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Subjects
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Chemistry HL

IB Sciences • HL

Chemistry HL

Browse the full topic structure and open study materials for Chemistry HL.

Structured practice

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Structure 1. Models of the particulate nature of matter

S1.1 Introduction to the particulate nature of matter

S1.1.1 Elements, Compounds and Mixtures

S1.1.2 The Kinetic Molecular Theory

S1.1.3 Temperature and Kinetic Energy

S1.2 The nuclear atom

S1.2.1 Atomic Structure

S1.2.2 Isotopes

S1.2.3 Mass Spectrometry (Higher Level Only)

S1.3 Electron configurations

S1.3.1 Emission spectra and energy levels

S1.3.2 Hydrogen emission spectrum

S1.3.3 Main energy levels

S1.3.4 Sublevels and orbitals

S1.3.5 Orbital configurations and rules

S1.3.6 Ionization energy (Higher Level Only)

S1.3.7 Successive ionization energies (Higher Level Only)

S1.4 Counting particles by mass: the mole

S1.4.1 The mole and Avogadro constant

S1.4.2 Relative atomic and formula masses

S1.4.3 Molar mass

S1.4.4 Empirical and molecular formulas

S1.4.5 Molar concentration

S1.4.6 Avogadro's law

S1.5 Ideal gases

S1.5.1 The ideal gas model

S1.5.2 Deviations from ideal gas behavior

S1.5.3 Molar volume of an ideal gas

S1.5.4 The ideal gas equation

Structure 2. Models of bonding and structure

S2.1 The ionic model

S2.1.1 Formation of ions

S2.1.2 Ionic bonds and binary compounds

S2.1.3 Lattice structures and properties

S2.2 The covalent model

S2.2.1 Formation of covalent bonds

S2.2.2 Single, double and triple bonds

S2.2.3 Coordination bonds

S2.2.4 VSEPR theory

S2.2.5 Bond polarity

S2.2.6 Molecular polarity

S2.2.7 Covalent network structures

S2.2.8 Intermolecular forces

S2.2.9 Intermolecular forces and physical properties

S2.2.10 Chromatography

S2.2.11 Resonance structures (Higher Level Only)

S2.2.12 Benzene (Higher Level only)

S2.2.13 Expanded Octet of Electrons (Higher Level Only)

S2.2.14 Formal Charge and Lewis Formulas (Higher Level Only)

S2.2.15 Sigma and Pi Bonds (Higher Level Only)

S2.2.16 Hybridization and Bonding (Higher Level Only)

S2.3 The metallic model

S2.3.1 Metallic bonding and properties of metals

S2.3.2 Strength of metallic bonds

S2.3.3 Transition elements and delocalized d-electrons (Higher Level Only)

S2.4 From models to materials

S2.4.1 Bonding as a continuum

S2.4.2 Position in the bonding triangle

S2.4.4 Polymers

S2.4.5 Addition polymers

S2.4.6 Condensation polymers (Higher Level)

Structure 3. Classification of matter

S3.1 The periodic table: classification of elements

S3.1.1 The structure of the periodic table

S3.1.2 Electron configuration and group trends

S3.1.3 Periodicity of properties

S3.1.4 Trends in chemical reactivity

S3.1.5 Metallic and non-metallic oxides

S3.1.6 Oxidation states

S3.1.7 Discontinuities in ionization energy trends (Higher Level Only)

S3.1.8 Properties of transition elements (Higher Level Only)

S3.1.9 Oxidations states of transition elements (Higher Level Only)

S3.1.10 Color of transition metal complexes (Higher Level Only)

S3.2 Functional groups: classification of organic compounds

S3.2.1 Representation of organic compounds

S3.2.2 Functional groups

S3.2.3 Homologous series

S3.2.4 Physical trends in homologous series

S3.2.5 IUPAC nomenclature

S3.2.6 Structural isomers

S3.2.7 Stereoisomers (Higher Level Only)

S3.2.8 Mass spectrometry (Higher Level Only)

S3.2.9 Infrared spectra (Higher Level Only)

S3.2.10 Proton nuclear magnetic resonance spectroscopy (Higher Level Only)

S3.2.11 H NMR spectra interpretation (Higher Level Only)

S3.2.12 Structural analysis (Higher Level Only)

Reactivity 1. What drives chemical reactions?

R1.1 Measuring enthalpy change

R1.1.1 Energy transfer in chemical reactions

R1.1.2 Endothermic and exothermic reactions

R1.1.3 Energy profiles

R1.1.4 Standard enthalpy change

R1.1.5 Practical considerations

R1.2 Energy cycles in reactions

R1.2.1 Bond enthalpy

R1.2.2 Hess's Law

R1.2.3 Standard enthalpy changes of combustion and formation (Higher Level Only)

R1.2.4 Hess's Law with combustion and formation data (Higher Level Only)

R1.2.5 Born-Haber Cycle (Higher Level Only)

R1.3 Energy from fuels

R1.3.1 Combustion fuels

R1.3.2 Incomplete combustion

R1.3.3 Fossil fuels

R1.3.4 Biofuels

R1.3.5 Fuel cells

R1.4 Entropy and spontaneity (Higher Level)

R1.4.1 Entropy (S) (Higher Level Only)

R1.4.2 Gibbs free energy (ΔG) (Higher Level Only)

R1.4.3 Spontaneity and Gibbs free energy (Higher Level Only)

R1.4.4 Gibbs free energy and equilibrium (Higher Level Only)

Reactivity 2. How much, how fast and how far?

R2.1 How much? The amount of chemical change

R2.1.1 Chemical equations and stoichiometry

R2.1.2 Using the mole ratio

R2.1.3 Limiting and excess reactants

R2.1.4 Percentage yield

R2.1.5 Atom economy

R2.2 How fast? The rate of chemical change

R2.2.1 Rate of reaction

R2.2.2 Collision theory

R2.2.3 Factors affecting the rate of reaction

R2.2.4 Activation energy

R2.2.5 Catalysts

R2.2.6 Reaction mechanisms and rate-determining steps (Higher Level Only)

R2.2.7 Energy profiles and transition states (Higher Level Only)

R2.2.8 Molecularity (Higher Level Only)

R2.2.9 Rate equations (Higher Level Only)

R2.2.10 Order of a reaction (Higher Level Only)

R2.2.11 Rate constant (Higher Level Only)

R2.2.12 Arrhenius equation (Higher Level Only)

R2.2.13 Arrhenius factor (Higher Level Only)

R2.3 How far? The extent of chemical change

R2.3.1 Dynamic equilibrium

R2.3.2 The equilibrium law and constant

R2.3.3 Magnitude of K and temperature dependence

R2.3.4 Le Châtelier’s principle

R2.3.5 Reaction quotient (Q) (Higher Level Only)

R2.3.6 Quantifying equilibrium concentrations (Higher Level Only)

R2.3.7 Gibbs free energy and equilibrium (Higher Level Only)

Reactivity 3. What are the mechanisms of chemical change?

R3.1 Proton transfer reactions

R3.1.1 Brønsted–Lowry acid-base theory

R3.1.2 Conjugate acid-base pairs

R3.1.3 Amphiprotic species

R3.1.4 pH and the hydrogen ion concentration

R3.1.5 The ion product of water (Kw)

R3.1.6 Strong and weak acids and bases

R3.1.7 Neutralization reactions

R3.1.8 pH curves for neutralization

R3.1.9 pOH scale (Higher Level Only)

R3.1.10 Acid and base strength and constants (Higher Level Only)

R3.1.11 Conjugate Acid-Base pair (Higher Level Only)

R3.1.12 The pH of a salt solution (Higher Level only)

R3.1.13 pH curves of Acid-Base combinations (Higher Level Only)

R3.1.14 Acid-Base indicators and pH changes (Higher Level Only)

R3.1.15 Appropriate indicators for titration (Higher Level Only)

R3.1.16 Buffer solutions (Higher Level Only)

R3.1.17 The pH of a buffer solution (Higher Level Only)

R3.2 Electron transfer reactions

R3.2.1 Oxidation and reduction definitions

R3.2.2 Redox half-equations

R3.2.3 Reactivity of elements based on periodic trends

R3.2.4 Acid-metal reactions

R3.2.5 Electrochemical cells: Oxidation and reduction

R3.2.6 Primary (voltaic) cells

R3.2.7 Secondary (rechargeable) cells

R3.2.8 Electrolytic cells

R3.2.9 Oxidation of organic compounds

R3.2.10 Reduction of functional groups

R3.2.11 Reduction of unsaturated compounds

R3.2.12 Standard electrode potentials (Higher Level Only)

R3.2.13 Standard cell potential (Higher Level Only)

R3.2.14 Gibbs free energy and cell potential (Higher Level Only)

R3.2.15 Electrolysis of aqueous solutions (Higher Level Only)

R3.2.16 Electroplating (Higher Level Only)

R3.3 Electron sharing reactions

R3.3.1 Radicals

R3.3.2 Homolytic fission

R3.3.3 Substitution reactions with alkanes

R3.4 Electron pair sharing reactions

R3.4.1 Nucleophiles

R3.4.2 Nucleophilic substitution reactions

R3.4.3 Heterolytic fission

R3.4.4 Electrophiles

R3.4.5 Electrophilic attack

R3.4.6 Lewis acid (Higher Level Only)

R3.4.7 Lewis acid-base reaction (Higher Level Only)

R3.4.8 Ligands and coordination bond (Higher Level Only)

R3.4.9 SN1 and SN2 mechanisms (Higher Level Only)

R3.4.10 Rate of the substitution reactions (Higher Level Only)

R3.4.11 Electrophilic addition (Higher Level only)

R3.4.12 The relative stability of carbocations (Higher Level Only)

R3.4.13 Reactions between benzene and electrophiles (Higher Level Only)