Assertion: The boiling points of aldehydes and ketone are higher than those of hydrocarbons and ethers of comparable molecular masses.

Reason: Aldehydes and ketones undergo intermolecular association due to dipole-dipole interactions.

Both Assertion and Reason are true and the Reason is the correct explanation of the Assertion.

The correct answer is option 1. Both Assertion and Reason are true and the Reason is the correct explanation of the Assertion.

Assertion: The boiling points of aldehydes and ketones are higher than those of hydrocarbons and ethers of comparable molecular masses.

The assertion is true. Aldehydes and ketones generally have higher boiling points than hydrocarbons and ethers of similar molecular masses. This is due to the stronger intermolecular forces present in aldehydes and ketones compared to hydrocarbons and ethers.

Reason: Aldehydes and ketones undergo intermolecular association due to dipole-dipole interactions.

The reason is true Aldehydes and ketones contain a polar carbonyl group (C=O). The difference in electronegativity between the carbon and oxygen atoms creates a dipole, with the oxygen being partially negative \((δ^-)\) and the carbon being partially positive \((δ^+)\). This polarity leads to dipole-dipole interactions between molecules of aldehydes and ketones. These interactions are stronger than the van der Waals forces present in non-polar hydrocarbons and ethers.

Explanation of the relationship:

Hydrocarbons:*Hydrocarbons (alkanes, alkenes, and alkynes) are non-polar molecules. Their boiling points are determined by weak van der Waals forces (London dispersion forces).

Ethers: Ethers have an oxygen atom bonded to two alkyl or aryl groups, but the C-O-C bond is less polar than the C=O bond in aldehydes and ketones. Thus, the intermolecular forces in ethers are weaker (dipole-dipole interactions in ethers are not as strong as those in carbonyl compounds).

Aldehydes and Ketones: The presence of a highly polar carbonyl group (C=O) in aldehydes and ketones leads to significant dipole-dipole interactions. These interactions are stronger than the van der Waals forces in hydrocarbons and the weaker dipole-dipole interactions in ethers.

Since both the assertion and the reason are true, and the reason correctly explains why aldehydes and ketones have higher boiling points than hydrocarbons and ethers of similar molecular masses, the correct answer is: Both Assertion and Reason are true and the Reason is the correct explanation of the Assertion.