The hydroxyl group in phenol is directly attached to the sp² hybridized carbon of the benzene ring, acting as an electron-withdrawing group. This, along with resonance structures, results in a positive charge on the oxygen, making phenols stronger acids than ...

Alkoxide ions are better proton acceptors than hydroxide ions, indicating stronger bases. Alcohols act as Bronsted bases due to the presence of unshared electron pairs on oxygen, making them capable of accepting protons.

Alcohols and phenols react with active metals (e.g., sodium, potassium, aluminum), forming alkoxides/phenoxides and releasing hydrogen. Phenols also react with aqueous sodium hydroxide to produce sodium phenoxides.

The polar nature of the O-H bond contributes to the acidic character of alcohols. Electron-releasing groups like –CH₃ and –C₂H₅ decrease the acid strength by increasing electron density on oxygen.

Alcohols and phenols, despite having comparable molecular masses with hydrocarbons, ethers, haloalkanes, and haloarenes, exhibit higher boiling points due to the presence of intermolecular hydrogen bonding, which is lacking in the other compound classes.