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
Kinetics I
Collision theory and factors affecting rate
- 3 things to know
- Papers 2 and 3
Overview
The activation energy and correct orientation a successful collision needs, and how raising concentration, pressure and surface area increases the frequency of collisions rather than the proportion that succeed.
What you need to know
Answer each one before you reveal it.
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Key term
Why does increasing the pressure of a gaseous reaction increase the rate?
Key term
What must happen between particles for a reaction to occur?
Questions from this subtopic
Each one with the model answer underneath.
- 1
What must happen between particles for a reaction to occur?
Model answer
Particles must collide with each other.
- 2
Besides colliding, what two conditions must a collision satisfy to be successful?
Model answer
The particles must collide with energy equal to or greater than the activation energy and with the correct orientation.
- 3
What does activation energy mean?
Model answer
The minimum energy that colliding particles must have for a reaction to take place.
- 4
Why does increasing the concentration of a reactant increase the rate of reaction?
Model answer
There are more reactant particles in a given volume, so collisions are more frequent.
- 5
Why does increasing the pressure of a gaseous reaction increase the rate?
Model answer
The gas particles are closer together in a smaller volume, so collisions are more frequent.
- 6
Why does increasing the surface area of a solid reactant increase the rate?
Model answer
More reactant particles are exposed at the surface, so collisions with them are more frequent.
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