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

1 Answer
anor277
Jul 5, 2017

Well, hydrogen bonding clearly operates for HF..........

Explanation:

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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