CLEP 
Chemistry
College · CLEP Chemistry · Certificate available
665 lessons 6.3h runtime 12 units 1,049 links between lessons Test yourself · 12 quizzes, a mid exam, and a final
StudyWalks exists to make learning clear, accessible, and free.
Short lessons. In order. Built for people who want to understand.
Begin with Unit 1: Essential Ideas: Matter, Measurement, and Uncertainty. It sets the foundation for everything that follows.
Nothing watched yet
Unit 1: Essential Ideas: Matter, Measurement, and Uncertainty 57 lessons, 3 lecture parts
- 0001 What Chemistry Studies
- 0004 The Scientific Method as a Process worked example
- 0008 Hypothesis
- 0009 Theory
- 0010 Scientific Law
- 0014 The Macroscopic Domain
- 0015 The Microscopic Domain
- 0016 The Symbolic Domain
- 0021 Matter Defined
- 0022 Solid
- 0023 Liquid
- 0024 Gas
- 0025 Plasma
- 0028 Mass
- 0029 Weight
- 0033 Conservation of Matter
- 0037 Pure Substance
- 0038 Element
- 0039 Compound
- 0043 Mixture
- 0044 Heterogeneous Mixture
- 0045 Homogeneous Mixture (Solution)
- 0049 Atom
- 0050 Molecule
- 0061 Physical Property
- 0062 Physical Change
- 0065 Chemical Property
- 0066 Chemical Change
- 0070 Extensive Property
- 0071 Intensive Property
- 0075 Metals, Nonmetals, and Metalloids
- 0079 The NFPA Hazard Diamond
- 0086 The Three Parts of a Measurement
- 0090 SI Base Units as a System
- 0091 The Meter
- 0092 The Kilogram
- 0093 The Second
- 0094 The Kelvin and Celsius
- 0098 Converting Between Metric Prefixes worked example
- 0102 Volume as a Derived Unit
- 0103 Density Defined
- 0107 Calculating Density from Mass and Volume worked example
- 0109 Volume by Water Displacement
- 0111 Converting Between Temperature Scales worked example
- 0121 Exact Numbers vs. Measured Numbers
- 0125 Significant Figures Defined
- 0129 Counting Significant Figures with Zeros worked example
- 0134 Significant Figures in Addition and Subtraction worked example
- 0138 Significant Figures in Multiplication and Division worked example
- 0142 Round-Half-to-Even Rule
- 0147 Precision
- 0148 Accuracy
- 0155 Dimensional Analysis
- 0156 Conversion Factor
- 0160 Single-Step Unit Conversion worked example
- 0164 Multi-Step Unit Conversion worked example
- 0170 Capstone: Identifying a Metal from Measured Data review
Unit 2: Atoms, Molecules, and Ions 56 lessons, 3 lecture parts
- 0181 Dalton's Atomic Theory
- 0184 The Law of Definite Proportions
- 0187 The Law of Multiple Proportions
- 0189 Applying the Law of Multiple Proportions worked example
- 0193 J. J. Thomson and the Discovery of the Electron (1897)
- 0196 Millikan's Oil-Drop Experiment (1913)
- 0199 Rutherford's Gold Foil Experiment (1911)
- 0202 The Nuclear Model of the Atom
- 0205 Proton
- 0208 Neutron
- 0211 Comparing the Three Subatomic Particles worked example
- 0214 Chemical Symbols
- 0217 Atomic Number
- 0219 Mass Number
- 0221 Isotope
- 0222 Ion
- 0225 Isotope Notation (Nuclear Symbol)
- 0228 Cation
- 0229 Anion
- 0232 The Atomic Mass Unit
- 0235 Average Atomic Mass as a Weighted Average
- 0238 Calculating Average Atomic Mass from Isotopic Data worked example
- 0241 Calculating Isotopic Abundance from Average Atomic Mass worked example
- 0244 Mass Spectrometry as the Method Behind Isotopic Data
- 0247 Standard Atomic Weight Is a Measured, Revisable Value
- 0249 Elements Without a Standard Atomic Weight
- 0252 Molecular Formula
- 0255 Structural Formula
- 0258 Empirical Formula
- 0261 Determining Empirical Formula from Molecular Formula worked example
- 0264 Diatomic Elements
- 0267 Isomers
- 0270 Mendeleev, Meyer, and the Periodic Table's Origin
- 0273 The Periodic Law
- 0276 Periods and Groups
- 0279 Metals, Nonmetals, and Metalloids at Periodic-Table Depth
- 0282 Main-Group, Transition, and Inner Transition Elements
- 0285 Named Families of the Periodic Table worked example
- 0288 Ionic Bond
- 0291 Covalent Bond
- 0294 Predicting Ionic vs. Molecular Bonding from the Periodic Table worked example
- 0297 Predicting Monatomic Ion Charge from Group Number
- 0300 Variable-Charge Metals
- 0303 Polyatomic Ion
- 0306 The -ate/-ite/per-/hypo- Oxyanion Naming Pattern worked example
- 0309 Writing Formulas for Ionic Compounds by Charge Balance worked example
- 0313 Naming Binary Ionic Compounds with Fixed-Charge Cations
- 0316 Naming Ionic Compounds with Variable-Charge Cations (Stock System)
- 0317 The Retired -ic/-ous Naming System
- 0320 Naming Ionic Hydrates
- 0323 Numerical Prefixes for Molecular Compound Names worked example
- 0327 Naming Binary Molecular Compounds
- 0330 Common Names That Override Systematic Rules
- 0333 Naming Binary Acids
- 0336 Naming Oxyacids
- 0340 Capstone: Classifying and Naming an Unknown Ionic Compound review
Unit 3: Composition, Solutions, and Stoichiometry 54 lessons, 3 lecture parts
- 0361 Formula Mass for Covalent Compounds
- 0364 Formula Mass for Ionic Compounds
- 0367 The Mole
- 0370 Avogadro's Number
- 0373 Molar Mass
- 0376 Converting Mass to Moles worked example
- 0379 Converting Moles to Number of Entities worked example
- 0382 Percent Composition
- 0385 Calculating Percent Composition from Experimental Mass Data worked example
- 0388 Determining Empirical Formula from Percent Composition worked example
- 0391 Determining Molecular Formula from Empirical Formula and Molar Mass worked example
- 0394 Solution, Solute, and Solvent
- 0397 Molarity
- 0400 Calculating Molarity from Solute Mass and Solution Volume worked example
- 0403 Calculating Solute Mass from Molarity and Volume worked example
- 0406 Strong and Weak Electrolytes
- 0407 Concentrated and Dilute
- 0410 Dilution of Solutions
- 0413 Performing a Dilution Calculation worked example
- 0416 Mass Percentage
- 0418 Volume Percentage
- 0419 Mass-Volume Percentage
- 0420 Parts per Million and Parts per Billion
- 0423 Writing a Chemical Equation
- 0426 Balancing Chemical Equations worked example
- 0429 Molecular Equations
- 0430 Complete Ionic Equations
- 0431 Net Ionic Equations and Spectator Ions
- 0434 Solubility
- 0435 Solubility Rules
- 0437 Predicting Precipitation Reactions worked example
- 0440 Acids and Bases
- 0443 Strong Acids and Strong Bases
- 0444 Weak Acids and Weak Bases
- 0447 Neutralization Reactions
- 0450 Writing Net Ionic Equations for Acid-Base Reactions worked example
- 0453 Oxidation Numbers
- 0456 Assigning Oxidation Numbers worked example
- 0459 Oxidation-Reduction (Redox) Reactions
- 0462 Combustion Reactions
- 0465 Single-Displacement Reactions
- 0468 Classifying a Reaction as Precipitation, Acid-Base, or Redox worked example
- 0471 Mole Ratios from a Balanced Equation
- 0474 Stoichiometric Calculations: Mass to Mass worked example
- 0477 Limiting Reactant
- 0480 Determining the Limiting Reactant worked example
- 0483 Theoretical Yield
- 0486 Percent Yield
- 0489 Calculating Percent Yield worked example
- 0492 Titration
- 0495 Titration Calculations worked example
- 0498 Gravimetric Analysis
- 0501 Combustion Analysis worked example
- 0510 Capstone: From Balanced Equation to Percent Yield review
Unit 4: Thermochemistry 36 lessons, 2 lecture parts
- 0621 Energy
- 0624 Potential and Kinetic Energy
- 0627 Law of Conservation of Energy
- 0630 Thermal Energy and Temperature
- 0633 Heat
- 0636 System and Surroundings
- 0637 Exothermic and Endothermic Processes
- 0640 The Joule and the Calorie
- 0643 Heat Capacity
- 0645 Specific Heat Capacity
- 0648 Calculating Heat from Mass, Specific Heat, and Temperature Change worked example
- 0651 Solving for an Unknown Specific Heat worked example
- 0654 Calorimetry
- 0657 The Coffee-Cup Calorimeter
- 0660 Calculating Heat Transfer Between Two Substances worked example
- 0663 Calculating Heat from Solution Calorimetry worked example
- 0666 The Bomb Calorimeter
- 0669 Calculating Heat from Bomb Calorimetry worked example
- 0672 Internal Energy and the First Law of Thermodynamics
- 0675 State Function
- 0678 Enthalpy
- 0681 Sign Convention for Enthalpy Change
- 0682 Scaling Enthalpy Change with a Thermochemical Equation's Coefficients
- 0685 Physical State in a Thermochemical Equation
- 0688 Determining Molar Enthalpy Change from a Limiting Reactant worked example
- 0691 Standard State and ΔH°
- 0694 Standard Enthalpy of Combustion
- 0697 Calculating Heat Released by Combustion of a Given Mass worked example
- 0700 Standard Enthalpy of Formation
- 0703 Writing and Solving Formation-Reaction Equations worked example
- 0706 Hess's Law worked example
- 0709 Stepwise Hess's Law Addition worked example
- 0712 Manipulating Reactions to Reach a Target Equation worked example
- 0715 The Summation Form of Hess's Law
- 0718 Applying the Summation Form to a Multi-Reactant Reaction worked example
- 0729 Capstone: From Calorimetry Data to a Hess's-Law Enthalpy Change review
Unit 5: Electronic Structure and Periodic Properties 48 lessons, 2 lecture parts
- 0761 Wavelength and Frequency
- 0763 Amplitude
- 0765 Wavelength and Frequency Are Inversely Related
- 0767 The Speed of Light as a Defining Constant
- 0769 Solving c = λν for Frequency worked example
- 0770 Solving c = λν for Wavelength worked example
- 0772 The Electromagnetic Spectrum
- 0775 Blackbody Radiation as a Puzzle for Classical Physics
- 0777 Planck's Hypothesis: Quantized Energy
- 0780 The Photoelectric Effect
- 0783 Wave-Particle Duality of Light
- 0788 Line Spectra Versus Continuous Spectra
- 0791 The Rydberg Equation's Structure
- 0793 Moseley and Atomic Number (1913)
- 0796 Bohr's Postulates
- 0799 The Bohr Model's Valid Domain
- 0801 The Bohr Model Is Not a Literal Planetary Picture
- 0804 Electron Transitions: Absorption and Emission
- 0810 De Broglie: Wave-Particle Duality of Matter
- 0813 The Heisenberg Uncertainty Principle
- 0816 The Quantum Mechanical Model
- 0818 Orbital
- 0819 Orbit Versus Orbital
- 0822 The Principal Quantum Number, n
- 0825 The Angular Momentum Quantum Number, l
- 0828 The Magnetic Quantum Number, ml
- 0831 The Spin Quantum Number, ms
- 0834 The s Orbital Shape
- 0836 The p Orbital Shape
- 0838 The d and f Orbitals
- 0844 The Pauli Exclusion Principle
- 0847 The Aufbau Principle
- 0850 Hund's Rule
- 0853 Electron Configuration Notation
- 0856 Orbital Diagrams
- 0859 Core Electrons Versus Valence Electrons
- 0862 Writing an Electron Configuration worked example
- 0865 Electron Configuration and Periodic Table Blocks
- 0868 Exceptions to the Aufbau Filling Order
- 0875 Effective Nuclear Charge (Zeff)
- 0878 Atomic Radius Trend
- 0881 Ionic Radius: Cations
- 0883 Ionic Radius: Anions
- 0886 First Ionization Energy Trend
- 0889 Successive Ionization Energies and the Core-Electron Jump
- 0892 Electron Affinity Trend
- 0895 Electronegativity, Named Structurally
- 0900 Capstone: Predicting a Periodic Trend from Electron Configuration and Zeff review
Unit 6: Chemical Bonding and Molecular Geometry 58 lessons, 3 lecture parts
- 0961 Ionic Bond Formation
- 0963 Ionic Compound Formula from Charge Balance
- 0966 Predicting Ionic Charge from Group Position
- 0969 Covalent Bond Formation
- 0972 Electronegativity's Periodic Trend
- 0975 Bond Polarity from Electronegativity Difference
- 0977 Pure Covalent, Polar Covalent, and Ionic as One Continuum
- 0980 Dipole Moment
- 0985 Lewis Symbol
- 0988 The Octet Rule
- 0991 Drawing a Lewis Structure worked example
- 0995 Incomplete Octet
- 0997 Expanded Octet
- 1000 Formal Charge, Defined
- 1003 Calculating Formal Charge from a Lewis Structure worked example
- 1006 Using Formal Charge to Choose the Best Structure
- 1009 Resonance
- 1011 Resonance Structures Are Contributing Forms
- 1013 The Single Fixed-Bond Misreading of Resonance
- 1018 Bond Length and Bond Order
- 1021 Covalent Bond Strength
- 1024 Estimating Reaction Enthalpy from Bond Energies worked example
- 1027 Lattice Energy
- 1030 Lattice Energy Trend with Charge and Radius
- 1035 VSEPR Theory's Core Assumption
- 1038 Electron-Pair Geometry
- 1040 Molecular Geometry
- 1043 Two-Domain Geometry: Linear
- 1045 Three-Domain Geometry: Trigonal Planar and Bent
- 1048 Four-Domain Geometry: Tetrahedral, Trigonal Pyramidal, and Bent
- 1051 Five-Domain Geometry: Trigonal Bipyramidal
- 1053 Six-Domain Geometry: Octahedral
- 1056 Assigning VSEPR Geometry from a Lewis Structure worked example
- 1060 Molecular Polarity from Bond Polarity and Geometry
- 1063 Polar Bonds Can Cancel to a Nonpolar Molecule
- 1065 The Polar-Bonds-Therefore-Polar-Molecule Misconception
- 1070 Capstone: From Lewis Structure to Molecular Polarity review
- 1080 Valence Bond Theory's Core Claim
- 1083 Sigma Bond
- 1085 Pi Bond
- 1090 Valence Bond Theory's Domain
- 1095 Orbital Hybridization, Defined
- 1098 sp Hybridization
- 1101 sp² Hybridization
- 1104 sp³ Hybridization
- 1107 sp³d and sp³d² Hybridization
- 1110 Predicting Hybridization from VSEPR Domain Count
- 1115 A Double Bond as Sigma Plus Pi
- 1117 A Triple Bond as Sigma Plus Two Pi
- 1120 Pi Bonding Restricts Rotation
- 1125 Molecular Orbital Theory's Core Claim
- 1128 Bonding Orbital Versus Antibonding Orbital
- 1132 Molecular Orbital Diagram
- 1135 Bond Order from a Molecular Orbital Diagram worked example
- 1138 Paramagnetism and Diamagnetism
- 1141 O2's Paramagnetism, Predicted by Molecular Orbital Theory worked example
- 1145 Molecular Orbital Theory's Domain
- 1200 Capstone: Two Bonding Models Applied to One Molecule review
Unit 7: Gases 45 lessons, 2 lecture parts
- 1201 Pressure, Defined
- 1203 The Pascal and Common Pressure Units
- 1206 Converting Among Pressure Units worked example
- 1210 Hydrostatic Pressure
- 1213 Barometer
- 1216 Manometer
- 1219 Calculating Gas Pressure from a Manometer Reading worked example
- 1224 Amontons's Law: Pressure and Temperature
- 1227 Charles's Law: Volume and Temperature
- 1230 Boyle's Law: Volume and Pressure
- 1233 Avogadro's Law: Volume and Amount
- 1236 The Ideal Gas Law
- 1239 Solving Problems with the Ideal Gas Law worked example
- 1243 The Combined Gas Law
- 1246 Ideal Gas Assumptions
- 1249 Standard Temperature and Pressure: the 1 atm Convention
- 1251 Standard Temperature and Pressure: the Current IUPAC Convention
- 1254 Standard Molar Volume, Computed Under Both STP Conventions worked example
- 1259 Gas Density from the Ideal Gas Law
- 1262 Determining Molar Mass from Measured Gas Properties worked example
- 1266 Dalton's Law of Partial Pressures
- 1269 Mole Fraction and Partial Pressure
- 1272 Calculating Partial Pressures in a Gas Mixture worked example
- 1276 Collecting a Gas Over Water
- 1279 Correcting for Water Vapor Pressure worked example
- 1283 Gas Volumes in Stoichiometric Ratios
- 1286 Gas Stoichiometry from Reaction Volumes worked example
- 1291 Diffusion
- 1294 Effusion
- 1297 Mean Free Path
- 1300 Graham's Law of Effusion
- 1302 The Direct-Proportionality Misreading of Graham's Law
- 1305 Calculating Relative Effusion Rates worked example
- 1308 Kinetic-Molecular Theory's Core Postulates
- 1311 Explaining the Gas Laws from Kinetic-Molecular Theory worked example
- 1315 Average Kinetic Energy and Temperature
- 1318 Maxwell-Boltzmann Speed Distribution
- 1321 Calculating Root-Mean-Square Speed worked example
- 1325 Kinetic-Molecular Theory Explains Graham's Law
- 1330 Real Gases Deviate from Ideal Behavior
- 1333 The Compressibility Factor
- 1336 Conditions Favoring Ideal Behavior
- 1339 The van der Waals Equation
- 1343 Calculating Pressure with the van der Waals Equation worked example
- 1350 Capstone: From Manometer Reading to Real-Gas Correction review
Unit 8: Liquids, Solids, Solutions, and Colloids 64 lessons, 3 lecture parts
- 1361 Condensed Phases and the IMF-KE Balance
- 1364 Intermolecular vs. Intramolecular Forces
- 1367 The "Breaking Bonds" Misreading of Boiling
- 1370 Dispersion Forces
- 1373 Ranking Boiling Points by Dispersion-Force Strength worked example
- 1376 Dipole-Dipole Attraction
- 1379 Hydrogen Bonding
- 1382 Why a Hydrogen Bond Is Not a Covalent Bond
- 1385 Predicting the Dominant IMF and Ranking Boiling Points worked example
- 1390 Viscosity
- 1393 Cohesive vs. Adhesive Forces
- 1396 Surface Tension
- 1399 Capillary Action
- 1404 Vaporization, Condensation, and Dynamic Equilibrium
- 1407 Equilibrium Vapor Pressure
- 1410 Boiling Point from Vapor Pressure
- 1413 The Normal Boiling Point
- 1416 Heating Curves and Phase-Change Plateaus
- 1419 Enthalpy of Fusion and Enthalpy of Vaporization
- 1424 The Clausius-Clapeyron Relation
- 1427 Estimating Enthalpy of Vaporization from Two Data Points worked example
- 1432 Constructing a Phase Diagram
- 1435 The Triple Point
- 1438 The Critical Point and the Supercritical Fluid
- 1441 Reading a Phase Diagram for a Given State worked example
- 1446 Water's Anomalous Melting-Point Slope
- 1451 Crystalline vs. Amorphous Solids
- 1454 Ionic Solids
- 1457 Metallic Solids
- 1460 Covalent Network Solids
- 1463 Molecular Solids
- 1466 Classifying an Unknown Solid from Its Properties worked example
- 1471 Crystal Defects
- 1476 The Unit Cell
- 1479 Coordination Number
- 1482 The Simple Cubic Unit Cell
- 1485 The Body-Centered Cubic Unit Cell
- 1488 The Face-Centered Cubic Unit Cell
- 1493 Computing a Metal's Density from Its Unit Cell worked example
- 1498 Ionic Crystal Unit Cells
- 1503 Capstone: From Dominant IMF to Crystal Structure review
- 1520 The Dissolution Process
- 1523 "Like Dissolves Like" as a Structural Heuristic
- 1526 Electrolytes vs. Nonelectrolytes
- 1529 Strong vs. Weak Electrolytes, Extended to the Van't Hoff Factor
- 1533 Saturated, Unsaturated, and Supersaturated Solutions
- 1536 Temperature's Effect on Solid and Gas Solubility
- 1539 Henry's Law for Gas Solubility
- 1544 Colligative Properties Defined
- 1547 Mole Fraction and Molality
- 1550 Converting Between Molarity and Molality worked example
- 1555 Raoult's Law and Vapor Pressure Lowering
- 1558 Calculating a Solution's Vapor Pressure Under Raoult's Law worked example
- 1561 Boiling Point Elevation
- 1564 Freezing Point Depression
- 1568 Calculating Boiling Point Elevation or Freezing Point Depression worked example
- 1573 Osmosis and Osmotic Pressure
- 1576 Calculating Osmotic Pressure worked example
- 1580 Determining Molar Mass from a Colligative Property worked example
- 1584 The van't Hoff Factor
- 1587 Freezing Point Depression for an Electrolyte Solution worked example
- 1591 Colloids Distinguished from Solutions and Suspensions
- 1594 The Tyndall Effect
- 1598 Capstone: One Aqueous Solution from IMF to Corrected Freezing Point review
Unit 9: Kinetics 43 lessons, 2 lecture parts
- 1601 Reaction Rate Defined
- 1604 Relative Reaction Rates from Stoichiometry
- 1607 Writing Relative Rate Expressions from a Balanced Equation worked example
- 1610 Average, Instantaneous, and Initial Rate
- 1615 Reactant Identity and Reaction Rate
- 1618 Physical State and Surface Area
- 1621 Temperature and Reaction Rate
- 1624 Concentration and Reaction Rate
- 1627 Catalysis Previewed as a Rate Factor
- 1632 The Rate Law and Reaction Order
- 1635 Overall Reaction Order
- 1638 Rate Laws Come From Experiment, Not Stoichiometric Coefficients
- 1641 The Stoichiometric-Coefficient Misreading of a Rate Law
- 1644 Determining a Rate Law by the Method of Initial Rates worked example
- 1649 Rate Constant Units Vary With Overall Order
- 1654 The Integrated Rate Law
- 1657 The First-Order Integrated Rate Law
- 1660 Solving the First-Order Integrated Rate Law for Time or Concentration worked example
- 1663 The Second-Order Integrated Rate Law
- 1666 Solving the Second-Order Integrated Rate Law worked example
- 1669 The Zero-Order Integrated Rate Law
- 1672 Half-Life Defined
- 1675 Half-Life's Order Dependence
- 1678 Calculating a First-Order Rate Constant From a Measured Half-Life worked example
- 1683 Collision Theory's Rate-Collision Proportionality
- 1686 Collision Orientation Requirement
- 1689 Activation Energy
- 1692 The Transition State
- 1695 The Arrhenius Equation
- 1698 Determining Activation Energy From Rate Constants at Two Temperatures worked example
- 1703 Elementary Reactions and Reaction Mechanisms
- 1706 Molecularity: Unimolecular and Bimolecular Steps
- 1709 Termolecular Elementary Reactions
- 1712 Reaction Intermediates
- 1715 The Rate-Determining Step
- 1718 An Elementary Step's Rate Law Follows From Its Molecularity
- 1721 Deriving a Rate Law from a Multistep Mechanism worked example
- 1726 Catalysts Lower Activation Energy Without Being Consumed
- 1729 The "Catalysts Shift Equilibrium" Misreading
- 1732 A Catalyst's Alternative, Lower-Energy Mechanism
- 1735 Homogeneous Catalysis
- 1738 Heterogeneous Catalysis
- 1740 Capstone: From Experimental Rate Law to Catalyzed Mechanism review
Unit 10: Equilibrium: Fundamentals, Acids and Bases, and Solubility 67 lessons, 3 lecture parts
- 1741 Dynamic Equilibrium: Equal Rates, Not Equal Concentrations
- 1743 Twin: "Equilibrium Means Equal Concentrations"
- 1746 Equilibrium as a Consequence of Kinetics
- 1749 Equilibrium Constant Expression Construction
- 1752 K Is Dimensionless
- 1755 K Depends Only on Temperature
- 1758 Homogeneous vs. Heterogeneous Equilibria
- 1761 Reaction Quotient Q Defined
- 1764 Comparing Q to K Predicts Direction
- 1766 K's Magnitude Read Qualitatively
- 1768 The ICE Table Method worked example
- 1771 The Small-x Approximation worked example
- 1774 Kp vs. Kc Relationship
- 1777 Converting Between Kp and Kc worked example
- 1780 Le Châtelier's Principle as a Q-vs-K Consequence
- 1783 Concentration Stress via Q vs. K
- 1786 Volume/Pressure Stress via Q vs. K
- 1789 Temperature Stress via Q vs. K
- 1792 Catalyst Has No Effect on Equilibrium Position
- 1795 Capstone: Predicting and Quantifying a Le Châtelier Shift review
- 1799 The Arrhenius Acid-Base Definition
- 1802 The Brønsted-Lowry Acid-Base Definition
- 1805 Conjugate Acid-Base Pairs
- 1807 Acid-Base Neutralization as a Reaction Type
- 1809 Amphiprotic Substances
- 1812 The Lewis Acid-Base Definition
- 1815 Nested Domains of Generality Among the Three Theories
- 1818 Autoionization of Water and Kw
- 1821 Kw's Temperature Dependence
- 1824 pH and pOH Scales and Their Relationship
- 1827 Strong Acids and Bases: Complete Dissociation
- 1829 The Recognized Strong Acids and Bases, Identified Structurally
- 1832 Calculating pH of a Strong Acid or Base Solution worked example
- 1835 Weak Acid Equilibrium and Ka
- 1838 Weak Base Equilibrium and Kb
- 1841 The Ka–Kb Relationship for a Conjugate Pair
- 1844 Solving for pH of a Weak Acid Solution worked example
- 1847 Percent Ionization Defined
- 1850 Calculating Percent Ionization worked example
- 1853 Polyprotic Acids: Stepwise Ionization
- 1856 Solving Polyprotic Acid pH via the Dominant First Ionization worked example
- 1859 Salt Hydrolysis: Predicting Acidic, Basic, or Neutral Salts
- 1862 Determining pH of a Salt Solution via Hydrolysis worked example
- 1865 Acid-Base Indicators: Mechanism
- 1868 Indicator Color-Change Range and Titration Indicator Choice
- 1871 Calculating Analyte Concentration from Titration Data worked example
- 1874 Titration Curve: Strong Acid–Strong Base Shape
- 1876 Titration Curve: Weak Acid–Strong Base Shape
- 1878 Titration Curve: Weak Base–Strong Acid Shape
- 1881 Equivalence Point vs. Endpoint Distinguished
- 1884 Reading Key Features of a Titration Curve worked example
- 1887 Buffers: How They Resist pH Change
- 1890 Buffer Composition Requirement
- 1893 Henderson-Hasselbalch Equation Application worked example
- 1896 Buffer Capacity
- 1899 Capstone: Buffer pH Calculation review
- 1903 Capstone: Titration Curve pH-at-Stages Synthesis review
- 1907 Solubility Product Ksp Defined
- 1910 Molar Solubility from Ksp worked example
- 1913 Common-Ion Effect on Solubility
- 1916 Molar Solubility with a Common Ion Present worked example
- 1919 Precipitation Prediction via Q vs. Ksp
- 1922 Precipitation as a Reaction Type
- 1925 Selective Precipitation
- 1928 Complex Ion Formation and Formation Constant Kf
- 1931 Complexation's Effect on Solubility
- 1935 Capstone: Ksp, Common-Ion, and Complexation Synthesis review
Unit 11: Thermodynamics and Electrochemistry 58 lessons, 4 lecture parts
- 2061 Spontaneous Process Defined
- 2063 Twin: Spontaneous Does Not Mean Fast
- 2066 A Spontaneous Direction Is Nonspontaneous Reversed
- 2069 Entropy as a Microstate-Counted State Function
- 2071 Twin: Entropy Is Not Disorder
- 2074 Entropy Rises with Accessible Microstates
- 2077 Entropy Trend Across Phases
- 2080 Entropy Rises with Temperature
- 2083 Entropy Rises with Molecular Complexity
- 2084 Entropy Rises with Mixing
- 2086 Predicting the Sign of ΔS worked example
- 2090 The Second Law of Thermodynamics
- 2093 The Third Law of Thermodynamics
- 2096 Standard Molar Entropy as an Absolute Quantity
- 2099 Calculating ΔS°rxn from Standard Molar Entropies worked example
- 2103 Gibbs Free Energy Defined
- 2106 Sign of ΔG Predicts Spontaneity
- 2109 The Four ΔH/ΔS Sign Combinations
- 2112 Temperature-Dependent Spontaneity and the Crossover Temperature
- 2115 Calculating the Crossover Temperature worked example
- 2118 Standard Free Energy of Formation ΔG°f
- 2121 Calculating ΔG°rxn from ΔG°f Values worked example
- 2124 ΔG as a Path-Independent State Function
- 2127 ΔG Under Nonstandard Conditions
- 2130 ΔG° Relates to K
- 2133 Calculating K from ΔG° worked example
- 2136 Capstone: Full Thermodynamic Profile of a Reaction review
- 2140 Oxidation and Reduction Defined by Electron Transfer
- 2143 Using Oxidation Numbers to Identify Oxidized and Reduced Species
- 2146 Balancing a Redox Equation by the Half-Reaction Method worked example
- 2150 Galvanic Cell: Spontaneous Redox Generates Current
- 2153 Anode and Cathode by Reaction, Not by Charge
- 2156 Twin: The Anode/Cathode Charge-Sign Reversal
- 2159 Salt Bridge Maintains Circuit and Neutrality
- 2162 Cell Notation Convention
- 2165 Cell Potential Defined
- 2168 The Standard Hydrogen Electrode
- 2171 Standard Reduction Potentials Tabulated
- 2174 Calculating Standard Cell Potential worked example
- 2178 Sign of E°cell Predicts Spontaneity
- 2181 Standard Reduction Potential Ranks Strength
- 2184 ΔG° Relates to E°cell
- 2187 Faraday's Constant
- 2190 E°cell, ΔG°, and K as One Fact
- 2193 Calculating K from E°cell worked example
- 2196 The Nernst Equation
- 2199 Applying the Nernst Equation worked example
- 2203 Concentration Cells
- 2206 Capstone: Full Electrochemical Profile of a Galvanic Cell review
- 2210 Battery as a Multi-Cell Galvanic Device
- 2213 Primary vs. Secondary Battery
- 2216 Fuel Cell Mechanism
- 2219 Corrosion as Unwanted Spontaneous Oxidation
- 2222 Cathodic Protection: Sacrificial Anode Principle
- 2225 Electrolysis: Nonspontaneous Redox Driven by Current
- 2228 Twin: Electrolytic Cell as the Forced-Reverse Galvanic Cell
- 2231 Calculating Product Quantity from Current and Time worked example
- 2235 Capstone: One Redox Couple, Three Cell Types review
Unit 12: Descriptive, Organic, and Nuclear Chemistry 79 lessons, 5 lecture parts
- 2281 Classifying Elements by Orbital Filling
- 2284 Metallic Character Tracks Ionization Energy
- 2287 Alkali Metal Reactivity Increases Down the Group
- 2290 Passivation Defined
- 2293 Alkaline Earth Metals Are Less Reactive Than Alkali Metals
- 2296 Group Oxidation State from Valence Electron Count
- 2299 Twin: The Inert Pair Effect
- 2302 Amphoterism at the Metal-Nonmetal Boundary
- 2305 Metalloids as Intermediate Semiconductors
- 2308 Boron's Electron Deficiency Drives Lewis Acidity
- 2311 Nonmetal Bonding Type from Electronegativity Difference
- 2314 Nonmetals Form Only Anions, Never Monatomic Cations
- 2317 Fluorine and Oxygen as the Strongest Oxidizers
- 2320 Nonmetal Hydride Acid Strength Trend
- 2323 Allotropes: Structure Sets Property
- 2326 Hydrogen's Dual Periodic-Table Position
- 2329 Nitrogen's Inertness and Nitrogen Fixation
- 2332 Oxygen's Allotropes and Oxidizing Strength
- 2335 Classifying Oxygen Compounds by O-O Bonding
- 2338 Sulfur's Allotropy and Variable Oxidation States
- 2341 Predicting Characteristic Oxidation State from Periodic Position worked example
- 2346 Halogen Physical State Tracks London Dispersion Forces
- 2349 Halogen Oxidizing Strength Decreases Down the Group
- 2352 Interhalogens Defined
- 2355 Noble Gas Unreactivity and the Xenon Exception
- 2360 Capstone: Predicting Bonding and Reactivity from Periodic Position review
- 2372 Transition Metals Defined by Partially Filled d Orbitals
- 2375 Multiple Oxidation States Peak Mid-First-Series
- 2378 Heavier d-Block Series Favor Higher Oxidation States
- 2381 Coordination Compounds as Lewis Acid-Base Adducts
- 2384 Coordination Number Sets Complex Geometry
- 2387 Monodentate vs. Polydentate Ligands
- 2390 Naming a Coordination Compound worked example
- 2394 Geometric Isomerism in Complexes
- 2397 Optical Isomerism (Enantiomers)
- 2400 Crystal Field Splitting in an Octahedral Complex
- 2403 The Spectrochemical Series: Weak- vs. Strong-Field Ligands
- 2406 Twin: The High-Spin Complex
- 2409 Twin: The Low-Spin Complex
- 2412 Complex Color from d-d Electron Transitions
- 2417 Capstone: Full Analysis of a Coordination Complex review
- 2429 Organic Compounds Defined by Carbon Catenation
- 2432 Alkanes: Saturated Hydrocarbons
- 2435 Structural Isomers Defined
- 2438 IUPAC Alkane Naming worked example
- 2442 Alkenes: Restricted Rotation at the Double Bond
- 2445 cis/trans Geometric Isomerism in Alkenes
- 2448 Alkynes: Linear Triple Bonds
- 2451 Twin: The Addition Reaction
- 2454 Twin: The Substitution Reaction
- 2457 Aromatic Delocalization Favors Substitution
- 2460 Alcohols: The Hydroxyl Functional Group
- 2463 Twin: The Aldehyde
- 2466 Twin: The Ketone
- 2469 Carboxylic Acids and Esters from the Carbonyl
- 2472 Amines: Weak Bases from a Nitrogen Lone Pair
- 2475 Amides Distinguished from Amines by the Carbonyl
- 2478 Determining an Organic Carbon's Oxidation Level worked example
- 2483 Capstone: Functional-Group Family Comparison review
- 2496 Nuclide Notation
- 2499 Mass Defect and Nuclear Binding Energy
- 2503 Calculating Binding Energy per Nucleon worked example
- 2507 The Band of Stability Predicts Decay Mode
- 2510 Twin: Alpha Decay
- 2513 Twin: Beta Decay
- 2516 Twin: Positron Emission and Electron Capture
- 2519 Gamma Emission Changes Neither Mass Nor Atomic Number
- 2522 Balancing a Nuclear Equation worked example
- 2526 Half-Life: Exponential Decay Defined and Measured worked example
- 2530 Radiometric Dating from a Decay Ratio worked example
- 2535 Twin: Nuclear Fission
- 2538 Twin: Nuclear Fusion
- 2541 Chain Reaction as a Self-Sustaining Threshold
- 2544 Reactor Components as Mechanism
- 2547 Radioisotope Tracers: Detection, Not Intervention
- 2550 Twin: Ionizing Radiation
- 2553 Twin: Nonionizing Radiation
- 2556 Direct vs. Indirect Radiation Damage
- 2561 Capstone: Decay Chain and Binding-Energy Profile review
Who this subject is for
- Students preparing for the CLEP Chemistry exam
- Nursing, pre-med and science majors
- Engineering students
- Adult learners finishing a degree
- Homeschool students
- Anyone who wants chemistry explained step by step
Why Chemistry matters
Chemistry explains what matter is made of and how it changes. It is the foundation for:
- Organic chemistry
- Biochemistry
- Pharmacology
- Physics
- Engineering
Time to complete
- of lessons (665, measured)
- 6.3 h
- of lectures (35)
- 18.2 h
- learning hours on the certificate, with quizzes and the final
- 29.5 h
Times are measured from the recordings and the exam time limits. Go at your own pace; nothing expires.
Featured pathway · $35
AI Foundations Pathway
Five micro-certificates (AI Literacy, Data Literacy, Critical Thinking, Cybersecurity Essentials and STEM Foundations) plus the Full Certificate in Computer Science. Hold all six and claim the pathway certificate, the badge and a verification number.
Explore the AI Foundations Pathway →Sources for Chemistry — the textbook it was written against, and the second source it was checked against.
This is free, and stays free. If it helped, here is what keeps it running.