Answer:
B => Mg° => Mg⁺² + 2e⁻
Explanation:
2Mg° + O₂ => 2MgO rewrite => Mg° + 1/2O₂ => 2MgO
Oxidation Half Rxn => Mg° => Mg⁺² + 2e⁻
Reduction Half Rxn => 1/2O₂ + 2e⁻ => 2O⁻
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FYI Note => For half-reactions one always finds the electrons listed on the product side of the reaction for oxidation reactions and for reduction reactions on the reactant side.
Mg° => Mg⁺² + 2e⁻ is the oxidation half-reaction for [tex]2Mg + O_2[/tex] → [tex]2Mgo[/tex]. Hence, option B is correct.
A reaction involving both oxidation and reduction simultaneously means one reactant gets oxidised, and the other gets reduced.
2Mg° + O₂ => 2MgO rewrite => Mg° + 1/2O₂ => 2MgO
Oxidation Half reaction => Mg° => Mg⁺² + 2e⁻
Reduction Half reaction => 1/2O₂ + 2e⁻ => 2O⁻
For half-reactions, one always finds the electrons listed on the product side of the reaction for oxidation reactions and for reduction reactions on the reactant side.
Hence, Mg° => Mg⁺² + 2e⁻ is the oxidation half-reaction for [tex]2Mg + O_2[/tex] → [tex]2Mgo[/tex].
Learn more about the redox reaction here:
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