Key term
Edexcel GCSE Chemistry 1CH0
Key Concepts in Chemistry
Topic overviewFormulae, word equations and balanced equationsHazard symbols and assessing riskThe changing model of the atomProtons, neutrons and electronsThe nucleus, mass number and atomic massElements and isotopesCalculating particle numbers and relative atomic massMendeleev's periodic tableHow the modern periodic table is arrangedElectronic configuration and the periodic tableHow ionic bonds formIons in ionic compoundsFormulae of ionic compounds and ionic equationsNaming compounds and the ionic latticeCovalent bonds and moleculesDot and cross diagrams for simple moleculesClassifying substances and the properties of ionic compoundsProperties of simple molecular substances, and forms of carbonGraphite and diamondFullerenes and graphenePolymers and models of bondingThe properties of metalsRelative formula mass and percentage compositionEmpirical and molecular formulaeConservation of mass in closed and open systemsReacting masses from balanced equationsConcentration in grams per cubic decimetreMoles and the Avogadro constantLimiting reactants and stoichiometry
States of Matter and Mixtures
Topic overviewThe three states of matter and changes of stateEnergy changes during changes of state, and predicting statePure substances and melting point dataChoosing a separation techniqueSeparating a mixture in practicePaper chromatography and interpreting a chromatogramInvestigating inks by distillation and chromatographyMaking water potable
Chemical Changes
Topic overviewAcids, alkalis and the pH scaleIndicators: litmus, methyl orange and phenolphthaleinHydrogen ion concentration and the pH scaleInvestigating pH change when neutralising an acidDilute and concentrated, weak and strong acidsBases and alkalisReactions of acids, and testing for hydrogen and carbon dioxideNeutralisation and its ionic equationPreparing soluble salts from insoluble and soluble reactantsPreparing pure, dry copper sulfate crystalsCarrying out an acid-alkali titrationSolubility rulesPredicting precipitates and preparing an insoluble saltElectrolytes and what electrolysis isMovement of ions and predicting the products of molten electrolysisElectrolysis with inert electrodesWriting half equationsOxidation and reduction at the electrodesElectrolysis of copper sulfate solutionInvestigating the electrolysis of copper sulfate
Extracting Metals and Equilibria
Topic overviewInvestigating the reactivity of metalsDisplacement reactions as redox reactionsThe reactivity seriesOres, oxidation and reductionChoosing a method to extract a metalBiological methods of metal extractionCorrosion resistance and recycling metalsLife cycle assessmentReversible reactions and dynamic equilibriumThe Haber process and its conditionsChanging the position of an equilibrium
Transition Metals, Quantitative Chemistry and Industrial Processes
Topic overviewTransition metals and their propertiesCorrosion and electroplatingPreventing rustingAlloys and alloy steelsHow the uses of metals relate to their propertiesConcentration in mol dm-3 and titration calculationsCarrying out an accurate titrationPercentage yieldAtom economy and choosing a reaction pathwayMolar volume of a gasAvogadro's law and gas volumesThe Haber processConditions used in industrial reactionsFertilisers and ammonium saltsPreparing ammonium sulfate in the lab and in industryChemical cells and fuel cellsEvaluating fuel cells
Groups in the Periodic Table
Topic overviewThe groups of the periodic table, and the alkali metalsReactions of the alkali metals with waterThe pattern in alkali metal reactivity and why it happensPhysical properties of the halogensThe test for chlorine, and halogens reacting with metalsHydrogen halides, and explaining halogen reactivityDisplacement reactions of the halogensGroup 0: the noble gases
Rates of Reaction and Energy Changes
Topic overviewInvestigating the rate of a reactionMeasuring rate and interpreting rate graphsCollision theory and factors affecting rateCatalysts and enzymesExothermic and endothermic changesBond breaking, bond making and the overall energy changeBond energies, activation energy and reaction profiles
Fuels and Earth Science
Topic overviewHydrocarbons and crude oilFractional distillation and the fractionsProperties of the fractions and homologous seriesComplete and incomplete combustionCarbon monoxide and sootPollutants and acid rainHydrogen and fossil fuels comparedCracking and why it is necessaryThe Earth's early atmosphereHow the oceans formed and how oxygen appearedThe test for oxygen and the greenhouse gasesToday's atmosphere and evidence for climate change
Chemical Analysis, Organic Chemistry and Materials
Topic overviewWhy an ion test must be unique, and flame testsTests for metal ions and for ammoniaTests for carbonate, sulfate and halide ionsIdentifying the ions in an unknown saltInstrumental methods and flame photometryAlkanes and why they are saturatedAlkenes and why they are unsaturatedReactions of alkenes, and combustionWhat a polymer is, and how poly(ethene) formsOther addition polymers, and monomers from polymersUses of polymers, and natural polymers including DNAPolyesters and condensation polymerisationProblems with polymers and recyclingAlcohols and the -OH functional groupComparing the energy released by alcohol fuelsMaking ethanol by fermentation and distillationCarboxylic acids and the -COOH functional groupOxidising alcohols to carboxylic acids, and homologous seriesThe size of nanoparticlesUses and risks of nanoparticlesChoosing a material for a use
Chemical Analysis, Organic Chemistry and Materials
- 21 subtopics
- 45 things to know
- Paper 2
What Chemical Analysis, Organic Chemistry and Materials covers
Chemical Analysis, Organic Chemistry and Materials is examined in Paper 2, Chemistry 2. It covers why an ion test must be unique, and flame tests, tests for metal ions and for ammonia, tests for carbonate, sulfate and halide ions, identifying the ions in an unknown salt, instrumental methods and flame photometry, alkanes and why they are saturated, alkenes and why they are unsaturated, reactions of alkenes, and combustion, what a polymer is, and how poly(ethene) forms, other addition polymers, and monomers from polymers, uses of polymers, and natural polymers including DNA, polyesters and condensation polymerisation, problems with polymers and recycling, alcohols and the -OH functional group, comparing the energy released by alcohol fuels, making ethanol by fermentation and distillation, carboxylic acids and the -COOH functional group, oxidising alcohols to carboxylic acids, and homologous series, the size of nanoparticles, uses and risks of nanoparticles and choosing a material for a use.
Where it is assessed
Paper 2
Chemistry 2: 1 hour 45 minutes, 100 marks, 50% of the GCSE.
Check the Pearson Edexcel specification ↗The 21 subtopics
Each one has its own page.
- Why an ion test must be unique, and flame testsWhy a test result must be unique to one ion and why known compounds are tested alongside, the flame colours of lithium, sodium, potassium, calcium and copper, and how the test is carried out.Open →
- Tests for metal ions and for ammoniaThe precipitates formed with sodium hydroxide solution by aluminium, calcium, copper, iron(II) and iron(III) ions, telling aluminium from calcium, the equation for copper(II) sulfate, and the tests for ammonium ions and ammonia gas with damp red litmus.Open →
- Tests for carbonate, sulfate and halide ionsThe acid and limewater test for carbonate ions, the acidified barium chloride test for sulfate ions, the acidified silver nitrate test for chloride, bromide and iodide ions and their precipitate colours, and why each acid is added first.Open →
- Identifying the ions in an unknown saltThe order of tests for an unknown salt, why the wire is cleaned and distilled water used, the sources of error and safety precautions, and naming salts from combined test results.Open →
- Instrumental methods and flame photometryWhat instrumental methods are and their advantages and disadvantages, using a calibration curve to find a concentration and diluting samples beyond its range, and identifying metal ions with a flame photometer by comparison with reference data.Open →
- Alkanes and why they are saturatedThe formulae and bonding of methane, ethane, propane and butane, the general formula CₙH₂ₙ₊₂, and why alkanes are saturated hydrocarbons containing only single bonds.Open →
- Alkenes and why they are unsaturatedThe formulae of ethene, propene and butene, the general formula CₙH₂ₙ, the structures of but-1-ene and but-2-ene, the C=C functional group, and why alkenes are unsaturated.Open →
- Reactions of alkenes, and combustionAddition reactions of ethene, propene and but-1-ene with bromine and their products, using bromine water to tell an alkane from an alkene, and the complete combustion of alkanes and alkenes as oxidation, with balanced equations.Open →
- What a polymer is, and how poly(ethene) formsWhat polymers, monomers and repeating units are and why a polymer's relative molecular mass is an average, and how ethene's double bond opens in addition polymerisation to form poly(ethene) with the repeating unit –CH₂–CH₂–.Open →
- Other addition polymers, and monomers from polymersPoly(propene), poly(chloroethene) and poly(tetrafluoroethene) and their monomers, why a monomer needs a C=C bond, working out a repeating unit from a monomer and a monomer from a repeating unit, and counting atoms in a chain.Open →
- Uses of polymers, and natural polymers including DNAThe properties that suit poly(ethene), poly(propene), PVC and PTFE to their uses, and the monomers of DNA, starch and proteins and why they count as polymers.Open →
- Polyesters and condensation polymerisationWhy forming a polyester is condensation polymerisation, the two monomers and the ester link, the water lost per link, how it differs from addition polymerisation, and why monomers need two functional groups.Open →
- Problems with polymers and recyclingPolymers made from finite crude oil, why non-biodegradable polymers fill landfill, the carbon dioxide, hydrogen chloride and carbon monoxide released by burning them, why sorting is needed, and the economic and environmental advantages and disadvantages of recycling polymers.Open →
- Alcohols and the -OH functional groupThe formulae and bonding of methanol, ethanol, propan-1-ol and butan-1-ol, the general formula CₙH₂ₙ₊₁OH, the –OH hydroxyl functional group, and dehydrating alcohols to form alkenes and water.Open →
- Comparing the energy released by alcohol fuelsComparing the temperature rise of water heated by burning ethanol, propanol, butanol and pentanol, the variables and weighing the spirit burner, heat loss and incomplete combustion as errors, the trend with chain length, and calculating the energy gained by the water.Open →
- Making ethanol by fermentation and distillationFermenting sugars with enzymes from yeast, the word and balanced equations, why the sugar is dissolved and why strong heating stops fermentation, and concentrating the dilute ethanol by fractional distillation using its boiling point of 78 °C.Open →
- Carboxylic acids and the -COOH functional groupThe formulae and bonding of methanoic, ethanoic, propanoic and butanoic acids, their general formula and the –COOH carboxyl group, their acidic reactions with litmus, metals, carbonates and alkalis, the salts formed, and vinegar.Open →
- Oxidising alcohols to carboxylic acids, and homologous seriesThe acids formed when methanol, ethanol, propan-1-ol and butan-1-ol are oxidised, the –COOH group, why wine turns sour, and predicting the reactions of other members of a homologous series.Open →
- The size of nanoparticlesThe 1 nm to 100 nm size range, how a nanoparticle compares with an atom, a molecule and a dust particle, and converting nanometres to metres in standard form.Open →
- Uses and risks of nanoparticlesHow surface area to volume ratio grows as particles shrink, why that suits catalysts and sunscreens, and the health and environmental risks that are not yet understood.Open →
- Choosing a material for a useThe properties of glass, clay ceramics, polymers and metals, what composites such as fibreglass and carbon fibre are and why they are useful, and choosing materials for wiring, furnaces, windows, saucepan handles, bridges and ropes from their properties.Open →
What you need to know
Answer each one before you reveal it.
Your recallNot started
Key term
Describe how a flame test is carried out on a solid sample, and why the wire loop is cleaned beforehand.
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Describe the tests for carbonate and sulfate ions, and why limewater and dilute hydrochloric acid are each part of them.
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Describe the chemical test for ammonia gas, explain why damp red litmus is used, and name one property besides the litmus change.
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Why must the flame test wire be cleaned between one unknown salt and the next?
Evaluation
Give three advantages of instrumental analysis over tests carried out by hand.
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What is the general formula of the alkenes?
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Write the balanced equation for the reaction between ethene and bromine.
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What is a polymer?
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What is the molecular formula of propene?
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Why is PVC used to insulate electrical cables?
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Why is the formation of a polyester described as condensation polymerisation?
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From which finite raw material are most polymers made?
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Give the formula of methanol.
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What is measured in order to compare the energy released by burning different alcohols?
Process
What is the name of the process that makes ethanol from sugars using yeast?
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Give the formula of methanoic acid.
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Which acid is produced when ethanol is oxidised?
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Give the approximate diameter of a single atom in nanometres.
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What happens to the surface area to volume ratio of a particle as the particle gets smaller?
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State two physical properties of glass.
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What is meant by saying that the result of an ion test is unique?
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What is seen when sodium hydroxide solution is added to a solution containing aluminium ions, Al³⁺?
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Describe the test that shows a substance contains carbonate ions.
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Why is distilled water used to dissolve an unknown salt before testing it?
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Explain why instrumental methods are more accurate than judging the colour of a precipitate by eye.
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How many covalent bonds are there in a molecule of ethane, and between which atoms?
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In a molecule of ethene, how many hydrogen atoms are joined to each carbon atom, and what joins the two carbon atoms?
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Describe what happens to the double bond when ethene reacts with bromine.
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Why is the relative molecular mass of a polymer described as an average rather than a fixed value?
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Which monomer is used to make PVC?
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Why is PVC suitable for window frames and drainpipes?
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Which two types of monomer react together to form a polyester?
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Why is the availability of starting materials a problem for polymer production?
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Give the formula of ethanol.
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Name the four alcohols burned in the investigation of temperature rise.
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Which organism supplies the enzymes needed for fermentation?
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Give the formula of ethanoic acid.
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Which acid is produced when methanol is oxidised?
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How does the diameter of a nanoparticle compare with that of a single atom?
Numbers
A cube of material has sides of 2 nm. Calculate its surface area to volume ratio.
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How do the densities of polymers compare with the densities of metals?
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A student claims that a white precipitate with sodium hydroxide solution proves calcium ions are present. Why is that conclusion unsafe?
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What is seen when sodium hydroxide solution is added to a solution containing calcium ions, Ca²⁺?
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What is seen immediately when dilute acid is added to a carbonate?
Take Chemical Analysis, Organic Chemistry and Materials further
The same content, four other ways.
Commonly confused
Pairs that lose marks when they are blurred together.
Alkane vs Alkene
Alkane: saturated hydrocarbon with only single carbon–carbon bonds, general formula CₙH₂ₙ₊₂. Alkene: unsaturated hydrocarbon with a carbon–carbon double bond, general formula CₙH₂ₙ.
Addition polymerisation vs Condensation polymerisation
Addition polymerisation: joining many alkene monomers into one long chain with no other product. Condensation polymerisation: joining two kinds of monomer through ester links, losing a water molecule each time.
Alcohol vs Carboxylic acid
Alcohol: compound with the –OH functional group, such as ethanol. Carboxylic acid: compound with the –COOH functional group, formed when the –OH group is oxidised.
Questions from this topic
Each one with the model answer underneath.
- 1
Why must a chemical test for an ion give a result that no other ion gives?
Model answer
Only a result unique to that ion allows a firm conclusion, because a shared result could have been caused by a different ion.
- 2
What is meant by saying that the result of an ion test is unique?
Model answer
The observation is produced by that one ion and by none of the other ions being looked for.
- 3
A student claims that a white precipitate with sodium hydroxide solution proves calcium ions are present. Why is that conclusion unsafe?
Model answer
Aluminium ions also give a white precipitate with sodium hydroxide solution, so this observation alone does not identify the ion.
- 4
Why is more than one test usually needed before an unknown salt can be named?
Model answer
One test identifies the positive ion and another identifies the negative ion, and neither result on its own names the whole compound.
- 5
Give one reason for testing a known compound alongside an unknown one.
Model answer
The known compound shows exactly what a positive result looks like, so the unknown observation can be compared with it.
- 6
What flame colour is produced by a lithium ion, Li⁺?
Model answer
Red.
What is inside Levo
Six ways to work the same material.
Chemical Analysis, Organic Chemistry and Materials revision questions
- What does Chemical Analysis, Organic Chemistry and Materials cover in Edexcel GCSE Chemistry?
- 21 subtopics: why an ion test must be unique, and flame tests, tests for metal ions and for ammonia, tests for carbonate, sulfate and halide ions, identifying the ions in an unknown salt, instrumental methods and flame photometry, alkanes and why they are saturated, alkenes and why they are unsaturated, reactions of alkenes, and combustion, what a polymer is, and how poly(ethene) forms, other addition polymers, and monomers from polymers, uses of polymers, and natural polymers including dna, polyesters and condensation polymerisation, problems with polymers and recycling, alcohols and the -oh functional group, comparing the energy released by alcohol fuels, making ethanol by fermentation and distillation, carboxylic acids and the -cooh functional group, oxidising alcohols to carboxylic acids, and homologous series, the size of nanoparticles, uses and risks of nanoparticles and choosing a material for a use. Each one has its own page with questions and model answers.
- How is Chemical Analysis, Organic Chemistry and Materials organised?
- By the Edexcel 1CH0 specification, subtopic by subtopic, so it matches the order you are taught it in.
Every question in Chemical Analysis, Organic Chemistry and Materials, on a schedule.
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