Alcohols Phenols And Ethers

1. The acidity of alcohols depends on the stability of the alkoxide ion (R-O ) formed after releasing a proton.
2. Alkyl groups are electron-releasing (+I effect). They increase electron density on the oxygen atom, destabilizing the negative charge on the alkoxide ion.
3. Primary alcohols ( ): Have one alkyl group. Least +I effect. Alkoxide is most stable. Strongest acid.
4. Secondary alcohols ( ): Have two alkyl groups. Moderate +I effect.
5. Tertiary alcohols ( ): Have three alkyl groups. Maximum +I effect. Alkoxide is least stable. Weakest acid.
Order of Acidity: .

1. Reaction: When phenol is treated with chloroform (CHCl ) in the presence of aqueous sodium hydroxide (NaOH) at 340K, followed by acid hydrolysis.
2. Mechanism: The reaction involves an electrophilic substitution where the electrophile is dichlorocarbene (:CCl ).
3. Product: An aldehyde group (-CHO) is introduced, predominantly at the ortho position to the phenolic -OH group.
4. Equation:
Phenol + CHCl + 3NaOH Salicylaldehyde (2-Hydroxybenzaldehyde) + 3NaCl + 2H O.

Step 1: Dehydration: Heat Propan-1-ol with concentrated H SO at 443 K to form Propene.
CH CH CH OH CH CH=CH + H O
Step 2: Hydration: Treat Propene with water in the presence of acid (Acid-catalyzed hydration). The addition follows Markovnikov's rule, where the OH group attaches to the more substituted carbon (the middle one).
CH CH=CH + H O CH CH(OH)CH (Propan-2-ol)

1. Alcohols (R-OH) contain a highly electronegative oxygen atom attached to a hydrogen atom, which allows them to form intermolecular hydrogen bonds.
2. These hydrogen bonds are strong attractive forces that require significant energy to break during boiling.
3. Haloalkanes (R-X) are polar but cannot form hydrogen bonds with each other; they only have weaker dipole-dipole interactions and Van der Waals forces.
4. Consequently, the boiling point of alcohols is much higher than that of haloalkanes of comparable molecular mass.