Benzene, \(\ce{C6H6}\), has the structure shown above. Considering the observation that benzene is only sparingly soluble in water, which of the following best describes the intermolecular forces of attraction between water and benzene?

Although it is correct that benzene is nonpolar and hydrophobic, there will still be intermolecular forces between water and benzene. Since water has a large dipole moment, it can induce a dipole in the benzene molecule. Additionally, nonpolar molecules also exhibit london dispersion forces.

Hydrogen bonding occurs between water molecules, but not necessarily much between benzene and water. The hydrogen and carbon atoms in benzene are similar in electronegativity, so the hydrogen does not have a partial positive dipole moment like the hydrogen in the water molecule.