What is the predominant intermolecular force in the liquid state of each of these compounds: hydrogen fluoride (hf), carbon tetrabromide (cbr4), and hydrogen chloride (hcl)?
a) dipole-dipole forces
b) hydrogen bonding
c) dispersion forces

Dipole dipole forces - HCL.

Hydrogen bonding - HF.

Dispersion forces - CBr4.

Explanation:

Dispersion forces work between all the molecules, but this is not the primary intramolecular force in hydrogen fluoride. The best to get intramolecular forces in the liquid state of the compounds are the normal boiling points:

HF boiling point is - 19.5 degree celsius.

HCl boiling point is - 39.6 degree celsius.

HCBr4 boiling point is - 76.2 degree celsius.

it is stable as it is in group 0 which have full outer shells of electrons

the answer your looking for is c).