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MCAT Test Prep General Chemistry Review Study Guide Part 1
>> YOUR LINK HERE: ___ http://youtube.com/watch?v=gzlVacEHVuw
This online video course tutorial focuses on the general chemistry section of the mcat. This video provides a lecture filled with notes and a sheet of formula and equations that will be useful as well as the fundamental concepts that go with. This study guide / review will help you to learn the most important topics in chemistry that you need to do well the physical science part of the MCAT. It has plenty of example problems and practice questions for you to test your knowledge on. • MCAT General Chemistry Part 1 - 8.5 Hour Review: • https://bit.ly/3xEWUuI • MCAT General Chemistry Part 2 - 7.5 Hour Review: • https://bit.ly/4awPGaI • MCAT Organic Chemistry Reactions Part 1 - 4 Hour Review: • https://bit.ly/43WXZuf • MCAT Organic Chemistry Reactions Part 2 - 5 Hour Review: • https://bit.ly/3TQXzkp • • • Here is a list of topics: • 1. Atoms, Molecules, Pure Elements, Ionic and Covalent Compounds • 2. Subatomic Particles – Electrons, Protons, and Neutrons • 3. The difference between an atom and an ion • 4. Cations vs Anions – Positive vs Negative Charged Ions • 5. Pure Substance and Mixtures – Homogeneous and Heterogeneous • 6. Density Practice Problems – Unit Conversion and Dimensional Analysis • 7. Temperature Conversions – Celsius, Fahrenheit, and Kelvin • 8. Atomic Number, Mass Number, and Charge • 9. Isotopes – C12 and C13 – Hydrogen, Deuterium and Tritium • 10. Allotropes of Carbon – Diamond and Graphite • 11. Alloys of Metals – Bronze, Brass, Steel, and Nichrome Wire • 12. 7 Diatomic Elements – H2, N2, O2, F2, Cl2, Br2, and I2 • 13. Monoatomic vs Polyatomic Ions – List to Memorize • 14. Nomenclature of Ionic and Molecular Compounds • 15. How To Write The Formula of Ionic and Covalent Compounds • 16. Strong and Weak Acids vs Strong and Weak Bases • 17. The pH Scale – Acidic vs Basic Conditions • 18. How To Name Acids – Nomenclature How To Write the Formula of an Acid • 19. Acid Base Conjugate Pairs – Conjugate Acid vs Conjugate Base • 20. Arrhenius Acid vs Arrhenius Base – H3O+ Hydronium Ions vs Hydroxide OH- Ions • 21. Bronsted Lowry Acid vs Bronsted Lowry Base – Proton Donors vs Proton Accetors • 22. Lewis Acid vs Lewis Base – Electron Pair Acceptors and Electron Pair Donors • 23. Acid water reaction vs base water reaction – reversible vs irreversible reactions – 1 or 2 arrows • 24. Acid Base Dissociation Reactions • 25. Molar Mass – Atomic mass, Molecular Weight and Formula Weight Calculations • 26. Mass Percent and Percent Composition Equation • 27. Grams to Moles Conversion and Moles to Gram • 28. Mole to Mole and Gram to Gram Stoichiometry • 29. Actual Yield, Theoretical Yield, Percent Yield and Percent Error Calculations • 30. How To Calculate The Amount of Excess Reactant That Remains • 31. How To Identify the Limiting and Excess Reactant • 32. Empirical Formula and Molecular Formula Determination Given Grams or Percent Composition • 33. Empirical Formula – Combusion Analysis • 34. Solubility Rules – Soluble vs Insoluble – Aqueous vs Solid Phase • 35. Strong, Weak and Nonelectrolytes – Electrical Conductivity of Solutions • 36. Concentration and Molarity Calculations – Moles of Solute and Liters of Solution • 37. Dilution Examples Problems – M1V1 M2V2 – Molarity, Volume and Mass in grams • 38. Solution Stoichiometry – Limiting and Excess Reactant – Theoretical Yield Calculations • 39. Acid Base Titration Problems – M1V1=M2V2 • 40. Chemical Reactions – Synthesis, Combination, Decomposition, Combustion, Redox Reactions, Single Replacement, Double Replacement Reactions, Acid Base Neutralization, Precipitation Reactions, and Gas Evolution Reactions • 41. Net Ionic Equations – Total Ionic and Molecular Equations – Spectator Ions • 42. Combined Gas Law Formula and Ideal Gas Law Equation – PV=nRT • 43. Boyle’s Law, Charles Law, Gay Lussac’s Law and Avogadro’s Law • 44. Pressure, Temperature, Volume and Moles – Direct vs Inverse Relationship • 45. Gas Density and Molar Mass Example Problems • 46. Dalton’s Law of Partial Pressures and Graham’s Law of Effusion • 47. Average Kinetic Energy of a Gas vs Temperature • 48. Partial Pressure, Mole Fraction, and Vapor Pressure • 49. Gas Law Stoichiometry Problems – STP – Standard Temperature and Pressure • 50. Molar Volume – 1 mole of gas = 22.4 Liters • 51. Kinetic Molecular Theory of Gases Postulate • 52. Units of Pressure – Torr, mm Hg, atm, Kpa, and Pa.
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