Final answer:
The compound with the highest boiling point is usually the one with the larger molecular size and stronger intermolecular forces, notably London dispersion forces and, where applicable, hydrogen bonding or other dipole interactions.
Step-by-step explanation:
When determining which compound has the highest boiling point, it's important to consider both molecular size and the type of intermolecular forces present. Compounds with larger molecular sizes generally exhibit stronger London dispersion forces, leading to higher boiling points. Additionally, compounds that are capable of hydrogen bonding or have polar functional groups will usually have higher boiling points compared to similar-sized nonpolar molecules.
(CH3)3CCl, also known as tert-butyl chloride, is a molecule that is relatively larger compared to simple alkanes like methane or ethane. Tert-butyl chloride will exhibit stronger London dispersion forces due to its larger molecular size. Additionally, the chlorine atom introduces some polarity to the molecule, although it will not contribute to hydrogen bonding as hydroxyl or amino groups would. Thus, while it may display some dipole-dipole interactions, London dispersion forces will be the dominant intermolecular force in determining its boiling point.