What are the predominant intermolecular forces in: Kr, CBr4, NaF, CH3OH, and ruby? Then rank by increasing boiling point.

Kr- dispersion forces

CBr4- dispersion forces

CH3OH - dispersion forces, dipole interaction, hydrogen bonding

NaF- ionic

Kr-<CBr4<CH3OH<NaF

Explanation:

The magnitude of intermolecular forces influences the boiling points of substances. The stronger the intermolecular forces the higher the boiling point.

The strongest intermolecular forces here is the Ionic bond hence it accounts for the highest boiling point followed by CH3OH having hydrogen bonding.

Though Krypton and CBr4 both have dipole interaction, the higher relative molecular mass of CBr4 makes it to have a higher boiling point than Kr

i just learnt this recently but i need to look through my notes again

i think it is true since you can test the answer and can use observations to complete it.