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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