Specification points

Edexcel International GCSE (9–1) Chemistry 4CH1

214 points in 4 topics, with Edexcel's codes and titles.

Codes and titles are read by a script from Edexcel's published specification and have not been checked by a person. What each point covers is in the specification itself: Edexcel’s specification.

1 Principles of chemistry

1a States of matter
1.1 The three states of matter
1.2 Changes of state
1.3 Diffusion and dilution experiments
1.4 Solvent, solute, solution and saturated solution
1.5C Solubility in g per 100 g of solvent
1.6C Solubility curves
1.7C Practical: solubility of a solid in water
1b Elements, compounds and mixtures
1.8 Classifying substances as elements, compounds or mixtures
1.9 Melting and boiling points of pure substances and mixtures
1.10 Techniques for separating mixtures
1.11 Chromatograms and the composition of mixtures
1.12 Rf values
1.13 Practical: paper chromatography
1c Atomic structure
1.14 Atoms and molecules
1.15 Structure of the atom
1.16 Atomic number, mass number, isotopes and relative atomic mass
1.17 Calculating relative atomic mass from isotopic abundances
1d The Periodic Table
1.18 Arrangement of the Periodic Table
1.19 Electronic configurations of the first 20 elements
1.20 Classifying elements as metals or non-metals
1.21 Metals and non-metals in the Periodic Table
1.22 Electronic configuration and position in the Periodic Table
1.23 Similar chemical properties within a group
1.24 Unreactivity of the noble gases
1e Chemical formulae, equations and calculations
1.25 Word and balanced chemical equations
1.26 Relative formula mass
1.27 The mole
1.28 Calculations with amount of substance
1.29 Reacting masses
1.30 Percentage yield
1.31 Finding formulae experimentally
1.32 Empirical and molecular formulae
1.33 Calculating empirical and molecular formulae
1.34C Concentration calculations in mol/dm³
1.35C Gas volumes and molar volume
1.36 Practical: formula of a metal oxide
1f Ionic bonding
1.37 Formation of ions
1.38 Charges of common ions
1.39 Formulae of ionic compounds
1.40 Dot-and-cross diagrams for ionic compounds
1.41 Ionic bonding as electrostatic attraction
1.42 Melting and boiling points of giant ionic lattices
1.43 Electrical conductivity of ionic compounds
1g Covalent bonding
1.44 Covalent bonds
1.45 Covalent bonding and electrostatic attraction
1.46 Dot-and-cross diagrams for covalent molecules
1.47 Properties of simple molecular substances
1.48 Relative molecular mass and boiling points
1.49 Properties of giant covalent structures
1.50 Diamond, graphite and C60 fullerene
1.51 Electrical conductivity of covalent compounds
1h Metallic bonding
1.52C Diagrams of metallic lattices
1.53C Metallic bonding as electrostatic attraction
1.54C Physical properties of metals
1i Electrolysis
1.55C Why covalent compounds do not conduct
1.56C When ionic compounds conduct electricity
1.57C Anions and cations
1.58C Electrolysis experiments with inert electrodes
1.59C Half-equations at the electrodes
1.60C Practical: electrolysis of aqueous solutions

2 Inorganic chemistry

2a Group 1 (alkali metals) – lithium, sodium and potassium
2.1 Group 1 metals as a family
2.2 Trend in reactivity in Group 1
2.3 Predicting properties of alkali metals
2.4C Group 1 reactivity and electronic configuration
2b Group 7 (halogens) – chlorine, bromine and iodine
2.5 Properties of the halogens
2.6 Predicting properties of halogens
2.7 Halogen displacement reactions
2.8C Group 7 reactivity and electronic configuration
2c Gases in the atmosphere
2.9 Composition of dry air
2.10 Percentage of oxygen in air
2.11 Combustion of elements in oxygen
2.12 Thermal decomposition of metal carbonates
2.13 Carbon dioxide and climate change
2.14 Practical: percentage of oxygen in air
2d Reactivity series
2.15 Reactivity series: water and dilute acids
2.16 Reactivity series: displacement reactions
2.17 Order of reactivity of metals
2.18 Conditions for rusting
2.19 Preventing rusting
2.20 Oxidation, reduction and redox
2.21 Practical: metals with dilute acids
2e Extraction and uses of metals
2.22C Metal ores and native metals
2.23C Extraction method and the reactivity series
2.24C Evaluating metal extraction processes
2.25C Uses of aluminium, copper, iron and steel
2.26C Alloys
2.27C Why alloys are harder than pure metals
2f Acids, alkalis and titrations
2.28 Indicators for acids and alkalis
2.29 The pH scale
2.30 Universal indicator
2.31 Hydrogen and hydroxide ions in acids and alkalis
2.32 Neutralisation
2.33C Acid-alkali titration
2g Acids, bases and salt preparations
2.34 Solubility rules for ionic compounds
2.35 Acids and bases as proton transfer
2.36 Proton donors and acceptors
2.37 Reactions of acids forming salts
2.38 Bases and alkalis
2.39 Preparing a soluble salt from an insoluble reactant
2.40C Preparing a soluble salt from an acid and alkali
2.41C Preparing an insoluble salt by precipitation
2.42 Practical: preparing copper(II) sulfate crystals
2.43C Practical: preparing lead(II) sulfate
2h Chemical tests
2.44 Tests for gases
2.45 Flame tests
2.46 Flame test colours
2.47 Tests for cations
2.48 Tests for anions
2.49 Test for water
2.50 Testing the purity of water

3 Physical chemistry

3a Energetics
3.1 Exothermic and endothermic reactions
3.2 Simple calorimetry experiments
3.3 Heat energy change: Q = mcΔT
3.4 Molar enthalpy change
3.5C Energy level diagrams
3.6C Bond breaking and bond making
3.7C Enthalpy change from bond energies
3.8 Practical: temperature changes in reactions
3b Rates of reaction
3.9 Experiments on rates of reaction
3.10 Factors affecting the rate of reaction
3.11 Collision theory and rate of reaction
3.12 Catalysts
3.13 How catalysts work
3.14C Reaction profile diagrams
3.15 Practical: marble chips and hydrochloric acid
3.16 Practical: catalysts for decomposing hydrogen peroxide
3c Reversible reactions and equilibria
3.17 Reversible reactions
3.18 Examples of reversible reactions
3.19C Dynamic equilibrium
3.20C Characteristics of dynamic equilibrium
3.21C Catalysts and the position of equilibrium
3.22C Temperature, pressure and the position of equilibrium

4 Organic chemistry

4a Introduction
4.1 Hydrocarbons
4.2 Representing organic molecules
4.3 Homologous series, functional groups and isomerism
4.4 IUPAC naming of organic compounds
4.5 Structural and displayed formulae from molecular formulae
4.6 Substitution, addition and combustion reactions
4b Crude oil
4.7 Crude oil as a mixture of hydrocarbons
4.8 Fractional distillation of crude oil
4.9 Fractions of crude oil and their uses
4.10 Trends in properties of crude oil fractions
4.11 Fuels
4.12 Complete and incomplete combustion
4.13 Carbon monoxide poisoning
4.14 Oxides of nitrogen from car engines
4.15 Sulfur dioxide from fuel impurities
4.16 Acid rain
4.17 Catalytic cracking
4.18 Why cracking is necessary
4c Alkanes
4.19 General formula of alkanes
4.20 Alkanes as saturated hydrocarbons
4.21 Formulae and names of alkanes
4.22 Reactions of alkanes with halogens
4d Alkenes
4.23 The alkene functional group
4.24 General formula of alkenes
4.25 Alkenes as unsaturated hydrocarbons
4.26 Formulae and names of alkenes
4.27 Reactions of alkenes with bromine
4.28 Bromine water test for alkenes
4e Alcohols
4.29C The alcohol functional group
4.30C Formulae and names of alcohols
4.31C Oxidation of ethanol
4.32C Manufacture of ethanol
4.33C Conditions for fermentation
4f Carboxylic acids
4.34C The carboxylic acid functional group
4.35C Formulae and names of carboxylic acids
4.36C Reactions of carboxylic acids
4.37C Vinegar
4g Esters
4.38C The ester functional group
4.39C Making ethyl ethanoate
4.40C Formulae of ethyl ethanoate
4.41C Formulae of esters
4.42C Properties and uses of esters
4.43C Practical: preparing an ester
4h Synthetic polymers
4.44 Addition polymers and monomers
4.45 Repeat units of addition polymers
4.46 Monomers from repeat units
4.47 Problems disposing of addition polymers
4.48C Condensation polymerisation and polyesters
4.49C Formulae of polyesters
4.50C Biopolyesters