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Strength and type of intermolecular forces (ion-ion, ion-dipole, dipole-dipole, dipole-induced dipole, induced dipole-induced dipole), as well as the shape of the molecule (rod-shaped [allows for dipoles to be closer together] vs. spherical) affects the boiling point. The stronger the intermolecular force means the more energy (heat) will be required to overcome the intermolecular forces, resulting in higher boiling points.
Ionic bonds typically have the highest boiling points due to their charges. Then, as mentioned, hydrogen bonds create very high boiling points. This is because it requires the greatest amount of energy to break the intermolecular bonds. Dipole-dipole bonds have a lower boiling point compared to hydrogen bonds and ionic bonds, but their higher boiling point is due to electronegativity difference between atoms. Finally is dispersion forces which have lowest boiling point of the four because these are instantaneous dipoles.
For this, you would probably have to see which has a stronger type of intermolecular bonds, the stronger the bond between molecules, the more energy would be required to sever them, which would lead that molecule/compound to have a higher boiling point.
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