See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Analysis of Aniline Base Strength The basicity of aniline derivatives depends on the electron density at the nitrogen atom. Electron-donating groups increase basicity; electron-withdrawing groups decrease it. ## Evaluating Each Option: **Option (A):** $NO_2$ groups are strong electron-withdrawing (deactivating). They significantly reduce electron density on $N$, making this a very weak base. **Option (B):** Single $NO_2$ is electron-withdrawing. The $Me$ group provides weak donation, but $NO_2$ dominates, making this weaker than options (C) and (D). **Option (C):** Two $Me$ groups (ortho and para positions) are electron-donating groups. They increase electron density on $N$ through resonance and inductive effects, **enhancing basicity**. **Option (D):** The $CN$ group is strongly electron-withdrawing (via $-I$ and resonance). It dramatically reduces the lone pair availability on $N$, making this the weakest base. ## Basicity Order: $$\text{(D)} < \text{(A)} < \text{(B)} < \text{(C)}$$ **Answer: (C)** has the highest basicity because the two methyl substituents donate electron density to the aromatic ring, increasing the nucleophilicity of the amino group and making it the least weak (i.e., strongest) of the given bases.