The bond length between central carbon atom and other carbon atom is minimum in

Options

A. Propene
B. Propyne
C. Propane
D. pentane

Answer

To determine the bond length between a central carbon atom and another carbon atom, we need to analyze the types of bonds formed between them: single, double, and triple bonds. The bond length is influenced by the bond type, which is related to the hybridization of the carbon atoms involved.

### Step-by-Step Solution:

1. **Identify the Types of Bonds**:
- The three types of carbon-carbon bonds we will consider are:
- Single bond (C-C)
- Double bond (C=C)
- Triple bond (C≡C)

2. **Understand Hybridization**:
- The hybridization of the carbon atoms affects the bond length:
- Single bond (C-C) involves sp³ hybridization.
- Double bond (C=C) involves sp² hybridization.
- Triple bond (C≡C) involves sp hybridization.

3. **Calculate Percentage s Character**:
- The percentage of s character in the hybridization affects bond strength and length:
- For sp³ (single bond): 25% s character
- For sp² (double bond): 33% s character
- For sp (triple bond): 50% s character

4. **Analyze Bond Strength and Length**:
- The greater the s character, the shorter and stronger the bond:
- Triple bond (C≡C) has the highest s character (50%), making it the shortest and strongest bond.
- Double bond (C=C) has 33% s character, making it longer than a triple bond but shorter than a single bond.
- Single bond (C-C) has the least s character (25%), making it the longest and weakest bond.

5. **Conclusion**:
- Therefore, the bond length between the central carbon atom and the other carbon atom is minimum in a triple bond (C≡C).

### Final Answer:
The bond length between the central carbon atom and the other carbon atom is minimum in a **triple bond**.

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