The boiling point of a substance can be predicted based on its type and strength of intermolecular forces because these forces play a crucial role in determining the amount of energy required to change the substance from a liquid to a gaseous state. The stronger the intermolecular forces, the higher the boiling point, as more energy is needed to overcome these forces and allow the molecules to separate and enter the gas phase.There are three main types of intermolecular forces: London dispersion forces, dipole-dipole interactions, and hydrogen bonding. London dispersion forces are the weakest, followed by dipole-dipole interactions, and hydrogen bonding being the strongest.Let's consider two different substances: water H2O and carbon dioxide CO2 .Water H2O has a boiling point of 100C 212F . The intermolecular forces present in water are hydrogen bonds, which are a type of strong dipole-dipole interaction. Hydrogen bonding occurs when a hydrogen atom is bonded to a highly electronegative atom such as oxygen, nitrogen, or fluorine and is attracted to another electronegative atom. In the case of water, the oxygen atom is highly electronegative, and the hydrogen atoms form hydrogen bonds with other oxygen atoms in neighboring water molecules. These strong hydrogen bonds require a significant amount of energy to break, resulting in a relatively high boiling point for water.Carbon dioxide CO2 has a boiling point of -78.5C -109.3F at 1 atm pressure. The intermolecular forces present in CO2 are London dispersion forces, which are the weakest type of intermolecular forces. CO2 is a linear, nonpolar molecule, meaning that there are no significant positive or negative charges on the molecule. As a result, the only intermolecular forces present are the temporary, weak London dispersion forces that arise from the random movement of electrons. Since these forces are much weaker than hydrogen bonds, less energy is required to overcome them, resulting in a lower boiling point for CO2 compared to water.In summary, the boiling point of a substance can be predicted based on the type and strength of its intermolecular forces. Stronger intermolecular forces, such as hydrogen bonding, result in higher boiling points, while weaker forces, like London dispersion forces, result in lower boiling points. In the example provided, water has a higher boiling point than carbon dioxide due to the presence of strong hydrogen bonds in water, while CO2 only has weak London dispersion forces.