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Mind Map: Alcohols, Phenols and Ethers
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FAQs on Mind Map: Alcohols, Phenols and Ethers
| 1. What's the difference between alcohols, phenols, and ethers in CBSE Chemistry? |  |
Ans. Alcohols contain a hydroxyl (-OH) group bonded to a carbon atom; phenols have -OH attached directly to an aromatic ring; ethers have two alkyl or aryl groups connected via oxygen. This structural distinction affects their chemical properties, reactivity patterns, and acidity levels significantly during NEET preparation.
| 2. Why are phenols more acidic than alcohols even though both have -OH groups? | |
Ans. Phenols are more acidic because the aromatic ring delocalises negative charge on the conjugate phenoxide ion through resonance, stabilising it. Alcohols lack this electron-delocalising ability, making their conjugate alkoxide ions much less stable and therefore less likely to donate protons readily.
| 3. How do you identify whether a compound is a primary, secondary, or tertiary alcohol? | |
Ans. Count the number of carbon atoms attached to the carbon bearing the -OH group. Primary alcohols have one carbon neighbour, secondary alcohols have two, and tertiary alcohols have three. This classification determines their oxidation patterns and reactivity in elimination and substitution reactions.
| 4. What are the main differences between SN1 and SN2 mechanisms in alcohol substitution reactions? | |
Ans. SN2 is a bimolecular, single-step mechanism requiring nucleophile attack with inversion of configuration; SN1 is unimolecular, forming a carbocation intermediate and allowing racemisation. Tertiary alcohols favour SN1, while primary alcohols predominantly undergo SN2 substitution under standard conditions.
| 5. Why can't phenols undergo typical alcohol reactions like esterification with carboxylic acids? | |
Ans. Phenols resist esterification because the aromatic ring's resonance delocalises electron density onto oxygen, making the -OH bond less nucleophilic and more difficult to protonate. However, phenols do react with acid anhydrides or acid chlorides to form esters, requiring stronger electrophilic reagents than simple carboxylic acids.
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