Question

Assertion (A): Ethers have lower boiling points than the boiling points of alcohols.
Reason (R): This is due to the presence of hydrogen bonding in alcohols.

• A. Both Assertion (A) and Reason (R) are true and Reason (R) is the correct explanation of the Assertion (A).
• B. Both Assertion (A) and Reason (R) are true, but Reason (R) is not the correct explanation of the Assertion (A).
• C. Assertion (A) is true, but Reason (R) is false.
• D. Assertion (A) is false, but Reason (R) is true.

Hint:

Alcohols form hydrogen bonds (O−H); ethers cannot, so alcohols boil higher.

Answer 1

The Correct Option is A

Concept: In an assertion-reason question, first check whether each statement is true by itself, then check whether the reason actually explains the assertion. Here the whole thing turns on hydrogen bonding.

Step 1: Check the Assertion
Alcohols have an O−H group, so their molecules can form hydrogen bonds with each other. Ethers have a C−O−C arrangement with no O−H, so they cannot form these hydrogen bonds. Hydrogen bonds hold molecules together strongly, so it takes more heat to boil alcohols. That means ethers really do boil at lower temperatures than alcohols, so the Assertion is true.

Step 2: Check the Reason
The Reason says the difference comes from hydrogen bonding in alcohols. That is exactly the cause we just used, so the Reason is true.

Step 3: Do they connect
Yes, the hydrogen bonding in alcohols is the very reason ethers boil lower, so the Reason correctly explains the Assertion.

Answer: Option (A), both are true and R correctly explains A.