Ethanol and dimethyl ether from a pair of functional isomers. The boiling point of Ethanol is higher than that of dimethyl ether, due to the presence of

Options

A. H - bonding in ethanol
B. H - bonding in dimethyl ether
C. `CH_(3)` gorup in ethanol
D. `CH_(3)` group in dimethyl ether

Explanation

To understand why ethanol has a higher boiling point than dimethyl ether, we need to analyze the structures and intermolecular forces present in both compounds.

### Step-by-Step Solution:

1. **Identify the Structures**:
- Ethanol (C₂H₅OH) is an alcohol with a hydroxyl (-OH) functional group.
- Dimethyl ether (C₂H₆O) is an ether with an oxygen atom bonded to two methyl (CH₃) groups.

2. **Functional Groups**:
- Ethanol contains a hydroxyl group, which is capable of forming hydrogen bonds.
- Dimethyl ether contains an ether functional group, which does not have the ability to form hydrogen bonds.

3. **Intermolecular Forces**:
- In ethanol, the presence of the hydroxyl group allows for hydrogen bonding between ethanol molecules. This is a strong intermolecular force that requires more energy to break.
- In dimethyl ether, the primary intermolecular forces are dipole-dipole interactions and Van der Waals forces, which are weaker than hydrogen bonds.

4. **Boiling Point Comparison**:
- The boiling point of a substance is influenced by the strength of its intermolecular forces. Stronger forces lead to higher boiling points.
- Since ethanol can form hydrogen bonds, it has stronger intermolecular attractions compared to dimethyl ether, which lacks hydrogen bonding.

5. **Conclusion**:
- Therefore, the boiling point of ethanol is higher than that of dimethyl ether due to the presence of hydrogen bonding in ethanol.

### Final Answer:
The boiling point of ethanol is higher than that of dimethyl ether due to the presence of hydrogen bonding in ethanol.

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