Oxidation-Reduction Reactions When copper metal is placed in a silver nitrate solution, a single-displacement reaction occurs. Silver deposits on the surface of the copper, and the solution turns blue because Cu^2+ ions form in the solution. (a) Write a balanced chemical equation for this reaction

Question

Oxidation-Reduction Reactions

When copper metal is placed in a silver nitrate solution, a single-displacement reaction occurs. Silver deposits on the surface of the copper, and the solution turns blue because Cu²⁺ ions form in the solution.

(a) Write a balanced chemical equation for this reaction.

(b) Identify the element oxidized and the element reduced.

(c) Identify the oxidizing and reducing agents.

(d) On a molecular level, describe what’s happening at the surface of the copper metal.

Accepted Answer

(a) As we did in Chapter 5, we begin by writing correct formulas for the reactants and products in this single-displacement reaction. Copper metal is one reactant; it is represented as Cu(s). The other reactant, silver nitrate, is an ionic compound composed of silver ions, each with a charge of 1+, and nitrate ions, each with a charge of 1-. Because this compound is soluble in water, we can represent it with the formula AgNO₃(aq). One of the products is a soluble ionic compound composed of copper ions, each with a charge of 2+, and nitrate ions. This product can be represented with the formula Cu(NO₃)₂(aq). The other product is silver metal that has the formula Ag(s).

The skeletal equation for this reaction is

Cu(s) + AgNO₃(aq) → Cu(NO₃)₂(aq) + Ag(s)

We can follow the rules described in Section 5.3 to balance the equation.

Cu(s) + 2AgNO₃(aq) → Cu(NO₃)₂(aq) + 2Ag(s)

(b) Copper atoms in the copper metal change from a charge of 0 to 2+, so Cu(s) is the reactant that is oxidized. The silver ion from silver nitrate changes from a charge of 1+ to 0, so the Ag⁺ ion is reduced.

(c) Because copper metal is the reactant that gives up electrons to cause the reduction of silver ion, it is the reducing agent. Silver ion is the oxidizing agent because it removes electrons from the copper metal, causing its oxidation.

(d) The solution becomes a pale blue as the reaction proceeds, indicating that Cu atoms are converted to Cu²⁺ ions. A coating of silver appears on the surface of the copper metal, indicating that silver ions, Ag⁺, are converted to silver atoms, which coat the surface of the copper metal.

Question 14.1: Oxidation-Reduction Reactions When copper metal is placed in...

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