Assertion : Ethers have specific dipole moment values
Reason : The C-O bond is polar nature.

Options

A. If both assertion and reason are correct and reason is correct explanation for assertion.
B. If both assertion and reason are correct but reason is not correct for assertion.
C. If assertion is correct but reason is incorrect.
D. If both assertion and reason are incorrect.

Explanation

To solve the question, we need to analyze the assertion and the reason provided.

### Step-by-Step Solution:

1. **Understanding the Assertion**:
- The assertion states that "Ethers have specific dipole moment values."
- Ethers are characterized by the presence of an oxygen atom bonded to two alkyl or aryl groups. The structure can be represented as R-O-R', where R and R' are hydrocarbon chains.

2. **Understanding the Reason**:
- The reason states that "The C-O bond is polar in nature."
- The oxygen atom is more electronegative than carbon, which means that in the C-O bond, the electrons are drawn closer to the oxygen atom, creating a dipole moment. This results in oxygen having a partial negative charge (δ-) and carbon having a partial positive charge (δ+).

3. **Analyzing the Dipole Moment**:
- The presence of polar C-O bonds contributes to the overall dipole moment of the ether molecule.
- Because ethers have a bent shape due to the presence of lone pairs on the oxygen atom, the dipole moments do not cancel out completely, leading to a net dipole moment.

4. **Conclusion**:
- Since both the assertion and the reason are true, and the reason accurately explains why ethers have specific dipole moment values, we conclude that both the assertion and the reason are correct.
- Therefore, the correct answer is that both the assertion and reason are true, and the reason is the correct explanation for the assertion.

### Final Answer:
Both assertion and reason are correct, and the reason is the correct explanation for the assertion.

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