* Intermolecular Forces: The strength of intermolecular forces directly impacts boiling point. Stronger forces require more energy to overcome, resulting in a higher boiling point.
* Propanone (Acetone): Acetone primarily exhibits dipole-dipole interactions due to its polar carbonyl group (C=O). These interactions are weaker than hydrogen bonds.
* Ethoxyethane (Diethyl ether): Diethyl ether has only weak London dispersion forces, which are the weakest type of intermolecular force. This is because its molecule is nonpolar.
Therefore, even though propanone has a larger molecular weight than ethoxyethane, its stronger dipole-dipole forces are still weaker than the hydrogen bonding present in many molecules with similar molecular weights. This is why ethoxyethane has a higher boiling point than propanone.
