Key term
AQA GCSE Chemistry 8462
Atomic Structure and the Periodic Table
Topic overviewAtoms, elements and compoundsWord equations, symbols and balanced equationsMixturesFrom the plum pudding model to the nuclear modelBohr, Chadwick and the modern model of the atomRelative electrical charges of subatomic particlesSize and mass of atomsRelative atomic mass and electronic structureThe periodic tableDevelopment of the periodic tableMetals and non-metalsGroup 0Group 1Group 7Transition metals, and how they differ from Group 1
Bonding, Structure, and the Properties of Matter
Topic overviewChemical bonds, including metallic bondingIonic bondingIonic compoundsCovalent bonding and how it is representedThe three states of matter and changes of statePredicting state, state symbols, and the limits of the particle modelProperties of ionic compoundsProperties of small moleculesPolymers and giant covalent structuresProperties of metals and alloys, and why metals conductDiamond and graphiteGraphene and fullerenesSizes of particles and their propertiesUses of nanoparticles
Chemical Analysis
Chemical Changes
Topic overviewThe reactivity seriesMetal oxides, extraction, and redox in terms of electronsAcids reacting with metals, neutralisation and saltsSoluble saltsThe pH scale and neutralisationTitrationsThe process of electrolysis, and molten ionic compoundsUsing electrolysis to extract metalsElectrolysis of aqueous solutions
Chemistry of the Atmosphere
Topic overviewThe Earth's early atmosphereHow oxygen increased and carbon dioxide decreasedThe gases in today's atmosphere, and which are greenhouse gasesHuman activities which contribute to an increase in greenhouse gases in the atmosphereGlobal climate change and carbon footprintsAtmospheric pollutants from fuels, and their effects
Energy Changes
Organic Chemistry
Topic overviewCrude oil, hydrocarbons and alkanesFractional distillation and petrochemicalsProperties of hydrocarbonsCracking, and testing alkenes with bromine waterWhy cracking is useful, and equations for itStructure and formulae of alkenesReactions of alkenesAlcoholsCarboxylic acidsAddition polymerisationAmino acids, DNA and naturally occurring polymers
Quantitative Chemistry
The Rate and Extent of Chemical Change
Using Resources
Topic overviewUsing the Earth's resources and sustainable developmentProducing potable water in the UKDesalination, and analysing water samplesWaste water treatmentLife cycle assessmentWays of reducing the use of resourcesCorrosion and its preventionAlloys as useful materialsGlass, clay ceramics and polymersComposites, and comparing materialsThe Haber processProduction and uses of NPK fertilisers
Chemical Analysis
Metal hydroxides
- 3 things to know
- Paper 2
Overview
Precipitating metal hydroxides with sodium hydroxide solution, the white precipitates of aluminium, calcium and magnesium and how excess tells them apart, the coloured precipitates of copper(II), iron(II) and iron(III), and their equations.
What you need to know
Answer each one before you reveal it.
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Key term
Why does adding sodium hydroxide solution to a solution of a metal salt often produce a solid?
Key term
Name the three metal ions that give a white precipitate with sodium hydroxide solution.
Questions from this subtopic
Each one with the model answer underneath.
- 1
Which reagent is added to a solution in order to identify metal ions by precipitation?
Model answer
Sodium hydroxide solution.
- 2
Why does adding sodium hydroxide solution to a solution of a metal salt often produce a solid?
Model answer
Many metal hydroxides are insoluble, so they come out of solution as a precipitate.
- 3
Name the three metal ions that give a white precipitate with sodium hydroxide solution.
Model answer
Aluminium ions, calcium ions and magnesium ions.
- 4
How can aluminium ions be distinguished from calcium and magnesium ions using sodium hydroxide solution?
Model answer
All three give a white precipitate at first, but only the aluminium hydroxide dissolves again when excess sodium hydroxide is added.
- 5
A solution gives a white precipitate with sodium hydroxide solution and the precipitate remains when more is added. Which ions could be present?
Model answer
Calcium ions or magnesium ions.
- 6
A white precipitate forms with sodium hydroxide solution and then disappears as more is added. Which ion is present?
Model answer
Aluminium ions.
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