Distinguish atoms, isotopes and ions
Use proton, neutron and electron counts to distinguish element identity, isotope and charge.
Chemistry and matter
Connect particle representations to quantities, changes and evidence.
This is the course outline. Open a unit to choose a lesson; every lesson opens on its own page. Explanations and experiments live inside those lesson pages.
Course scope and preparation
Forty-six lessons connect atomic structure and bonding to chemical quantities, solutions, measurement, gases and energy. The sequence then develops rates, equilibrium, acids and bases, electrochemistry, polymers and material recovery. Thirty-four quantitative models, one qualitative corrosion investigation and one published-data comparison support predictions, investigations and explanations.
Arithmetic, ratios, units and scientific notation are explained where needed; programming is not required. The module list below shows the available topics. The bounded teaching sequence and retained investigation workflow are available; notebook completion does not establish practical laboratory proficiency.
Each lesson supports saved predictions, experiment captures, reflections and practice. Notebook completion records the presence of work; it does not establish mastery. Scientific inquiry provides optional preparation in measurement and fair comparisons.
Particles, formulas and conservation
Read formulas without changing the substance
Distinguish a molecular formula from a coefficient and count atoms across several species.
Balance atoms and identify what remains
Explain a balanced reaction using atom conservation and account for a limiting inventory.
Electron structure, bonding and molecular shape
Connect electron arrangements to atomic structure
Reconcile proton count, neutral electron count, shell totals and subshell notation for the first eighteen elements.
Use periodic patterns without turning trends into laws
Use main-group electron patterns to compare chemical behavior while distinguishing composition, charge and qualitative trends.
Build ionic formulas from charge and structure
Derive a neutral formula ratio from specified ion charges and relate ionic structure to mobility and material properties.
Repair covalent structures with two electron checks
Diagnose missing, excess and misplaced electrons in supplied Lewis structures, including single, double and triple bonds.
Connect molecular shape to bond-polarity cancellation
Explain why bond polarity and molecular polarity are different, using geometry, symmetry and explicit model assumptions.
Explain boiling-point evidence with intermolecular attractions
Distinguish dispersion, dipole interactions and hydrogen bonding, and explain the limits of a structure–boiling-point comparison.
Connect metallic bonding to charge transport
Connect metallic bonding to electrical conduction and ductility without treating electrons as consumed fuel or ions as the current carriers in a solid wire.
Choose a conductor using two explicit constraints
Use quantitative evidence to select a supported conductor design and state which missing properties could change the decision.
Mass, moles and reaction quantities
Connect a measured mass to a particle amount
Convert mass to amount using molar mass and distinguish equal masses from equal molecule numbers.
Predict product mass without rounding away reactants
Identify a limiting reactant from stoichiometric amounts and reconcile product plus leftover mass.
Diagnose product yield and impure isolates
Calculate theoretical and corrected yield, distinguish mass loss from matter destruction, and diagnose conflicting evidence.
Solution amount, concentration and preparation
Distinguish solution amount from concentration
Calculate molarity with explicit volume units and distinguish a larger sample from a more concentrated solution.
Dilute a stock solution without losing the solute ledger
Derive a dilution from conserved solute and distinguish filling to volume from adding a stated solvent volume.
Density, displacement and evidence quality
Find density from the volume a sample displaces
Calculate density from displacement and explain when the measurement assumptions fail.
Decide what a coarse density measurement can establish
Construct conservative density bounds and explain why a coarse displacement can lack a finite upper bound.
Mixtures, solubility and separation
Distinguish a dissolved mixture from a pure substance
Distinguish a homogeneous solution from the whole heterogeneous sample and explain saturation without confusing it with dissolution rate.
Design a separation and account for every fraction
Explain selective separation, recovery and contamination using stage-specific component balances.
Gas states, temperature and mixtures
Explain gas pressure with a controlled volume comparison
Use absolute pressure, units and controlled comparisons to explain ideal-gas compression and identify model limits.
Use absolute temperature and specify what is held fixed
Compare equilibrium gas states using kelvin temperatures and explicit amount, volume and pressure constraints.
Account for each gas in a mixture
Apply an additive ideal-mixture pressure ledger without confusing mole fraction, mass fraction or occupied volume.
Heat, phase changes and reaction energy
Track energy through warming and melting
Predict temperature and liquid fraction from a conserved energy ledger.
Account for heat in the samples, cup and surroundings
Close a signed heat balance and explain why the final temperature is not a simple average.
Explain reaction enthalpy using a bond ledger
Calculate signed reaction enthalpy without confusing bond energies with activation energy.
Reaction rates and time-dependent evidence
Measure reaction rates over a chosen interval
Calculate and compare average disappearance rates with explicit signs, units and observation windows.
Test a constant-fraction reaction model
Explain first-order decay using equal fractional changes and test what it predicts about concentration and rate.
Explain temperature effects using activation barriers
Interpret an activation-energy diagram and use absolute temperature in an Arrhenius comparison without confusing rate constants with rates.
Speed both directions without moving equilibrium
Explain why a catalyst changes the approach to equilibrium while preserving its position at fixed temperature.
Reversible reactions and equilibrium
Explain equilibrium with two continuing reactions
Predict net reaction direction and explain a dynamic equilibrium using a conserved concentration ledger.
Acids, bases and neutralization
Connect proton transfer, water ions and pH
Distinguish acid strength, concentration and pH, and explain why acidic solutions are still electrically neutral.
Account for neutralization before calculating pH
Determine excess strong acid or base and calculate final ion concentrations without discarding spectator ions.
Separate acid strength, concentration and percent ionization
Use Ka, analytical concentration and conservation to explain pH and fractional ionization without treating strength as concentration.
Test why buffers resist change but have finite capacity
Explain buffer action using reacting amounts, equilibrium and charge balance, while distinguishing initial pH from resistance to a challenge.
Distinguish titration equivalence, detection and sampling
Calculate a strong-acid titration state and explain how endpoint choice and finite sampling affect an inferred concentration.
Oxidation, reduction and electron accounting
Balance oxidation and reduction without losing charge
Identify oxidation, reduction and agents, then reconcile half-reaction electron transfer with a balanced net ionic equation.
Trace both pathways through a galvanic cell
Explain why sustained discharge needs two charge pathways and calculate transferred charge from balanced electron stoichiometry.
Use electrode potentials without multiplying the voltage
Calculate a standard cell potential with a consistent convention and explain its thermodynamic scope.
Connect voltage, charge and reaction free energy
Calculate standard reaction free energy and keep reaction normalization, thermodynamic direction and rate distinct.
Predict voltage from unequal ion concentrations
Calculate and interpret a concentration-cell potential, reverse its direction and identify the equal-activity condition.
Convert electrical current into reaction amount
Apply electron stoichiometry to electrolysis while keeping current, charge, reaction amount and energy distinct.
Separate target product from total charge
Calculate product amount and required duration using an assigned current efficiency, including zero-charge and zero-efficiency cases.
Diagnose corrosion and protection at a damaged surface
Distinguish barrier protection, sacrificial protection and galvanic attack, and identify which route remains after a connection is interrupted.
Polymers and material resource decisions
Track atoms and end groups as polymer units join
Distinguish monomers, repeat units and finite end groups, and conserve atoms through an illustrative condensation process.
Distinguish collection from usable material recovery
Conserve material across a recovery process and distinguish collection rate, usable yield, recycled content and environmental evidence.
Projects, practice and evidence
Cumulative virtual investigation
Identify an unknown sample within a measurement budget, justify a separation and save a report snapshot for review. Public simulated evidence and text completeness do not establish independent mastery.
Investigate an unknown sampleCumulative practice and transfer
Connect quantities, mechanisms and evidence in twelve public cases. First responses, feedback exposure and editable reasoning drafts are saved separately from lesson completion.
Open chemistry transfer casesFurther study beyond this bounded sequence
Further empirical measurement and classification investigations, further electronic-structure evidence, further covalent structures and measured structure-property evidence, broader quantitative investigations, temperature-dependent solubility, measured/nonideal gas behavior, expanded thermochemistry, experimental rate laws, measured temperature and catalyst effects, equilibrium perturbations, weak-base and salt equilibria, broader buffer evidence, weak-acid titration and measured endpoint evidence are directions for additional study and investigations beyond the listed sequence. Authentic project evidence, independent assessment and practical participation still require real learner and educator records. Unauthored extensions do not award completion credit.
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