Chemical Forums
Chemistry Forums for Students => Organic Chemistry Forum => Topic started by: aspiringphysician on September 05, 2013, 01:50:13 PM
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Why is a carboxylic acid a stronger deactivator (i.e. more electron-withdrawing) than an ester?
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Why is a carboxylic acid a stronger deactivator (i.e. more electron-withdrawing) than an ester?
Can you explain to us why either acids or esters are deactivators first of all?
I.e. what mechanism makes them deactivate an aromatic ring.