Log In Get Started

The learning loop

See all features →

Build understanding

Clear explanations. Connected ideas. Help when you need it.

Put it into practice

Try it, get feedback, and learn from every attempt.

Know what to work on next

See your progress and find a clearer next step.

Key Stage 3

Coming soon

GCSE

Biology
Chemistry
Physics
Biology (Combined)
Chemistry (Combined)
Physics (Combined)
Maths
Geography

IGCSE

Biology
Chemistry
Physics

A-Level

Biology
Chemistry
Physics

11+

Coming soon

Product

See all features →

Build understanding

Clear explanations. Connected ideas. Help when you need it.

Put it into practice

Try it, get feedback, and learn from every attempt.

Know what to work on next

See your progress and find a clearer next step.

Log In Get Started

Home Subjects Analytics SageAI Lessons Notes Flashcards Questions Feedback

Notes/A-Level/Chemistry/Edexcel/Edexcel A-level Chemistry — 9CH0

Syllabus

Edexcel A-level Chemistry — 9CH0

- •The nature of ionic bonding2.1
  •Ionic radius, charge and bond strength2.2
  •Ion formation by electron loss and gain2.3
  •Dot-and-cross diagrams of ions2.4
  •Trends in ionic radii2.5
  •Experimental evidence for ions2.6
  •The nature of covalent bonding2.7
  •Dot-and-cross diagrams of covalent and coordinate bonds2.8
  •Covalent bond lengths and strengths2.9
  •Electron-pair repulsion and molecular shape2.10
  •Shapes and bond angles with up to six electron pairs2.11
  •Predicting unfamiliar molecular shapes and bond angles2.12
  •Electronegativity2.13
  •The bonding continuum and bond polarity2.14
  •Predicting molecular polarity2.15
  •Types of intermolecular forces2.16
  •Hydrogen bonding in water, ammonia and hydrogen fluoride2.17
  •Hydrogen bonding and anomalous properties of water2.18
  •Predicting hydrogen bonding2.19
  •Intermolecular forces and boiling temperature trends2.20
  •Choosing solvents using intermolecular forces2.21
  •The nature of metallic bonding2.22
- •Giant ionic, covalent and metallic lattices2.23
  •Simple molecular structures2.24
  •Diamond, graphite and graphene2.25
  •Deducing structure and bonding from data2.26
  •Predicting physical properties from structure and bonding2.27
- •Interpreting molecular ions and fragmentation patterns7.1
- •Identifying functional groups using infrared spectroscopy7.2
- •The definition of lattice energy13.1
  •Enthalpy of atomisation and electron affinity13.2
  •Born–Haber cycles and calculations13.3
  •Lattice energy and ionic bond strength13.4
  •Experimental and theoretical lattice energies and covalent character13.5
  •Polarisation of ions13.6
  •Factors affecting cation polarising power13.7
  •Factors affecting anion polarisability13.8
  •Enthalpies of solution and hydration13.9
  •Energy cycles involving solution, hydration and lattice energy13.10
  •Ionic charge and radius effects on lattice and hydration energies13.11
- •Why enthalpy alone does not determine feasibility13.12
  •Entropy, disorder and the direction of change13.13
  •Entropy changes in physical and chemical processes13.14
  •System, surroundings and total entropy change13.15
  •Calculating entropy changes of the system13.16
  •Calculating entropy changes of the surroundings and total entropy13.17
  •Gibbs energy, enthalpy and entropy13.18
  •Predicting feasibility and feasible temperatures using Gibbs energy13.19
  •Gibbs energy and equilibrium constants13.20
  •Why negative Gibbs energy does not guarantee a reaction13.21
  •Kinetic inhibition of thermodynamically feasible reactions13.22
- •Electronic configurations of Period 4 d-block atoms and ions15.1
  •The definition of a transition metal15.2
  •Variable oxidation states in transition metals15.3
  •The meaning of a ligand15.4
  •Coordinate bonding in complex ions15.5
  •The structure of a complex ion15.6
  •Coloured transition-metal ions in solution15.7
  •Ligand-induced d-orbital splitting and colour15.8
  •Why some metal ions and complexes are colourless15.9
  •Factors causing colour changes in transition-metal ions15.10
  •Coordination number15.11
  •Water, hydroxide and ammonia as monodentate ligands15.12
  •Octahedral complexes with coordination number six15.13
  •Tetrahedral complexes with large ligands15.14
  •Square planar complexes and cis-platin15.15
  •Cis-platin isomerism and cancer treatment15.16
  •Bidentate and multidentate ligands15.17
  •Haemoglobin as an iron(II) complex15.18
  •Carbon monoxide ligand exchange in haemoglobin15.19
- •Colours of vanadium oxidation states15.20
  •Vanadium redox reactions and electrode potentials15.21
  •Redox interconversions of chromium ions15.22
  •The chromate-dichromate equilibrium15.23
  •Metal-ion reactions with hydroxide and ammonia15.24
  •Distinguishing ligand exchange from amphoteric behaviour15.25
  •Ligand exchange and colour changes in copper and cobalt complexes15.26
  •Ligand size, charge and coordination-number changes15.27
  •The chelate effect and entropy15.28
  •Transition metals as heterogeneous and homogeneous catalysts15.29
  •The action of heterogeneous catalysts15.30
  •Vanadium(V) oxide catalysis in the contact process15.31
  •Catalytic converters: adsorption, reaction and desorption15.32
  •Homogeneous catalysts and intermediates15.33
  •Iron(II) catalysis of the iodide-peroxodisulfate reaction15.34
  •Manganese(II) autocatalysis of the manganate(VII)-ethanedioate reaction15.35

Syllabus

Edexcel A-level Chemistry — 9CH0

- •The nature of ionic bonding2.1
  •Ionic radius, charge and bond strength2.2
  •Ion formation by electron loss and gain2.3
  •Dot-and-cross diagrams of ions2.4
  •Trends in ionic radii2.5
  •Experimental evidence for ions2.6
  •The nature of covalent bonding2.7
  •Dot-and-cross diagrams of covalent and coordinate bonds2.8
  •Covalent bond lengths and strengths2.9
  •Electron-pair repulsion and molecular shape2.10
  •Shapes and bond angles with up to six electron pairs2.11
  •Predicting unfamiliar molecular shapes and bond angles2.12
  •Electronegativity2.13
  •The bonding continuum and bond polarity2.14
  •Predicting molecular polarity2.15
  •Types of intermolecular forces2.16
  •Hydrogen bonding in water, ammonia and hydrogen fluoride2.17
  •Hydrogen bonding and anomalous properties of water2.18
  •Predicting hydrogen bonding2.19
  •Intermolecular forces and boiling temperature trends2.20
  •Choosing solvents using intermolecular forces2.21
  •The nature of metallic bonding2.22
- •Giant ionic, covalent and metallic lattices2.23
  •Simple molecular structures2.24
  •Diamond, graphite and graphene2.25
  •Deducing structure and bonding from data2.26
  •Predicting physical properties from structure and bonding2.27
- •Interpreting molecular ions and fragmentation patterns7.1
- •Identifying functional groups using infrared spectroscopy7.2
- •The definition of lattice energy13.1
  •Enthalpy of atomisation and electron affinity13.2
  •Born–Haber cycles and calculations13.3
  •Lattice energy and ionic bond strength13.4
  •Experimental and theoretical lattice energies and covalent character13.5
  •Polarisation of ions13.6
  •Factors affecting cation polarising power13.7
  •Factors affecting anion polarisability13.8
  •Enthalpies of solution and hydration13.9
  •Energy cycles involving solution, hydration and lattice energy13.10
  •Ionic charge and radius effects on lattice and hydration energies13.11
- •Why enthalpy alone does not determine feasibility13.12
  •Entropy, disorder and the direction of change13.13
  •Entropy changes in physical and chemical processes13.14
  •System, surroundings and total entropy change13.15
  •Calculating entropy changes of the system13.16
  •Calculating entropy changes of the surroundings and total entropy13.17
  •Gibbs energy, enthalpy and entropy13.18
  •Predicting feasibility and feasible temperatures using Gibbs energy13.19
  •Gibbs energy and equilibrium constants13.20
  •Why negative Gibbs energy does not guarantee a reaction13.21
  •Kinetic inhibition of thermodynamically feasible reactions13.22
- •Electronic configurations of Period 4 d-block atoms and ions15.1
  •The definition of a transition metal15.2
  •Variable oxidation states in transition metals15.3
  •The meaning of a ligand15.4
  •Coordinate bonding in complex ions15.5
  •The structure of a complex ion15.6
  •Coloured transition-metal ions in solution15.7
  •Ligand-induced d-orbital splitting and colour15.8
  •Why some metal ions and complexes are colourless15.9
  •Factors causing colour changes in transition-metal ions15.10
  •Coordination number15.11
  •Water, hydroxide and ammonia as monodentate ligands15.12
  •Octahedral complexes with coordination number six15.13
  •Tetrahedral complexes with large ligands15.14
  •Square planar complexes and cis-platin15.15
  •Cis-platin isomerism and cancer treatment15.16
  •Bidentate and multidentate ligands15.17
  •Haemoglobin as an iron(II) complex15.18
  •Carbon monoxide ligand exchange in haemoglobin15.19
- •Colours of vanadium oxidation states15.20
  •Vanadium redox reactions and electrode potentials15.21
  •Redox interconversions of chromium ions15.22
  •The chromate-dichromate equilibrium15.23
  •Metal-ion reactions with hydroxide and ammonia15.24
  •Distinguishing ligand exchange from amphoteric behaviour15.25
  •Ligand exchange and colour changes in copper and cobalt complexes15.26
  •Ligand size, charge and coordination-number changes15.27
  •The chelate effect and entropy15.28
  •Transition metals as heterogeneous and homogeneous catalysts15.29
  •The action of heterogeneous catalysts15.30
  •Vanadium(V) oxide catalysis in the contact process15.31
  •Catalytic converters: adsorption, reaction and desorption15.32
  •Homogeneous catalysts and intermediates15.33
  •Iron(II) catalysis of the iodide-peroxodisulfate reaction15.34
  •Manganese(II) autocatalysis of the manganate(VII)-ethanedioate reaction15.35

Dot-and-cross diagrams of ions

Edexcel·Chemistry·2.4

Notes Coming Soon

The concept content for this specification point is being prepared. Check back soon.