See image — GOC and Organic Chemistry Basics Chemistry Question

💡 Solution & Explanation

# Analysis of p-Nitrophenoxide Ion Resonance Structures **Structure of p-Nitrophenoxide:** The ion has a nitro group ($NO_2^+$) at para position to an oxide group ($O^-$) on benzene. **Evaluating each option:** **(A)** Both oxygens on N have formal charges $\bar{O}$ and $O^-$ — violates charge distribution; nitro group is $NO_2$ not $NO_2^+$ **(B)** N with $O^+$ and $O^-$ — represents canonical form with N=O double bond; aromatic ring properly conjugated; **valid resonance structure** **(D)** Shows aromatic C=O double bond opposite to $O^-$ on nitro group — creates unfavorable double negative charge region; poor charge separation **(C)** Has both oxygens on nitrogen as $\bar{O}$ (radicals) with negative charge on phenolic oxygen — **most unlikely because:** - Creates two unpaired electrons on N (radical character) - Violates octet rule for nitrogen - Nitro group becomes $NO_2^{3-}$ (impossible oxidation state) - Disrupts conjugation without stabilization benefit - Much higher energy than other resonance forms **Answer: (C)** is the most unlikely representation because it introduces radical character on nitrogen and creates an untenable charge distribution that violates basic valency and octet principles.