Table of contents

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

20. Electrochemistry

Cell Notation

General Chemistry

20. Electrochemistry

Cell Notation

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Multiple Choice

Write the half reactions as well as the overall net ionic equation for the following line notation:
Fe (s) | Fe²⁺(aq) || Mg²⁺(aq) | Mg (s)

Anode: Fe (s) → Fe²⁺ (aq) + 2e^-

Cathode: Mg²⁺ (aq) + 2e^- → Mg (s)

Overall: Fe (s) + Mg²⁺ (aq) → Fe²⁺ (aq) + Mg (s)

Anode: Fe (s) → Fe²⁺ (aq) + 2e^-

Cathode: Mg²⁺ (aq) + 2e^- → Mg (s)

Overall: Fe²⁺ (aq) + Mg (s) → Fe (s) + Mg²⁺ (aq)

Anode: Fe (s) → Fe²⁺ (aq) + 2e^-

Cathode: Mg (s) → Mg²⁺ (aq) + 2e^-

Overall: Fe (s) + Mg²⁺ (aq) → Fe²⁺ (aq) + Mg (s)

Anode: Fe²⁺ (aq) + 2e^- → Fe (s)

Cathode: Mg²⁺ (aq) + 2e^- → Mg (s)

Overall: Fe (s) + Mg²⁺ (aq) → Fe²⁺ (aq) + Mg (s)

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Verified step by step guidance

Identify the components of the line notation: Fe (s) | Fe2+ (aq) || Mg2+ (aq) | Mg (s). The single vertical line '|' separates different phases, while the double vertical line '||' represents the salt bridge or membrane separating the two half-cells.

Determine the oxidation and reduction processes. Oxidation occurs at the anode, where Fe (s) is converted to Fe2+ (aq) by losing electrons. Reduction occurs at the cathode, where Mg2+ (aq) gains electrons to form Mg (s).

Write the oxidation half-reaction for the anode: Fe (s) → Fe2+ (aq) + 2e-. This shows the loss of electrons by iron as it is oxidized.

Write the reduction half-reaction for the cathode: Mg2+ (aq) + 2e- → Mg (s). This shows the gain of electrons by magnesium ions as they are reduced.

Combine the two half-reactions to write the overall net ionic equation: Fe (s) + Mg2+ (aq) → Fe2+ (aq) + Mg (s). This represents the complete redox reaction occurring in the electrochemical cell.