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(B) The acidic strength of phenols is determined by the stability of the corresponding phenoxide ion. Electron-withdrawing groups $(EWG)$ increase aci

Vedclass · Accepted Answer

$IV > III > I > II$

Vedclass · Answer

(B) The acidic strength of phenols is determined by the stability of the corresponding phenoxide ion. Electron-withdrawing groups $(EWG)$ increase acidity by stabilizing the phenoxide ion,while electron-donating groups $(EDG)$ decrease acidity by destabilizing it.$1.$ $IV$ ($p$-nitrophenol): The $-NO_2$ group at the $p$-position exerts both a strong $-I$ effect and a strong $-M$ (mesomeric) effect,which significantly stabilizes the phenoxide ion.$2.$ $III$ ($m$-nitrophenol): The $-NO_2$ group at the $m$-position exerts only a $-I$ effect (no $-M$ effect),providing less stabilization than at the $p$-position.$3.$ $I$ (Phenol): This is the reference compound.$4.$ $II$ ($p$-methylphenol): The $-CH_3$ group at the $p$-position exerts a $+I$ effect and hyperconjugation $(+H)$,which donates electron density and destabilizes the phenoxide ion,making it the least acidic.Therefore,the correct order of acidic strength is $IV > III > I > II$.

Arrange the following in the correct order of their acidic strength:

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