General Chemistry
This page is for the first year undergraduate General Chemistry course (commonly referred to as Gen Chem). This page is built on the principle that mastery of the concepts comes from active problem-solving rather than passive reading. Instead of dense textbook chapters or lecture transcripts, the focus is on practice problems to develop more rigorous problem-solving skills, deeper conceptual understanding, and an emphasis on scientific reasoning.
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Course Topics
General Chemistry 1 (First Semester)
Measurement and Problem-Solving
Unit conversions
Scientific notation
Significant figures
Accuracy and precision
Percent error
Density calculations
Graphical data analysis
Matter and Atomic Structure
Matter classification
Physical vs. chemical changes
Intensive vs. extensive properties
Conservation of mass
Subatomic particles & Isotope Notation
Average atomic mass
Formulas and Nomenclature
Ionic Compound Naming
Ionic formula writing
Covalent/ molecular compound naming
Covalent molecular formula writing
Acid naming formula writing
Hydrate naming
The Mole and Chemical Composition
Molar mass
Mass, mole, particle conversions
Percent composition
Empirical formula & Molecular formula
Combustion Analysis
Hydrate formula determination
Chemical Equations and Reaction Types
Equation balancing
Reaction classification & prediction
Intro Oxidation-Reduction
Stoichiometry
Limiting Reactant
Excess Reactant
Theoretical & Percent Yield
Mixture composition problems
Aqueous Reactions
Molarity
Dilution
Ion-concentration
Solution mixing & Solubility Rule
Complete and Net Ionic Equations
Neutralization Stoichiometry
Titrations, introduction
Gases
Pressure Conversions
Gas Laws
Ideal Gas Law
Gas Density
Molar Mass Determination
Gas Stoichiometry
Partial Pressure & Gas over Water
Thermochemistry
Heat Flow
Internal Energy & Pressure-Volume work
Calorimetry
Specific Heat
Reaction Enthalpies
Hess’s Law
Enthalpy of Formation
Bond Enthalpies
Quantum Theory
Wavelength, frequency, energy, photons
Electromagnetic spectrum
Hydrogen transition calculations
Emission Spectrum Interpretations
de Broglie wavelength
Quantum numbers
Orbital Identification & Capacity
Electron Configurations and Periodicity
Electron Configuration
Ion configuration writing
Orbital-diagrams
Paramagnetism and diamagnetism
Atomic Trends (radius, ion radius, ionization, electronegativity)
Ionic Bonding
Ionic formula prediction
Coulombic Comparisons
Lattice energy
Born-Haber cycle
Covalent Bonding
Lewis Structures
Octet Exceptions
Resonance
Formal Charges
Bond order, length, strength
Bond polarity
Bond enthalpy
Molecular Geometry and Bonding
Lewis Structures
Formal Charges
Molecular & Electron Geometry (VESPR, bond angle)
Molecular Polarity
Hybridization & Orbital overlap
Molecular Orbital diagrams
Magnetic Property Prediction
Intermolecular Forces and Phases
Intermolecular Forces
Physical Properties (Boiling point, vapor pressure, viscosity, surface tension)
Phase Changes & Heating Curve
Phase Diagram
Clausius–Clapeyron calculations
Unit Cell Density
General Chemistry 2 (Second Semester)
Solutions
Molarity & Molality
Mole fraction
Dilutions
Solution mixing & Ion concentration
Solubility curve interpretation
Henry’s Law
Colligative Properties
Vapor pressure
Raoult’s-law
Boiling point elevation & Freezing-point depression
Osmotic pressure
Molar mass determination
van ’t Hoff-factor determination
Ideal-solution comparisons
Chemical Kinetics
Average Rate & Instantaneous Rate
Rate Law
Reaction Order determination
Rate constant units
Integrated Rate Law
Half Life
Kinetic-plot interpretation
Mechanisms and Catalysis
Elementary step, Molecularity, Intermediate & Catalyst identification
Rate-determining-step identification
Mechanism validation
Rate-law derivation
Reaction coordinate diagrams
Activation energy
Arrhenius equation
Chemical Equilibrium
Equilibrium Expression
Equilibrium Constant
Kc-to-Kp conversions
K vs Q (Reaction Quotient)
ICE table calculations
Le Châtelier predictions
Acid–Base Theory
Acid-base classification
Conjugate-pair identification
Lewis acid-base
Strong acid & base pH calculations
pH-pOH conversions
Kw calculations
Strong-acid–base mixing / Neutralization
Weak-Acid and Weak-Base Equilibria
Weak-acid pH calculations
Weak-base pH calculations
Ka determination
Kb determination
Percent ionization
Polyprotic acids
Salt hydrolysis
Buffers and Titrations
Henderson–Hasselbalch calculations
Buffer component determination
Buffer preparation
Added-acid & base buffer calculations
Buffer-capacity comparisons
Titration-curve calculations
Equivalence-point pH
Indicator selection
Solubility Equilibria
Ksp
Molar solubility
Common-ion solubility
Precipitation prediction
Selective-precipitation calculations
pH-dependent solubility
Complex-ion equilibrium
Qualitative-ion separation
Entropy and Spontaneity
Entropy
Phase-transition entropy
Microstate comparisons
Spontaneity determination
Reversible-process comparisons
Entropy-versus-temperature analysis
Gibbs Free Energy
Free energy calculations
Temperature-threshold calculations
Nonstandard Free energy
ΔG to K conversions
Coupled-reaction calculations
Thermodynamic-versus-kinetic control
Electrochemistry
Redox equation balancing
Anode-cathode identification
Cell-notation writing
Standard-cell-potential
Spontaneous-cell prediction
Nernst-equation
Electrolysis calculations
Nuclear Chemistry
Nuclear equation balancing
Decay-mode identification
Daughter-nuclide prediction
Half-life
Binding energy
Fission energy
Coordination Chemistry
Complex ion naming & formula writing
Coordination-number determination
Ligand identification
d-electron counting
Geometric isomers
Optical isomers
Crystal field splitting diagrams
Magnetic properties
Organic Chemistry
Hydrocarbon naming
Structural formula drawing
Functional groups
Constitutional isomer drawing
Geometric-isomer identification
Organic-reaction prediction
Biomolecule classification
We don't teach general chemistry by dropping the Henderson-Hasselbalch equation and expecting buffers to make sense. We talk about it by comparing a buffer to a shock absorber, something built to soak up small hits without the whole system swinging wildly, so students understand what the equation is actually protecting against. If you've ever had to calculate a buffer's pH correctly but freeze when asked why adding a strong acid barely moves it, that's will soon change.