Strongest C-H bond is present in

Options

A. ethane
B. ethene
C. ethyne
D. `CH_(3)OH`

Answer

To determine where the strongest C-H bond is present among the given compounds (ethane, ethene, ethyne, and methanol), we will analyze the hybridization of carbon in each compound and the bond order of the C-H bonds.

### Step-by-Step Solution:

1. **Identify the Compounds**: The compounds given are:
- Ethane (C2H6)
- Ethene (C2H4)
- Ethyne (C2H2)
- Methanol (CH3OH)

2. **Determine the Hybridization of Carbon**:
- **Ethane (C2H6)**: Each carbon is sp³ hybridized (4 sigma bonds).
- **Ethene (C2H4)**: Each carbon is sp² hybridized (3 sigma bonds and 1 pi bond).
- **Ethyne (C2H2)**: Each carbon is sp hybridized (2 sigma bonds and 2 pi bonds).
- **Methanol (CH3OH)**: The carbon is sp³ hybridized (4 sigma bonds).

3. **Analyze the C-H Bonds**:
- The strength of a bond is influenced by the hybridization of the carbon atom. Generally, the order of bond strength is:
- sp > sp² > sp³
- This means that C-H bonds involving sp hybridized carbon will be stronger than those involving sp² or sp³ hybridized carbon.

4. **Compare the C-H Bonds**:
- In **ethane**, the C-H bond is formed between sp³ hybridized carbon and hydrogen.
- In **ethene**, the C-H bond is formed between sp² hybridized carbon and hydrogen.
- In **ethyne**, the C-H bond is formed between sp hybridized carbon and hydrogen.
- In **methanol**, the C-H bond is also formed between sp³ hybridized carbon and hydrogen.

5. **Conclusion**:
- The strongest C-H bond is found in **ethyne** because the carbon is sp hybridized, leading to a stronger bond compared to the other compounds.

### Final Answer:
The strongest C-H bond is present in **ethyne (C2H2)**.