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 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

9. Quantum Mechanics

Introduction to Quantum Mechanics

General Chemistry

9. Quantum Mechanics

Introduction to Quantum Mechanics

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Multiple Choice

How many quantum numbers are required to designate a particular orbital?

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Understand that quantum numbers are used to describe the properties of atomic orbitals and the properties of electrons in orbitals.

Recognize that there are four quantum numbers: the principal quantum number (n), the azimuthal quantum number (l), the magnetic quantum number (m_l), and the spin quantum number (m_s).

Identify that to designate a particular orbital, you need the first three quantum numbers: n, l, and m_l.

The principal quantum number (n) indicates the energy level and size of the orbital.

The azimuthal quantum number (l) defines the shape of the orbital, and the magnetic quantum number (m_l) specifies the orientation of the orbital in space.