Table of contents

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1. Intro to General Chemistry3h 48m
2. Atoms & Elements4h 16m
3. Chemical Reactions4h 10m
4. BONUS: Lab Techniques and Procedures1h 36m
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

8. Thermochemistry

Nature of Energy

General Chemistry

8. Thermochemistry

Nature of Energy

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Multiple Choice

In chemical reactions, how is energy typically released?

By decreasing the pressure of the system

Through the breaking of chemical bonds

Through the formation of chemical bonds

By increasing the temperature of the reactants

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Verified step by step guidance

Understand that chemical reactions involve the rearrangement of atoms, which leads to the breaking and forming of chemical bonds.

Recognize that energy is required to break chemical bonds, while energy is released when new bonds are formed.

Consider the concept of bond energy, which is the amount of energy needed to break a bond or the energy released when a bond is formed.

Realize that in exothermic reactions, the energy released from forming new bonds is greater than the energy required to break the initial bonds, resulting in a net release of energy.

Conclude that the typical release of energy in chemical reactions occurs through the formation of chemical bonds, as this process releases energy into the surroundings.