CHEM 1A03
Mac
Course Overview
Grade Boosters
Lessons & Practice
I. Welcome
1. Unit 1 and 2: Fundamental Skills Review
4hr2. Unit 3: Atomic Structure and Theory
5hr2.2.1. Quantum Numbers2.2.2. Quantum Numbers Cheatsheet2.2.3. Example2.2.4. Example2.2.5. Example2.2.6. Practice2.2.7. Shapes (aka Boundary Diagrams) of Atomic Orbitals2.2.8. Drawing Atomic Orbitals2.2.9. Example2.2.10. Practice2.2.11. Angular and Radial Nodes2.2.12. Wave Properties of Electrons2.2.13. Plotting Radial Electron Probability2.2.14. Example2.2.15. Example2.2.16. Example2.2.17. Practice2.2.18. Relative Energies of Atomic Orbitals2.2.19. Rules for Orbital Filling2.2.20. Example2.2.21. Example2.2.22. Practice2.2.23. Practice
2.3.1. The Basics of Absorption and Emission Spectra2.3.2. Bohr's Atomic Model 2.3.3. Absorption vs Emission of a Photon2.3.4. Example2.3.5. Example2.3.6. Bohr Model Equations2.3.7. Example2.3.8. Example2.3.9. Practice 2.3.10. The Bohr Model and Atomic Line Spectra2.3.11. Relating Electronic Transitions to Emission Spectra2.3.12. Example2.3.13. Practice2.3.14. Practice
2.6.1. Electronic Configurations of Atoms2.6.2. Electron Configurastions Cheatsheet2.6.3. Electron Configuration Exceptions2.6.4. Example2.6.5. Example2.6.6. Practice2.6.7. Practice2.6.8. Practice 2.6.9. Electron Configurations of Ions of Main Group Elements2.6.10. Electron Configuration of Ions of Transition Elements2.6.11. Example2.6.12. Example2.6.13. Practice2.6.14. Diamagnetic Vs Paramagnetic 2.6.15. Example2.6.16. Practice2.6.17. Ground State Vs Excited State Electron Configurations2.6.18. Example2.6.19. Example2.6.20. Practice2.6.21. Practice
3. Unit 4: Periodic Table Trends
2.8hr4. Unit 5: Chemical Bonding
3hr5. Unit 6: Solubility and Chemical Equilibrium
3hr5.3.1. Three Ways to Write Out Chemical Reactions5.3.2. Practice5.3.3. Relating Net Ionic Equations to Ionization of Acids and Bases5.3.4. Introduction to Equilibrium 5.3.5. Understanding Equilibrium5.3.6. Equilibrium Constant (K)5.3.7. The Magnitude of the Equilibrium Constant, K5.3.8. Practice5.3.9. Practice5.3.10. Predicting Equilibria: The Reaction Quotient (Q) 5.3.11. Example5.3.12. Practice5.3.13. Practice
5.6.1. Solubility5.6.2. Example: Ksp5.6.3. Practice: Calculating Molar Solubility5.6.4. Practice: Solubility5.6.5. Factors that Affect Solubility5.6.6. Practice: Ranking Solubility5.6.7. Common-ion Effect Introduction5.6.8. Common-ion Effect Problem 5.6.9. common-ion effect5.6.10. Practice: Molar Solubility
6. Unit 7: Acids and Bases
2.2hr7. Unit 8: Thermodynamics
3hr- 7.I. Chapter Intro
7.4.1. Heat, Work, and Internal Energy Continued 7.4.2. Practice: Summary For Exam!7.4.3. Enthalpy7.4.4. Energy Equations for Gases 7.4.5. deltaH and deltaU7.4.6. Practice: deltaH and q7.4.7. Exam Like Practice Problem 7.4.8. Monoatomic and Diatomic Ideal Gases 7.4.9. Exam Like Practice Problem #27.4.10. Exam Like Practice Problem #37.4.11. Exam-Like Practice Problem #47.4.12. Calorimetry7.4.13. Example: Monoatomic Gas Question7.4.14. Practice7.4.15. Practice
8. Unit 9: Phase Transitions and Phase Diagrams
1hr9. Unit 10: Entropy and Free Energy
42min9.2.1. Gibbs Free Energy and Spontaneity (w/o chemical potential)9.2.2. Spontaneity 9.2.3. Example: Spontaneity of a Reaction9.2.4. Predicting Spontaneity Based off Entropy9.2.5. Chemical Equilibrium and ΔG Equations9.2.6. DeltaGo and K 9.2.7. Chemical Equilibrium and ΔG Practice 9.2.8. Chemical Equilibrium and ΔG Practice #29.2.9. Chemical Equilibrium and ΔG Practice #39.2.10. Van't Hoff Practice Problem
10. Unit 11: Electrochemistry
2.4hr11. Unit 12: Intermolecular Forces and Physical Properties
2.9hrTerm Test 2 Overview
Available Term Test 2 Grade Boosters
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Course Notes
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