Specification points
Edexcel GCSE Chemistry 1CH0
253 points in 10 topics, with Edexcel's codes and titles.
Grade boundaries·Edexcel command words
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.
0 Formulae, equations and hazards
1 Key concepts in chemistry
- 1.1 Development of the model of the atom
- 1.2 Structure of an atom
- 1.3 Relative charge and mass of subatomic particles
- 1.4 Equal numbers of protons and electrons
- 1.5 Size of the nucleus
- 1.6 Mass concentrated in the nucleus
- 1.7 Mass number
- 1.8 Proton number unique to each element
- 1.9 Isotopes
- 1.10 Numbers of protons, neutrons and electrons in atoms
- 1.11 Isotopes and non-integer relative atomic masses
- 1.12 Calculating relative atomic mass
- 1.13 Mendeleev's periodic table
- 1.14 Mendeleev's predictions of undiscovered elements
- 1.15 Mendeleev's ordering and relative atomic mass
- 1.16 Atomic number and position in the periodic table
- 1.17 Periods and groups in the periodic table
- 1.18 Metals and non-metals in the periodic table
- 1.19 Electronic configurations of the first 20 elements
- 1.20 Electronic configuration and periodic table position
- 1.21 Formation of ionic bonds
- 1.22 Definition of an ion
- 1.23 Protons, neutrons and electrons in simple ions
- 1.24 Formation of ions in ionic compounds
- 1.25 The endings -ide and -ate
- 1.26 Formulae of ionic compounds
- 1.27 Ionic lattice structures
- 1.28 Formation of covalent bonds
- 1.29 Covalent bonding forming molecules
- 1.30 Size of atoms and small molecules
- 1.31 Dot and cross diagrams of simple molecules
- 1.32 Classifying substances by structure and bonding
- 1.33 Properties of ionic compounds
- 1.34 Properties of simple molecular compounds
- 1.35 Graphite and diamond as giant covalent substances
- 1.36 Structures of graphite and diamond
- 1.37 Uses of graphite and diamond
- 1.38 Fullerenes and graphene
- 1.39 Simple polymers such as poly(ethene)
- 1.40 Properties of metals
- 1.41 Limitations of models and representations
- 1.42 Physical properties of metals and non-metals
- 1.43 Relative formula mass and percentage by mass
- 1.44 Empirical formulae from reacting masses
- 1.45 Empirical and molecular formulae
- 1.46 Experiment to find an empirical formula
- 1.47 Conservation of mass
- 1.48 Reacting masses from equations
- 1.49 Concentration in g dm⁻³
- 1.50 The mole and the Avogadro constant
- 1.51 Calculating moles and numbers of particles
- 1.52 Limiting reactants
- 1.53 Stoichiometry from reacting masses
2 States of matter and mixtures
- 2.1 Particles in the three states of matter
- 2.2 Changes of state
- 2.3 Particle changes during changes of state
- 2.4 Predicting physical state from data
- 2.5 Pure substances and mixtures
- 2.6 Melting point and purity
- 2.7 Separation techniques
- 2.8 Choosing a separation technique
- 2.9 Paper chromatography
- 2.10 Interpreting chromatograms
- 2.11 Core practical: composition of inks
- 2.12 Producing potable water
3 Chemical changes
- 3.1 Acids and alkalis as sources of ions
- 3.2 The pH scale
- 3.3 Indicators
- 3.4 Ion concentration and pH
- 3.5 Tenfold changes in hydrogen ion concentration
- 3.6 Core practical: pH change in neutralisation
- 3.7 Dilute and concentrated solutions
- 3.8 Strong and weak acids
- 3.9 Bases
- 3.10 Alkalis as soluble bases
- 3.11 Reactions of acids forming salts
- 3.12 Tests for hydrogen and carbon dioxide
- 3.13 Neutralisation
- 3.14 Neutralisation in terms of ions
- 3.15 Soluble salts from insoluble reactants
- 3.16 Soluble salts by titration
- 3.17 Core practical: copper sulfate crystals
- 3.18 Acid-alkali titration to prepare a salt
- 3.19 Solubility rules
- 3.20 Predicting precipitates
- 3.21 Preparing an insoluble salt
- 3.22 Electrolytes
- 3.23 Electrolysis
- 3.24 Movement of ions in electrolysis
- 3.25 Products of electrolysis with inert electrodes
- 3.26 Electrolysis of molten binary compounds
- 3.27 Half equations in electrolysis
- 3.28 Oxidation and reduction as electron transfer
- 3.29 Oxidation and reduction at the electrodes
- 3.30 Electrolysis of copper sulfate and purifying copper
- 3.31 Core practical: electrolysis of copper sulfate
4 Extracting metals and equilibria
- 4.1 Relative reactivity of metals
- 4.2 Displacement reactions as redox
- 4.3 The reactivity series
- 4.4 Metal ores and native metals
- 4.5 Oxidation and reduction as oxygen gain and loss
- 4.6 Extraction of metals by reduction
- 4.7 Choosing a method of metal extraction
- 4.8 Biological methods of metal extraction
- 4.9 Resistance to oxidation and reactivity
- 4.10 Recycling metals
- 4.11 Life-cycle assessment
- 4.12 Evaluating life-cycle assessment data
- 4.13 Reversible reactions
- 4.14 Dynamic equilibrium
- 4.15 Formation of ammonia
- 4.16 Conditions for the Haber process
- 4.17 Effects of conditions on equilibrium position
5 Separate chemistry 1
- 5.1C Properties of transition metals
- 5.2C Corrosion
- 5.3C Preventing rusting
- 5.4C Electroplating
- 5.5C Alloys and strength
- 5.6C Alloy steels
- 5.7C Uses of metals and alloys
- 5.8C Concentration in mol dm⁻³
- 5.9C Core practical: acid-alkali titration
- 5.10C Titration calculations
- 5.11C Percentage yield
- 5.12C Reasons for lower actual yields
- 5.13C Atom economy
- 5.14C Calculating atom economy
- 5.15C Choosing a reaction pathway
- 5.16C Molar volume of a gas
- 5.17C Calculations with molar volume
- 5.18C Avogadro's law and gas volumes
- 5.19C The Haber process
- 5.20C Rate of attainment of equilibrium
- 5.21C Choosing conditions in industrial reactions
- 5.22C Fertilisers: nitrogen, phosphorus and potassium
- 5.23C Ammonia and nitric acid making fertiliser
- 5.24C Making ammonium sulfate in the lab and industry
- 5.25C Chemical cells
- 5.26C Hydrogen-oxygen fuel cells
- 5.27C Strengths and weaknesses of fuel cells
6 Groups in the periodic table
- 6.1 Alkali metals, halogens and noble gases
- 6.2 Physical properties of alkali metals
- 6.3 Reactions of alkali metals with water
- 6.4 Reactivity pattern of alkali metals
- 6.5 Alkali metal reactivity and electronic configuration
- 6.6 Colours and states of the halogens
- 6.7 Physical properties of the halogens
- 6.8 Test for chlorine
- 6.9 Halogens reacting with metals
- 6.10 Hydrogen halides
- 6.11 Halogen displacement reactions
- 6.12 Halogen displacement as redox
- 6.13 Halogen reactivity and electronic configuration
- 6.14 Inertness of the noble gases
- 6.15 Uses of noble gases
- 6.16 Physical properties of the noble gases
7 Rates of reaction and energy changes
- 7.1 Core practical: conditions and rates of reaction
- 7.2 Methods for measuring rate of reaction
- 7.3 Collisions and rate of reaction
- 7.4 Factors affecting rate of reaction
- 7.5 Interpreting rate graphs
- 7.6 Catalysts
- 7.7 Catalysts and activation energy
- 7.8 Enzymes as catalysts in making alcoholic drinks
- 7.9 Heat energy changes in reactions
- 7.10 Exothermic changes
- 7.11 Endothermic changes
- 7.12 Bond breaking and bond making
- 7.13 Overall energy change from bond energies
- 7.14 Calculating energy change from bond energies
- 7.15 Activation energy
- 7.16 Reaction profiles
8 Fuels and Earth science
- 8.1 Hydrocarbons
- 8.2 Crude oil
- 8.3 Fractional distillation of crude oil
- 8.4 Crude oil fractions and their uses
- 8.5 How fractions differ
- 8.6 Homologous series
- 8.7 Complete combustion of hydrocarbons
- 8.8 Incomplete combustion
- 8.9 Toxicity of carbon monoxide
- 8.10 Problems of carbon monoxide and soot
- 8.11 Sulfur dioxide from fuel impurities
- 8.12 Acid rain
- 8.13 Oxides of nitrogen from engines
- 8.14 Hydrogen versus petrol as a car fuel
- 8.15 Non-renewable fossil fuels
- 8.16 Cracking
- 8.17 Why cracking is necessary
- 8.18 Volcanic origin of the early atmosphere
- 8.19 Composition of the early atmosphere
- 8.20 Formation of the oceans
- 8.21 Carbon dioxide dissolving in the oceans
- 8.22 Photosynthesis increasing atmospheric oxygen
- 8.23 Test for oxygen
- 8.24 The greenhouse effect
- 8.25 Evidence for human activity causing climate change
- 8.26 Today's atmosphere and effects of greenhouse gases
9 Separate chemistry 2
- 9.1C Why ion tests must be unique
- 9.2C Flame tests
- 9.3C Tests for metal ions
- 9.4C Test for ammonia
- 9.5C Tests for negative ions
- 9.6C Core practical: identifying ions in unknown salts
- 9.7C Identifying ions from test results
- 9.8C Instrumental methods of analysis
- 9.9C Flame photometry
- 9.10C Formulae and structures of alkanes
- 9.11C Alkanes as saturated hydrocarbons
- 9.12C Formulae and structures of alkenes
- 9.13C Alkenes as unsaturated hydrocarbons
- 9.14C Addition of bromine to alkenes
- 9.15C Bromine water test for alkenes
- 9.16C Complete combustion of alkanes and alkenes
- 9.17C Polymers
- 9.18C Polymerisation of ethene
- 9.19C Other addition polymers
- 9.20C Monomers and addition polymers
- 9.21C Uses and properties of polymers
- 9.22C Polyesters as condensation polymers
- 9.23C Problems associated with polymers
- 9.24C Recycling polymers
- 9.25C Naturally occurring polymers
- 9.26C Formulae and structures of alcohols
- 9.27C Alcohol functional group and dehydration
- 9.28C Core practical: combustion of alcohols
- 9.29C Formulae and structures of carboxylic acids
- 9.30C Carboxylic acid functional group and properties
- 9.31C Oxidation of alcohols to carboxylic acids
- 9.32C Predicting reactions from functional groups
- 9.33C Ethanol by fermentation
- 9.34C Concentrating ethanol by fractional distillation
- 9.35C Size of nanoparticles
- 9.36C Properties and uses of nanoparticulate materials
- 9.37C Risks of nanoparticulate materials
- 9.38C Properties of ceramics, polymers, composites and metals
- 9.39C Selecting materials for a given use