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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3: minutes

Problem 9

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.

Verified step by step guidance

Step 1: Write the unbalanced chemical equation for the reaction. Potassium (K) reacts with bromine (Br₂) to form potassium bromide (KBr). The unbalanced equation is:

K + {Br}_{2} \to KBr

Step 2: Balance the equation by ensuring the number of atoms of each element is the same on both sides. Potassium and bromine are diatomic in their elemental forms, so you need to balance the equation as follows:

2 K + {Br}_{2} \to 2 KBr

Step 3: Identify the oxidizing agent. Bromine (Br₂) gains electrons during the reaction, transforming into bromide ions (Br⁻). Since bromine is reduced, it acts as the oxidizing agent.

Step 4: Identify the reducing agent. Potassium (K) loses electrons during the reaction, transforming into potassium ions (K⁺). Since potassium is oxidized, it acts as the reducing agent.

Step 5: Summarize the reaction. Potassium is oxidized (loses electrons) and bromine is reduced (gains electrons). The balanced equation is

2 K + {Br}_{2} \to 2 KBr

, with potassium as the reducing agent and bromine as the oxidizing agent.

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Key Concepts

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

Balancing Chemical Equations

Balancing chemical equations involves ensuring that the number of atoms for each element is the same on both sides of the equation. This reflects the law of conservation of mass, which states that matter cannot be created or destroyed in a chemical reaction. In this case, potassium (K) and bromine (Br) react to form potassium bromide (KBr), and the equation must be balanced to accurately represent the reaction.

Oxidation and Reduction

Oxidation and reduction are processes that involve the transfer of electrons between substances. Oxidation refers to the loss of electrons, while reduction refers to the gain of electrons. In the reaction between potassium and bromine, potassium is oxidized (loses electrons) and bromine is reduced (gains electrons), allowing for the identification of the oxidizing agent (bromine) and the reducing agent (potassium).

Identifying Oxidizing and Reducing Agents

The oxidizing agent is the substance that causes oxidation by accepting electrons, while the reducing agent is the substance that causes reduction by donating electrons. In the given reaction, potassium acts as the reducing agent because it donates electrons, and bromine acts as the oxidizing agent because it accepts those electrons. Understanding these roles is crucial for analyzing redox reactions.

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Related Practice

Multiple Choice

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

Ba (s) + Cl₂ (g) → BaCl₂ (aq)

Which element is oxidized and which is reduced in the following reaction?

Hg (aq) + HgCl₂ (aq) → Hg₂Cl₂

Which of the following represents an oxidation-reduction reaction?

I. PCl₃ (aq) + Cl₂ (g) → PCl₅ (aq)

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

III. CO₂ (g) + 2 LiOH (aq) → Li₂CO₃ (aq) + H₂O (l)

IV. FeCl₂ (aq) + 2 NaOH (aq) → Fe(OH)₂ (aq) + 2 NaCl (aq)

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

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⁺

813

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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

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Multiple Choice