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Chemistry · Electronic concepts of oxidation and reduction, redox reactions, oxidation number, rules for assigning oxidation number and balancing of redox reactions

Consider the following reaction. \[ \left.\right|_{\mathbf{C H O}} ^{\mathbf{C H

Consider the following reaction. \[ \left.\right|_{\mathbf{C H O}} ^{\mathbf{C H O}}+\left.\mathbf{O H}^{-} \longrightarrow\right|_{\mathbf{C H}_{2} \mathbf{O H}} ^{\mathbf{O O}^{-}} \]

  • A. It is not a disproportionation reaction
  • B. It is intramolecular redox reaction
  • C. \( O H^{-} \) is reducing as well as oxidising agent
  • D. \( (C H O)_{2} \) is a reducing as well as oxidising agent

Step-by-step solution

In the reaction, (CHO)2 (likely glyoxal) undergoes disproportionation in the presence of OH-: one aldehyde group is reduced to CH2OH, while the other is oxidized to OO- (likely a peroxy or carboxylate species). The same compound (CHO)2 acts as both reducing agent (losing electrons) and oxidizing agent (gaining electrons), making option D correct. Option A is false because it is a disproportionation. Option B is not necessarily true if the reaction is intermolecular (two separate molecules), but even if intramolecular, the key property is that (CHO)2 serves dual redox roles. Option C is false as OH- acts as a base, not as a redox agent.
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