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
Atomic Structure and the Periodic Table
Ionisation energy and the evidence for sub-shells
- 3 things to know
- Papers 1 and 3
Overview
Recall questions on the definition of first ionisation energy, the trends across a period and down a group, and how successive ionisation energies reveal shells and sub-shells.
What you need to know
Answer each one before you reveal it.
Your recallNot started
Key term
What are successive ionisation energies?
Key term
Explain why ionisation energy increases with greater nuclear charge.
Questions from this subtopic
Each one with the model answer underneath.
- 1
Define first ionisation energy.
Model answer
The energy required to remove one electron from each atom in one mole of gaseous atoms to form one mole of gaseous unipositive ions
- 2
What are successive ionisation energies?
Model answer
The energies required to remove each subsequent electron from an increasingly positive ion
- 3
Explain why ionisation energy increases with greater nuclear charge.
Model answer
More protons in the nucleus create a stronger attraction for the electrons, making them harder to remove
- 4
How does electron shielding affect ionisation energy?
Model answer
Greater electron shielding from inner shells reduces the effective nuclear charge felt by outer electrons, decreasing ionisation energy
- 5
Why are electrons in higher energy sub-shells easier to remove?
Model answer
Electrons in higher energy sub-shells are further from the nucleus and experience less nuclear attraction, so less energy is needed to remove them
- 6
Explain why first ionisation energy generally increases across a period.
Model answer
Nuclear charge increases across a period while shielding remains similar, so electrons are held more tightly
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