General

CH4 intermolecular forces aren't nearly as strong as they are for the other 3 substances.
The other 3 substances are all held together with hydrogen bonds, which are extremely strong.

CH4 methane = non polar; non polar molecules are held together by the "weak force" aka london dispersion force.
H2O = polar => H-O bonds are held together by hydrogen bonds, very very strong intermolecular forces (but not as strong as ionic bonds).
HF = polar => H-F bonds also held together by hydrogen bonds.
NH3 = polar => H-N forces are also held together by hydrogen bonds.

Basically, hydrogen bonds are formed between elements with small radius and high electronegativity (F, N, O); or with an high electronegative difference of approx. 1.5 or greater.

The stronger the [b]intermolecular bonds[/b] (bonds that holds one molecule with another molecule), the higher the boiling point, because it requires more energy to break the bonds. In phase changes such as boiling/freezing we are talking about breaking the intermolecular bonds, and the main force that holds CH4 molecules together is the weak force. You do not want to get confused with the strong "dipole-dipole" C-H [b]intramolecular bonds[/b] (bonds that holds the atom to form a molecule) because we are not breaking those bonds in phase changes.

hydrogen bonding for H2O, all i remember from chem

rest are polar? lol van der waalz. stronger the bonds, the higher the BP