Answer:
Hydrogen bonds.
Explanation:
The intermolecular forces are the forces that are presented between molecules in a substance. As higher is the force, as closer are the molecules, and more difficult will be to separate them.
Because of that, the solids have stronger forces than the liquids, which have stronger forces than the gases. Also, as strong the force, as higher will be the boiling point.
The ionic bond is the strongest and it's presented at ionic compounds, which are solids at room temperature and have high boiling points.
The covalent bonds are presented in the molecules and are formed when atoms share pairs of electrons. Between these molecules, the forces can be London forces, dipole-dipole forces, or hydrogen bonds.
The London forces are the weaker, they are presented at the nonpolar molecules, so it's easy to boil it. For a compound with low molar mass and London forces, it'll probably be at the gas phase at room temperature.
The dipole-dipole forces are presented at the polar molecules, and it's strong than the London forces. And the hydrogen bonds are a specific type of dipole-dipole forces, which is stronger and is formed between hydrogen and F, O, or N.
Because hydrogen has a low molar mass (1 g/mol), the compounds formed by it intends to have a low molar mass. So, to be liquid at room temperature, low mass, and high boiling point, it's more probable that the compound has hydrogen bonds.
