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.

"the periodic table is arranged in order of atomic number."

periodic trends is an atom that gets larger as the number of electronic shells increase, the radius of atoms increases as you go down a certain group in the periodic table of elements. in general, the size of an atom will decrease as you move from left to right of a certain period.