Question

Benzene C6 H6 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 the attraction between water and benzene?

1) Dipole-dipole forces
2) Hydrogen bonding
3) London dispersion forces
4) Ionic bonding

Answer 1

Benzene is only sparingly soluble in water due to the nonpolar nature of benzene resulting in predominant London dispersion forces between benzene and water molecules.

Step-by-step explanation:

Considering that benzene (C6H6) is only sparingly soluble in water, the intermolecular forces of attraction between water and benzene are primarily London dispersion forces. This is because benzene is a nonpolar molecule and does not form dipole-dipole interactions or hydrogen bonds with water, which are both polar. Benzene's solubility characteristics and boiling points are similar to those of cyclohexane, another hydrocarbon which also doesn't mix well with water. It is important to note that aromatic hydrocarbons like benzene have special bonding described by the resonance hybrid concept or the delocalization concept, but this does not significantly affect intermolecular interactions with water.