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The stronger the IMFs, the higher the boiling point. For example, it takes more energy to break dipole-dipole IMFs than to break London dispersion IMFs because dipole dipole forces are stronger. Therefore, by looking at the IMFs, we can predict which substances have a higher boiling point.
It is also important to remember that boiling does not break bonds. So when explaining the effect that boiling point has, my TA suggested avoiding using the phrase "break bonds" and use "overcome intermolecular forces" instead.
When something has stronger intermolecular forces, the boiling point is generally higher. For example, if a molecule has H-bonds, it'll have a higher boiling point than a molecule with only London Dispersion Forces, as LDF are weaker than H-bonds.
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