Question

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

Answer 1

The predominant intermolecular force in the liquid state of HF is hydrogen bonding, in CBr4 is dispersion forces, and in HCl is dipole-dipole forces.

Step-by-step explanation:

The predominant intermolecular force in the liquid state of hydrogen fluoride (HF) is hydrogen bonding. Hydrogen bonding occurs when a hydrogen atom is bonded to one of the more electronegative atoms, such as fluorine. The strong dipole-dipole interaction in hydrogen fluoride leads to the formation of hydrogen bonds between molecules.

The predominant intermolecular force in the liquid state of carbon tetrabromide (CBr4) is dispersion forces. Dispersion forces occur as a result of temporary dipoles that form due to asymmetric distribution of electrons. Since carbon tetrabromide is a nonpolar molecule, dispersion forces are the main intermolecular force.

The predominant intermolecular force in the liquid state of hydrogen chloride (HCl) is dipole-dipole forces. Dipole-dipole interactions occur between polar molecules due to the electrostatic attraction between the positive end of one molecule and the negative end of another molecule.

Answer 2

Dipole dipole forces - HCL.

Hydrogen bonding - HF.

Dispersion forces - CBr4.

Step-by-step 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.