctuations in electron distribution around the molecules, creating temporary dipoles that attract other molecules. Since London dispersion forces are weaker than hydrogen bonding, methane has a much lower boiling point of -161.5C -258.7F .In summary, the strength of intermolecular forces directly affects the boiling point of a substance. Water, with its strong hydrogen bonding, has a higher boiling point than methane, which has weaker London dispersion forces.