The strength and type of intermolecular forces present in a substance have a significant impact on its boiling point. Intermolecular forces are the forces that exist between molecules, and they play a crucial role in determining the physical properties of substances, such as boiling point, melting point, and viscosity.There are three main types of intermolecular forces:1. London dispersion forces also known as van der Waals forces : These are the weakest intermolecular forces and occur between all molecules, including nonpolar molecules. They result from temporary fluctuations in electron distribution, which create temporary dipoles that attract other molecules.2. Dipole-dipole forces: These forces occur between polar molecules, where there is a permanent separation of charge partial positive and partial negative charges within the molecule. The positive end of one molecule is attracted to the negative end of another molecule.3. Hydrogen bonding: This is a special type of dipole-dipole interaction that occurs when hydrogen is bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine . Hydrogen bonding is stronger than regular dipole-dipole forces due to the significant difference in electronegativity between hydrogen and the electronegative atom.The boiling point of a substance is the temperature at which it changes from a liquid to a gas. The stronger the intermolecular forces in a substance, the more energy is required to overcome these forces and change the substance from a liquid to a gas. Consequently, substances with stronger intermolecular forces will have higher boiling points.In general, the strength of intermolecular forces follows the order: London dispersion forces < dipole-dipole forces < hydrogen bonding. Therefore, substances with predominantly London dispersion forces will have lower boiling points compared to those with dipole-dipole forces or hydrogen bonding.For example, consider the boiling points of methane CH4 , ammonia NH3 , and water H2O . Methane, a nonpolar molecule, has weak London dispersion forces and a boiling point of -161.5C. Ammonia, a polar molecule with dipole-dipole forces, has a boiling point of -33.3C. Water, which forms hydrogen bonds, has a boiling point of 100C. This demonstrates the influence of the strength and type of intermolecular forces on the boiling points of substances.