Here's why:

* Nonpolar: Methane is a nonpolar molecule due to its tetrahedral shape and the equal sharing of electrons between carbon and hydrogen.

* No Dipole-Dipole: Nonpolar molecules do not have permanent dipoles, so dipole-dipole interactions are not present.

* No Hydrogen Bonding: Hydrogen bonding requires a hydrogen atom directly bonded to a highly electronegative atom like oxygen, nitrogen, or fluorine. Methane doesn't have any of these.

London Dispersion Forces (LDFs): These are the weakest type of intermolecular force and arise from temporary fluctuations in electron distribution around the molecule. Even though methane is nonpolar on average, these temporary fluctuations create temporary dipoles that can induce dipoles in neighboring methane molecules, resulting in weak attractions.

Therefore, the only intermolecular force present in methane is London dispersion forces.