Match List-I with List-II with their boiling points.

Choose the correct answer from the options given below:

(A)-(III), (B)-(IV), (C)-(I), (D)-(II)

The correct answer is Option (1) → (A)-(III), (B)-(IV), (C)-(I), (D)-(II)

Boiling point depends mainly on intermolecular forces:

• Hydrogen bonding → highest boiling point • Dipole forces → moderate • London forces → lowest

$H_2O$ (Water): Extensive hydrogen bonding occurs between water molecules. Each molecule can form up to four hydrogen bonds. This leads to the highest boiling point in this set.

• Boiling Point: 373 K (I)

$CH_3CH_2OH$ (Ethanol): Contains an $-OH$ group, allowing for intermolecular hydrogen bonding. However, the bonding is less extensive than in water.

• Boiling Point: 351 K (III)

$CH_3CH_2OCH_2CH_3$ (Diethyl ether): This is a larger ether molecule. It lacks hydrogen bonding but has dipole-dipole interactions and significantly stronger London dispersion forces (due to higher molecular mass) compared to dimethyl ether.

• Boiling Point: 348 K (II)

$CH_3OCH_3$ (Dimethyl ether): This is the smallest molecule here and an ether. It only has weak dipole-dipole interactions and no hydrogen bonding.

• Boiling Point: 248 K (IV)