Chlorine has a boiling point of $238~mathrmK$ while hydrogen chloride has a boiling point of $188~mathrmK$.

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Hydrogen chloride has dipole-dipole forces so I would expect it to have greater inter-molecular forces and thus a higher boiling point. However, since this is not the case, this must mean that chlorine has a greater intermolecular forces due to London dispersion forces.

But why? I thought London dispersion forces were miniscule and only had a notable effect in large molecules. Shouldn"t the dipole-dipole forces be way stronger than the London dispersion forces?



This is because $ceCl2$ has close to double the mass and is also a larger molecule compared to $ceHCl$. You were correct in saying that London dispersion forces are weaker but because of $ceCl2$s size they overcome the dipole-dipole forces in $ceHCl$.


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