The shape of a benzene molecule is planar and exhibits a hexagonal configuration with alternating single and double bonds. This arrangement allows for delocalized electrons across the carbon atoms, contributing to its stability and aromatic properties. In contrast, cyclohexane adopts a three-dimensional chair conformation, which is non-planar and allows for more staggered interactions between hydrogen atoms, minimizing steric strain.
When it comes to boiling points, cyclohexane generally has a higher boiling point compared to benzene. This is primarily due to the higher molecular weight and the fact that cyclohexane is a larger and more polarizable molecule, which increases the Van der Waals forces acting between its molecules. Consequently, these intermolecular forces require more energy to overcome, leading to a higher boiling point compared to benzene, which also experiences π-π stacking interactions but lacks the same degree of polarizability.