What is the predominant intermolecular force in the liquid state of each of these compounds: hydrogen fluoride (HF), carbon tetrabromide (CBr4), and nitrogen trifluoride (NF3)? Force(s): Dipole-dipole Hydrogen Bonding Dispersion

Hydrogen bonding occurs when hydrogen is covalently bonded to a highly electronegative atom such as fluorine, chlorine nitrogen, oxygen etc. Hence the dominant intermolecular force in HF is hydrogen bonding.

CBr4 is nonpolar because the molecule is tetrahedral and the individual C-Br dipole moments cancel out leaving the molecule with a zero dipole moment hence the dominant intermolecular force are the dispersion forces.

NF3 has a resultant dipole moment hence the molecules are held together by dipole-dipole interaction.

adioabiola adioabiola · Answer 2 · 2021-12-02T16:27:06+01:00

The predominant intermolecular force in the liquid state of the compounds are as follows:

HF - hydrogen bonding

HF - hydrogen bondingCBr4 - Dispersion

HF - hydrogen bondingCBr4 - DispersionNF3 - Dipole-dipole

Discussion:

Hydrogen bonding is a bonding characterized covalent bonding of hydrogen to a highly electronegative atom such as fluorine, chlorine nitrogen, oxygen etc.

In essence, the dominant intermolecular force in HF is hydrogen bonding.

Carbon tetrabromide, CBr4 is nonpolar because the molecule is tetrahedral and the individual C-Br dipole moments neutralise leaving the molecule with a zero dipole moment hence the dominant intermolecular force are the dispersion forces.

Nitrogen trifluoride, NF3 has its molecules held together by dipole-dipole interaction as a result of its resultant dipole moment.