Log In
Log In
Two papers · twelve modules · taught by simulacra of chemistry’s foundational figures
The complete Pearson Edexcel GCSE Chemistry 1CH0 specification, taught one-on-one by simulacra of the people who built chemistry as a discipline. Each module covers one Topic of the spec in full — from atoms and isotopes, through the periodic table and bonding, the calculations and the mole, states of matter and mixtures, chemical changes (acids, bases, electrolysis), the extraction of metals and equilibria, and the quantitative-and-transition chemistry that closes Paper 1, to the groups in the periodic table, rates and energy changes, fuels and Earth science, and organic chemistry, polymers, and analysis (Paper 2).
What is distinctive is who teaches. John Dalton — the schoolmaster who in 1808 published A New System of Chemical Philosophy establishing the modern atomic theory — opens the programme on atoms and isotopes. Dmitri Mendeleev walks the student through the periodic table he himself constructed in 1869. Linus Pauling teaches bonding and structure, the territory of his 1939 Nature of the Chemical Bond. Berzelius teaches the calculations and the mole; Robert Boyle teaches states of matter and mixtures; Antoine Lavoisier teaches chemical changes including all three core practicals on pH, salt preparation, and electrolysis. Humphry Davy teaches the extraction of metals and equilibria; Michael Faraday closes Paper 1 with the quantitative and transition-metal chemistry. Paper 2 is led by Mendeleev returning for the periodic groups, Svante Arrhenius on rates and energy, James Lovelock on fuels and Earth science, and Friedrich August Kekulé on organic chemistry, polymers, and analysis.
The twelve modules are independently enrolable. A student preparing the full Edexcel paper works through all twelve in order. A student revising one specific topic — bonding, electrolysis, the Haber process, the H–R diagram, organic mechanisms — can take that module alone. The format is Oxford-Cambridge tutorial throughout: one student, one simulacrum, ZPD-paced, with the host’s real disciplinary voice and habits of mind operative throughout the conversation. All Core Practicals (2.11, 3.6, 3.17, 3.31, 5.9C, 7.1, 9.6C, 9.28C) are integrated into the relevant modules.
Eight modules covering Topics 1 through 5: the atomic and bonding foundations, states of matter, the central acid-base-redox chemistry, metal extraction and equilibria, and the quantitative-transition closer.
The opening module establishes the atomic theory every chemical fact in the rest of the course will rest on. Led by John Dalton, whose 1808 A New System of Chemical Philosophy established that matter consists of indivisible atoms in fixed-ratio combinations, the module covers atomic structure (protons, neutrons, electrons), atomic and mass number, isotopes, and the calculation of relative atomic mass from isotopic data.
The second module turns to the central organisation of chemistry. Led by Dmitri Mendeleev, who in 1869 arranged the 63 known elements into the periodic table, left gaps for elements not yet discovered, and predicted gallium, scandium, and germanium with their properties before they were found. The module covers Mendeleev’s 1869 arrangement, his anomalies and Moseley’s 1913 atomic-number resolution, the modern table’s structure, the metal/non-metal divide, and electronic configurations of the first 20 elements.
The largest module of Paper 1: 22 spec points covering ionic bonding (with dot-and-cross diagrams for groups 1, 2, 6, 7), covalent bonding (with the spec’s six required small molecules), the four bonding classes and their physical properties, giant covalent (diamond, graphite, fullerenes, graphene), polymers, metallic bonding via the cation-and-electron-sea model, and the limitations of structural representations. Led by Linus Pauling, whose 1939 The Nature of the Chemical Bond applied quantum mechanics to chemistry and won the 1954 Nobel Prize.
The quantitative spine of the course: relative formula mass, percentage composition, empirical and molecular formulae, conservation of mass, balanced-equation calculations, and (Higher) the mole, Avogadro’s constant, limiting reactants, and stoichiometry from experimental data. Led by Jöns Jacob Berzelius, who between 1813 and 1828 gave chemistry its alphabet — the symbol notation that lets every chemical statement be written precisely.
The first explicit experimental module: the particle model in three states, the six interconversions, distinguishing pure substances from mixtures via melting-point evidence, the five separation techniques, paper chromatography with Rf calculations, Core Practical 2.11 on inks, and water treatment for potability. Led by Robert Boyle, the seventeenth-century natural philosopher whose 1661 Sceptical Chymist drew the line between alchemy and chemistry.
The largest module in Paper 1 alongside Module 3: 31 spec points and three Core Practicals covering acids, alkalis, the pH scale (with Higher-tier factor-of-ten H+ reasoning), the four acid-reaction patterns, neutralisation, salt preparation by both insoluble-base and titration routes (Core Practical 3.17), the solubility rules and precipitation, and electrolysis (with Core Practical 3.31). Also Core Practical 3.6 on the pH change with calcium hydroxide. Led by Antoine Lavoisier, whose 1789 Traité Élémentaire de Chimie established modern chemistry by destroying the phlogiston theory.
The reactivity series and metal extraction (carbon reduction vs electrolysis) including (Higher) biological extraction, life-cycle assessment, and recycling; reversible reactions and dynamic equilibrium; the Haber process and (Higher) the prediction of equilibrium response to changes in temperature, pressure, and concentration. Led by Sir Humphry Davy, the Cornish chemist who between 1807 and 1808 isolated potassium, sodium, calcium, magnesium, strontium, and barium for the first time by electrolysing their molten compounds.
The closing module of Paper 1, all Higher Tier and Separate Chemistry only: transition metals, corrosion and rust prevention, electroplating, alloys, concentration in mol dm−3, Core Practical 5.9C on accurate titrations, percentage yield and atom economy, molar volume and Avogadro’s law, the Haber process at industrial detail with NPK fertilisers, and chemical and hydrogen-oxygen fuel cells. Led by Michael Faraday, the bookbinder’s apprentice who became Davy’s assistant and the most important experimentalist of the nineteenth century.
Four modules covering Topics 6 through 9: the periodic groups, rates and energy changes, fuels and Earth science, and the organic-polymers-and-analysis closer.
Group 1 alkali metals (with the spec-required reactions of Li, Na, K with water and the reactivity-trend explanation), Group 7 halogens (with metal-halide and hydrogen-halide reactions, displacement reactivity, and the chlorine test), and Group 0 noble gases (inertness, uses, physical trends). Led by Mendeleev returning from Module 2 — this is the chemistry of his table’s columns.
Collision theory and the four rate factors (temperature, concentration, surface area, pressure), catalysts and activation energy, exothermic and endothermic reactions, the bond-energy basis of ΔH (with Higher-tier quantitative calculations), and reaction profiles. Includes Core Practical 7.1 on rates by gas production and the disappearing-cross method. Led by Svante Arrhenius, the Swedish physical chemist whose 1889 equation k = Ae−Ea/RT gave rate-temperature its quantitative form.
Hydrocarbons and crude oil, fractional distillation and the six required fractions, the homologous series (alkanes), complete and incomplete combustion (with CO toxicity and incomplete-combustion hazards), SO2 and NOx pollution and acid rain, hydrogen vs petrol, cracking, the Earth’s atmospheric history (volcanic outgassing, ocean formation, CO2 removal into limestone, oxygen accumulation from photosynthesis), the greenhouse effect, and the modern climate-change evidence and mitigation question. Led by James Lovelock, whose Gaia hypothesis reframed Earth as a coupled biological-chemical system.
The largest single module in the course (39 spec points), all Higher Tier and Separate Chemistry only: cation flame-tests and NaOH precipitation tests; carbonate, sulfate, halide anion tests; Core Practical 9.6C on identifying ions; instrumental analysis (spectroscopy, mass spectrometry); alkanes, alkenes, the bromine-water test, addition reactions; addition polymerisation; condensation polymerisation and natural polymers; alcohols and Core Practical 9.28C on alcohol oxidation; carboxylic acids; fermentation; nanoparticles. Led by Friedrich August Kekulé, who in 1865 dreamed of an ouroboros and woke knowing the structure of benzene.