Balance each redox reaction occurring in basic aqueous solution. c. Cl₂(g) → Cl^–(aq) + ClO^–(aq)

Verified step by step guidance

1. Identify the oxidation and reduction half-reactions. In this case, Cl2 is being reduced to Cl- and oxidized to ClO-. Write the half-reactions: Cl2 → Cl- and Cl2 → ClO-.
2. Balance the atoms other than oxygen and hydrogen in each half-reaction. For the reduction half-reaction, Cl2 → 2Cl-. For the oxidation half-reaction, Cl2 → ClO-.
3. Balance the oxygen atoms by adding H2O molecules. For the oxidation half-reaction, add one H2O to the right side: Cl2 → ClO- + H2O.
4. Balance the hydrogen atoms by adding OH- ions. For the oxidation half-reaction, add two OH- to the left side: Cl2 + 2OH- → ClO- + H2O.
5. Balance the charges by adding electrons. For the reduction half-reaction, add two electrons to the right side: Cl2 + 2e- → 2Cl-. For the oxidation half-reaction, add two electrons to the left side: Cl2 + 2OH- + 2e- → ClO- + H2O.

Key Concepts

Redox Reactions

Redox reactions, or reduction-oxidation reactions, involve the transfer of electrons between species. In these reactions, one species is oxidized (loses electrons) while another is reduced (gains electrons). Understanding the oxidation states of the elements involved is crucial for identifying which species undergo oxidation and reduction.

Balancing Redox Reactions in Basic Solution

Balancing redox reactions in basic solutions requires a specific approach. First, the half-reactions for oxidation and reduction are written separately. Then, hydroxide ions (OH⁻) are added to neutralize any hydrogen ions (H⁺) that may appear, and water molecules are used to balance the oxygen atoms. Finally, the overall reaction is combined and simplified.

Oxidation States

Oxidation states are a way to keep track of electron transfer in redox reactions. Each element in a compound is assigned an oxidation state based on a set of rules, which helps determine how many electrons are gained or lost during the reaction. In the given reaction, recognizing the changes in oxidation states of chlorine is essential for correctly balancing the equation.