# 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

Jul 5, 2017

Well, hydrogen bonding clearly operates for $H F$..........

#### Explanation:

Whereas dipole-dipole interaction operates for $\text{methylene chloride}$, and dispersion forces are the primary intermolecular force in $\text{carbon tetrachloride}$. And note that dispersion forces operate between all molecules, but in $H F$ 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........

$H F ,$ $\text{normal boiling point} = 19.5$ ""^@C;

$C {H}_{2} C {l}_{2} ,$ $\text{normal boiling point} = 39.6$ ""^@C;

${\text{CCl}}_{4} ,$ $\text{normal boiling point} = 76.2$ ""^@C.

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