Final answer:
Cyclohexanol, which can form hydrogen bonds due to its hydroxyl group, will have a higher boiling point compared to cyclohexene, which lacks this group and can only exhibit weaker London dispersion forces.
Step-by-step explanation:
When comparing the boiling points of cyclohexene and cyclohexanol, it is important to consider the types of intermolecular forces present within each molecule. Cyclohexanol contains a hydroxyl group (-OH), which allows it to participate in hydrogen bonding, a strong type of dipole-dipole interaction. In contrast, cyclohexene has a double bond and does not have the ability to form hydrogen bonds as it lacks the hydroxyl group.
Due to the presence of hydrogen bonding, cyclohexanol will have a higher boiling point than cyclohexene. This is similar to the example where methanol, which can form an extensive hydrogen bonding network, has a higher boiling point compared to nonpolar molecules that only exhibit London dispersion forces.
Therefore, cyclohexanol, with its ability to form hydrogen bonds, will exhibit a higher boiling point than cyclohexene, which can only participate in weaker van der Waals forces, specifically London dispersion forces.