* Hydrogen Bonding: This is the strongest intermolecular force present in methanol. The hydrogen atom bonded to the highly electronegative oxygen atom (O-H) creates a dipole moment, allowing for strong hydrogen bonding between the oxygen atom of one methanol molecule and the hydrogen atom of another.

* Dipole-Dipole Interactions: The polar O-H bond in methanol results in a permanent dipole moment across the molecule. These dipoles interact with each other, creating dipole-dipole forces.

* London Dispersion Forces: These are the weakest intermolecular forces present in all molecules, including methanol. They arise from temporary fluctuations in electron distribution, creating temporary dipoles that induce dipoles in neighboring molecules.

Overall: Hydrogen bonding is the dominant intermolecular force in methanol, giving it a relatively high boiling point compared to other molecules with similar molecular weight.