IB Chemistry Higher Level
International Baccalaureate (IB) Diploma Programme Chemistry - Higher Level
Welcome, students! This specialized academic portal provides in-depth resources for the IB Chemistry Higher Level (HL) curriculum. Here, you will find exhaustive syllabus checklists, vertical revision notes, targeted practice question banks, and official subject guides and data booklets—all mathematically and chemically formatted to optimize your learning and help you achieve a Grade 7.
1. Course Introduction
IB Chemistry Higher Level (HL) is a rigorous and highly challenging academic pathway designed for students aiming to pursue careers in Medicine, Pharmacy, Chemical Engineering, or Material Sciences at world-class universities. The curriculum covers the fundamental core concepts (Standard Level Core) along with 95 hours of advanced high-level extension topics (Additional Higher Level - AHL), emphasizing structural models and chemical reactivity.
Assessment Outline
| Assessment Component | Duration | Calculator & Resource Policy | Marks | Weighting |
|---|---|---|---|---|
| Paper 1 (MCQ & Data Analysis) | 120 minutes (2 hours) | Calculator & Data Booklet allowed | 75 marks | 36% |
| Paper 2 (Free Response) | 150 minutes (2.5 hours) | Calculator & Data Booklet allowed | 90 marks | 44% |
| Internal Assessment (IA) - Exploration | Independent research (12-20 pages) | No restrictions | 24 marks | 20% |
Syllabus Structure
The IB Chemistry syllabus is structured around two main pillars: Structure (how matter is put together) and Reactivity (how matter behaves and reacts). The Higher Level course integrates both the Standard Level core topics and the advanced High-Level extension topics (SL Core & HL Extensions):
S1.1 Introduction to the particulate nature of matter
1.1.1 Elements, compounds, and mixtures.
1.1.2 The kinetic molecular theory explains physical properties and state changes.
1.1.3 Temperature (K) as a measure of average kinetic energy.
S1.2 The nuclear atom
1.2.1 Atomic structure: protons, neutrons, and electrons.
1.2.2 Isotopes: same element, different neutron numbers.
1.2.3 [AHL] Mass spectra determine relative atomic masses.
S1.3 Electron configurations
1.3.1 Emission spectra: photons emitted during electron transitions.
1.3.2 Hydrogen line spectrum as evidence for discrete energy levels.
1.3.3 Main energy level (n) holds a maximum of 2n2 electrons.
1.3.4 Main energy level division into s, p, d, and f sublevels.
1.3.5 Orbitals hold two electrons of opposite spin; filling principles.
1.3.6 [AHL] Convergence limit corresponds to ionization.
1.3.7 [AHL] Successive ionization energy data reveals electron configuration.
S1.4 Counting particles by mass: The mole
1.4.1 The mole (mol) and the Avogadro constant.
1.4.2 Relative atomic mass (Ar) and relative formula mass (Mr).
1.4.3 Molar mass (M) in g mol-1.
1.4.4 Empirical and molecular formulas.
1.4.5 Molar concentration.
1.4.6 Avogadro’s law for gases.
S1.5 Ideal gases
1.5.1 Ideal gas model assumptions.
1.5.2 Real gases deviate from the ideal model (low T, high P).
1.5.3 Molar volume of an ideal gas.
1.5.4 Ideal gas equation (PV=nRT) and combined gas law.
S2.1 The ionic model
2.1.1 Cations (from metals) and anions (from non-metals).
2.1.2 Ionic bond: electrostatic attraction between ions.
2.1.3 Ionic compounds exist as 3D lattice structures.
S2.2 The covalent model
2.2.1 Covalent bond: electrostatic attraction for a shared pair of electrons; octet rule.
2.2.2 Single, double, and triple bonds (length and strength).
2.2.3 Coordination bond: shared pair originates from one atom.
2.2.4 VSEPR model predicts molecular shapes.
2.2.5 Bond polarity from electronegativity differences.
2.2.6 Molecular polarity depends on bond polarity and geometry.
2.2.7 Covalent network structures (C allotropes, Si, SiO2).
2.2.8 Intermolecular forces (London, dipole-dipole, H-bonding).
2.2.9 Relative strengths of intermolecular forces.
2.2.10 Chromatography separates mixtures based on relative attractions.
2.2.11 [AHL] Resonance structures (delocalization).
2.2.12 [AHL] Benzene (C6H6) structure as an example of resonance.
2.2.13 [AHL] Atoms with an expanded octet.
2.2.14 [AHL] Formal charge determines the preferred Lewis formula.
2.2.15 [AHL] Sigma (σ) bonds (head-on combination) and pi (π) bonds (lateral combination).
2.2.16 [AHL] Hybridization (sp, sp2, sp3) forms new hybrid orbitals.
S2.3 The metallic model
2.3.1 Metallic bond: electrostatic attraction between cations and delocalized electrons.
2.3.2 Strength of metallic bond (ion charge, ion radius).
2.3.3 [AHL] Transition elements have delocalized d-electrons.
S2.4 From models to materials
2.4.1 Bonding continuum (ionic, covalent, metallic) represented by a bonding triangle.
2.4.2 Position in bonding triangle determined by electronegativity.
2.4.3 Alloys: mixtures with enhanced properties.
2.4.4 Polymers: macromolecules from repeating monomers.
2.4.5 Addition polymers form by breaking double bonds.
2.4.6 [AHL] Condensation polymers form via reaction between functional groups.
S3.1 The periodic table: Classification of elements
3.1.1 Periodic table structure: periods, groups, blocks.
3.1.2 Period number (outer energy level) and group number (valence electrons).
3.1.3 Periodicity: trends in properties (radius, IE, electronegativity).
3.1.4 Trends in Group 1 (alkali metals) and Group 17 (halogens).
3.1.5 Continuum of properties (metallic/non-metallic); oxide trends.
3.1.6 Oxidation state: assigned number (charge if ionic).
3.1.7 [AHL] Discontinuities in first IE as evidence for sublevels.
3.1.8 [AHL] Transition element properties from incomplete d-sublevels.
3.1.9 [AHL] Variable oxidation states in transition elements.
3.1.10 [AHL] Coloured complexes due to d-sublevel splitting.
S3.2 Functional groups: Classification of organic compounds
3.2.1 Representation of organic compounds (formulas, models).
3.2.2 Functional groups give characteristic properties.
3.2.3 Homologous series: family differing by a structural unit (e.g., CH2).
3.2.4 Trends in physical properties within a homologous series.
3.2.5 IUPAC nomenclature (systematic names).
3.2.6 Structural isomers (same formula, different connectivity).
3.2.7 [AHL] Stereoisomers (cis-trans and optical isomers/enantiomers).
3.2.8 [AHL] Mass spectrometry (MS) fragmentation patterns.
3.2.9 [AHL] Infrared (IR) spectra identify bond types.
3.2.10 [AHL] Proton nuclear magnetic resonance (¹H NMR) shows H environments.
3.2.11 [AHL] ¹H NMR splitting patterns (singlets, doublets, etc.).
3.2.12 [AHL] Combined data for structural determination.
R1.1 Measuring enthalpy changes
1.1.1 Chemical reactions involve energy transfer; total energy conserved.
1.1.2 Endothermic (energy absorbed) and exothermic (energy released) reactions.
1.1.3 Relative stability of reactants/products determines endo/exothermic.
1.1.4 Standard enthalpy change (ΔH⊖) determined from temperature change (Q=mcΔT).
R1.2 Energy cycles in reactions
1.2.1 Bond-breaking absorbs energy; bond-forming releases energy (average bond enthalpy).
1.2.2 Hess’s law: enthalpy change is pathway independent.
1.2.3 [AHL] Standard enthalpy changes of combustion (ΔHc⊖) and formation (ΔHf⊖).
1.2.4 [AHL] Calculating ΔH⊖ using ΔHf⊖ or ΔHc⊖ data.
1.2.5 [AHL] Born-Haber cycle (application of Hess’s law for ionic compounds).
R1.3 Energy from fuels
1.3.1 Combustion reactions occur when heated in oxygen.
1.3.2 Incomplete combustion produces CO and/or C.
1.3.3 Fossil fuels (advantages and disadvantages).
1.3.4 Biofuels (from biological fixation of carbon).
1.3.5 Fuel cells convert chemical energy to electrical energy.
R1.4 Entropy and spontaneity (AHL)
1.4.1 [AHL] Entropy (S): measure of matter/energy dispersal.
1.4.2 [AHL] Gibbs energy: ΔG⊖=ΔH⊖−TΔS⊖.
1.4.3 [AHL] Spontaneous change occurs if ΔG is negative.
1.4.4 [AHL] At equilibrium, ΔG=0; ΔG⊖=−RTlnK.
R2.1 How much? The amount of chemical change
2.1.1 Chemical equations show reactant/product ratios.
2.1.2 Mole ratios determine masses, volumes, or concentrations.
2.1.3 Limiting reactant determines theoretical yield.
2.1.4 Percentage yield (experimental/theoretical).
2.1.5 Atom economy (measure of efficiency).
R2.2 How fast? The rate of chemical change
2.2.1 Rate of reaction: change in concentration per unit time.
2.2.2 Collision theory: requires sufficient energy and proper orientation.
2.2.3 Factors influencing reaction rate (pressure, conc, surface area, temp, catalyst).
2.2.4 Activation energy (Ea): minimum energy for successful collision.
2.2.5 Catalysts provide an alternative pathway with lower Ea.
2.2.6 [AHL] Reaction mechanisms occur in elementary steps; slowest step is rate-determining.
2.2.7 [AHL] Energy profiles for multistep reactions.
2.2.8 [AHL] Molecularity (unimolecular, bimolecular, termolecular).
2.2.9 [AHL] Rate equations determined experimentally.
2.2.10 [AHL] Order of reaction (zero, first, second).
2.2.11 [AHL] Rate constant (k) is temperature dependent.
2.2.12 [AHL] Arrhenius equation relates k, T, and Ea.
2.2.13 [AHL] Arrhenius factor (A).
R2.3 How far? The extent of chemical change
2.3.1 Dynamic equilibrium: closed system, forward/backward rates equal.
2.3.2 Equilibrium law and equilibrium constant (K).
2.3.3 Magnitude of K indicates reaction extent; temperature dependent.
2.3.4 Le Châtelier’s principle predicts effects of changes.
2.3.5 [AHL] Reaction quotient (Q) predicts direction of shift.
2.3.6 [AHL] Solving equilibrium problems (calculating concentrations).
2.3.7 [AHL] Relationship between K and ΔG.
R3.1 Proton transfer reactions
3.1.1 Brønsted-Lowry acid (proton donor) and base (proton acceptor).
3.1.2 Conjugate acid-base pair (differ by one proton).
3.1.3 Amphiprotic species (act as acid or base).
3.1.4 The pH scale: pH=−log10[H+].
3.1.5 Ion product constant of water (Kw=[H+][OH−]).
3.1.6 Strong vs. weak acids/bases (extent of ionization).
3.1.7 Neutralization reactions (acid + base).
3.1.8 pH curves for strong acid-strong base titrations.
3.1.9 [AHL] The pOH scale: pOH=−log10[OH−].
3.1.10 [AHL] Ka,Kb,pKa,pKb describe weak acid/base strength.
3.1.11 [AHL] Relationship for conjugate pairs: Ka×Kb=Kw.
3.1.12 [AHL] pH of salt solutions (hydrolysis).
3.1.13 [AHL] pH curves for all strong/weak combinations.
3.1.14 [AHL] Acid-base indicators are weak acids.
3.1.15 [AHL] Choosing an appropriate indicator (end point vs. equivalence point).
3.1.16 [AHL] Buffer solutions resist pH change.
3.1.17 [AHL] pH of a buffer solution (depends on pKa/pKb and concentration ratio).
R3.2 Electron transfer reactions
3.2.1 Oxidation and reduction definitions (e- transfer, oxidation state).
3.2.2 Half-equations show oxidation and reduction separately.
3.2.3 Predicting redox ease from periodic table position.
3.2.4 Acids react with reactive metals to release H2.
3.2.5 Anode (oxidation) and cathode (reduction) in electrochemical cells.
3.2.6 Primary (voltaic) cells (spontaneous redox).
3.2.7 Secondary (rechargeable) cells (reversible redox).
3.2.8 Electrolytic cells (non-spontaneous redox).
3.2.9 Oxidation of organic compounds (alcohols).
3.2.10 Reduction of organic compounds (carboxylic acids, ketones).
3.2.11 Reduction of unsaturated compounds (addition of H2).
3.2.12 [AHL] Standard electrode potential (E⊖) (relative to H2 half-cell).
3.2.13 [AHL] Standard cell potential (E⊖cell); positive for spontaneous reactions.
3.2.14 [AHL] Relationship: ΔG⊖=−nFE⊖.
3.2.15 [AHL] Electrolysis of aqueous solutions (competing reactions).
3.2.16 [AHL] Electroplating.
R3.3 Electron sharing reactions
3.3.1 Radicals: molecular entities with an unpaired electron.
3.3.2 Radicals produced by homolytic fission (UV or heat).
3.3.3 Radicals take part in substitution reactions with alkanes.
R3.4 Electron-pair sharing reactions
3.4.1 Nucleophile: reactant that donates an electron pair.
3.4.2 Nucleophilic substitution: nucleophile donates e- pair, leaving group departs.
3.4.3 Heterolytic fission: bond breaks, both electrons go to one fragment.
3.4.4 Electrophile: reactant that accepts an electron pair.
3.4.5 Electrophilic addition: alkenes susceptible due to high e- density.
3.4.6 [AHL] Lewis acid (e- pair acceptor) and Lewis base (e- pair donor).
3.4.7 [AHL] Lewis acid-base reactions form coordination bonds.
3.4.8 [AHL] Ligands (Lewis bases) form complex ions with transition elements.
3.4.9 [AHL] Nucleophilic substitution mechanisms (SN1, SN2).
3.4.10 [AHL] Rate of substitution influenced by the leaving group.
3.4.11 [AHL] Electrophilic addition mechanisms (symmetrical alkenes).
3.4.12 [AHL] Carbocation stability (unsymmetrical alkenes); major product.
3.4.13 [AHL] Electrophilic substitution mechanisms (benzene).
Official Academic Resources
Download official IB Chemistry resources and curriculum guides below:
2. Study Notes
Access our curated study notes summarizing fundamental chemical concepts and advanced theories:
Save My Exams Revision Notes & Practice Resources * A comprehensive guide covering all topics mapped to the IB Chemistry syllabus. * Access specialized revision notes, multiple-choice practice questions, and structured question banks for each syllabus subtopic below:
| Syllabus Topic & Subtopic | Revision Notes | Multiple Choice | Structured Qs |
|---|---|---|---|
| S1. Models of the particulate nature of matter | |||
| S1.1 Introduction to the particulate nature of matter | Notes | MCQ Qs | Struct Qs |
| S1.2 The nuclear atom | Notes | MCQ Qs | Struct Qs |
| S1.3 Electron configurations | Notes | MCQ Qs | Struct Qs |
| S1.4 Counting particles by mass: The mole | Notes | MCQ Qs | Struct Qs |
| S1.5 Ideal gases | Notes | MCQ Qs | Struct Qs |
| S2. Models of bonding and structure | |||
| S2.1 The ionic model | Notes | MCQ Qs | Struct Qs |
| S2.2 The covalent model | Notes | MCQ Qs | Struct Qs |
| S2.3 The metallic model | Notes | MCQ Qs | Struct Qs |
| S2.4 From models to materials | Notes | MCQ Qs | Struct Qs |
| S3. Classification of matter | |||
| S3.1 The periodic table: Classification of elements | Notes | MCQ Qs | Struct Qs |
| S3.2 Functional groups: Classification of organic compounds | Notes | MCQ Qs | Struct Qs |
| R1. What drives chemical reactions? | |||
| R1.1 Measuring enthalpy changes | Notes | MCQ Qs | Struct Qs |
| R1.2 Energy cycles in reactions | Notes | MCQ Qs | Struct Qs |
| R1.3 Energy from fuels | Notes | MCQ Qs | Struct Qs |
| R1.4 Entropy and spontaneity (AHL) | Notes | MCQ Qs | Struct Qs |
| R2. How much, how fast and how far? | |||
| R2.1 How much? The amount of chemical change | Notes | MCQ Qs | Struct Qs |
| R2.2 How fast? The rate of chemical change | Notes | MCQ Qs | Struct Qs |
| R2.3 How far? The extent of chemical change | Notes | MCQ Qs | Struct Qs |
| R3. What are the mechanisms of chemical change? | |||
| R3.1 Proton transfer reactions | Notes | MCQ Qs | Struct Qs |
| R3.2 Electron transfer reactions | Notes | MCQ Qs | Struct Qs |
| R3.3 Electron sharing reactions | Notes | MCQ Qs | Struct Qs |
| R3.4 Electron-pair sharing reactions | Notes | MCQ Qs | Struct Qs |
| Tools | |||
| Tool 1: Experimental techniques | Notes | N/A | N/A |
| Tool 2: Technology | Notes | N/A | N/A |
| Tool 3: Mathematics | Notes | N/A | N/A |
| Inquiry | |||
| Collecting Data in Chemistry | Notes | N/A | N/A |
| Exploring and Designing in Chemistry | Notes | N/A | N/A |
3. Practice Questions
Access targeted conceptual questions modeled after actual exam formats:
2025 Syllabus Practice Questions
Practice questions mapped to the new 2025 IB Chemistry syllabus themes and subtopics.
| Topic | Question Bank |
|---|---|
| S1 — Models of the Particulate Nature of Matter | Full Theme |
| S1.1 — Introduction to the Particulate Nature of Matter | Open PDF |
| S1.2 — The Nuclear Atom | Open PDF |
| S1.3 — Electron Configurations | Open PDF |
| S1.4 — The Mole | Open PDF |
| S1.5 — Ideal Gases | Open PDF |
| S2 — Models of Bonding & Structure | Full Theme |
| S2.1 — The Ionic Model | Open PDF |
| S2.2 — The Covalent Model | Open PDF |
| S2.3 — The Metallic Model | Open PDF |
| S2.4 — From Models to Materials | Open PDF |
| S3 — Classification of Matter | Full Theme |
| S3.1 — The Periodic Table - Classification of Elements | Open PDF |
| S3.2 — Functional Groups - Classification of Organic Compounds | Open PDF |
| R1 — What Drives Chemical Reactions? | Full Theme |
| R1.1 — Measuring Enthalpy Changes | Open PDF |
| R1.2 — Energy Cycles in Reactions | Open PDF |
| R1.3 — Energy From Fuels | Open PDF |
| R1.4 — Entropy & Spontaneity | Open PDF |
| R2 — How Much, How Fast & How Far? | Full Theme |
| R2.1 — The Amount of Chemical Change | Open PDF |
| R2.2 — The Rate of Chemical Change | Open PDF |
| R2.3 — The Extent of Chemical Change | Open PDF |
| R3 — Mechanisms of Chemical Change | Full Theme |
| R3.1 — Proton Transfer Reactions | Open PDF |
| R3.2 — Electron Transfer Reactions | Open PDF |
| R3.3 — Electron Sharing Reactions | Open PDF |
| R3.4 — Electron-pair Sharing Reactions | Open PDF |
| T — Tools & Inquiries | Full Theme |
| I2 — Collecting & Processing Data | Open PDF |
| I3 — Concluding & Evaluating | Open PDF |
| T1 — Experimental Techniques | Open PDF |
| T3 — Mathematics Tools | Open PDF |
IB Chemistry HL — 2016 Syllabus Practice Questions
Practice questions organized by the pre-2025 IB Chemistry topic structure.
| Topic | Question Paper | Mark Scheme |
|---|---|---|
| Topic 1: Stoichiometric Relationships | QP | MS |
| Topic 2: Atomic Structure | QP | MS |
| Topic 3: Periodicity | QP | MS |
| Topic 4: Chemical Bonding & Structure | QP | MS |
| Topic 5: Energetics / Thermochemistry | QP | MS |
| Topic 6: Chemical Kinetics | QP | MS |
| Topic 7: Equilibrium | QP | MS |
| Topic 8: Acids & Bases | QP | MS |
| Topic 9: Redox Processes | QP | MS |
| Topic 10: Organic Chemistry | QP | MS |
| Topic | Paper 1 | Paper 2 |
|---|---|---|
| Topic 1: Stoichiometric Relationships | ||
| Topic 2: Atomic Structure | ||
| Topic 3: Periodicity | ||
| Topic 4: Chemical Bonding & Structure | ||
| Topic 5: Energetics / Thermochemistry | ||
| Topic 6: Chemical Kinetics | ||
| Topic 7: Equilibrium | ||
| Topic 8: Acids & Bases | ||
| Topic 9: Redox Processes | ||
| Topic 10: Organic Chemistry | ||
| Topic 11: Measurement & Data Processing | N/A |
| Topic | Question Bank |
|---|---|
| Topic 1: Stoichiometric Relationships | |
| Matter & Chemical Change | Open PDF |
| Reacting Masses and Volumes | Open PDF |
| Stoichiometric Relationships | Open PDF |
| The Mole Concept | Open PDF |
| Topic 2: Atomic Structure | |
| Atomic Structure | Open PDF |
| Atomic Structure (HL) | Open PDF |
| Electron Configuration | Open PDF |
| The Nuclear Atom | Open PDF |
| Topic 3: Periodicity | |
| Coloured Complexes | Open PDF |
| First-Row D-Block Elements | Open PDF |
| Periodic Table | Open PDF |
| Periodic Trends | Open PDF |
| Periodicity | Open PDF |
| The Periodic Table - the Transition Metals (HL) | Open PDF |
| Topic 4: Chemical Bonding & Structure | |
| Chemical Bonding & Structure | Open PDF |
| Chemical Bonding & Structure (HL) | Open PDF |
| Covalent Bonding | Open PDF |
| Covalent Bonding, Electron Domain, and Molecular Geometries | Open PDF |
| Covalent Structures | Open PDF |
| Hybridization | Open PDF |
| Intermolecular Forces | Open PDF |
| Ionic Bonding & Structure | Open PDF |
| Metallic Bonding | Open PDF |
| Topic 5: Energetics / Thermochemistry | |
| Bond Enthalpies | Open PDF |
| Chemical Kinetics (HL) | Open PDF |
| Energetics _ Thermochemistry | Open PDF |
| Energetics _ Thermochemistry (HL) | Open PDF |
| Energy Cycles | Open PDF |
| Hess's Law | Open PDF |
| Measuring Energy Changes | Open PDF |
| Topic 6: Chemical Kinetics | |
| Activation Energy | Open PDF |
| Chemical Kinetics | Open PDF |
| Collision Theory and Rates of Reaction | Open PDF |
| Entropy & Spontanaeity | Open PDF |
| Rate Expression & Reaction Mechanism | Open PDF |
| Topic 7: Equilibrium | |
| Equilibrium | Open PDF |
| Equilibrium (HL) | Open PDF |
| Topic 8: Acids & Bases | |
| Acid Deposition | Open PDF |
| Acids & Bases | Open PDF |
| Acids & Bases (HL) | Open PDF |
| Calculations Involving Acids & Bases | Open PDF |
| Lewis Acids & Bases | Open PDF |
| Properties of Acids & Bases | Open PDF |
| Strength of Acids & Bases | Open PDF |
| The pH Scale | Open PDF |
| Theories of Acids & Bases | Open PDF |
| pH Curves | Open PDF |
| Topic 9: Redox Processes | |
| Electrochemical Cells | Open PDF |
| Oxidation & Reduction | Open PDF |
| Redox Processes | Open PDF |
| Redox Processes (HL) | Open PDF |
| Topic 10: Organic Chemistry | |
| Functional Groups | Open PDF |
| Fundamentals of Organic Chemistry | Open PDF |
| Organic Chemistry | Open PDF |
| Organic Chemistry (HL) | Open PDF |
| Stereoisomerism | Open PDF |
| Synthetic Routes | Open PDF |
| Types of Organic Reactions | Open PDF |
| Topic 11: Measurement & Data Processing | |
| Graphical Techniques | Open PDF |
| Measurement & Analysis (HL) | Open PDF |
| Measurement & Data Processing | Open PDF |
| Spectroscopic Identification of Organic Compounds | Open PDF |
| Uncertainties & Errors in Measurement & Results | Open PDF |
4. Topical Past Paper Questions
Topical collection of past exam questions sorted by syllabus and paper to help you focus on specific areas of the curriculum:
| Topics | Paper 1A Questions | Paper 2 Questions |
|---|---|---|
| Chapter 1: Introduction to the Particulate Nature of Matter | Part 1 | Part 1 |
| Chapter 2: The Nuclear Atom | Part 1 | Part 1 |
| Chapter 3: Electron Configurations | Part 1 | Part 1 |
| Chapter 4: Counting Particles by Mass: The Mole | Part 1 | Part 1 |
| Chapter 5: Ideal Gases | Part 1 | Part 1 |
| Chapter 6: The Ionic Model | Part 1 | Part 1 |
| Chapter 7: The Covalent Model | Part 1 | Part 1 |
| Chapter 8: The Metallic Model | Part 1 | Part 1 |
| Chapter 9: From Models to Materials | Part 1 | Part 1 |
| Chapter 10: The Periodic Table: Classification of Elements | Part 1 | Part 1 |
| Chapter 11: Functional Groups: Classification of Organic Compounds | Part 1 | Part 1 |
| Chapter 12: Measuring Enthalpy Change | Part 1 | Part 1 |
| Chapter 13: Measuring Enthalpy Change | Part 1 | Part 1 |
| Chapter 14: Energy Cycles in Reactions | Part 1 | Part 1 |
| Chapter 15: Energy from Fuels | Part 1 | Part 1 |
| Chapter 16: Entropy and Spontaneity | Part 1 | Part 1 |
| Chapter 17: How Much: The Amount of Chemical Change | Part 1 | Part 1 |
| Chapter 18: How Fast: The Rate of Chemical Change | Part 1 | Part 1 |
| Chapter 19: How Far: The Extent of Chemical Change | Part 1 | Part 1 |
| Chapter 20: Proton Transfer Reactions | Part 1 | Part 1 |
| Chapter 21: Electron Transfer Reactions | Part 1 | Part 1 |
| Chapter 22: Electron Sharing Reactions | Part 1 | Part 1 |
| Chapter 23: Electron-Pair Sharing Reactions | Part 1 | Part 1 |
| Topics | Paper 1 Questions | Paper 2 Questions |
|---|---|---|
| Chapter 1: Stoichiometric Relationships | Part 1 Part 2 Part 3 | Part 1 Part 2 |
| Chapter 2: Atomic Structure | Part 1 Part 2 | Part 1 Part 2 |
| Chapter 3: Periodicity | Part 1 Part 2 Part 3 | Part 1 Part 2 |
| Chapter 4: Chemical Bonding and Structure | Part 1 Part 2 Part 3 Part 4 Part 5 | Part 1 Part 2 |
| Chapter 5: Energetics and Thermochemistry | Part 1 Part 2 Part 3 Part 4 | Part 1 Part 2 |
| Chapter 6: Chemical Kinetics | Part 1 Part 2 Part 3 | Part 1 Part 2 |
| Chapter 7: Equilibrium | Part 1 Part 2 | Part 1 Part 2 |
| Chapter 8: Acids and Bases | Part 1 Part 2 Part 3 Part 4 | Part 1 Part 2 |
| Chapter 9: Redox Processes | Part 1 Part 2 Part 3 | Part 1 Part 2 |
| Chapter 10: Organic Chemistry | Part 1 Part 2 Part 3 Part 4 Part 5 Part 6 | Part 1 Part 2 |
| Chapter 11: Measurement and Data Processing | Part 1 Part 2 | Part 1 Part 2 |