International Baccalaureate®︎ Chemistry
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Course Topics
The topics listed below may appear in a variety of International Baccalaureate (IB) Chemistry courses, including IB Chemistry Standard Level (SL) and Higher Level (HL). These study pages are based on the principle that true mastery comes from active problem-solving. Rather than relying solely on textbook explanations or passive notes, these resources focus on strengthening your conceptual understanding through the typical types of problems, exam-style questions, and quantitative challenges you will encounter throughout the IB Chemistry curriculum.
Structure 1: Models of the Particulate Nature of Matter
Structure 1.1 – Introduction to the particulate nature of matter
1.1 Classify matter and separations
1.2 Explain states and transitions
1.3 Interpret thermal energy changes
Structure 1.2 – The nuclear atom
2.1 Explain basic atomic structure
2.2 Define atomic isotopes
2.3 Determine relative atomic mass
Structure 1.3 – Electron configurations
3.1. Explain atomic emission spectra
3.2. Prove discrete energy levels
3.3. Calculate energy level capacity
3.4. Describe electron sub-levels
3.5. Define orbital electron capacity
3.6. Relate convergence to ionization
3.7. Analyze successive ionization energies
Structure 1.4 – Counting particles by mass: The mole
4.1. Define the mole concept
4.2. Define relative atomic mass
4.3. Express molar mass units
4.4. Compare empirical molecular formulas
4.5. Determine molar concentration
4.6. Apply Avogadro's gas law
Structure 1.5 – Ideal gases
5.1. Define ideal gas model
5.2. Explain real gas deviations
5.3. Define molar gas volume
5.4. Apply ideal gas laws
Structure 2: Models of Bonding and Structure
Structure 2.1 – The ionic model
1.1. Explain ion formation
1.2. Define ionic bonding
1.3. Describe ionic lattice structures
Structure 2.2 – The covalent model
2.1. Define covalent bonding
2.2. Compare covalent bond types
2.3. Define coordinate covalent bonds
2.4. Apply VSEPR molecular theory
2.5. Explain bond polarity cause
2.6. Determine overall molecular polarity
2.7. Describe covalent network structures
2.8. Identify intermolecular force determinants
2.9. Compare intermolecular force strengths
2.10. Explain chromatography separation mechanisms
2.11. Explain molecular resonance structures
2.12. Analyze benzene resonance model
2.13. Describe expanded octet molecules
2.14. Calculate atomic formal charges
2.15. Describe sigma bond formation
2.16. Define atomic orbital hybridization
Structure 2.3 – The metallic model
3.1. Define metallic bonding
3.2. Explain metallic bond strength
3.3. Explain delocalized d-electrons
Structure 2.4 – From models to materials
4.1. Explain bonding triangle continuum
4.2. Determine bonding triangle position
4.3. Describe metal alloy properties
4.4. Define basic polymer structure
4.5. Explain addition polymer formation
4.6. Explain condensation polymer formation
Structure 3: Classification of Matter
Structure 3.1 – The periodic table: Classification of elements
1.1. Describe periodic table structure
1.2. Explain period energy levels
1.3. Define periodic property trends
1.4. Describe group property trends
1.5. Explain oxide property trends
1.6. Define atomic oxidation states
1.7. Explain ionization energy anomalies
1.8. Describe transition metal properties
1.9. Explain variable oxidation states
1.10. Explain transition complex colors
Structure 3.2 – Organic structures and functional groups
2.1. Classify organic formula types
2.2. Define functional group roles
2.3. Define homologous series structure
2.4. Analyze homologous series trends
2.5. Apply IUPAC systematic naming
2.6. Define structural isomerism
2.7. Explain stereoisomer spatial arrangements
2.8. Explain mass spectrometry fragmentation
2.9. Identify bonds with infrared
2.10. Analyze proton NMR environments
2.11. Interpret NMR peak splitting
2.12. Combine analytical structural data
Reactivity 1: What Drives Chemical Reactions?
Reactivity 1.1 – Measuring enthalpy changes
1.1. Explain chemical energy conservation
1.2. Classify endothermic exothermic reactions
1.3. Relate stability to energetics
1.4. Define standard enthalpy change
Reactivity 1.2 – Energy cycles in reactions
2.1. Explain bond energy changes
2.2. Define Hess's law
2.3. Use standard enthalpy data
2.4. Calculate reaction enthalpy changes
2.5. Apply Born-Haber cycles
Reactivity 1.3 – Bonding and enthalpy
3.1. Describe basic combustion reactions
3.2. Explain incomplete combustion products
3.3. Compare fossil fuel types
3.4. Explain biofuel carbon fixation
3.5. Describe fuel cell operation
Reactivity 1.4 – Entropy and spontaneity (HL)*
4.1. Define system entropy
4.2. Relate Gibbs energy variables
4.3. Determine reaction spontaneity
4.4. Relate equilibrium to ΔG
Reactivity 2: How Much, How Fast, and How Far?
Reactivity 2.1 – How much? The amount of chemical change
1.1. Interpret chemical equation ratios
1.2. Apply mole ratio calculations
1.3. Identify limiting reactants
1.4. Calculate percentage yield
1.5. Measure reaction atom economy
Reactivity 2.2 – How fast? The rate of chemical change
2.1. Define reaction rate
2.2. State collision theory
2.3. Identify rate factors
2.4. Define activation energy
2.5. Explain catalyst mechanisms
2.6. Identify rate-determining step
2.7. Interpret energy profiles
2.8. Define reaction molecularity
2.9. Determine rate equations experimentally
2.10. Define reaction order
2.11. Analyze rate constant
2.12. Apply Arrhenius equation
2.13. Define Arrhenius factor
Reactivity 2.3 – How far? The extent of chemical change
3.1. Define dynamic equilibrium
3.2. State the equilibrium law.
3.3. Interpret equilibrium constant magnitude
3.4. Apply Le Châtelier's principle
3.5. Calculate reaction quotient Q
3.6. Quantify equilibrium mixture composition
3.7. Relate equilibrium to ΔG
Reactivity 3: What Are the Mechanisms of Chemical Change?
Reactivity 3.1 – Proton transfer reactions
1.1. Define Brønsted–Lowry acids and bases
1.2. Identify conjugate acid–base pairs
1.3. Describe amphiprotic species behavior
1.4. Calculate pH and hydrogen concentration
1.5. Apply water ion product constant
1.6. Compare strong and weak acids
1.7. Describe acid–base neutralization reactions
1.8. Interpret neutralization pH curves
Reactivity 3.2 – Electron transfer reactions
2.1. Define oxidation and reduction
2.2. Construct redox half-equations
2.3. Predict elemental redox trends
2.4. Describe acid–metal reactions
2.5. Identify cell electrode processes
2.6. Explain primary voltaic cells
2.7. Describe secondary rechargeable cells
2.8. Explain electrolytic cell operation
2.9. Describe organic group oxidation
2.10. Describe organic group reduction
2.11. Explain unsaturated compound reduction
Reactivity 3.3 – Electron sharing reactions
3.1. Define free radical properties
3.2. Explain homolytic radical formation
3.3. Describe radical alkane substitution
Reactivity 3.4 – Electron-pair sharing reactions
4.1. Define nucleophile electron donation
4.2. Explain nucleophilic substitution mechanism
4.3. Define heterolytic bond fission
4.4. Define electrophile electron acceptance
4.5. Explain alkene electrophilic addition