CHEM 1040
University of Guelph
Course Overview
Grade Boosters
Lessons & Practice
I. Welcome
1 min1. Review: Measurement/ Significant Figures / Atoms, Molecules and Ions
57min2. Atomic Structure / Periodic Trends / Lewis Structures / VSEPR and Bonding
8hr2.1.1. Electromagnetic Spectrum2 min2.1.2. Photon Equations5 min2.1.3. Photon Equations (Cntd.)9 min2.1.4. Example4 min2.1.5. Example3 min2.1.6. Practice1 min2.1.7. Practice4 min2.1.8. The Photoelectric Effect8 min2.1.9. The Photoelectric Effect Equation11 min2.1.10. Example5 min2.1.11. Practice3 min2.1.12. Practice5 min2.1.13. The Basics of Absorption and Emission Spectra3 min2.1.14. Bohr's Atomic Model 12 min2.1.15. Absorption vs Emission of a Photon3 min2.1.16. Example4 min2.1.17. Example3 min2.1.18. Wave-Particle Duality 8 min2.1.19. Example1 min2.1.20. Practice2.1.21. Practice3 min2.1.22. The Bohr Model Vs The Quantum Model6 min2.1.23. Quantum Numbers11 min2.1.24. Quantum Numbers Cheatsheet2.1.25. Example3 min2.1.26. Example5 min2.1.27. Example1 min2.1.28. Practice1 min2.1.29. Shapes (aka Boundary Diagrams) of Atomic Orbitals7 min2.1.30. Drawing Atomic Orbitals7 min2.1.31. Example3 min2.1.32. Practice2.1.33. Electronic Configurations of Atoms11 min2.1.34. Electron Configurastions Cheatsheet2.1.35. Electron Configuration Exceptions5 min2.1.36. Example3 min2.1.37. Example3 min2.1.38. Practice2.1.39. Practice4 min2.1.40. Practice 2.1.41. Electron Configurations of Ions of Main Group Elements9 min2.1.42. Electron Configuration of Ions of Transition Elements2 min2.1.43. Example5 min2.1.44. Example5 min2.1.45. Practice3 min2.1.46. Diamagnetic Vs Paramagnetic 7 min2.1.47. Example8 min2.1.48. Practice
2.2.1. Atomic Radius7 min2.2.2. Atomic Radius Theory7 min2.2.3. Example2 min2.2.4. Example3 min2.2.5. Practice1 min2.2.6. Ionization Energy 5 min2.2.7. Comparing 1st, 2nd, and 3rd Ionization Energies9 min2.2.8. Practice2 min2.2.9. Practice2 min2.2.10. Practice5 min2.2.11. Electron Affinity 10 min2.2.12. Example2 min2.2.13. Practice2 min2.2.14. Practice4 min2.2.15. Effective Nuclear Charge 9 min2.2.16. Example1 min2.2.17. Practice2 min
2.3.1. Drawing Lewis Structures 17 min2.3.2. Example11 min2.3.3. Example7 min2.3.4. Practice2.3.5. Practice7 min2.3.6. Electronegativity 4 min2.3.7. Example47 sec2.3.8. Practice3 min2.3.9. Resonance Structures Theory7 min2.3.10. Equivalent Vs Non-Equivalent Resonance Structures5 min2.3.11. Example7 min2.3.12. Example13 min2.3.13. Practice2.3.14. Practice
2.4.1. VSEPR Theory20 min2.4.2. Example10 min2.4.3. Example6 min2.4.4. Practice 2.4.5. Practice2.4.6. VSEPR and Molecular Shapes Cheatsheet2.4.7. Review of Polar Covalent Bonds2.4.8. Molecular Polarity 8 min2.4.9. Example8 min2.4.10. Practice2.4.11. Practice3 min2.4.12. Introduction to Valence Bond Theory6 min2.4.13. Example: Valence Bond Theory4 min2.4.14. Introduction to Hybridization5 min2.4.15. Determining Hybridization7 min2.4.16. Example8 min2.4.17. Example4 min2.4.18. Practice2.4.19. Sigma and Pi Bonds2 min2.4.20. Sigma and Pi Bonds 3 min2.4.21. Practice
3. The Mole / Stoichiometry / Chemical Reactions
4hr3.2.1. Balancing Reactions3 min3.2.2. Intro to Stoichiometry4 min3.2.3. Stoichiometry: Putting it All Together6 min3.2.4. Example5 min3.2.5. Example6 min3.2.6. Practice6 min3.2.7. Practice7 min3.2.8. Mass Percentage2 min3.2.9. Example3.2.10. Practice3.2.11. Empirical Vs Molecular Formulas1 min3.2.12. Example3.2.13. Example #17 min3.2.14. Example #25 min3.2.15. Practice3.2.16. Practice3.2.17. Introduction to Limiting Reagents5 min3.2.18. Example5 min3.2.19. Example3 min3.2.20. Example7 min3.2.21. Practice3 min3.2.22. Percent Yield 5 min3.2.23. Example7 min3.2.24. Practice5 min3.2.25. Practice
3.3.1. Solubility Chart 8 min3.3.2. Example5 min3.3.3. Example5 min3.3.4. Practice3.3.5. Definitions of Acids and Bases 3 min3.3.6. Acids 2 min3.3.7. Bases2 min3.3.8. Neutralization Reactions3.3.9. Three Ways to Write Out Chemical Reactions11 min3.3.10. Practice3.3.11. Relating Net Ionic Equations to Ionization of Acids and Bases8 min3.3.12. Solution Properties3 min3.3.13. Solutions4 min3.3.14. Practice3.3.15. Titration Problem Introduction4 min3.3.16. Example7 min3.3.17. Measurable Properties of Gases8 min3.3.18. Gas Laws7 min3.3.19. Molar Volume4 min3.3.20. Example: Pressure Conversions3 min3.3.21. Example: Gas Laws2 min3.3.22. Example: Molar Volume3 min3.3.23. Practice Level 155 sec3.3.24. Practice Level 22 min3.3.25. Practice Level 33 min3.3.26. The Ideal Gas Law5 min3.3.27. Example2 min3.3.28. Example7 min3.3.29. Practice8 min
4. Equilibrium
2.3hr4.1.1. Introduction to Equilibrium 2 min4.1.2. Understanding Equilibrium3 min4.1.3. Concentration vs Time Graphs4 min4.1.4. Practice3 min4.1.5. Practice6 min4.1.6. Equilibrium Constant (K)10 min4.1.7. The Magnitude of the Equilibrium Constant, K8 min4.1.8. Practice2 min4.1.9. Practice4 min4.1.10. Solving for Kc vs Kp 5 min4.1.11. Manipulating Equilibrium Constants5 min4.1.12. Practice7 min4.1.13. Predicting Equilibria: The Reaction Quotient (Q) 6 min4.1.14. Example4 min4.1.15. Practice3 min4.1.16. Practice4.1.17. Intro to ICE Tables4.1.18. Example 19 min4.1.19. Example 29 min4.1.20. Example 33 min4.1.21. Example 49 min4.1.22. Example 512 min4.1.23. Le Chatelier's Priniciple14 min4.1.24. Practice6 min4.1.25. Practice
5. Acids and Bases / Salts and Buffers / Titration Curves
5hr5.1.1. Definitions of Acids and Bases 10 min5.1.2. Identifying Conjugate Acid and Base Pairs 7 min5.1.3. Practice2 min5.1.4. Relationships Between the Strength of an Acid/Base and its Conjugate Base/Acid5 min5.1.5. How to Tell the Stronger Acid by Looking at Conjugate Bases14 min5.1.6. Acidity of Oxyacids4 min5.1.7. Autoionization of Water (Kw) 4 min5.1.8. pH Scale 7 min5.1.9. Example2 min5.1.10. Example6 min5.1.11. Practice5.1.12. Indicators8 min5.1.13. Practice5.1.14. Acids and their Equations7 min5.1.15. Practice4 min5.1.16. Bases and their Equations6 min5.1.17. Types of Acid or Base Reactions and pH Calculations Summary5.1.18. Example5.1.19. Example21 min5.1.20. Percent Ionization or Dissociation4 min5.1.21. Example: Percent Ionization4 min5.1.22. Acid Base Equations Cheatsheet5.1.23. Acid/Base Important Relationships Cheatsheet
5.2.1. Acidic, Basic, and Neutral Salts 8 min5.2.2. Salts (Cntd.)3 min5.2.3. Example1 min5.2.4. Practice5.2.5. Salts Cheatsheet5.2.6. Example5 min5.2.7. Strong Base + Strong Acid Reactions3 min5.2.8. Strong Base + Weak Acid Reactions4 min5.2.9. Weak Base + Strong Acid Reactions3 min5.2.10. Practice9 min5.2.11. Introduction to Buffers6 min5.2.12. Buffers Problem Type 16 min5.2.13. Example3 min5.2.14. Buffers Problem Type 22 min5.2.15. Example6 min5.2.16. Buffers Problem Type 32 min5.2.17. Example6 min5.2.18. Practice5.2.19. Example5 min5.2.20. Forming Buffers6 min5.2.21. Example4 min5.2.22. Example2 min5.2.23. Effective Buffer Range5 min5.2.24. Practice2 min
6. Introduction to Organic Chemistry / Intermolecular Forces
1.5hr6.1.1. What is Organic Chemistry?2 min6.1.2. Line Bond Drawing6 min6.1.3. Concept Clarifier6.1.4. Hydrocarbons2 min6.1.5. Naming Simple Hydrocarbons4 min6.1.6. Hydrocarbon Example2 min6.1.7. Practice: Hydrocarbon Naming6.1.8. Practice: Hydrocarbon Naming 26.1.9. Functional Groups3 min6.1.10. 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 Theory2 min6.1.16. Addition Polymerization4 min6.1.17. Polymer Formation Questions6.1.18. Practice: Identify the Monomer6.1.19. Condensation Polymers Theory5 min6.1.20. Practice: Identify the Monomer #2
6.2.1. Intramolecular vs Intermolecular Forces5 min6.2.2. Intermolecular Forces Theory15 min6.2.3. Example6.2.4. Example 6.2.5. Practice9 min6.2.6. Phases of Matter3 min6.2.7. Intermolecular Forces and Boiling Point11 min6.2.8. Other Physical Properties and Intermolecular Forces6 min6.2.9. Example9 min6.2.10. Example4 min6.2.11. 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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