The overlapping of orbitals in benzene is of the type

Options

A. `sp^(2) - sp^(2)`
B. `sp^(3)-sp^(3)`
C. `sp-sp`
D. `p-p`

Explanation

To determine the type of orbital overlapping in benzene, we can follow these steps:

### Step 1: Understand the Structure of Benzene
Benzene (C₆H₆) is a cyclic compound consisting of six carbon atoms arranged in a hexagonal ring. Each carbon atom is bonded to one hydrogen atom.

**Hint:** Recall the molecular formula of benzene and its hexagonal structure.

### Step 2: Identify the Hybridization of Carbon Atoms
In benzene, each carbon atom undergoes sp² hybridization. This means that one s orbital and two p orbitals combine to form three sp² hybrid orbitals, while one p orbital remains unhybridized.

**Hint:** Remember that sp² hybridization involves one s orbital and two p orbitals.

### Step 3: Determine the Bonding in Benzene
Each carbon atom forms sigma (σ) bonds with its two neighboring carbon atoms and one hydrogen atom using the sp² hybrid orbitals. The unhybridized p orbital on each carbon atom is perpendicular to the plane of the ring.

**Hint:** Sigma bonds are formed by head-on overlapping of orbitals, while p orbitals are involved in pi bonding.

### Step 4: Analyze the Overlapping of p Orbitals
The unhybridized p orbitals from adjacent carbon atoms overlap sideways to form pi (π) bonds. This results in a delocalized electron cloud above and below the plane of the benzene ring.

**Hint:** Pi bonds are formed by the lateral overlap of p orbitals.

### Step 5: Conclusion on the Type of Overlapping
The overlapping of orbitals in benzene is primarily of the type p-p overlapping, which leads to the formation of the delocalized π system.

**Hint:** Look for the type of orbital involved in the bonding when considering the overlapping.

### Final Answer
The overlapping of orbitals in benzene is of the type **p-p overlapping**.