The presence of delocalised `pi` electrons in benzene indicates that it is

Options

A. Less stable than cyclohexatriene
B. more stable than cyclohexatriene
C. more basic than cyclohexatriene
D. both(2)(3)

Answer

To answer the question regarding the presence of delocalized π electrons in benzene, we can break down the explanation into a step-by-step solution:

### Step-by-Step Solution

1. **Understanding Benzene Structure**:
- Benzene (C6H6) is a cyclic compound with a hexagonal structure consisting of six carbon atoms.
- Each carbon atom is sp² hybridized, forming three sigma bonds: two with adjacent carbon atoms and one with a hydrogen atom.

**Hint**: Recall the structure of benzene and its hybridization.

2. **Delocalized π Electrons**:
- In benzene, there are six π electrons that are not localized between two specific carbon atoms. Instead, they are delocalized over the entire ring structure.
- This delocalization occurs because the p orbitals of the carbon atoms overlap, allowing the π electrons to move freely across the entire ring.

**Hint**: Think about how p orbitals interact in a cyclic structure.

3. **Aromaticity**:
- The delocalization of π electrons contributes to the aromatic nature of benzene. Aromatic compounds are characterized by their stability due to this electron delocalization.
- Benzene follows Huckel's rule, which states that a compound is aromatic if it has (4n + 2) π electrons, where n is a non-negative integer. For benzene, n = 1, giving it 6 π electrons.

**Hint**: Remember Huckel's rule for aromaticity.

4. **Stability of Benzene**:
- The delocalized π electrons provide extra stability to benzene compared to non-aromatic compounds. This stability is why benzene does not readily undergo addition reactions like alkenes do; instead, it tends to undergo substitution reactions.

**Hint**: Compare the reactivity of benzene with that of alkenes.

5. **Bond Lengths**:
- The delocalization of electrons results in equivalent bond lengths in benzene. The carbon-carbon bonds in benzene are neither single nor double but are of an intermediate length, indicating that all bonds are equivalent due to the resonance structure.

**Hint**: Consider how resonance affects bond lengths in benzene.

### Conclusion
The presence of delocalized π electrons in benzene indicates that it is an aromatic compound, which is more stable than non-aromatic compounds due to the delocalization of electrons across the entire ring structure.