Edexcel International A Level (IAL) Chemistry (YCH11) Study Notes - New Syllabus
Edexcel International A Level (IAL) Chemistry (YCH11) Study Notes
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Edexcel International A Level (IAL) Chemistry (YCH11) Study Notes
Unit 1: Structure, Bonding and Introduction to Organic Chemistry
Topic 1: Formulae, Equations and Amount of Substance
- 1.1 Chemical terms and formulae
- 1.2 The mole and Avogadro constant
- 1.3 Balanced full equations
- 1.4 Relative atomic, molecular and molar mass; ppm
- 1.5 Concentration (mol dm−3, g dm−3)
- 1.6 Empirical and molecular formulae (experimental)
- 1.7 Reacting masses calculations
- 1.8 Gas volumes and ideal gas equation (pV = nRT)
- 1.9 Percentage yield and atom economy
- 1.10 Determining formulae /equations experimentally
- 1.11 CORE PRACTICAL 1: Molar volume of a gas
- 1.12 Ionic equations linked to observations
Topic 2: Atomic Structure and the Periodic Table
- 2.1–2.2 Structure of the atom; relative mass and charge
- 2.3–2.4 Atomic number, mass number and ions
- 2.5 Isotopes
- 2.6–2.7 Mass spectrometry and spectra interpretation
- 2.8–2.9 I, II ,III Ionisation energy
- 2.10 Factors affecting ionisation energy
- 2.11 Successive IE and sub-shell evidence
- 2.12 Shapes of s and p orbitals
- 2.13 Orbital filling and spin
- 2.14–2.15 Electron configuration and chemical properties
- 2.16 Periodic table blocks (s, p, d)
- 2.17 Graphical representation of IE
- 2.18 Period 2 & 3 trends
Topic 3: Bonding and Structure
Ionic Bonding
- 3.1–3.2 Evidence and formation of ions
- 3.3 Dot-and-cross diagrams (ions)
- 3.4 Ionic lattices
- 3.5 Electrostatic attraction in ionic bonding
- 3.6 Ionic radius and charge effects
- 3.7 Isoelectronic ions and trends
- 3.8–3.9 Polarisation, polarising power and polarisability
Covalent Bonding
- 3.10 Covalent bonding (electron density evidence)
- 3.11 Dot-and-cross (single, double, triple, dative)
- 3.12 Giant covalent structures
- 3.13 Electronegativity
- 3.14 Bonding continuum
- 3.15 Polar bonds and polar molecules
Shapes of Molecules
- 3.16 Electron-pair repulsion theory
- 3.17 Bond length and bond angle
- 3.18 Shapes and bond angles (examples)
- 3.19 Predicting analogous shapes
Metallic Bonding
Topic 4: Introductory Organic Chemistry and Alkanes
Introduction
- 4.1–4.3 Hazard, risk assessment and risk reduction
- 4.4 Homologous series and functional groups
- 4.5 IUPAC naming and formulae
- 4.6 Classification of reactions
- 4.7 Homolytic and heterolytic bond fission
- 4.8 Free radicals and electrophiles
Alkanes
- 4.9 General formula; saturated hydrocarbons
- 4.10 Structural isomerism
- 4.11 Naming structural isomers
- 4.12 Alkanes as fuels
- 4.13 Combustion pollutants
- 4.14 Environmental impact of combustion
- 4.15 Sustainability and alternative fuels
- 4.16 Carbon neutrality
- 4.17 Reactions of alkanes
- 4.18 Free radical substitution mechanism
Topic 5: Alkenes
Unit 2: Energetics, Group Chemistry, Halogenoalkanes and Alcohols
Topic 6: Energetics
- 6.1 Enthalpy change (ΔH) and standard conditions
- 6.2 Exothermic and endothermic reactions
- 6.3 Enthalpy level diagrams
- 6.4 Standard enthalpy changes (formation, combustion, etc.)
- 6.5 Calorimetry calculations (q = mcΔT)
- 6.6 Hess’s Law and enthalpy cycles
- 6.7 CORE PRACTICAL 2: Hess’s Law
- 6.8 Evaluation of experimental errors and uncertainty
- 6.9–6.10 Bond enthalpy and calculations
- 6.11 Bond enthalpy and reaction insights
Topic 7: Intermolecular Forces
- 7.1 Types of intermolecular forces
- 7.2 Hydrogen bonding (H₂O, NH₃, HF)
- 7.3 Anomalous properties of water
- 7.4 Predicting hydrogen bonding
- 7.5 IMF and physical properties
- 7.6 Solvent choice and intermolecular forces
Topic 8: Redox Chemistry and Groups 1, 2 and 7
8A: Redox Chemistry
- 8.1–8.2 Oxidation numbers and calculations
- 8.3–8.4 Oxidation states and formula writing
- 8.5 Oxidation and reduction (electron transfer)
- 8.6 Oxidising and reducing agents
- 8.7 Disproportionation reactions
- 8.8 Oxidation number in classification
- 8.9 Formation of ions
- 8.10 Ionic half-equations
8B: Groups 1 and 2
- 8.11 Ionisation energy trends
- 8.12 Reactivity trends
- 8.13 Reactions with O₂, Cl₂ and H₂O
- 8.14 Reactions of oxides and hydroxides
- 8.15 Solubility trends
- 8.16 Thermal stability trends
- 8.17 Flame colours
- 8.18 Thermal decomposition and flame tests
- 8.19 Tests for CO₃²⁻, SO₄²⁻, NH₄⁺
- 8.20 Solution concentration and titrations
- 8.21 CORE PRACTICAL 3: HCl concentration
- 8.22 Uncertainty in volumetric analysis
- 8.23 CORE PRACTICAL 4: Standard solution
8C: Group 7 (Halogens)
- 8.24 Trends (mp, bp, electronegativity, reactivity)
- 8.25 Redox reactions of halogens
- 8.26 Halogen reactions (oxidation and disproportionation)
- 8.27 Reactions of halides
- 8.28 Predictions for F and At
Topic 9: Introduction to Kinetics and Equilibria
9A: Kinetics
- 9.1 Collision theory
- 9.2 Activation energy
- 9.3 Rate calculations
- 9.4 Maxwell–Boltzmann distribution
- 9.5 Catalysts and activation energy
- 9.6 Reaction profiles
- 9.7 Catalysts in industry
- 9.8 Catalyst action
9B: Equilibria
Topic 10: Organic Chemistry – Halogenoalkanes, Alcohols and Spectra
10A: General Principles
- 10.1 Types of reactions
- 10.2 Reaction mechanisms
- 10.3–10.4 Heterolytic fission and nucleophiles
- 10.5 Bond polarity and mechanism type
10B: Halogenoalkanes
- 10.6 Nomenclature and structures
- 10.7 Primary, secondary and tertiary halogenoalkanes
- 10.8 Reactions of halogenoalkanes
- 10.9 Nucleophilic substitution mechanisms
- 10.10 Hydrolysis rate comparisons
- 10.11 CORE PRACTICAL 5: Hydrolysis rates
- 10.12 Reactivity trends
- 10.13 Bond enthalpy and reactivity
- 10.14 CORE PRACTICAL 6: Chlorination
10C: Alcohols
- 10.15 Nomenclature and structures
- 10.16 Types of alcohols
- 10.17 Reactions of alcohols
- 10.18 Oxidation of alcohols
- 10.19 Preparation and purification
- 10.20 CORE PRACTICAL 7: Oxidation of propan-1-ol
10D: Spectroscopy
Unit 4: Rates, Equilibria and Further Organic Chemistry
Topic 11: Kinetics
- 11.1 Kinetics Definitions
- 11.2 Half-life calculations and first-order identification
- 11.3 Experimental techniques
- 11.4 Initial-rate and continuous monitoring methods
- 11.5 Order determination (all graphical and rate methods)
- 11.6 Iodination of propanone
- 11.7 Rate-determining step from rate equation
- 11.8 Mechanism from rate equation
- 11.9 SN1 and SN2 from rate equations
- 11.10 Activation energy from data (Arrhenius)
- 11.11 Heterogeneous catalysis
- 11.12 Core Practical: iodine-propanone & clock reaction
- 11.13 Core Practical: activation energy
Topic 12: Entropy and Energetics
- 12.1 Enthalpy vs feasibility
- 12.2 Entropy as disorder
- 12.3 Entropy and temperature/states
- 12.4 Direction of change (ΔS)
- 12.5 Entropy changes (state, dissolving, moles)
- 12.6 ΔS_total = ΔS_system + ΔS_surroundings
- 12.7 ΔS_system calculations
- 12.8 ΔS_surroundings = −ΔH/T
- 12.9–12.10 Feasibility, temperature and ΔS_total
- 12.11 Thermodynamic vs kinetic stability
- 12.12 Enthalpy of atomisation, electron affinity, lattice energy
- 12.13 Born-Haber cycles
- 12.14 Experimental vs theoretical lattice energy
- 12.15 Polarisation and covalency
- 12.16 Enthalpy of solution and hydration
- 12.17 Energy cycles for ΔH_solution
- 12.18 Ionic charge and radius effects
- 12.19 Solubility using ΔH and ΔS
Topic 13: Chemical Equilibria
- 13.1–13.2 Kc and Kp expressions
- 13.3 Equilibrium constant calculations
- 13.4 Effects of temperature, pressure, catalyst
- 13.5 Independence of K from concentration/pressure
- 13.6 Temperature effect on K
- 13.7 Equilibrium explained using K
- 13.8 Entropy relationship (ΔS_total = R ln K)
- 13.9 Extent of reaction from K
Topic 14: Acid-base Equilibria
- 14.1–14.2 Brønsted–Lowry theory and conjugate pairs
- 14.3–14.5 pH and [H⁺] relationships
- 14.6–14.7 Strong acids and pH of strong acids
- 14.8 Ka expression
- 14.9 pH of weak acids (Ka, pKa)
- 14.10–14.12 Kw, pKa and pKw definitions
- 14.13 Experimental pH analysis
- 14.14 Ka from experimental data
- 14.15 Titration curves
- 14.16 Indicator selection
- 14.17–14.18 Buffer solutions and buffer action
- 14.19 Buffer pH calculations
- 14.20 Buffer preparation calculations
- 14.21 Titration curves (Ka & buffer region)
- 14.22 Biological buffers
- 14.23 Core Practical: Ka determination
Topic 15: Organic Chemistry: Carbonyls, Carboxylic Acids and Chirality
15A: Chirality
- 15.1–15.2 Optical isomerism and enantiomers
- 15.3 Optical activity
- 15.4 Racemic mixtures
- 15.5 Optical evidence for mechanisms
15B: Carbonyl compounds
- 15.6 Nomenclature and structures
- 15.7 Hydrogen bonding and properties
- 15.8 Reactions of carbonyls
15C: Carboxylic acids
- 15.9 Nomenclature and structures
- 15.10 Hydrogen bonding and properties
- 15.11 Preparation methods
- 15.12 Reactions
15D: Carboxylic acid derivatives
- 15.13 Nomenclature (acyl chlorides, esters)
- 15.14 Reactions of acyl chlorides
- 15.15 Ester hydrolysis
- 15.16 Polyesters
15E: Spectroscopy and chromatography
- 15.17–15.18 Mass spectrometry and 13C NMR basics
- 15.19 13C NMR interpretation
- 15.20 1H NMR interpretation
- 15.21 Chromatography principles
- 15.22 Rf values
- 15.23 HPLC and GC
Unit 5: Transition Metals and Organic Nitrogen Chemistry
Topic 16: Redox Equilibria
- 16.1 Oxidation and reduction (electron transfer & oxidation number)
- 16.2–16.3 Standard electrode potential (E°) and standard conditions
- 16.4 Standard hydrogen electrode
- 16.5 Measurement of electrode potentials
- 16.6 Core Practical: electrochemical cells
- 16.7 Standard emf (E°cell)
- 16.8 Cell diagrams
- 16.9 Conditions affecting electrode potential
- 16.10 Feasibility using E°
- 16.11 Relationship: E°cell, entropy and lnK
- 16.12 Limitations of E° predictions
- 16.13 Electrochemical series
- 16.14 Disproportionation using E°
- 16.15 Redox titration calculations
- 16.16 Uncertainty in measurements
- 16.17 Core Practicals: redox titrations (KMnO₄ & iodine)
- 16.18–16.19 Fuel cells and hydrogen–oxygen fuel cell reactions
Topic 17: Transition Metals
- 17.1 Transition metals (d-block, incomplete d orbitals)
- 17.2 Electronic configurations (Sc–Zn)
- 17.3 Variable oxidation states
- 17.4–17.6 Ligands, dative bonding and complex ions
- 17.7 Coloured ions
- 17.8 d-orbital splitting and colour
- 17.9 Lack of colour
- 17.10 Coordination number
- 17.11 Colour changes (oxidation state, ligand, coordination)
- 17.12 Monodentate ligands (H₂O, OH⁻, NH₃)
- 17.13–17.14 Octahedral and tetrahedral complexes
- 17.15 Square planar complexes (cisplatin)
- 17.16 Bidentate and hexadentate ligands (EDTA)
- 17.17 Haemoglobin and ligand exchange
- 17.18 Vanadium oxidation states (colours)
- 17.19 Vanadium redox reactions
- 17.20 Dichromate redox reactions
- 17.21 Chromate–dichromate equilibrium
- 17.22–17.23 Reactions with NaOH/NH₃ and amphoteric behaviour
- 17.24 Ligand exchange reactions (Cu²⁺, Co²⁺)
- 17.25 Stability of complexes (entropy)
- 17.26–17.27 Transition metals as catalysts and heterogeneous catalysis
- 17.28 V₂O₅ catalyst (contact process)
- 17.29 Catalytic converters
- 17.30 Homogeneous catalysis
- 17.31 Fe²⁺ catalysis (I⁻ & S₂O₈²⁻)
- 17.32 Mn²⁺ autocatalysis
- 17.33 Core Practical: transition metal complex
Topic 18: Arenes
- 18.1–18.2 Benzene structure and delocalised π bonding
- 18.3 Resistance to addition reactions
- 18.4 Reactions of benzene
- 18.5 Electrophilic substitution mechanisms
- 18.6 Phenol reactions
Topic 19: Organic Nitrogen Compounds
- 19.1 Nomenclature (amines, amides, amino acids)
- 19.2 Reactions of amines
- 19.3 Basicity and hydrogen bonding
- 19.4 Preparation of amines
- 19.5 Aromatic amines preparation
- 19.6 Diazotisation and azo dyes
- 19.7 Amides from acyl chlorides
- 19.8–19.9 Polymerisation and polymer repeat units
- 19.10 Polymer properties and solubility
- 19.11 Amino acids (zwitterions, optical activity, peptide bonds)
- 19.12 Core Practical: analysis of unknowns
Topic 20: Organic Synthesis
- 20.1–20.3 Structure determination and multi-step synthesis
- 20.2 Chain extension (Grignard reagents)
- 20.4 Core Practical: aspirin synthesis
- 20.5 Purification techniques