The correct order of acidity of the above com | vedclass

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(C) The acidity of phenols depends on the stability of the phenoxide ion formed after the loss of a proton. Electron-withdrawing groups $(EWG)$ stabil

Vedclass · Accepted Answer

$IV > III > I > II$

Vedclass · Answer

(C) The acidity of phenols depends on the stability of the phenoxide ion formed after the loss of a proton. Electron-withdrawing groups $(EWG)$ stabilize the phenoxide ion and increase acidity, while electron-donating groups $(EDG)$ destabilize it and decrease acidity.$1$. Compound $(IV)$ has a $-NO_2$ group, which is a strong electron-withdrawing group ($-R$ and $-I$ effect), making it the most acidic.$2$. Compound $(III)$ has a $-CH=CH_2$ group, which is an electron-withdrawing group ($-R$ effect), making it more acidic than $(I)$ and $(II)$.$3$. Compound $(I)$ has a $-CH_3$ group, which is an electron-donating group ($+I$ and hyperconjugation), making it less acidic than $(III)$ but more acidic than $(II)$.$4$. Compound $(II)$ has a $-NMe_2$ group, which is a very strong electron-donating group ($+R$ effect), making it the least acidic.Therefore, the correct order of acidity is $(IV) > (III) > (I) > (II)$.

The correct order of acidity of the above compounds is:

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