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

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Hydrogen chloride has actually dipole-dipole forces so I would suppose it to have actually greater inter-molecular pressures and therefore a higher boiling point. However before, because this is not the situation, this must mean that chlorine has actually a greater intermolecular forces as a result of London dispersion pressures.

But why? I assumed London dispersion pressures were miniscule and only had a noteworthy impact in large molecules. Shouldn"t the dipole-dipole pressures be method stronger than the London dispersion forces?



This is because $ceCl2$ has actually close to double the mass and is also a bigger molecule compared to $ceHCl$. You were correct in saying that London dispersion forces are weaker yet bereason of $ceCl2$s dimension they get over the dipole-dipole pressures in $ceHCl$.


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