The strongest intermolecular interactions between methane (CH4) molecules arise from b) London dispersion forces.
Methane is a nonpolar molecule due to its symmetric tetrahedral shape, which means there is an equal distribution of electron density. As a result, it does not possess a permanent dipole and cannot engage in dipole-dipole interactions or hydrogen bonding. In nonpolar molecules like methane, the only significant type of intermolecular force present is the London dispersion forces. These forces arise from temporary fluctuations in electron distribution within the molecules, creating momentary dipoles that induce similar dipoles in neighboring molecules. While these forces are generally weak compared to other types of intermolecular interactions, they are the primary forces operating in pure methane.