Step 1: Understanding the Concept:
Intermolecular forces are the forces of attraction and repulsion between atoms, molecules, and ions. The nature of these forces depends entirely on the polarity of the participating species.
- **Ammonia (\(NH_3\)):** Nitrogen is more electronegative than hydrogen, and the molecule has a lone pair. Due to its trigonal pyramidal geometry, the bond dipoles do not cancel out. Thus, \(NH_3\) is a **polar** molecule with a permanent dipole.
- **Benzene (\(C_6H_6\)):** It is a planar, hexagonal ring with a highly symmetrical distribution of electrons. The individual \(C-H\) dipoles cancel each other out. Thus, benzene is a **non-polar** molecule.
Step 2: Detailed Explanation:
When a polar molecule like ammonia approaches a non-polar molecule like benzene, the permanent dipole of the ammonia molecule induces a temporary dipole in the benzene molecule.
The positive end of the ammonia dipole attracts the electron cloud of benzene, or the negative end repels it, causing a shift in electron density within the benzene ring.
This results in an "induced dipole" in benzene. The resulting attractive force between the permanent dipole of \(NH_3\) and the induced dipole of benzene is called a **dipole-induced dipole interaction**, also known as **Debye forces**.
Let's evaluate other options:
- **Hydrogen bonding:** Although ammonia can form H-bonds with itself or water, benzene does not have a highly electronegative atom (N, O, F) with a lone pair to act as a significant H-bond acceptor in a standard context.
- **Dipole-dipole:** This requires both molecules to be polar.
- **Ion-dipole:** This requires an ion (like \(Na^+\)) and a polar molecule.
Step 3: Final Answer:
The interaction between a polar molecule (\(NH_3\)) and a non-polar molecule (Benzene) is dipole-induced dipole.
Hence, the correct option is (B).