Maximum bond energy of C-H bonds is found in the compound

Options

A. Ethane
B. Ethene
C. Ethyne
D. Equal in all the three

Explanation

To determine the compound with the maximum bond energy of C-H bonds, we need to analyze the types of hybridization present in different hydrocarbons and how they affect the bond strength between carbon and hydrogen.

### Step-by-Step Solution:

1. **Identify the Compounds**: We will consider three hydrocarbons:
- Ethane (C2H6) - with C-C single bonds and C-H bonds.
- Ethene (C2H4) - with C=C double bonds and C-H bonds.
- Ethyne (C2H2) - with C≡C triple bonds and C-H bonds.

2. **Determine the Hybridization**:
- In **Ethane (C2H6)**, the carbon atoms are **sp³ hybridized**. Each C-H bond is formed by the overlapping of an sp³ orbital from carbon and an s orbital from hydrogen.
- In **Ethene (C2H4)**, the carbon atoms are **sp² hybridized**. Each C-H bond is formed by the overlapping of an sp² orbital from carbon and an s orbital from hydrogen.
- In **Ethyne (C2H2)**, the carbon atoms are **sp hybridized**. Each C-H bond is formed by the overlapping of an sp orbital from carbon and an s orbital from hydrogen.

3. **Analyze the S-character**:
- The s-character of the hybrid orbitals affects the bond strength:
- **sp³ hybridization** has 25% s-character.
- **sp² hybridization** has 33% s-character.
- **sp hybridization** has 50% s-character.

4. **Relate S-character to Bond Strength**:
- As the s-character increases, the bond strength also increases. This is because orbitals with higher s-character are closer to the nucleus, leading to stronger bonds.
- Therefore, the order of bond strength for C-H bonds in these compounds is:
- Ethane (sp³) < Ethene (sp²) < Ethyne (sp).

5. **Conclusion**:
- Since Ethyne has the highest s-character (50%) due to its sp hybridization, it will have the maximum bond energy for the C-H bonds compared to Ethane and Ethene.

### Final Answer:
The compound with the maximum bond energy of C-H bonds is **Ethyne (C2H2)**.