Process
Edexcel A-Level Chemistry 9CH0
Atomic Structure and the Periodic Table
Bonding and Structure
Inorganic Chemistry and the Periodic Table
Topic overviewFlame tests and how they workThermal decomposition of nitrates and carbonatesCarrying out flame tests and testing the gasesGroup 2 elements and their compoundsTrends in Group 7 and predicting fluorine and astatineHalogen displacement reactionsDisproportionation and the reactions of chlorineHalides with concentrated sulfuric acid, and the hydrogen halidesTesting for halide ions with silver nitrateTesting for carbonate and hydrogencarbonate ionsTesting for sulfate and ammonium ions
Formulae, Equations and Amounts of Substance
Topic overviewThe mole, molar mass and empirical formulaThe ideal gas equation and molar volumeEquations, concentration and reacting quantitiesStandard solutions, titration and uncertaintyPercentage yield, atom economy and acid reactionsCore practicals 1 to 3Empirical formula and water of crystallisation by experimentApparatus, uncertainty and mathematical skills
Organic Chemistry I
Topic overviewFormulae, homologous series and functional groupsIUPAC nomenclatureTypes of organic reaction and structural isomerismStereoisomerism and E/Z nomenclaturePractical techniques in organic chemistryAlkanes, crude oil and combustion pollutantsRadical substitutionAlkenes, the double bond and hydrogenationElectrophilic addition, Markovnikov's rule and the test for an alkeneAddition polymers and waste polymersNucleophilic substitution of halogenoalkanesRates of hydrolysis and the SN1 and SN2 mechanismsClassifying and oxidising alcoholsAlcohols: practical techniques and the core practicals
Modern Analytical Techniques I
Energetics I
Kinetics I
Equilibrium I
Acid-Base Equilibria
Energetics II
Redox II
Transition Metals
Topic overviewElectron configuration and what makes a transition metalComplex ions, ligands and the colour of transition metal ionsCoordination number, monodentate ligands and the shapes of complexesBidentate and multidentate ligands, and ligand exchangeVanadium and chromium chemistryReactions with sodium hydroxide and ammoniaCobalt and copper complexesLigand exchange, amphoteric behaviour and the chelate effectTransition metals as catalysts
Kinetics II
Organic Chemistry II
Topic overviewChiralityAldehydes, ketones and their oxidationReduction and nucleophilic addition of HCNTesting for a carbonyl group: 2,4-DNPH and the iodoform reactionCarboxylic acids and their reactionsEsters and acyl chloridesReflux, extraction and recrystallisationDistillation, melting temperature and working safely
Organic Chemistry III
Topic overviewThe structure of benzene and the evidence for itElectrophilic substitution of benzeneNitration, halogenation, Friedel-Crafts and phenolAmines: structure and basicityReactions of amines and preparing themAmides and condensation polymersAmino acids, zwitterions and proteinsEmpirical and molecular formulae from analytical dataGrignard reagents and multi-step synthesisPurification techniques and the aspirin preparation
Transition Metals
Cobalt and copper complexes
- 3 things to know
- Papers 1 and 3
Overview
Cobalt(II) and copper(II) ions with sodium hydroxide and ammonia and which precipitates dissolve in excess, ligand exchange to deep blue [Cu(NH₃)₄(H₂O)₂]²⁺ in excess ammonia and its equation, and the colours of [Cu(H₂O)₆]²⁺ and the copper hydroxide precipitate.
What you need to know
Answer each one before you reveal it.
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Key term
Explain why the solution turns deep blue when excess ammonia is added to Cu²⁺(aq).
Key term
Does the precipitate formed when Co²⁺(aq) reacts with NaOH(aq) dissolve in excess sodium hydroxide?
Questions from this subtopic
Each one with the model answer underneath.
- 1
Does the precipitate formed when Co²⁺(aq) reacts with NaOH(aq) dissolve in excess sodium hydroxide?
Model answer
No, the precipitate remains unchanged in excess NaOH(aq).
- 2
What is observed when dilute ammonia is added to Co²⁺(aq)?
Model answer
A blue-green precipitate of Co(OH)₂ forms.
- 3
What happens when excess ammonia is added to the precipitate formed from Co²⁺(aq), and what does this demonstrate?
Model answer
The precipitate dissolves to form a straw/yellow-brown solution containing [Co(NH₃)₆]²⁺, demonstrating ligand exchange.
- 4
What is observed when dilute NaOH is added to Cu²⁺(aq)?
Model answer
A pale blue precipitate of Cu(OH)₂ forms.
- 5
What happens when excess sodium hydroxide solution is added to Cu²⁺(aq)?
Model answer
No change occurs; the pale blue precipitate remains.
- 6
Explain why Cu(OH)₂ does not dissolve when excess NaOH(aq) is added.
Model answer
Cu(OH)₂ does not undergo ligand exchange or form a soluble complex with hydroxide ions, so the pale blue precipitate remains.
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