In benzene, carbon uses all the three p-orbitals for hybridisation .

Explanation

To determine whether the statement "In benzene, carbon uses all three p-orbitals for hybridization" is true or false, we can follow these steps:

### Step 1: Understand the Structure of Benzene
Benzene (C₆H₆) is a cyclic compound with a hexagonal structure. It consists of six carbon atoms connected by alternating double and single bonds. Each carbon atom is bonded to one hydrogen atom.

### Step 2: Analyze the Hybridization of Carbon in Benzene
To find the hybridization of carbon in benzene, we need to consider the bonding and the number of sigma (σ) and pi (π) bonds formed by each carbon atom.

1. Each carbon atom in benzene forms three sigma bonds:
- One sigma bond with the adjacent carbon atom.
- Two sigma bonds with two hydrogen atoms.

2. The remaining p-orbital on each carbon atom is used to form a pi bond with the adjacent carbon atom, contributing to the delocalized π-electron system in benzene.

### Step 3: Determine the Hybridization Type
Since each carbon atom forms three sigma bonds and has no lone pairs, we can determine the hybridization:
- The hybridization of carbon in benzene is sp² because:
- The three sigma bonds are formed using one s orbital and two p orbitals.
- The remaining p orbital (the third p orbital) is not hybridized and is used for π bonding.

### Step 4: Conclusion
Since carbon in benzene uses only two p-orbitals for hybridization (sp²) and one p-orbital for π bonding, the statement "In benzene, carbon uses all three p-orbitals for hybridization" is **false**.

### Final Answer
The statement is **false**.

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