The term Van der Waals refers to a set of intermolecular forces that arise from the interactions between molecules. These forces include dipole-dipole interactions, London dispersion forces, and dipole-induced dipole forces. Van der Waals forces are generally weaker than covalent and ionic bonds, yet they play a crucial role in determining the physical properties of substances, such as boiling and melting points. For example, they are responsible for the condensation of gases into liquids and the formation of molecular solids. The strength of these forces can be described quantitatively using the Van der Waals equation, which modifies the ideal gas law to account for molecular size and intermolecular attraction:
In this equation, represents pressure, is volume, is the number of moles, is the ideal gas constant, is temperature, and and are specific constants for a given gas that account for the attractive forces and volume occupied by the gas molecules, respectively.
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