Textbook Question
Identify the oxidized reactant, the reduced reactant, the oxidizing agent, and the reducing agent in the following reactions:a. Fe(s)+Cu₂+(aq) → Fe₂+(aq)+Cu(s) b. Mg(s)+Cl₂(g) → MgCl₂(s)c. 2 Al(s)+Cr₂O₃(s) → 2 Cr(s) + Al₂O₃(s)
16. Oxidation and Reduction
Redox Reactions
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Identify the oxidizing agent and reducing agent from the following redox reaction.
Ba (s) + Cl2 (g) → BaCl2 (aq)
A
Ba:oxidizing agent; Cl2 reducing agent
B
Ba:reducing agent; Cl2 oxidizing agent
Verified step by step guidance1
Understand the concept of oxidation and reduction: Oxidation involves the loss of electrons, while reduction involves the gain of electrons. In a redox reaction, the substance that gets oxidized is the reducing agent, and the substance that gets reduced is the oxidizing agent.
Identify the oxidation states of the elements in the reactants and products. For elemental barium (Ba), the oxidation state is 0. For chlorine gas (Cl2), each chlorine atom also has an oxidation state of 0.
Determine the changes in oxidation states: In the product BaCl2, barium (Ba) has an oxidation state of +2, and each chlorine atom (Cl) has an oxidation state of -1.
Analyze the changes: Barium (Ba) goes from an oxidation state of 0 to +2, indicating it loses electrons and is oxidized. Chlorine (Cl2) goes from an oxidation state of 0 to -1, indicating it gains electrons and is reduced.
Conclude the roles: Since barium (Ba) is oxidized, it acts as the reducing agent. Since chlorine (Cl2) is reduced, it acts as the oxidizing agent.
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