Ethanol and dimethyl ether form a pair of 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 ethyl alcohol
B. H-bonding in dimethyl ether
C. `CH_(3)` group in ethyl alcohol
D. `CH_(3)` group in demethyl ether

Explanation

To solve the question regarding the boiling points of ethanol and dimethyl ether, we will follow these steps:

### Step 1: Identify the Compounds
Ethanol (C2H5OH) and dimethyl ether (C2H6O) are both isomers, meaning they have the same molecular formula (C2H6O) but different structural formulas.

### Step 2: Understand the Structures
- **Ethanol** has a hydroxyl (-OH) group, which is characteristic of alcohols.
- **Dimethyl ether** has an ether functional group, consisting of an oxygen atom bonded to two methyl groups (CH3-O-CH3).

### Step 3: Analyze the Intermolecular Forces
- **Ethanol** can form hydrogen bonds due to the presence of the -OH group. Hydrogen bonding occurs when a hydrogen atom covalently bonded to a highly electronegative atom (like oxygen) is attracted to another electronegative atom.
- **Dimethyl ether**, on the other hand, cannot form hydrogen bonds because it lacks an -OH group. Instead, it exhibits weaker dipole-dipole interactions.

### Step 4: Compare Boiling Points
The boiling point of a substance is influenced by the strength of its intermolecular forces:
- **Ethanol** has strong intermolecular hydrogen bonding, leading to higher molecular association and a higher boiling point.
- **Dimethyl ether** has weaker dipole-dipole interactions, resulting in lower molecular association and a lower boiling point.

### Step 5: Conclusion
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 ethyl alcohol.

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