The Question is from NEET guide , and it was created by the author Mr. S M HUSSAIN

Question

What is the bond length between carbon atoms in benzene?

Mr. S M HUSSAIN · Accepted Answer

## CORE INFORMATION
✓ **Answer**: C
## CONCEPT FRAMEWORK
 **Primary Concept**:  Bond Length and Resonance
 **Related Topics**: Delocalized electrons, Aromatic compounds, Hybridization
 **Prerequisites**: Understanding of single, double, and resonance structures.
## SOLUTION PATHWAY
**Given Information**:
  The question asks about the C-C bond length in benzene ($C_6H_6$).
  [Important conditions]: Benzene is an aromatic compound with a cyclic structure.
**Method & Steps**:
 1. Benzene's structure involves alternating single and double bonds between carbon atoms in a cyclic structure.
  Reasoning:  A simple representation shows alternating single and double bonds. However, this is not the complete picture.
  Formula/Rule: None directly applicable, but understanding of resonance is crucial.
 2. Due to resonance, the electrons in the $\pi$ system are delocalized across all six carbon atoms.
  Working: This means that the electrons are not localized in specific double bonds, but are spread out over the entire ring.  This leads to a bond order of 1.5 for each C-C bond.
  Key Point: The delocalization is what makes benzene unusually stable.
 3. A bond order of 1.5 implies a bond length intermediate between a single and a double bond.
  Result: The C-C bond length in benzene is intermediate between a single and double bond.
  Verification: Experimental data confirms that the C-C bond length in benzene is indeed intermediate between single and double bonds.
 ## OPTION ANALYSIS
A :x:  A single C-C bond is longer than the bond in benzene.
B :x: A double C=C bond is shorter than the bond in benzene.
C ✓: The bond length is intermediate due to resonance and delocalization.
D :x: The bond is shorter than a double bond because of the resonance effect.
 ## LEARNING AIDS
 **Common Mistakes**:
  1.Thinking that benzene has distinct single and double bonds: Remember the delocalization of electrons.
  2.Confusing bond order with bond length: While related, they are not directly interchangeable.  Higher bond order means shorter bond length.
 **Quick Tips**:
  1.Remember the key characteristics of aromatic compounds like benzene, particularly the delocalized $\pi$ system.
  2.Visualize the resonance structures of benzene to understand the electron distribution.

Mr. S M HUSSAIN · Answer

Same as a single bond

Mr. S M HUSSAIN · Answer

Same as a double bond

Mr. S M HUSSAIN · Answer

The correct Option is "Intermediate between single and double bond"

Mr. S M HUSSAIN · Answer

Longer than a double bond

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