Match List-I with List-II with their boiling points.
|
List-I Compound Name |
List-II Boiling Point |
|
(A) $CH_3CH_2OH$ |
(I) 373K |
|
(B) $CH_3OCH_3$ |
(II) 348K |
|
(C) $H_2O$ |
(III) 351K |
|
(D) $CH_3CH_2OCH_2CH_3$ |
(IV) 248K |
Choose the correct answer from the options given below:
Answer & explanation
Correct answer: option 1
The correct answer is Option (1) → (A)-(III), (B)-(IV), (C)-(I), (D)-(II)
|
List-I Compound Name |
List-II Boiling Point |
|
(A) $CH_3CH_2OH$ |
(III) 351K |
|
(B) $CH_3OCH_3$ |
(IV) 248K |
|
(C) $H_2O$ |
(I) 373K |
|
(D) $CH_3CH_2OCH_2CH_3$ |
(II) 348K |
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)