* Hydrogen Bonding: Methylamine (CH3NH2) can form hydrogen bonds. The nitrogen atom in the amine group (NH2) has a lone pair of electrons that can form a hydrogen bond with a hydrogen atom on another molecule. This strong intermolecular interaction requires more energy to break, leading to a higher boiling point.
* Van Der Waals Forces: Ethane (CH3CH3) only exhibits weaker Van der Waals forces (London dispersion forces) due to its nonpolar nature. These forces are weaker than hydrogen bonds.
In summary: The ability of methylamine to form hydrogen bonds, a stronger intermolecular force compared to the Van der Waals forces in ethane, results in a higher boiling point for methylamine.
