Genchem Bonding Periodic>Intermolecular Forces Practice Test

Dimethyl ether has stronger dipole–dipole interactions because its oxygen has two lone pairs, so it boils higher than methanol.

Methanol is less polar, so it relies less on dispersion forces and consequently boils at a higher temperature.

Both molecules experience only London dispersion forces, so methanol's higher boiling point arises from resonance stabilization.

Methanol can donate and accept hydrogen bonds via its O–H group, leading to stronger intermolecular attraction than in dimethyl ether.