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(A) To determine the basic strength,we look at the availability of the lone pair on the nitrogen atom:$(ii)$ Benzylamine $(C_6H_5CH_2NH_2)$: The lone

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$iv < iii < i < ii$

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(A) To determine the basic strength,we look at the availability of the lone pair on the nitrogen atom:$(ii)$ Benzylamine $(C_6H_5CH_2NH_2)$: The lone pair on the nitrogen is localized (not involved in resonance),making it the strongest base.$(i)$ Aniline $(C_6H_5NH_2)$: The lone pair on the nitrogen is delocalized into the benzene ring due to resonance,reducing its basicity.$(iii)$ $o$-Nitroaniline $(o-NO_2-C_6H_4NH_2)$: The $-NO_2$ group is a strong electron-withdrawing group ($-I$ and $-M$ effect),which further decreases the electron density on the nitrogen compared to aniline.$(iv)$ Benzamide $(C_6H_5CONH_2)$: The lone pair on the nitrogen is involved in resonance with the adjacent carbonyl group $(C=O)$,making it the least basic.Therefore,the correct order of basic strength is: $iv < iii < i < ii$.

Arrange the following compounds in the correct order of their basic strength:

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