Your journey to excellence inChemistry
By Revision Genie
Solids, liquids and gases in the particle model (arrangement, movement, energy)
Questions are written as you practise.
Melting and freezing as particle/energy changes
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Boiling and condensing as particle/energy changes
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Evaporation as particle/energy changes
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Sublimation and deposition as particle/energy changes
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Dilution of coloured solutions explained with particles
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Diffusion of gases explained with particles
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Solvent, solute, solution and saturated solution
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Solubility in g per 100 g of solvent
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Plotting solubility curves
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Interpreting solubility curves
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Practical: solubility of a solid in water at a specific temperature
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Classifying substances as element, compound or mixture
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Pure substances vs mixtures using melting/boiling behaviour
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Simple distillation: separating a solvent from a solution
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Fractional distillation: separating liquids with different boiling points
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Filtration: separating an insoluble solid from a liquid
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Crystallisation: obtaining a soluble solid from a solution
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Paper chromatography: separating dissolved substances
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Reading a chromatogram to identify how many components are present
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Using Rf values to identify components
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Practical: paper chromatography using inks/food colourings
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What “atom” and “molecule” mean
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Subatomic particles: positions, relative masses and relative charges
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Atomic number and mass number
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Isotopes: what changes (neutrons) vs what stays the same (protons)
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Relative atomic mass (Ar) as a weighted mean
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Calculating Ar from isotopic abundances
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How the Periodic Table is arranged by atomic number
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Groups and periods: what they represent
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Deducing electron configurations for the first 20 elements
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Using electrical conductivity to classify metals vs non-metals
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Using oxide acid–base character to classify metals vs non-metals
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Identifying metal/non-metal from Periodic Table position
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Linking electron configuration to position in the Periodic Table
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Why elements in the same group have similar chemical properties
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Why noble gases are unreactive
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Writing word equations for reactions you’ve studied
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Writing balanced symbol equations (including state symbols)
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Calculating Mr from Ar values
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The mole as a unit for amount of substance
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Converting between moles, mass and Mr/Ar
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Using balanced equations to calculate reacting masses
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Percentage yield calculations
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Finding formulae experimentally: metal oxides (combustion/reduction idea)
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Water of crystallisation: recognising hydrated salts from formulae
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Empirical formula vs molecular formula
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Calculating empirical formula from experimental data
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Calculating molecular formula from empirical formula and Mr
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Concentration calculations in mol/dm³
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Gas volume calculations using molar volume at rtp (24 dm³)
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Practical: determine the formula of a metal oxide by combustion or reduction
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Building a reactivity series from reactions with water
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Building a reactivity series from reactions with dilute acids
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Displacement: metals displacing other metals from oxides
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Displacement: metals displacing other metals from salt solutions
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The required metal order in the reactivity series
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Rusting conditions for iron
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Preventing rust: barrier methods
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Preventing rust: galvanising
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Preventing rust: sacrificial protection
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Oxidation, reduction and redox (oxygen transfer definitions)
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Oxidation, reduction and redox (electron transfer definitions)
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Oxidising agents and reducing agents
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Practical: reactions of dilute acids with metals (Mg, Zn, Fe)
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Ores and metals in the Earth’s crust
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Why some unreactive metals are found native
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Extraction by reduction with carbon (iron as the example)
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Extraction by electrolysis (aluminium as the example)
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Comparing extraction methods using reactivity
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Commenting on an extraction process from unfamiliar information
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Aluminium: linking properties to uses
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Copper: linking properties to uses
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Iron and steel: linking properties to uses
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Types of steel: mild, high-carbon and stainless
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What an alloy is
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Why alloys are harder than pure metals
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Using litmus to identify acids and alkalis
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Using phenolphthalein to identify acids and alkalis
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Using methyl orange to identify acids and alkalis
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The pH scale (0–14) and what it measures
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Classifying solutions by pH (strong/weak acid/alkali, neutral)
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Using universal indicator to estimate pH
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Acids as a source of hydrogen ions (H⁺) in water
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Alkalis as a source of hydroxide ions (OH⁻) in water
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Neutralisation as acid + alkali
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Describing an acid–alkali titration method
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Solubility rules: Group 1 and ammonium compounds
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Solubility rules: nitrates
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Solubility rules: chlorides (including key exceptions)
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Solubility rules: sulfates (including key exceptions)
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Solubility rules: carbonates (including key exceptions)
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Solubility rules: hydroxides (including key exceptions)
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Acids and bases as proton transfer
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Acid as proton donor; base as proton acceptor
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Acid + metal reactions (HCl and H₂SO₄)
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Acid + base reactions (metal oxides/hydroxides, ammonia)
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Acid + carbonate reactions (CO₂ test link)
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Alkalis vs bases (soluble bases)
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Preparing a soluble salt from an insoluble reactant (method + reasons)
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Preparing a soluble salt from an acid and alkali (method + reasons)
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Preparing an insoluble salt by precipitation (two soluble reactants)
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Practical: make hydrated copper(II) sulfate crystals from copper(II) oxide
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Practical: prepare lead(II) sulfate
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Exothermic vs endothermic reactions (definitions)
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Recognising exothermic/endothermic from observations and temperature change
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Calorimetry basics: measuring temperature change safely and consistently
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Using Q = mcΔT to calculate heat energy change
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Converting Q to molar enthalpy change (ΔH)
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Energy level diagrams for exothermic reactions
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Energy level diagrams for endothermic reactions
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Bond breaking as endothermic; bond making as exothermic
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Using bond energies to calculate reaction enthalpy change
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Practical: temperature changes for dissolving, neutralisation, displacement, combustion
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What a hydrocarbon is
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Empirical vs molecular vs general formula in organic chemistry
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Structural vs displayed formulae (what each shows)
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Homologous series (patterns in formulae and properties)
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Functional groups (how they define families)
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Isomerism (same formula, different structure)
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IUPAC naming rules for simple organics (up to 6 carbons)
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Writing possible structures from a molecular formula
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Classifying reactions: substitution
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Classifying reactions: addition
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Classifying reactions: combustion
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Crude oil as a mixture of hydrocarbons
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Fractional distillation of crude oil (how it works)
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Main fractions: names and typical uses
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Trends across fractions: colour
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Trends across fractions: boiling point
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Trends across fractions: viscosity
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Fuels as energy-releasing substances
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Complete combustion products of hydrocarbons
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Incomplete combustion products of hydrocarbons
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Why carbon monoxide is poisonous (oxygen transport idea)
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Formation of nitrogen oxides in car engines (high temperature)
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Sulfur dioxide from impurities in fuels
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How SO₂ and NOₓ contribute to acid rain
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Catalytic cracking (conditions and catalyst)
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Why cracking is needed (supply and demand)
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General formula for alkanes
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Saturated hydrocarbons and what “saturated” means
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Drawing structural formulae for alkanes up to 5 carbons
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Drawing displayed formulae for alkanes up to 5 carbons
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Naming unbranched alkanes
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Naming unbranched-chain isomers (up to 5 carbons)
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Substitution with halogens under UV light
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Writing word/symbol equations for mono-substitution
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The C=C functional group
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General formula for alkenes
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Unsaturated hydrocarbons and what “unsaturated” means
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Drawing structural formulae for alkenes up to 4 carbons
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Drawing displayed formulae for alkenes up to 4 carbons
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Naming unbranched alkenes
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Naming unbranched-chain isomers (up to 4 carbons)
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Addition with bromine to form dibromoalkanes
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Bromine water test: telling an alkane from an alkene
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Forming ions by electron loss and gain
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Predicting ion charges from Group number (Groups 1, 2, 3, 5, 6, 7)
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Common named ions and charges (NH₄⁺, OH⁻, CO₃²⁻, NO₃⁻, SO₄²⁻)
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Writing ionic formulae from ion charges
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Dot-and-cross diagrams for ionic compounds (electron transfer)
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Ionic bonding as electrostatic attraction
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Giant ionic lattices and high melting/boiling points
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Conductivity: solid vs molten/aqueous ionic compounds
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Covalent bonds as shared pairs of electrons
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Covalent bonding as electrostatic attraction (shared pair and nuclei)
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Dot-and-cross: diatomic molecules (H₂, O₂, N₂, halogens)
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Dot-and-cross: hydrogen halides
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Dot-and-cross: H₂O, NH₃, CO₂
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Dot-and-cross: small organics up to two carbons (methane, ethane, ethene)
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Simple molecular substances: low melting/boiling points
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Intermolecular forces as attractions between molecules
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Boiling points increase with relative molecular mass (simple molecules)
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Giant covalent structures: why melting/boiling points are high
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Diamond: structure linked to hardness and conductivity
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Graphite: structure linked to conductivity and softness
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C₆₀ fullerene: structure linked to properties
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Why covalent compounds usually do not conduct electricity
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Representing a metallic lattice in 2D
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Metallic bonding as electrostatic attraction (ions and delocalised electrons)
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Electrical conductivity in metals explained by delocalised electrons
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Malleability in metals explained by layer movement
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Why covalent substances do not conduct (link to bonding)
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Why ionic substances conduct only when molten or in solution
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Cations and anions: definitions
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Electrolysis of molten lead(II) bromide: predicting products
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Electrolysis of aqueous sodium chloride: predicting products
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Electrolysis of dilute sulfuric acid: predicting products
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Electrolysis of aqueous copper(II) sulfate: predicting products
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Writing half-equations at the cathode and anode
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Electrolysis as redox (oxidation at anode, reduction at cathode)
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Practical: investigating electrolysis of aqueous solutions
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Similar reactions with water as evidence of a “family”
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Reactions with air and water as evidence of a reactivity trend
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Predicting properties of other Group 1 metals from trends
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Explaining Group 1 reactivity trend using electron configurations
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Colours and physical states of chlorine, bromine and iodine
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Trends in Group 7 physical properties
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Predicting properties of other halogens from trends
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Displacement reactions: halogens displacing halides
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Using displacement to deduce reactivity order
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Explaining Group 7 reactivity trend using electron configurations
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Percentages by volume of the four most abundant gases in dry air
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Measuring oxygen percentage using metal reactions (e.g. iron)
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Measuring oxygen percentage using non-metal reactions (e.g. phosphorus)
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Combustion in oxygen: magnesium
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Combustion in oxygen: hydrogen
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Combustion in oxygen: sulfur
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Thermal decomposition of carbonates to produce CO₂ (e.g. copper carbonate)
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Carbon dioxide as a greenhouse gas
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Linking increased CO₂ to climate change (basic understanding)
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Practical: determine oxygen percentage in air
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Test for hydrogen (pop test)
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Test for oxygen (relights a glowing splint)
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Test for carbon dioxide (limewater)
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Test for ammonia (damp red litmus turning blue)
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Test for chlorine (bleaches damp litmus)
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Flame test method (how to carry it out)
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Flame test colours: Li⁺, Na⁺, K⁺, Ca²⁺, Cu²⁺
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Test for NH₄⁺ using sodium hydroxide and the gas produced
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Test for Cu²⁺ using sodium hydroxide (precipitate)
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Test for Fe²⁺ using sodium hydroxide (precipitate)
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Test for Fe³⁺ using sodium hydroxide (precipitate)
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Test for Cl⁻/Br⁻/I⁻ using acidified silver nitrate
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Test for SO₄²⁻ using acidified barium chloride
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Test for CO₃²⁻ using hydrochloric acid and identifying CO₂
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Test for water using anhydrous copper(II) sulfate
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Physical purity test for water (sharp melting/boiling point)
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Measuring rate: what you can observe and record
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Designing rate experiments (variables and fair testing)
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Surface area effect on rate (describing and explaining)
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Concentration effect on rate (describing and explaining)
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Temperature effect on rate (describing and explaining)
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Pressure effect on rate (gases) (describing and explaining)
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Catalysts: definition and what “unchanged” means
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Collision theory: linking rate to collision frequency and energy
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Catalysts and activation energy (alternative pathway)
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Reaction profile diagrams showing ΔH and activation energy
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Practical: marble chips + hydrochloric acid (surface area and concentration)
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Practical: catalytic decomposition of hydrogen peroxide
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Identifying reversible reactions and using the ⇌ symbol
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Reversible: hydrated copper(II) sulfate dehydration/rehydration
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Reversible: heating ammonium chloride
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Dynamic equilibrium in a sealed container
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Features of dynamic equilibrium (equal rates; constant concentrations)
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Why a catalyst does not change the position of equilibrium
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Temperature changes and equilibrium position (endo/exo direction)
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Pressure changes and equilibrium position (moles of gas idea)
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The −OH functional group
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Drawing and naming methanol
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Drawing and naming ethanol
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Drawing and naming propan-1-ol (propanol)
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Drawing and naming butan-1-ol (butanol)
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Ethanol oxidation by complete combustion
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Ethanol oxidation by microbial oxidation to ethanoic acid
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Ethanol oxidation using acidified potassium dichromate(VI)
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Manufacturing ethanol by hydration of ethene (conditions and catalyst)
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Manufacturing ethanol by fermentation of glucose (conditions)
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Why fermentation needs no air and an optimum temperature
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The carboxyl functional group
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Drawing and naming unbranched carboxylic acids up to 4 carbons
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Carboxylic acids reacting with metals
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Carboxylic acids reacting with carbonates
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Vinegar as ethanoic acid solution
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The ester functional group
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Making ethyl ethanoate from ethanol + ethanoic acid (acid catalyst)
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Structural and displayed formula of ethyl ethanoate
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Working out an ester structure from the alcohol + carboxylic acid
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Working backwards from an ester to its alcohol + carboxylic acid
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Esters as volatile substances with distinctive smells
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Ester uses: food flavourings and perfumes
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Practical: preparing an ester (e.g. ethyl ethanoate)
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Addition polymerisation and the idea of monomers
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Drawing repeat units: poly(ethene)
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Drawing repeat units: poly(propene)
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Drawing repeat units: poly(chloroethene)
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Drawing repeat units: (poly)tetrafluoroethene
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Deducing a monomer from an addition polymer repeat unit
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Deducing a repeat unit from a monomer
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Disposal problems: inertness and non-biodegradability
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Disposal problems: toxic gases from burning some polymers
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Condensation polymerisation: diol + dicarboxylic acid → polyester + water
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Writing a polyester repeat unit from given monomers (incl. ethanedioic acid + ethanediol)
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Biopolyesters and biodegradability
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Turning a research question into a testable hypothesis
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Identifying independent, dependent and control variables
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Choosing apparatus and measurement methods for precision
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Recording observations in a clear, repeatable method
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Presenting data in tables with headings and units
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Plotting graphs with sensible scales and labelled axes
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Drawing conclusions that match the evidence
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Spotting anomalies and suggesting reasons
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Reliability: repeats and identifying random error
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Accuracy vs precision (and how to improve both)
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Validity: controlling variables and fair testing
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Evaluating a method (limitations, improvements)
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Safe practical technique and risk control in chemistry contexts
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Using decimal numbers and standard form in chemistry contexts
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Ratios, fractions and percentages in chemistry problems (yield, composition)
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Using appropriate significant figures
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Using means/averages for repeated measurements
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Bar charts and frequency representations for data
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Scatter graphs to identify patterns and trends
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Changing the subject of an equation (e.g. Q = mcΔT, concentration equations)
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Substituting values with correct units
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Solving simple equations for unknowns
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Finding gradient and intercept from linear graphs
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Using a tangent to estimate rate of change on a curve
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Estimating area under a curve by counting squares
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Thermal decomposition of different carbonates (compare ease)
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Comparing energy released by different fuels (temperature rise)
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Burning candles: air used up and products formed
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Calcium compounds: CaCO₃ decomposition; CaO + water; CaCO₃ + acid
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Neutralisation reactions using oxides/hydroxides/carbonates
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Electrolysis of seawater or acidified water
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Investigating rusting of iron (variables and prevention)
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Oxidation/reduction in combustion and competition reactions
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Fractional distillation of synthetic crude oil (fractions + properties)
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Cracking paraffin oil
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Testing precipitate predictions when mixing soluble salts
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Ion tests to identify unknown compounds
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Heating a hydrated salt to find water of crystallisation
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