What is the predominant intermolecular force in the liquid state of each of these compounds: hydrogen fluoride (HF), carbon tetrachloride (CCl4), and dichloromethane (CH2Cl2)? Either Dipole-dipole forces, Hydrogen bonding or Dispersion forces

Md Ariful Islam

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Md Ariful Islam

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Whereas dipole-dipole interaction operates for $"methylene chloride"$, and dispersion forces are the primary intermolecular force in $"carbon tetrachloride"$. And note that dispersion forces operate between all molecules, but in $HF$ it is not the primary intermolecular force.

And how do we get a handle on intermolecular force? Well, the best metric are the normal boiling points........

$HF,$ $"normal boiling point"=19.5$ $""^@C$;

$CH_2Cl_2,$ $"normal boiling point"=39.6$ $""^@C$;

$"CCl"_4,$ $"normal boiling point"=76.2$ $""^@C$.

The heavy, many electron, carbon tet molecule is the most involatile material, even tho' hydrogen bonding clearly operates for $HF$.

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