Step 1: Understanding the Concept:
Intermolecular forces are determined by the electronic structure and polarity of the molecules involved.
Ammonia (\(NH_3\)) is a polar molecule because the electronegativity of Nitrogen is much higher than Hydrogen, and its trigonal pyramidal shape prevents the bond dipoles from canceling out.
Benzene (\(C_6H_6\)) is a non-polar molecule. It is a highly symmetrical hydrocarbon ring where individual \(C-H\) bond dipoles cancel each other out perfectly.
Step 2: Detailed Explanation:
When a polar molecule like Ammonia approaches a non-polar molecule like Benzene, the permanent dipole of Ammonia creates an electric field.
This field distorts the electron cloud of the Benzene molecule, effectively "inducing" a temporary dipole in the non-polar Benzene.
The attraction between the permanent dipole of the Ammonia and the induced dipole of the Benzene is called a **dipole-induced dipole interaction**.
Evaluation of other options:
- Hydrogen bonding: Ammonia can act as an H-bond donor, but Benzene lacks a highly electronegative atom (\(N, O, F\)) to act as an acceptor for a traditional H-bond.
- Dipole-dipole: This requires both molecules to be polar.
- Ion-dipole: This requires one species to be a charged ion.
Step 3: Final Answer:
The interaction is dipole-induced dipole interaction.