IBDP Chemistry SL
This AccelaStudy domain covers the complete IB Diploma Programme Chemistry Standard Level curriculum as specified in the IB Chemistry guide (first assessment 2025). The course is organized around two interlocking strands — Structure and Reactivity — that together build a coherent, conceptual understanding of chemistry rather than a collection of isolated facts.The Structure strand (Themes 1–3) develops models of matter from the sub-atomic level upward: atomic structure and electron configuration, periodic trends, moles and stoichiometry, bonding models (ionic, covalent, metallic), molecular geometry via VSEPR, intermolecular forces, and the classification of organic and inorganic matter including spectroscopic identification techniques.The Reactivity strand (Themes 4–6) addresses the driving forces, rates, and mechanisms of chemical change: thermochemistry and Hess's law, entropy and Gibbs free energy, redox chemistry and electrochemical cells, collision theory and kinetics, chemical equilibrium and Le Chatelier's principle, acid–base chemistry and pH calculations, and organic reaction mechanisms including substitution, addition, condensation, and hydrolysis pathways.Experimental and inquiry skills are woven throughout, culminating in the Internal Assessment — an individual scientific investigation of the student's own design. The domain provides dedicated coverage of measurement uncertainty, data processing, graphical analysis, and the criteria used to assess the IA.Nature of Science (NOS) threads are integrated across all themes, encouraging students to reflect on how chemical knowledge is constructed, validated, and revised, and on the ethical responsibilities that accompany scientific practice.All content is mapped to the four IB assessment objectives (AO1–AO4) and aligned with the command terms used in IB Chemistry examinations. Adaptive practice questions, contrastive pairs, and worked examples are calibrated to Paper 1 (data-based and multiple-choice) and Paper 2 (structured and extended-response) formats.
210
Minutes
90
Questions
4/7
Passing Score
$173
Exam Cost
Who Should Take This
This domain is designed for IB Diploma students taking Chemistry at Standard Level, typically in Years 1–2 of the Diploma Programme. It is ideal for students who plan to pursue university studies in medicine, pharmacy, biology, environmental science, engineering, or any discipline that requires a solid grounding in chemical principles. It is also well-suited to students who want to strengthen their quantitative reasoning and experimental skills in a globally recognized framework. No prior formal chemistry course is strictly required, though familiarity with basic atomic concepts and algebra is assumed.
What's Covered
1Atomic structure, the periodic table and periodic trends, moles and stoichiometry, ideal gases
2Ionic bonding, covalent bonding, Lewis structures, VSEPR, molecular polarity, intermolecular forces, metallic bonding, solid structures
3Organic functional groups and nomenclature, isomerism, mixtures and separation techniques, spectroscopic identification (IR and ¹H NMR at SL)
4Thermochemistry, enthalpy, Hess's law, bond enthalpies, entropy, Gibbs free energy, redox and electrochemistry
5Reaction kinetics, collision theory, Maxwell–Boltzmann distributions, chemical equilibrium, Le Chatelier's principle, Kc, acids and bases, pH, buffers
6Free-radical substitution, electrophilic addition, nucleophilic substitution, condensation and hydrolysis, addition and condensation polymerization, multi-step synthesis
71,500–2,500 word individual investigation assessed on personal engagement, exploration, analysis, evaluation, and communication; teacher-marked and externally moderated
What's Included in AccelaStudy® AI
Adaptive Knowledge Graph
Practice Questions
Lesson Modules
Console Simulator Labs
Exam Tips & Strategy
13 Activity Formats
Course Outline
1Structure 1: Models of the Particulate Nature of Matter 3 topics
Atomic Structure
- Describe the nuclear model of the atom, identifying the relative masses and charges of protons, neutrons, and electrons, and define atomic number, mass number, and isotopes with reference to specific examples.
- Explain the evidence for quantized energy levels in atoms using emission spectra, describing how electron transitions between energy levels produce characteristic lines in the hydrogen spectrum.
- State the electron configurations of atoms and ions up to Z=36 using subshell notation (1s²2s²2p⁶…) and identify the relationship between configuration and position in the periodic table.
- Calculate the relative atomic mass of an element from isotopic masses and abundances given as percentages, applying the weighted-average formula and expressing the answer to appropriate significant figures.
The Periodic Table — Periodic Trends
- Describe the organization of the periodic table into periods, groups, blocks (s, p, d), and the distinction between metals, metalloids, and non-metals, identifying trends in physical properties across periods and down groups.
- Explain the periodic trends in atomic radius, ionic radius, ionization energy, and electronegativity across Period 3 and down Group 1 and Group 17, linking each trend to nuclear charge, shielding, and electron configuration.
- Evaluate the limitations of periodic trends by discussing anomalies such as the ionization energy dip between Groups 2 and 13 and between Groups 15 and 16, explaining these in terms of electron sub-shell and spin-pairing effects.
Moles and Stoichiometry
- Define the mole concept and Avogadro's constant, and calculate the number of particles, molar mass, and amount in moles for elements, compounds, and mixtures given mass or particle data.
- Determine empirical and molecular formulas from percentage composition or combustion analysis data, showing stepwise mole-ratio calculations and verifying consistency with given molar mass values.
- Calculate theoretical yield, percentage yield, and atom economy for chemical reactions, identifying the limiting reagent and explaining the significance of atom economy in the context of green chemistry principles.
- Apply the ideal gas law (PV = nRT) and molar volume at STP to calculate the volume, pressure, temperature, or amount of a gas, and explain the assumptions of the ideal gas model and conditions under which real gases deviate.
2Structure 2: Models of Bonding and Structure 4 topics
Ionic Bonding and Structure
- Describe the formation of ionic bonds through electron transfer between metals and non-metals, and explain how lattice enthalpy, ion charge, and ion size determine the physical properties of ionic compounds including melting point and electrical conductivity.
- Draw the electron-dot (Lewis) structures of common ionic compounds, correctly representing the transfer of electrons and the resulting noble-gas configurations of the ions formed.
Covalent Bonding and Molecular Geometry
- Draw Lewis (electron-dot) structures for molecules and polyatomic ions, including resonance structures, formal charges, and expanded octets for Period 3 elements, applying the octet rule and its exceptions correctly.
- Predict the three-dimensional shape and bond angles of molecules and ions using VSEPR theory, distinguishing between electron-domain geometry and molecular geometry for species with two to six electron domains.
- Explain bond polarity using electronegativity differences and determine whether a molecule is polar or non-polar by considering both bond polarity and molecular geometry, providing examples such as CO₂, H₂O, NH₃, and CH₄.
Intermolecular Forces and Physical Properties
- Describe and compare the three types of intermolecular forces — London dispersion forces, dipole–dipole interactions, and hydrogen bonding — explaining the structural features required for each and ranking their relative strengths.
- Explain trends in boiling points, solubility, and viscosity of molecular substances by relating the type and strength of intermolecular forces to the energy required to overcome them, using specific examples from Groups 14–17 hydrides.
Metallic Bonding and Giant Structures
- Describe the metallic bonding model as a lattice of positive ions surrounded by a delocalized sea of electrons, and explain how this model accounts for the electrical conductivity, malleability, ductility, and high melting points of metals.
- Compare the four types of solid structures — ionic, covalent network, metallic, and molecular — by evaluating their bonding, representative examples, and resulting physical properties including melting point, hardness, and electrical conductivity.
3Structure 3: Classification of Matter 3 topics
Functional Groups and Organic Nomenclature
- Identify and name the principal organic functional groups — alkane, alkene, alkyne, arene, haloalkane, alcohol, aldehyde, ketone, carboxylic acid, ester, amine, and amide — and apply IUPAC nomenclature rules to compounds with up to six carbon atoms.
- Distinguish between structural isomers (chain, position, and functional-group isomers) and stereoisomers (cis–trans and optical isomers), drawing and naming examples and explaining the conditions required for each type of isomerism.
Mixtures, Solutions, and Separation Techniques
- Describe the principles and applications of common separation techniques — filtration, distillation, recrystallization, paper and thin-layer chromatography, and column chromatography — explaining the physical or chemical basis of each method.
- Calculate and interpret Rf values from chromatography data, and explain how polarity of the stationary and mobile phases determines the separation of components in thin-layer and paper chromatography.
Spectroscopic Identification of Organic Compounds
- Identify functional groups and structural features of organic molecules using infrared (IR) spectroscopy data, interpreting characteristic absorption wavenumbers for O–H, N–H, C=O, and C–H bonds from provided spectra or data tables.
- Interpret ¹H NMR spectra at SL level by identifying the number of chemically distinct proton environments, relative integration values, and chemical shift ranges to deduce or confirm the structural formula of an organic compound.
4Reactivity 1: What Drives Chemical Reactions? 3 topics
Thermochemistry and Enthalpy
- Define enthalpy change (ΔH) and distinguish between exothermic and endothermic reactions using energy-level diagrams, identifying the sign convention for ΔH and the standard conditions (298 K, 100 kPa) used in thermochemical data.
- Calculate the enthalpy change of a reaction using calorimetry data (q = mcΔT), applying appropriate unit conversions and mole calculations, and evaluate sources of experimental error that cause the measured value to differ from the standard value.
- Apply Hess's law to calculate unknown enthalpy changes by constructing energy cycles or combining thermochemical equations, including the use of standard enthalpies of formation and combustion from data booklet values.
- Calculate average bond enthalpies to estimate ΔH for gas-phase reactions, explaining why values calculated from bond enthalpies are approximations compared to those obtained from Hess's law cycles using standard formation enthalpies.
Entropy and Spontaneity
- Describe entropy (S) as a measure of the dispersal of energy and matter, predict the sign of ΔS for physical and chemical changes, and explain why entropy increases with temperature, dissolution, and reactions that increase the number of gas-phase particles.
- Calculate the Gibbs free energy change (ΔG = ΔH − TΔS) for a reaction at a given temperature and determine whether the reaction is spontaneous, non-spontaneous, or at equilibrium, explaining the temperature dependence of spontaneity for each ΔH/ΔS combination.
Electrochemistry — Redox and Cells
- Identify oxidation and reduction in terms of electron transfer and changes in oxidation state, assign oxidation numbers to atoms in compounds and ions using established rules, and identify oxidizing and reducing agents in redox reactions.
- Construct balanced half-equations and overall ionic equations for redox reactions in acidic and neutral aqueous solution using the half-equation method, ensuring conservation of atoms, charge, and electrons.
- Determine the standard cell potential (E°cell) of a galvanic cell from standard electrode potentials, predict the direction of spontaneous electron flow, and explain the relationship between E°cell and the spontaneity of the redox reaction.
- Describe the operation of electrolytic cells, predict the products of electrolysis of molten and aqueous electrolytes using the activity series and standard electrode potentials, and apply Faraday's laws to calculate the mass of product deposited.
5Reactivity 2: How Much, How Fast, and How Far? 3 topics
Reaction Kinetics
- Define rate of reaction and describe how it is measured experimentally using changes in concentration, volume of gas, mass, or absorbance over time, including the calculation of average and instantaneous rates from graphical data.
- Explain the effect of concentration, temperature, surface area, and catalysts on reaction rate using collision theory and Maxwell–Boltzmann distribution diagrams, distinguishing between the effect on activation energy and on collision frequency.
- Construct and interpret Maxwell–Boltzmann distribution curves for a sample of gas molecules at different temperatures, annotating the activation energy threshold and explaining why a small temperature increase causes a large increase in reaction rate.
Chemical Equilibrium
- Describe the characteristics of dynamic chemical equilibrium, explain why the equilibrium constant Kc is temperature-dependent but unaffected by concentration changes or catalysts, and write Kc expressions for homogeneous equilibria from balanced equations.
- Apply Le Chatelier's principle to predict the direction of equilibrium shift in response to changes in concentration, pressure, and temperature, and explain the industrial significance of these factors using the Haber process as a case study.
- Calculate equilibrium concentrations and the value of Kc from initial concentrations and equilibrium data using ICE (Initial–Change–Equilibrium) tables, and determine whether a system is at equilibrium by comparing the reaction quotient Q with Kc.
Acids, Bases, and Buffers
- Define acids and bases using the Brønsted–Lowry model, identify conjugate acid–base pairs in proton-transfer reactions, and distinguish between strong and weak acids and bases in terms of degree of dissociation and relative values of Ka and Kb.
- Calculate pH of strong acids, strong bases, and weak acids using the expressions pH = −log[H⁺], pOH = −log[OH⁻], and the Ka expression, applying the assumption that dissociation of weak acids is small relative to initial concentration where appropriate.
- Interpret acid–base titration curves for strong acid–strong base and weak acid–strong base combinations, identifying the equivalence point, half-equivalence point, and buffer region, and explaining the choice of appropriate indicator for each titration.
- Explain how a buffer solution resists changes in pH when small amounts of acid or base are added, describing the composition of acidic buffers and the role of the weak acid–conjugate base equilibrium in maintaining near-constant pH.
6Reactivity 3: What Are the Mechanisms of Chemical Change? 2 topics
Organic Reaction Pathways
- Describe the conditions, reagents, and products of free-radical substitution of alkanes with halogens, explaining the initiation, propagation, and termination steps and the reason why a mixture of products is formed.
- Explain the electrophilic addition reactions of alkenes with hydrogen, halogens, hydrogen halides, and water, predicting the major product of addition to unsymmetrical alkenes using Markovnikov's rule and explaining the carbocation intermediate.
- Describe the nucleophilic substitution of haloalkanes with hydroxide, cyanide, and ammonia nucleophiles, identifying the nucleophile, electrophilic carbon, and leaving group, and explaining how the reaction enables functional group interconversion in synthesis.
- Outline multi-step organic synthesis routes converting between functional groups, selecting appropriate reagents and conditions for each step and justifying the sequence chosen to achieve the target molecule from a given starting material.
Condensation and Hydrolysis Reactions
- Describe the formation of esters by condensation of carboxylic acids with alcohols and the hydrolysis of esters under acidic and basic conditions, writing balanced equations and explaining the reversibility of esterification and the role of acid catalysis.
- Explain the formation of condensation polymers (polyesters and polyamides) from bifunctional monomers, drawing the repeating unit of the polymer and identifying the small molecule eliminated in each condensation step.
- Compare addition polymerization and condensation polymerization in terms of monomer requirements, the presence or absence of a small-molecule by-product, and the structural features of the resulting polymer chains, using named examples of each type.
7Experimental and Inquiry Skills (Internal Assessment) 2 topics
Measurement, Uncertainty, and Data Processing
- Identify and distinguish between random and systematic errors in experimental measurements, explaining how each type affects accuracy and precision, and suggesting specific improvements to reduce each source of error in a given experimental context.
- Calculate absolute and percentage uncertainties for measured quantities and propagate uncertainties through addition, subtraction, multiplication, division, and power operations, expressing final results with appropriate significant figures and uncertainty.
- Construct and interpret graphs of experimental data, including drawing best-fit lines and curves, calculating gradients with uncertainty, identifying anomalous data points, and using graphical linearization to determine the relationship between variables.
Scientific Investigation Design and Evaluation
- Design a controlled scientific investigation by formulating a focused research question, stating a testable hypothesis with scientific justification, identifying independent, dependent, and controlled variables, and describing a safe and ethical experimental procedure.
- Evaluate the reliability and validity of experimental data by assessing the impact of identified errors and limitations on the conclusion, comparing results with literature values where available, and proposing realistic modifications to improve the investigation.
- Communicate scientific findings in a structured investigation report, presenting processed data in appropriate tables and graphs, constructing a conclusion that directly addresses the research question, and citing sources using a consistent referencing format.
8Nature of Science and Cross-Cutting Concepts 1 topic
Models, Evidence, and Scientific Thinking
- Evaluate the role of models in chemistry — including atomic models, bonding models, and kinetic-molecular theory — by discussing their predictive power, limitations, and the historical evidence that led to their development or revision.
- Discuss the ethical responsibilities of chemists in relation to the development and use of chemical substances, including the environmental impact of industrial processes, the role of green chemistry principles, and the societal implications of chemical research.
Scope
Included Topics
- All five SL core themes: Structure 1 (Models of the particulate nature of matter), Structure 2 (Models of bonding and structure), Structure 3 (Classification of matter), Reactivity 1 (What drives chemical reactions?), Reactivity 2 (How much, how fast and how far?), Reactivity 3 (What are the mechanisms of chemical change?)
- All SL prescribed practical activities and experimental skills: measurement and data processing, graphical analysis, uncertainty propagation, and laboratory safety
- Nature of Science (NOS) strand integrated across all themes: scientific method, models and limitations, paradigm shifts, ethical dimensions of chemistry
- Mathematical skills required at SL: significant figures, unit conversions, logarithms (pH), proportional reasoning, graphical analysis, basic statistical treatment of data
- Internal Assessment: individual scientific investigation (10 hours, 1,500–2,500 words) assessed on personal engagement, exploration, analysis, evaluation, and communication
- Two external assessment components: Paper 1 (data-based and multiple-choice, 36%), Paper 2 (structured and extended-response, 44%)
- All IB Chemistry SL assessment objectives: AO1 (knowledge and understanding), AO2 (application and analysis), AO3 (synthesis and evaluation), AO4 (use and application of appropriate skills)
- IB Chemistry SL command terms taxonomy across all assessment objectives
- Conceptual understandings and guiding questions as specified in the IB Chemistry guide (first assessment 2025)
Not Covered
- All HL-only sub-topics and extensions: additional spectroscopic techniques (13C NMR, mass spectrometry fragmentation patterns beyond SL), advanced organic mechanisms (electrophilic addition detail, nucleophilic substitution SN1/SN2 distinction), crystal field theory, advanced electrochemistry (Nernst equation), formal treatment of reaction mechanisms beyond SL scope
- University-level quantum mechanics beyond the Bohr and quantum-mechanical models described in the SL syllabus
- Detailed industrial process engineering beyond illustrative context (e.g., Haber process economics, detailed reactor design)
- Vendor-specific laboratory software or instrument calibration procedures beyond general principles
- Country-specific environmental regulations cited only as illustrative context
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