Halogen derivatives have greater polarity and higher molecular mass compared to parent hydrocarbons, resulting in stronger intermolecular forces of attraction (dipole-dipole and van der Waals). This leads to higher boiling points in chlorides, bromides, and iodides compared to hydrocarbons of similar molecular mass.
Why do halogen derivatives of organic compounds generally have higher boiling points than their parent hydrocarbons?
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Halogen derivatives of organic compounds generally have higher boiling points than their parent hydrocarbons due to the influence of halogen atoms on intermolecular forces. Halogens, with their high electronegativity, induce dipole-dipole interactions and van der Waals forces between molecules. These additional intermolecular forces increase the boiling point by requiring more energy to overcome the attractive forces and transition from the liquid to the gaseous phase. The larger the halogen, the greater the impact on boiling points due to increased surface area and stronger van der Waals forces. This phenomenon is evident in halogenated compounds like chloroform or bromobenzene compared to their hydrocarbon counterparts.