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AP Chemistry Concept List

This file contains 500 concepts for the AP Chemistry learning graph, organized by course unit with foundational and cross-cutting concepts.

Foundational Concepts (1-25)

  1. Matter
  2. Energy
  3. Atoms
  4. Elements
  5. Compounds
  6. Mixtures
  7. Physical Properties
  8. Chemical Properties
  9. Physical Changes
  10. Chemical Changes
  11. Scientific Method
  12. Measurement
  13. SI Units
  14. Significant Figures
  15. Dimensional Analysis
  16. Density
  17. Temperature Scales
  18. Scientific Notation
  19. Accuracy and Precision
  20. Percent Error
  21. Laboratory Safety
  22. Data Collection
  23. Graphing Data
  24. Conservation Laws
  25. Atomic Theory History

Unit 1: Atomic Structure and Properties (26-80)

  1. Subatomic Particles
  2. Protons
  3. Neutrons
  4. Electrons
  5. Atomic Number
  6. Mass Number
  7. Isotopes
  8. Atomic Mass
  9. Average Atomic Mass
  10. Mass Spectrometry
  11. Mass Spectrum Analysis
  12. Relative Abundance
  13. Mole Concept
  14. Avogadro's Number
  15. Molar Mass
  16. Mole Calculations
  17. Percent Composition
  18. Empirical Formula
  19. Molecular Formula
  20. Combustion Analysis
  21. Bohr Model
  22. Quantum Mechanical Model
  23. Energy Levels
  24. Principal Quantum Number
  25. Subshells
  26. Orbitals
  27. Orbital Shapes
  28. Electron Configuration
  29. Aufbau Principle
  30. Pauli Exclusion Principle
  31. Hund's Rule
  32. Valence Electrons
  33. Core Electrons
  34. Noble Gas Notation
  35. Electron Config of Ions
  36. Electromagnetic Spectrum
  37. Wavelength
  38. Frequency
  39. Photon Energy
  40. Planck's Equation
  41. Photoelectric Effect
  42. Emission Spectra
  43. Absorption Spectra
  44. Photoelectron Spectroscopy
  45. PES Data Interpretation
  46. Periodic Table Organization
  47. Periods and Groups
  48. Periodic Trends
  49. Atomic Radius
  50. Ionic Radius
  51. Ionization Energy
  52. Successive Ionization Energy
  53. Electron Affinity
  54. Electronegativity
  55. Effective Nuclear Charge

Unit 2: Molecular and Ionic Compound Structure (81-140)

  1. Chemical Bonds
  2. Ionic Bonds
  3. Covalent Bonds
  4. Metallic Bonds
  5. Bond Formation Energy
  6. Ionic Compounds
  7. Crystal Lattice
  8. Lattice Energy
  9. Cation Formation
  10. Anion Formation
  11. Polyatomic Ions
  12. Naming Ionic Compounds
  13. Writing Ionic Formulas
  14. Transition Metal Ions
  15. Lewis Dot Symbols
  16. Lewis Structures
  17. Octet Rule
  18. Single Bonds
  19. Double Bonds
  20. Triple Bonds
  21. Lone Pairs
  22. Bonding Pairs
  23. Resonance Structures
  24. Resonance Hybrid
  25. Formal Charge
  26. Formal Charge Calculation
  27. Expanded Octets
  28. Incomplete Octets
  29. Exceptions to Octet Rule
  30. Bond Order
  31. Bond Length
  32. Bond Energy
  33. VSEPR Theory
  34. Electron Geometry
  35. Molecular Geometry
  36. Linear Geometry
  37. Trigonal Planar Geometry
  38. Tetrahedral Geometry
  39. Trigonal Bipyramidal
  40. Octahedral Geometry
  41. Bent Geometry
  42. Trigonal Pyramidal
  43. Bond Angles
  44. Lone Pair Repulsion
  45. Orbital Hybridization
  46. sp Hybridization
  47. sp2 Hybridization
  48. sp3 Hybridization
  49. Sigma Bonds
  50. Pi Bonds
  51. Bond Polarity
  52. Electronegativity Difference
  53. Polar Covalent Bonds
  54. Nonpolar Covalent Bonds
  55. Dipole Moment
  56. Molecular Polarity
  57. Polar Molecules
  58. Nonpolar Molecules
  59. Naming Covalent Compounds
  60. Network Covalent Solids

Unit 3: Intermolecular Forces and Properties (141-200)

  1. Intermolecular Forces
  2. Intramolecular Forces
  3. IMF vs Chemical Bonds
  4. London Dispersion Forces
  5. Polarizability
  6. Dipole-Dipole Forces
  7. Hydrogen Bonding
  8. Hydrogen Bond Requirements
  9. Ion-Dipole Forces
  10. IMF Strength Comparison
  11. States of Matter
  12. Kinetic Molecular Theory
  13. Solids
  14. Crystalline Solids
  15. Amorphous Solids
  16. Liquids
  17. Surface Tension
  18. Viscosity
  19. Capillary Action
  20. Gases
  21. Gas Pressure
  22. Atmospheric Pressure
  23. Ideal Gas Law
  24. Ideal Gas Constant
  25. Boyle's Law
  26. Charles's Law
  27. Avogadro's Law
  28. Dalton's Law
  29. Partial Pressures
  30. Mole Fraction
  31. Gas Stoichiometry
  32. Molar Volume
  33. Real Gases
  34. Van der Waals Equation
  35. Deviations from Ideality
  36. Phase Changes
  37. Melting and Freezing
  38. Boiling and Condensation
  39. Sublimation and Deposition
  40. Heating Curves
  41. Cooling Curves
  42. Heat of Fusion
  43. Heat of Vaporization
  44. Phase Diagrams
  45. Triple Point
  46. Critical Point
  47. Vapor Pressure
  48. Solutions
  49. Solvent and Solute
  50. Solubility
  51. Like Dissolves Like
  52. Saturated Solutions
  53. Concentration Units
  54. Molarity
  55. Dilution Calculations
  56. Beer-Lambert Law
  57. Spectrophotometry
  58. Colligative Properties
  59. Boiling Point Elevation
  60. Freezing Point Depression

Unit 4: Chemical Reactions (201-265)

  1. Chemical Equations
  2. Balancing Equations
  3. Coefficients
  4. State Symbols
  5. Reaction Types Overview
  6. Synthesis Reactions
  7. Decomposition Reactions
  8. Single Replacement
  9. Double Replacement
  10. Combustion Reactions
  11. Activity Series
  12. Solubility Rules
  13. Precipitation Reactions
  14. Complete Ionic Equations
  15. Net Ionic Equations
  16. Spectator Ions
  17. Stoichiometry
  18. Mole-to-Mole Ratios
  19. Mass-to-Mass Calculations
  20. Limiting Reagent
  21. Excess Reagent
  22. Theoretical Yield
  23. Actual Yield
  24. Percent Yield
  25. Solution Stoichiometry
  26. Titration
  27. Titration Curves
  28. Equivalence Point
  29. Indicator Selection
  30. Gravimetric Analysis
  31. Oxidation States
  32. Assigning Oxidation Numbers
  33. Oxidation
  34. Reduction
  35. Redox Reactions
  36. Half Reactions
  37. Balancing Redox Equations
  38. Oxidizing Agents
  39. Reducing Agents
  40. Electron Transfer
  41. Conservation of Mass
  42. Conservation of Charge
  43. Gas Evolution Reactions
  44. Acid-Carbonate Reactions
  45. Molecular Equations
  46. Reaction Prediction
  47. Qualitative Analysis
  48. Flame Tests
  49. Precipitate Identification
  50. Volumetric Analysis
  51. Standard Solutions
  52. Primary Standards
  53. Endpoint vs Equivalence
  54. Titration Calculations
  55. Percent Purity
  56. Empirical Formula from Data
  57. Molar Ratios in Solutions
  58. Serial Dilutions
  59. Driving Force of Reactions
  60. Metathesis Reactions
  61. Acid-Metal Reactions
  62. Disproportionation
  63. Color of Solutions
  64. Chemical Analysis
  65. Back Titration

Unit 5: Kinetics (266-320)

  1. Reaction Rate
  2. Rate of Disappearance
  3. Rate of Appearance
  4. Average Rate
  5. Instantaneous Rate
  6. Initial Rate
  7. Rate Law
  8. Rate Constant
  9. Reaction Order
  10. Zero Order Reactions
  11. First Order Reactions
  12. Second Order Reactions
  13. Determining Reaction Order
  14. Method of Initial Rates
  15. Integrated Rate Laws
  16. Zero Order Integrated Law
  17. First Order Integrated Law
  18. Second Order Integrated Law
  19. Half-Life
  20. First Order Half-Life
  21. Graphical Rate Analysis
  22. Concentration vs Time
  23. Linearization Rate Data
  24. Collision Theory
  25. Activation Energy
  26. Activated Complex
  27. Transition State
  28. Effective Collisions
  29. Orientation Factor
  30. Arrhenius Equation
  31. Arrhenius Plot
  32. Frequency Factor
  33. Temperature and Rate
  34. Energy Diagrams
  35. Exothermic Diagrams
  36. Endothermic Diagrams
  37. Reaction Mechanisms
  38. Elementary Steps
  39. Molecularity
  40. Unimolecular Reactions
  41. Bimolecular Reactions
  42. Rate-Determining Step
  43. Reaction Intermediates
  44. Mechanism Validation
  45. Catalysis
  46. Homogeneous Catalysis
  47. Heterogeneous Catalysis
  48. Enzyme Catalysis
  49. Catalyst Effect on Ea
  50. Catalyst and Equilibrium
  51. Catalyzed vs Uncatalyzed
  52. Surface Area and Rate
  53. Concentration and Rate
  54. Factors Affecting Rate
  55. Kinetics Experiments

Unit 6: Thermodynamics (321-375)

  1. Thermodynamics
  2. System and Surroundings
  3. Open Systems
  4. Closed Systems
  5. Isolated Systems
  6. Exothermic Reactions
  7. Endothermic Reactions
  8. Heat and Temperature
  9. Heat Transfer
  10. Specific Heat Capacity
  11. Heat Capacity
  12. Calorimetry
  13. Coffee Cup Calorimeter
  14. Bomb Calorimeter
  15. Enthalpy
  16. Enthalpy Change
  17. Standard Enthalpy
  18. Enthalpy of Formation
  19. Standard Formation Values
  20. Enthalpy of Combustion
  21. Enthalpy of Reaction
  22. Hess's Law
  23. Hess's Law Calculations
  24. Born-Haber Cycle
  25. Bond Enthalpy
  26. Bond Enthalpy Calculations
  27. Entropy
  28. Entropy Change
  29. Standard Entropy
  30. Entropy and Disorder
  31. Microstates
  32. Boltzmann Equation
  33. Second Law Thermodynamics
  34. Third Law Thermodynamics
  35. Entropy of Phase Changes
  36. Entropy Predictions
  37. Gibbs Free Energy
  38. Gibbs Free Energy Equation
  39. Standard Free Energy
  40. Free Energy of Formation
  41. Spontaneity
  42. Nonspontaneous Processes
  43. Temperature Dependence
  44. Gibbs and Equilibrium
  45. Free Energy and Work
  46. Coupled Reactions
  47. Thermodynamic Stability
  48. Kinetic Stability
  49. State Functions
  50. Path Functions
  51. Internal Energy
  52. First Law Thermodynamics
  53. PV Work
  54. Enthalpy vs Internal Energy
  55. Calorimetry Calculations

Unit 7: Equilibrium (376-420)

  1. Chemical Equilibrium
  2. Dynamic Equilibrium
  3. Equilibrium State
  4. Forward Reaction
  5. Reverse Reaction
  6. Equilibrium Constant Kc
  7. Equilibrium Constant Kp
  8. Kc and Kp Relationship
  9. Writing K Expressions
  10. Homogeneous Equilibrium
  11. Heterogeneous Equilibrium
  12. Equilibrium Position
  13. Reaction Quotient Q
  14. Q vs K Comparison
  15. Predicting Direction
  16. ICE Tables
  17. ICE Table Calculations
  18. Small K Approximation
  19. Quadratic in Equilibrium
  20. Le Chatelier's Principle
  21. Concentration Changes
  22. Pressure Changes
  23. Volume Changes
  24. Temperature Changes on K
  25. Effect of Catalyst on Eq
  26. Adding Inert Gas
  27. Equilibrium Shifts
  28. Solubility Equilibria
  29. Solubility Product Ksp
  30. Molar Solubility
  31. Common Ion Effect
  32. Predicting Precipitation
  33. Selective Precipitation
  34. Complex Ion Formation
  35. Formation Constants
  36. Ksp Calculations
  37. Ion Product
  38. Temperature and Solubility
  39. Henry's Law
  40. Equilibrium and Free Energy
  41. Relationship K and Delta G
  42. Manipulating K Expressions
  43. Reversing Reactions K
  44. Adding Reactions K
  45. Industrial Equilibrium

Unit 8: Acids and Bases (421-475)

  1. Acids
  2. Bases
  3. Arrhenius Theory
  4. Bronsted-Lowry Theory
  5. Lewis Acid-Base Theory
  6. Conjugate Acid-Base Pairs
  7. Conjugate Acid
  8. Conjugate Base
  9. Amphiprotic Substances
  10. Autoionization of Water
  11. Ion Product of Water Kw
  12. pH Scale
  13. pH Calculation
  14. pOH
  15. pH and pOH Relationship
  16. Strong Acids
  17. Strong Bases
  18. Strong Acid pH
  19. Strong Base pH
  20. Weak Acids
  21. Weak Bases
  22. Acid Dissociation Ka
  23. Base Dissociation Kb
  24. Ka and Kb Relationship
  25. Percent Ionization
  26. Weak Acid pH Calculation
  27. Weak Base pH Calculation
  28. Polyprotic Acids
  29. Diprotic Acid Equilibria
  30. Acid Strength Factors
  31. Binary Acid Trends
  32. Oxyacid Strength
  33. Salt Hydrolysis
  34. Acidic Salts
  35. Basic Salts
  36. Neutral Salts
  37. Buffer Solutions
  38. Buffer Composition
  39. Henderson-Hasselbalch
  40. Buffer Capacity
  41. Buffer pH Calculations
  42. Buffer Preparation
  43. Acid-Base Titration
  44. Strong Acid-Strong Base
  45. Weak Acid-Strong Base
  46. Strong Acid-Weak Base
  47. Titration Curve Analysis
  48. Half-Equivalence Point
  49. Buffer Region
  50. Indicators and pH Range
  51. Selecting Indicators
  52. Neutralization Reactions
  53. Net Ionic Acid-Base
  54. Dilute Acid Calculations
  55. pH of Mixed Solutions

Unit 9: Applications of Thermodynamics / Electrochemistry (476-500)

  1. Electrochemistry
  2. Galvanic Cells
  3. Voltaic Cell Components
  4. Anode and Cathode
  5. Salt Bridge
  6. Electron Flow Direction
  7. Cell Notation
  8. Standard Reduction Potential
  9. Standard Hydrogen Electrode
  10. Cell Potential Calculation
  11. Spontaneous Cell Reactions
  12. Nernst Equation
  13. Nonstandard Conditions
  14. Concentration Cells
  15. Free Energy and Cell EMF
  16. Delta G and E Relation
  17. Faraday's Constant
  18. Electrolytic Cells
  19. Electrolysis
  20. Electrolysis of Water
  21. Electroplating
  22. Faraday's Laws
  23. Stoichiometry Electrolysis
  24. Batteries and Fuel Cells
  25. Corrosion

Addendum: Concepts from Bloom's Taxonomy Learning Objectives (501-508)

These concepts are explicitly named in the course description's Bloom's Taxonomy learning objectives but were not included in the original 500-concept learning graph. They are covered in the chapters indicated.

  1. Coulombic Attraction
  2. Molecular Orbital Theory
  3. Bonding Molecular Orbitals
  4. Antibonding Molecular Orbitals
  5. MO Energy Diagrams
  6. Bond Order from MO Theory
  7. Paramagnetism and Diamagnetism
  8. Error Propagation