Table of contents

1. Matter and Measurements4h 31m
2. Atoms and the Periodic Table5h 23m
3. Ionic Compounds2h 18m
4. Molecular Compounds2h 18m
5. Classification & Balancing of Chemical Reactions3h 17m
6. Chemical Reactions & Quantities2h 27m
7. Energy, Rate and Equilibrium3h 46m
8. Gases, Liquids and Solids3h 25m
9. Solutions4h 10m
10. Acids and Bases3h 29m
11. Nuclear Chemistry56m
BONUS: Lab Techniques and Procedures1h 38m
BONUS: Mathematical Operations and Functions47m
12. Introduction to Organic Chemistry1h 34m
13. Alkenes, Alkynes, and Aromatic Compounds2h 12m
14. Compounds with Oxygen or Sulfur1h 6m
15. Aldehydes and Ketones1h 1m
16. Carboxylic Acids and Their Derivatives1h 11m
17. Amines39m
18. Amino Acids and Proteins1h 51m
19. Enzymes1h 37m
20. Carbohydrates1h 41m
21. The Generation of Biochemical Energy2h 8m
22. Carbohydrate Metabolism2h 22m
23. Lipids2h 26m
24. Lipid Metabolism1h 45m
25. Protein and Amino Acid Metabolism1h 37m
26. Nucleic Acids and Protein Synthesis2h 54m

5. Classification & Balancing of Chemical Reactions

Redox Reactions

GOB Chemistry

5. Classification & Balancing of Chemical Reactions

Redox Reactions

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1:04 minutes

Problem 49

Textbook Question

In each of the following, tell whether the substance gains electrons or loses electrons in a redox reaction:
a. An oxidizing agent
b. A reducing agent
c. A substance undergoing oxidation
d. A substance undergoing reduction

Verified step by step guidance

Understand the key concepts: In a redox reaction, oxidation involves the loss of electrons, while reduction involves the gain of electrons. An oxidizing agent is the substance that causes oxidation by gaining electrons, and a reducing agent is the substance that causes reduction by losing electrons.

For part (a): An oxidizing agent gains electrons because it is reduced in the process of oxidizing another substance.

For part (b): A reducing agent loses electrons because it is oxidized in the process of reducing another substance.

For part (c): A substance undergoing oxidation loses electrons, as oxidation is defined as the loss of electrons.

For part (d): A substance undergoing reduction gains electrons, as reduction is defined as the gain of electrons.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Oxidizing Agent

An oxidizing agent is a substance that gains electrons in a redox reaction, causing another substance to be oxidized. By accepting electrons, it undergoes reduction itself. This process is crucial in various chemical reactions, including combustion and respiration, where the oxidizing agent facilitates the transfer of electrons.

Reducing Agent

A reducing agent is a substance that loses electrons in a redox reaction, thereby causing another substance to be reduced. By donating electrons, it undergoes oxidation. Reducing agents are essential in many chemical processes, such as metal extraction and organic synthesis, where they help convert compounds to their reduced forms.

Oxidation and Reduction

Oxidation refers to the process where a substance loses electrons, resulting in an increase in oxidation state. Conversely, reduction is the gain of electrons, leading to a decrease in oxidation state. These two processes are interconnected in redox reactions, where one substance is oxidized while another is reduced, highlighting the conservation of charge.

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Related Practice

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)

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Textbook Question

Potassium, a silvery metal, reacts with bromine, a corrosive, reddish liquid, to yield potassium bromide, a white solid. Write the balanced equation, and identify the oxidizing and reducing agents.

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Textbook Question

Identify each of the following as an oxidation or a reduction:

c. Cr³⁺(aq) + 3e^– → Cr(s)

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Textbook Question

In the mitochondria of human cells, energy is provided by the oxidation and reduction reactions of the iron ions in the cytochromes in electron transport. Identify each of the following as an oxidation or a reduction:

a. Fe³⁺ + e^– → Fe²⁺

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Multiple Choice

Which element is being reduced in the following reaction?

Cr₂O₇^2- + 3 HNO₂ + 5 H⁺→ 2 Cr³⁺ + 3NO₃^- + 4 H₂O

Identify the oxidizing agent and reducing agent from the following redox reaction.

Ba (s) + Cl₂ (g) → BaCl₂ (aq)