CHEM*1040
University of Guelph
Course Overview
Grade Boosters
Lessons & Practice
I. Welcome
1. Review: Measurement/ Significant Figures / Atoms, Molecules and Ions
57min2. Atomic Structure / Periodic Trends / Lewis Structures / VSEPR and Bonding
8hr2.1.1. Electromagnetic Spectrum2.1.2. Photon Equations2.1.3. Photon Equations (Cntd.)2.1.4. Example2.1.5. Example2.1.6. Practice2.1.7. Practice2.1.8. The Photoelectric Effect2.1.9. The Photoelectric Effect Equation2.1.10. Example2.1.11. Practice2.1.12. Practice2.1.13. The Basics of Absorption and Emission Spectra2.1.14. Bohr's Atomic Model 2.1.15. Absorption vs Emission of a Photon2.1.16. Example2.1.17. Example2.1.18. Wave-Particle Duality 2.1.19. Example2.1.20. Practice2.1.21. Practice2.1.22. The Bohr Model Vs The Quantum Model2.1.23. Quantum Numbers2.1.24. Quantum Numbers Cheatsheet2.1.25. Example2.1.26. Example2.1.27. Example2.1.28. Practice2.1.29. Shapes (aka Boundary Diagrams) of Atomic Orbitals2.1.30. Drawing Atomic Orbitals2.1.31. Example2.1.32. Practice2.1.33. Electronic Configurations of Atoms2.1.34. Electron Configurastions Cheatsheet2.1.35. Electron Configuration Exceptions2.1.36. Example2.1.37. Example2.1.38. Practice2.1.39. Practice2.1.40. Practice 2.1.41. Electron Configurations of Ions of Main Group Elements2.1.42. Electron Configuration of Ions of Transition Elements2.1.43. Example2.1.44. Example2.1.45. Practice2.1.46. Diamagnetic Vs Paramagnetic 2.1.47. Example2.1.48. Practice
2.2.1. Atomic Radius2.2.2. Atomic Radius Theory2.2.3. Example2.2.4. Example2.2.5. Practice2.2.6. Ionization Energy 2.2.7. Comparing 1st, 2nd, and 3rd Ionization Energies2.2.8. Practice2.2.9. Practice2.2.10. Practice2.2.11. Electron Affinity 2.2.12. Example2.2.13. Practice2.2.14. Practice2.2.15. Effective Nuclear Charge 2.2.16. Example2.2.17. Practice
2.4.1. VSEPR Theory2.4.2. Example2.4.3. Example2.4.4. Practice 2.4.5. Practice2.4.6. VSEPR and Molecular Shapes Cheatsheet2.4.7. Review of Polar Covalent Bonds2.4.8. Molecular Polarity 2.4.9. Example2.4.10. Practice2.4.11. Practice2.4.12. Introduction to Valence Bond Theory2.4.13. Example: Valence Bond Theory2.4.14. Introduction to Hybridization2.4.15. Determining Hybridization2.4.16. Example2.4.17. Example2.4.18. Practice2.4.19. Sigma and Pi Bonds2.4.20. Sigma and Pi Bonds 2.4.21. Practice
3. The Mole / Stoichiometry / Chemical Reactions
4hr3.2.1. Balancing Reactions3.2.2. Intro to Stoichiometry3.2.3. Stoichiometry: Putting it All Together3.2.4. Example3.2.5. Example3.2.6. Practice3.2.7. Practice3.2.8. Mass Percentage3.2.9. Example3.2.10. Practice3.2.11. Empirical Vs Molecular Formulas3.2.12. Example3.2.13. Example #13.2.14. Example #23.2.15. Practice3.2.16. Practice3.2.17. Introduction to Limiting Reagents3.2.18. Example3.2.19. Example3.2.20. Example3.2.21. Practice3.2.22. Percent Yield 3.2.23. Example3.2.24. Practice3.2.25. Practice
3.3.1. Solubility Chart 3.3.2. Example3.3.3. Example3.3.4. Practice3.3.5. Definitions of Acids and Bases 3.3.6. Acids 3.3.7. Bases3.3.8. Neutralization Reactions3.3.9. Three Ways to Write Out Chemical Reactions3.3.10. Practice3.3.11. Relating Net Ionic Equations to Ionization of Acids and Bases3.3.12. Solution Properties3.3.13. Solutions3.3.14. Practice3.3.15. Titration Problem Introduction3.3.16. Example3.3.17. Measurable Properties of Gases3.3.18. Gas Laws3.3.19. Molar Volume3.3.20. Example: Pressure Conversions3.3.21. Example: Gas Laws3.3.22. Example: Molar Volume3.3.23. Practice Level 13.3.24. Practice Level 23.3.25. Practice Level 33.3.26. The Ideal Gas Law3.3.27. Example3.3.28. Example3.3.29. Practice
4. Equilibrium
2.3hr4.1.1. Introduction to Equilibrium 4.1.2. Understanding Equilibrium4.1.3. Concentration vs Time Graphs4.1.4. Practice4.1.5. Practice4.1.6. Equilibrium Constant (K)4.1.7. The Magnitude of the Equilibrium Constant, K4.1.8. Practice4.1.9. Practice4.1.10. Solving for Kc vs Kp 4.1.11. Manipulating Equilibrium Constants4.1.12. Practice4.1.13. Predicting Equilibria: The Reaction Quotient (Q) 4.1.14. Example4.1.15. Practice4.1.16. Practice4.1.17. Intro to ICE Tables4.1.18. Example 14.1.19. Example 24.1.20. Example 34.1.21. Example 44.1.22. Example 54.1.23. Le Chatelier's Priniciple4.1.24. Practice4.1.25. Practice
5. Acids and Bases / Salts and Buffers / Titration Curves
5hr5.1.1. Definitions of Acids and Bases 5.1.2. Identifying Conjugate Acid and Base Pairs 5.1.3. Practice5.1.4. Relationships Between the Strength of an Acid/Base and its Conjugate Base/Acid5.1.5. How to Tell the Stronger Acid by Looking at Conjugate Bases5.1.6. Acidity of Oxyacids5.1.7. Autoionization of Water (Kw) 5.1.8. pH Scale 5.1.9. Example5.1.10. Example5.1.11. Practice5.1.12. Indicators5.1.13. Practice5.1.14. Acids and their Equations5.1.15. Practice5.1.16. Bases and their Equations5.1.17. Types of Acid or Base Reactions and pH Calculations Summary5.1.18. Example5.1.19. Example5.1.20. Percent Ionization or Dissociation5.1.21. Example: Percent Ionization5.1.22. Acid Base Equations Cheatsheet5.1.23. Acid/Base Important Relationships Cheatsheet
5.2.1. Acidic, Basic, and Neutral Salts 5.2.2. Salts (Cntd.)5.2.3. Example5.2.4. Practice5.2.5. Salts Cheatsheet5.2.6. Example5.2.7. Strong Base + Strong Acid Reactions5.2.8. Strong Base + Weak Acid Reactions5.2.9. Weak Base + Strong Acid Reactions5.2.10. Practice5.2.11. Introduction to Buffers5.2.12. Buffers Problem Type 15.2.13. Example5.2.14. Buffers Problem Type 25.2.15. Example5.2.16. Buffers Problem Type 35.2.17. Example5.2.18. Practice5.2.19. Example5.2.20. Forming Buffers5.2.21. Example5.2.22. Example5.2.23. Effective Buffer Range5.2.24. Practice
6. Introduction to Organic Chemistry / Intermolecular Forces
1.5hr6.1.1. What is Organic Chemistry?6.1.2. Line Bond Drawing6.1.3. Concept Clarifier6.1.4. Hydrocarbons6.1.5. Naming Simple Hydrocarbons6.1.6. Hydrocarbon Example6.1.7. Practice: Hydrocarbon Naming6.1.8. Practice: Hydrocarbon Naming 26.1.9. Functional Groups6.1.10. Identifying Functional Groups Problem 16.1.11. Functional Groups of Vitamin C6.1.12. Practice: Identifying Functional Groups6.1.13. Practice Question6.1.14. Functional Groups6.1.15. Polymers Theory6.1.16. Addition Polymerization6.1.17. Polymer Formation Questions6.1.18. Practice: Identify the Monomer6.1.19. Condensation Polymers Theory6.1.20. Practice: Identify the Monomer #2
6.2.1. Intramolecular vs Intermolecular Forces6.2.2. Intermolecular Forces Theory6.2.3. Example6.2.4. Example 6.2.5. Practice6.2.6. Phases of Matter6.2.7. Intermolecular Forces and Boiling Point6.2.8. Other Physical Properties and Intermolecular Forces6.2.9. Example6.2.10. Example6.2.11. Practice6.2.12. Practice
CHEM*1040 Flashcards
1/86
Dalton's Atomic Theory
Describes matter in terms of atoms where each element is composed of identical atoms, different elements have different types of atoms, atoms combine in specific ratios to form compounds, and atoms are indivisible in chemical processes.
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