Dipole-dipole forces and hydrogen bonds are intermolecular forces which are interactions that keep molecules together and are electrostatic forces.
Dipole-dipole forces are attraction’s forces between polar molecules because these molecules attract each other when the positive end of one is near the negative end of the other.
The hydrogen bonds are a type of dipole-dipole forces but in these interactions, we have a molecule that has in its structure hydrogen and another atom with high electronegativity, like oxygen, Fluor, nitrogen and sulfur. Due to the high electronegativity difference between these atoms these forces are stronger, so more energy is needed to put the molecules apart, hence the melting and boiling points of compounds that possess this interactios are higher.
I think the correct answer from the choices listed above is the first option. Compared to compounds that possess only dipole-dipole intermolecular forces, compounds that possess hydrogen bonding generally have <span>higher melting points. This is because hydrogen bonding is a stronger force than dipole-dipole.</span>
