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

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

General Chemistry

6. Chemical Quantities & Aqueous Reactions

Redox Reactions

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Multiple Choice

Which of the following chemical equations represent oxidation-reduction reactions?

3) AgNO3(aq) + NaI(aq) → AgI(s) + NaNO3(aq)

2) 2 H2(g) + O2(g) → 2 H2O(l)

1) Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s)

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Verified step by step guidance

Step 1: Understand the concept of oxidation-reduction (redox) reactions. These are reactions where there is a transfer of electrons between species, leading to changes in oxidation states.

Step 2: Identify the oxidation states of each element in the reactants and products for each equation. This will help determine if there is a change in oxidation state, indicating a redox reaction.

Step 3: For equation 1) Zn(s) + CuSO4(aq) → ZnSO4(aq) + Cu(s), assign oxidation states: Zn is 0 in Zn(s) and +2 in ZnSO4(aq); Cu is +2 in CuSO4(aq) and 0 in Cu(s). Notice the change in oxidation states, indicating a redox reaction.

Step 4: For equation 2) 2 H2(g) + O2(g) → 2 H2O(l), assign oxidation states: H is 0 in H2(g) and +1 in H2O(l); O is 0 in O2(g) and -2 in H2O(l). Notice the change in oxidation states, indicating a redox reaction.

Step 5: For equation 3) AgNO3(aq) + NaI(aq) → AgI(s) + NaNO3(aq), assign oxidation states: Ag is +1 in AgNO3(aq) and +1 in AgI(s); Na is +1 in NaI(aq) and +1 in NaNO3(aq); I is -1 in NaI(aq) and -1 in AgI(s). There is no change in oxidation states, indicating it is not a redox reaction.