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Chad's Prep®
Chad's Prep®

DAT, MCAT, OAT & Science Prep

  • Home
  • College Courses
    • High School Chemistry
      • Chad’s High School Chemistry Videos (FREE)
      • Chad’s High School Chemistry Master Course
    • General Chemistry
      • Chad’s General Chemistry Videos (FREE)
      • Chad’s General Chemistry Master Course
    • Organic Chemistry
      • Chad’s Organic Chemistry Videos (FREE)
      • Chad’s Organic Chemistry Master Course
      • Chad’s Organic Chemistry Refresher for the ACS Final Exam
    • General Physics
      • Chad’s General Physics Videos (FREE)
      • Chad’s General Physics Master Course
    • Chad’s Biochemistry Videos (FREE)
    • Chad’s Physical Chemistry Videos (FREE)
    • Ultimate Bundle
  • Pre-Health Courses
    • DAT
    • MCAT
    • OAT
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  • Pricing
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  • Chapter 1 – Matter and Measurement
    • 1.1 Matter
    • 1.2 Significant Figures
    • 1.3 Units and Conversions
  • Chapter 2 – Atoms, Molecules, and Ions
    • 2.1 Atomic Structure and Introduction to the Periodic Table
    • 2.2 Naming Ionic Compounds
    • 2.3 Naming Molecular Compounds
    • 2.4 Naming Acids
  • Chapter 3 – Stoichiometry
    • 3.1 Chemical Reactions & Chemical Equations
    • 3.2 Calculations With Moles
    • 3.3 Mass Percent and Empirical and Molecular Formulas
    • 3.4 Limiting Reagent Calculations
  • Chapter 4 – Aqueous Reactions and Solution Stoichiometry
    • 4.1 Solutions and Electrolytes
    • 4.2 Double Displacement Reactions
    • 4.3 Oxidation-Reduction Reactions
    • 4.4 Molarity and Dilutions
    • 4.5 Solution Stoichiometry
  • Chapter 5 – Thermochemistry
    • 5.1 First Law of Thermodynamics and Enthalpy
    • 5.2 Calorimetry
    • 5.3 Hess’s Law and Enthalpies of Formation
  • Chapter 6 – Electronic Structure
    • 6.1 Nature of Light and the Photoelectric Effect
    • 6.2 Electronic Transitions (Absorption and Emission)
    • 6.3 The de Broglie Relation and the Heisenberg Uncertainty Principle
    • 6.4 Quantum Numbers and Atomic Orbitals
    • 6.5 Electronic Configuration
  • Chapter 7 – Periodic Trends
    • 7.1 Atomic Radius
    • 7.2 Ionization Energy
    • 7.3 Electron Affinity & Electronegativity
    • 7.4 Properties of Elements & Compounds
  • Chapter 8 – Bonding and Lewis Structures
    • 8.1 Ionic Bonding
    • 8.2 Lewis Dot Structures
    • 8.3 Bond Enthalpy
  • Chapter 9 – Molecular Geometry
    • 9.1 VSEPR Theory and Molecular Geometry
    • 9.2 Polarity
    • 9.3 Hybridization
    • 9.4 Sigma and Pi Bonds
    • 9.5 Molecular Orbital Theory
  • Chapter 10 – Gases
    • 10.1 Properties of Gases
    • 10.2 Gas Laws Including the Ideal Gas Law
    • 10.3 Additional Gas Laws
    • 10.4 Real Gases & the Van der Waals Equation
  • Chapter 11 – Intermolecular Forces, Liquids, and Solids
    • 11.1 Intermolecular Forces
    • 11.2 Phase Diagrams
    • 11.3 Structures of Solids
  • Chapter 13 – Solutions
    • 13.1 Solution Formation and Solubility
    • 13.2 Units of Concentration
    • 13.3 Colligative Properties
  • Chapter 14 – Kinetics
    • 14.1 Rate Expressions and the Rate of Reaction
    • 14.2 Rate Laws
    • 14.3 Reaction Mechanisms, Catalysts, and Reaction Coordinate Diagrams
    • 14.4 Collision Theory and the Arrhenius Equation
    • 14.5 Integrated Rate Laws
  • Chapter 15 – Equilibrium
    • 15.1 Equilibrium and Equilibrium Constants
    • 15.2 Le Chatelier’s Principle
    • 15.3 Equilibrium Calculations (ICE Tables)
  • Chapter 16 – Acids and Bases
    • 16.1 Introduction to Acids and Bases
    • 16.2 Binary Acids, Oxoacids, and Polyprotic Acids
    • 16.3 Introduction to the pH Scale and pH Calculations
    • 16.4 pH Calculations for Strong Acids and Bases
    • 16.5 pH Calculations for Weak Acids and Bases
    • 16.6 Acidity and Basicity of Salts
  • Chapter 17 – Buffers, Titrations, and Solubility
    • 17.1 Buffers
    • 17.2 Titrations and Titration Curves
    • 17.3 pH Calculations Involving Titrations
    • 17.4 Solubility and Ksp
    • 17.5 Common Ion Effect and Precipitation
    • 17.6 pH Effects on Solubility
  • Chapter 18 – Thermodynamics
    • 18.1 The Laws of Thermodynamics
    • 18.2 Entropy
    • 18.3 Gibbs Free Energy and the Relationship between ΔG, ΔH, & ΔS
    • 18.4 ΔG, ΔH, ΔS, and Formation Reactions
    • 18.5 Gibbs Free Energy and the Equilibrium Constant
  • Chapter 19 – Electrochemistry
    • 19.1 How to Assign Oxidation Numbers
    • 19.2 How to Balance Oxidation Reduction Reactions
    • 19.3 Galvanic Cells
    • 19.4 How to Calculate Standard Cell Potential
    • 19.5 How to Calculate Nonstandard Cell Potential [Nernst Equation]
    • 19.6 Cell Potential, Delta G, and the Equilibrium Constant
    • 19.7 Electrolytic Cells
    • 19.8 Electrolysis Calculations
  • Chapter 20 – Nuclear Chemistry
    • 20.1 Introduction to Nuclear Chemistry
    • 20.2 Balancing Nuclear Reactions
    • 20.3 Spontaneous Routes of Nuclear Decay, Fission, & Fusion
    • 20.4 Kinetics of Nuclear Decay
    • 20.5 Energy of Nuclear Reactions and Nuclear Binding Energy
  • Chapter 21 – Coordination Chemistry
    • 21.1 Introduction to Coordination Chemistry
    • 21.2 Naming Complex Ions and Coordination Compounds
    • 21.3 Isomers in Coordination Chemistry
    • 21.4 Crystal Field Theory
    • 21.5 Color & Paramagnetism of Coordination Compounds
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