Which of these molecules would you expect to have the lowest boiling point? Select the single best answer. CClClClHtrichloromethane CHNHHHHmethylamine CHHIHiodomethane

To determine which molecule has the lowest boiling point, we need to consider the types of intermolecular forces present in each molecule.

1. CCl3H (trichloromethane): This molecule has dipole-dipole interactions due to the difference in electronegativity between carbon and chlorine atoms. It also has London dispersion forces.

2. CH3NH2 (methylamine): This molecule has dipole-dipole interactions and also hydrogen bonding due to the presence of a nitrogen atom bonded to a hydrogen atom. Hydrogen bonding is a stronger intermolecular force than dipole-dipole interactions.

3. CH3I (iodomethane): This molecule has dipole-dipole interactions and London dispersion forces. Iodine atoms are larger and have more electrons than chlorine atoms, so iodomethane will have stronger London dispersion forces than trichloromethane.

Considering these factors, we can expect that the molecule with the weakest intermolecular forces will have the lowest boiling point. In this case, that would be CCl3H (trichloromethane) because it only has dipole-dipole interactions and London dispersion forces, and does not have hydrogen bonding like methylamine. Also, its London dispersion forces are weaker than those in iodomethane due to the smaller size and fewer electrons of chlorine atoms compared to iodine atoms.