Final answer:
Van der Waals forces are weak intermolecular forces that include dipole-dipole, dipole-induced dipole, and London dispersion forces, which can occur between polar and nonpolar molecules without relying on polarity.
Step-by-step explanation:
Van der Waals forces are a form of intermolecular attractive forces that contribute to the behaviour of liquids and solids. Interestingly, van der Waals forces do not rely on the polarity of molecules. These forces include dipole-dipole interactions between polar molecules and London dispersion forces which are relevant for nonpolar molecules. Furthermore, these interactions can occur between polar and covalently bound atoms in different molecules due to temporary partial charges that arise when electrons move around a nucleus, leading to slight attractions known as van der Waals interactions. The van der Waals forces are commonly grouped into three types—dipole-dipole, dipole-induced dipole, and the London dispersion forces. Dipole-dipole attractions result from the electrostatic attraction between the partial charges of different polar molecules. On the other hand, London dispersion forces are a result of temporary dipole moments occurring due to the uneven distribution of electrons within nonpolar molecules or atoms, making even nonpolar substances capable of van der Waals interactions. The Van der Waals Equation of State enhances the Ideal Gas Law by considering the volume occupied by gas molecules and the attractive forces between them. These attractive forces can have a significant impact on the properties of gases and liquids. Johannes van der Waals, a Dutch physicist, developed this theory which explains how real gases deviate from ideal behavior.