Textbook Question
Indicate whether each of the following statements is true or false: (a) If something is reduced, it is formally losing electrons. (b) A reducing agent gets oxidized as it reacts.
6. Chemical Quantities & Aqueous Reactions
Redox Reactions
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In the reaction 4Li(s) + O2(g) → 2Li2O(s), identify the oxidizing agent and the reducing agent.
A
Oxidizing agent: Li2O, Reducing agent: O2
B
Oxidizing agent: O2, Reducing agent: Li
C
Oxidizing agent: Li, Reducing agent: O2
D
Oxidizing agent: O2, Reducing agent: Li2O
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 oxidizing agent is the substance that gets reduced (gains electrons), and the reducing agent is the substance that gets oxidized (loses electrons).
Examine the chemical equation: 4Li(s) + O2(g) → 2Li2O(s). Identify the elements involved in the reaction and their initial and final states.
Determine the oxidation states: Lithium (Li) starts as a neutral element with an oxidation state of 0 and ends up in Li2O with an oxidation state of +1. Oxygen (O2) starts as a neutral molecule with an oxidation state of 0 and ends up in Li2O with an oxidation state of -2.
Identify the changes in oxidation states: Lithium goes from 0 to +1, indicating it loses electrons and is oxidized. Oxygen goes from 0 to -2, indicating it gains electrons and is reduced.
Assign the roles: Since lithium is oxidized, it acts as the reducing agent. Since oxygen is reduced, it acts as the oxidizing agent.
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