Which of the following is the strongest base?

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(D) The basicity of amines depends on the availability of the lone pair of electrons on the nitrogen atom. In $C_6H_5NH_2$ (aniline),the lone pair is

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$C_6H_5CH_2NH_2$

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(D) The basicity of amines depends on the availability of the lone pair of electrons on the nitrogen atom. In $C_6H_5NH_2$ (aniline),the lone pair is involved in resonance with the benzene ring,reducing its availability. In $p-NO_2-C_6H_4NH_2$ and $m-NO_2-C_6H_4NH_2$,the $-NO_2$ group is a strong electron-withdrawing group ($-I$ and $-M$ effect),which further decreases the electron density on the nitrogen atom,making them weaker bases than aniline. In $C_6H_5CH_2NH_2$ (benzylamine),the $-NH_2$ group is attached to a $CH_2$ group,not directly to the benzene ring. Therefore,the lone pair is not involved in resonance with the benzene ring. Thus,$C_6H_5CH_2NH_2$ is the strongest base among the given options.

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