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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 38m
5. BONUS: Mathematical Operations and Functions48m
6. Chemical Quantities & Aqueous Reactions3h 53m
7. Gases3h 49m
8. Thermochemistry2h 37m
9. Quantum Mechanics2h 58m
10. Periodic Properties of the Elements3h 9m
11. Bonding & Molecular Structure3h 29m
12. Molecular Shapes & Valence Bond Theory1h 57m
13. Liquids, Solids & Intermolecular Forces2h 23m
14. Solutions3h 1m
15. Chemical Kinetics2h 53m
16. Chemical Equilibrium2h 29m
17. Acid and Base Equilibrium5h 1m
18. Aqueous Equilibrium4h 47m
19. Chemical Thermodynamics1h 50m
20. Electrochemistry2h 42m
21. Nuclear Chemistry2h 36m
22. Organic Chemistry5h 7m
23. Chemistry of the Nonmetals2h 39m
24. Transition Metals and Coordination Compounds3h 16m

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

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Multiple Choice

What element is undergoing reduction in the following reaction? Zn(s) + 2 AgNO3(aq) → Zn(NO3)2(aq) + 2 Ag(s)

Zinc (Zn)

Nitrogen (N)

Silver (Ag)

Oxygen (O)

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Verified step by step guidance

Identify the oxidation states of each element in the reactants and products. For example, in Zn(s), the oxidation state of Zn is 0, and in Zn(NO3)2, the oxidation state of Zn is +2.

Determine the oxidation state of Ag in AgNO3. In AgNO3, Ag has an oxidation state of +1.

Determine the oxidation state of Ag in the products. In the product 2 Ag(s), the oxidation state of Ag is 0.

Compare the oxidation states of Ag in the reactants and products. Notice that the oxidation state of Ag changes from +1 in AgNO3 to 0 in Ag(s).

Conclude that the element undergoing reduction is the one whose oxidation state decreases. Since the oxidation state of Ag decreases from +1 to 0, Ag is the element undergoing reduction.