- A redox reaction is a chemical reaction that involves the transfer of electrons, resulting in changes in the oxidation states of atoms. - Oxidation is an increase in oxidation state (loss of electrons). - Reduction is a decrease in oxidation state (gain of electrons). - Let's analyze the oxidation states in each reaction: - A) AlCl₃ (+3, -1) + H₂O (+1, -2) → Al(OH)₃ (+3, -2, +1) + HCl (+1, -1). Oxidation states of all elements remain unchanged. - B) 2NaH (+1, -1) → 2Na (0) + H₂ (0). Na changes from +1 to 0 (reduction), H changes from -1 to 0 (oxidation). Redox. - C) 4Fe (0) + 3O₂ (0) → 2Fe₂O₃ (+3, -2). Fe changes from 0 to +3 (oxidation), O changes from 0 to -2 (reduction). Redox. - D) CuSO₄ (+2, -2) + Zn (0) → Cu (0) + ZnSO₄ (+2, -2). Cu changes from +2 to 0 (reduction), Zn changes from 0 to +2 (oxidation). Redox.
Which one of the following is not an example of a redox reaction?
Asked in UPSC NDA 1 2022 · Topic: Inorganic Chemistry (Inorganic Reaction Mechanisms)
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