Here’s a clear comparison of alcohols, ethers, and phenols:
1. Alcohols
- Functional group: –OH (hydroxyl group) attached to a saturated carbon atom (sp³).
- General formula: R–OH
- Example: Ethanol (CH₃CH₂OH)
- Properties:
- Polar due to O–H bond.
- Can form hydrogen bonds.
- Higher boiling points than ethers of similar mass.
- Soluble in water (small-chain alcohols).
- Uses: Solvents, fuels, antiseptics, beverages.
2. Ethers
- Functional group: –O– (oxygen atom connected to two alkyl/aryl groups).
- General formula: R–O–R′
- Example: Diethyl ether (CH₃CH₂–O–CH₂CH₃)
- Properties:
- Less polar than alcohols (no –OH group).
- Cannot form hydrogen bonds with themselves (but can with water).
- Lower boiling points than alcohols of similar mass.
- Fairly volatile and flammable.
- Uses: Solvents, anesthetics, intermediates in organic synthesis.
3. Phenols
- Functional group: –OH group directly attached to an aromatic benzene ring.
- General formula: Ar–OH
- Example: Phenol (C₆H₅OH)
- Properties:
- More acidic than alcohols (due to resonance stabilization of phenoxide ion).
- Can form hydrogen bonds.
- Higher boiling points than hydrocarbons but lower than similar alcohols.
- Distinct antiseptic smell.
- Uses: Antiseptics (Dettol contains phenolic compounds), plastics, resins, dyes.
Key Difference Summary
- Alcohols: –OH on aliphatic carbon.
- Ethers: Oxygen between two carbons (R–O–R).
- Phenols: –OH directly attached to aromatic ring.