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Chemistry
Atoms, bonds, reactions and the chemistry of everyday life, from the periodic table to organic molecules.
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Chemistry on LearnViz HighSchoolEdu has 150 interactive topics. Each one has a plain-English explanation, a live animation you can control, key ideas to remember and a quick quiz. Chemistry explains medicine, food, cleaning products, fuels and building materials.
Matter and Measurement
1What Is Matter?Matter is anything that has mass and takes up space.2States of MatterSolids, liquids and gases differ in how particles are arranged and move.3Physical and Chemical ChangesPhysical changes alter form; chemical changes create new substances.4Pure Substances and MixturesPure substances have fixed composition; mixtures can vary.5Separation TechniquesFiltration, distillation and chromatography separate mixtures.6Elements, Compounds and MoleculesElements are one kind of atom; compounds bond different kinds.7SI Units and MeasurementChemistry uses SI units like kilogram, metre, litre and mole.8Significant FiguresSignificant figures show the precision of a measurement.9Density in ChemistryDensity links mass and volume and identifies substances.10Scientific Method in the LabHypothesis, experiment, data and conclusion drive chemistry.Atomic Structure
11The AtomAtoms are the tiny building blocks of matter.12Historical Atomic ModelsFrom Dalton to quantum mechanics, models of the atom keep improving.13Atomic Number and Mass NumberAtomic number is the number of protons; mass number is protons plus neutrons.14IsotopesIsotopes are atoms of one element with different numbers of neutrons.15IonsIons are atoms that have gained or lost electrons.16Electron ShellsElectrons occupy shells that hold 2, 8, 8 … electrons.17Electron ConfigurationElectron configuration lists where electrons live in orbitals.18Orbitals and Quantum NumbersOrbitals are regions where electrons are likely to be found.19Valence ElectronsOuter-shell electrons control how an atom bonds.20Atomic Mass and the MoleThe mole counts particles: 6.022 × 10²³ per mole.21Emission SpectraExcited atoms emit light at specific wavelengths.22Radioactive DecayUnstable nuclei emit radiation to become stable.23Nuclear EquationsNuclear equations balance mass numbers and atomic numbers.24Fission and Fusion in ChemistryNuclear reactions release far more energy than chemical ones.The Periodic Table
25Organising the Periodic TableElements are arranged by atomic number in periods and groups.26Metals, Non-metals and MetalloidsProperties change across the table.27Alkali MetalsGroup 1 metals are soft and violently reactive with water.28Alkaline Earth MetalsGroup 2 metals are reactive but less so than group 1.29HalogensGroup 17 non-metals form salts and are strong oxidisers.30Noble GasesGroup 18 elements have full shells and rarely react.31Transition MetalsTransition metals have variable charges and coloured compounds.32Atomic Radius TrendAtoms shrink across a period and grow down a group.33Ionization EnergyThe energy needed to remove an electron.34ElectronegativityElectronegativity measures how strongly an atom attracts bonding electrons.35Periodic Trends SummaryTrends in radius, ionization energy and electronegativity follow nuclear charge and shielding.36Naming Elements and SymbolsSymbols come from names, often Latin.Chemical Bonding
37Ionic BondingIonic bonds form when metals transfer electrons to non-metals.38Covalent BondingCovalent bonds share electron pairs.39Metallic BondingMetal atoms share a sea of delocalised electrons.40Lewis Dot StructuresLewis structures show valence electrons and bonds.41The Octet RuleAtoms bond to have eight valence electrons.42Polar and Nonpolar BondsUnequal sharing makes a polar bond.43Molecular GeometryVSEPR predicts shapes from electron-pair repulsion.44Intermolecular ForcesForces between molecules decide boiling points.45Hydrogen BondingHydrogen bonds link H to N, O or F on neighbouring molecules.46Properties of Ionic CompoundsIonic solids are hard, brittle, and conduct when dissolved or molten.47Properties of Covalent CompoundsMolecular substances have low melting points and rarely conduct.48Giant StructuresDiamond, graphite and silica are giant covalent structures.49Bond Energy and LengthStronger bonds are shorter and need more energy to break.50Resonance StructuresSome molecules are best described by several Lewis structures at once.Formulas and Naming
51Chemical FormulasA formula shows which atoms and how many are in a substance.52Naming Ionic CompoundsName the metal then the non-metal with an -ide ending.53Naming Covalent CompoundsGreek prefixes show the number of atoms.54Polyatomic IonsGroups of atoms carry a charge together.55Molar MassMolar mass sums the atomic masses in a formula.56Percent CompositionPercent composition shows each element's share of mass.Stoichiometry
57Balancing Chemical EquationsAtoms are conserved, so equations must balance.58The Mole ConceptThe mole converts between particles, mass and volume.59Mole RatiosCoefficients give mole ratios between substances.60Mass-to-Mass StoichiometryGrams → moles → mole ratio → moles → grams.61Limiting ReactantThe reactant that runs out first limits the product.62Percent YieldPercent yield compares actual to theoretical yield.63Empirical FormulaThe simplest whole-number ratio of atoms in a compound.64Molecular Formula from EmpiricalMultiply the empirical formula by a whole number.65Concentration and MolarityMolarity is moles of solute per litre of solution.66DilutionsAdding solvent lowers concentration without changing moles.67Titration CalculationsTitrations find an unknown concentration using a reaction with a known solution.68Gas StoichiometryGas volumes relate to moles at the same conditions.69Stoichiometry Word ProblemsTranslate words to balanced equations and ratios.70Law of Conservation of MassMass is neither created nor destroyed in chemical reactions.Gases and States of Matter
71Kinetic Molecular TheoryGas particles are tiny, far apart and in constant random motion.72Gas PressurePressure comes from particle collisions with container walls.73Boyle's LawAt constant temperature, P and V are inversely proportional.74Charles's LawAt constant pressure, V is proportional to Kelvin temperature.75Gay-Lussac's LawAt constant volume, P is proportional to Kelvin temperature.76Combined and Ideal Gas LawsPV = nRT combines every gas law.77Dalton's Law of Partial PressuresThe total pressure is the sum of each gas's partial pressure.78Graham's Law of EffusionLighter gases effuse faster.79Phase Changes and Heating CurvesTemperature plateaus during melting and boiling.80Vapor Pressure and BoilingA liquid boils when its vapor pressure equals external pressure.81Solids and Crystal StructureCrystalline solids have particles in repeating patterns.82Plasma and Other StatesPlasma is an ionized gas; Bose–Einstein condensates form near absolute zero.Solutions
83Solutions and SolubilityA solution is a solute dissolved in a solvent.84Solubility CurvesGraphs show how much dissolves at each temperature.85ElectrolytesElectrolytes form ions in water and conduct electricity.86Precipitation ReactionsMixing solutions can form an insoluble solid.87Colligative PropertiesDissolved particles change freezing and boiling points.88Osmosis and Diffusion in SolutionsParticles move from high to low concentration.89Colloids and SuspensionsLarger particles stay suspended without dissolving.90Concentration UnitsPercent, ppm and molarity express concentration.91Water as a SolventPolar water dissolves ionic and polar substances.92Heat of SolutionDissolving can absorb or release heat.Chemical Reactions
93Types of ReactionsReactions fall into synthesis, decomposition, single and double replacement and combustion.94Combustion ReactionsCombustion burns fuel in oxygen to release heat.95Single Replacement and the Activity SeriesA more reactive element displaces a less reactive one.96Double Replacement ReactionsIons swap partners, often forming a precipitate, gas or water.97Decomposition ReactionsOne compound breaks into simpler substances.98Net Ionic EquationsShow only the species that actually react.99Writing and Predicting ProductsUse reaction types to predict what forms.100Catalysts and EnzymesCatalysts speed reactions without being consumed.Energy and Rates
101Exothermic and Endothermic ReactionsExothermic reactions release heat; endothermic absorb it.102Enthalpy and Hess's LawTotal enthalpy change is independent of the path.103Activation EnergyReactions need a minimum energy to start.104Collision TheoryReactions occur when particles collide with enough energy and the right orientation.105Reaction RatesRate measures how fast reactants disappear or products appear.106Rate LawsRate = k[A]ᵐ[B]ⁿ links rate to concentration.107Chemical EquilibriumAt equilibrium forward and reverse rates are equal.108Le Chatelier's PrincipleA system at equilibrium shifts to oppose a disturbance.109Equilibrium ConstantK compares product to reactant concentrations at equilibrium.110Entropy and SpontaneityReactions favour more disorder and lower energy.Acids, Bases and Redox
111Acids and BasesAcids donate H⁺; bases accept H⁺ or donate OH⁻.112The pH ScalepH = −log[H⁺] measures acidity.113Strong and Weak AcidsStrong acids ionize completely; weak ones partly.114NeutralizationAcid plus base gives salt and water.115BuffersBuffers resist changes in pH.116Acid Rain and Environmental ChemistryPollutants lower rain pH and harm ecosystems.117Oxidation and ReductionOxidation loses electrons; reduction gains electrons.118Balancing Redox ReactionsBalance atoms and charges using half-reactions.119Galvanic CellsSpontaneous redox reactions make electricity.120ElectrolysisElectricity drives a non-spontaneous reaction.121Corrosion and RustingIron rusts when it meets oxygen and water.Organic and Applied Chemistry
122Introduction to Organic ChemistryOrganic chemistry studies carbon compounds.123AlkanesAlkanes are saturated hydrocarbons with single bonds.124Alkenes and AlkynesDouble and triple bonds make hydrocarbons unsaturated.125IsomersIsomers share a formula but have different structures.126Functional GroupsA functional group sets a molecule's reactions.127Alcohols and Carboxylic AcidsAlcohols contain –OH; carboxylic acids contain –COOH.128PolymersPolymers are long chains made from repeating monomers.129Biochemistry BasicsCarbohydrates, proteins, lipids and nucleic acids run life.130Petroleum and Fractional DistillationCrude oil is separated by boiling point into fuels.131Green ChemistryGreen chemistry reduces hazard and waste.132Chemical Safety and Lab SkillsSafe practices protect people and results.133Chemistry of Everyday LifeCooking, cleaning and cars all rely on chemistry.134Water TreatmentChemistry makes water safe to drink.135Atmospheric ChemistryThe atmosphere is a mix of gases that cycle through reactions.Applications and Extensions
136Mendeleev and the History of the Periodic TableMendeleev ordered elements by mass and left gaps for undiscovered ones.137Allotropes of CarbonDiamond, graphite, graphene and fullerenes are all pure carbon.138AlloysAlloys mix metals to improve strength or corrosion resistance.139Soaps and DetergentsSoap molecules have a water-loving head and a grease-loving tail.140Fertilisers and AgriculturePlants need nitrogen, phosphorus and potassium.141The Haber ProcessNitrogen and hydrogen combine to make ammonia under pressure.142The Contact Process and Sulfuric AcidSulfur dioxide is oxidised to make the world's most-made acid.143Extracting MetalsMetals are extracted from ores by reduction or electrolysis.144Chemistry of FireworksMetal salts burn in colours and oxidisers drive the show.145NanomaterialsMaterials at the nanometre scale have new properties.146Radiocarbon DatingCarbon-14 decays so we can date organic remains.147SpectroscopySpectroscopy identifies substances by how they interact with light.148Chromatography in DetailDifferent components travel at different speeds through a medium.149Chemistry in MedicineDrugs are molecules that fit receptors or block enzymes.150Sustainable Materials and RecyclingRecycling and bio-based materials cut waste.No topics match.
Frequently asked questions
What topics are in Chemistry?
There are 150 topics, including What Is Matter?, States of Matter, Physical and Chemical Changes, Pure Substances and Mixtures, Separation Techniques, and more.
Who is Chemistry on LearnViz for?
High school students who want to understand chemistry visually, teachers who want a quick classroom demonstration, and parents helping with homework.
Do I have to study the topics in order?
No. The list follows the order of the course, but every topic has its own page, so you can start wherever you need help.
How do I track my progress?
Open a topic and press “Mark as learned”. This subject page then shows how many topics you have completed. Progress is saved in your own browser.
How is Chemistry used in real life?
Chemistry explains medicine, food, cleaning products, fuels and building materials.