Benzene C6H6 is an aromatic hydrocarbon compound. The primary intermolecular forces present in benzene are London dispersion forces also known as van der Waals forces and - interactions.1. London dispersion forces: These are weak, temporary attractive forces that arise due to the instantaneous dipoles created by the movement of electrons in the molecule. Since benzene is a nonpolar molecule, these forces are the primary intermolecular forces between benzene molecules.2. - interactions: Benzene has a planar hexagonal structure with alternating single and double carbon-carbon bonds, which creates a delocalized electron cloud above and below the plane of the molecule. These electrons can interact with the electrons of neighboring benzene molecules, leading to weak attractive forces known as - interactions.These intermolecular forces contribute to the physical properties of benzene in the following ways:1. Boiling and melting points: Due to the relatively weak London dispersion forces and - interactions, benzene has a low boiling point 80.1C and melting point 5.5C compared to compounds with stronger intermolecular forces like hydrogen bonding.2. Volatility and vapor pressure: The weak intermolecular forces in benzene result in a relatively high volatility and vapor pressure at room temperature, making it easy for benzene to evaporate.3. Solubility: Benzene is nonpolar and has weak intermolecular forces, which makes it more soluble in nonpolar solvents like other hydrocarbons, and less soluble in polar solvents like water.4. Viscosity: The weak intermolecular forces in benzene lead to a low viscosity, meaning it flows easily as a liquid.Overall, the London dispersion forces and - interactions in benzene contribute to its relatively low boiling and melting points, high volatility, nonpolar solubility, and low viscosity.