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Official source: IB Chemistry curriculum

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Chemistry SL

6 topics41 outcomesLocal syllabus version: 2025

S1: Models of the Particulate Nature of Matter

6 outcomes

Open
  1. S1.1.1Describe the nuclear model of the atom: protons and neutrons in a nucleus surrounded by electrons; define atomic number, mass number, and isotopes
  2. S1.1.2Calculate relative atomic mass from isotopic masses and abundances; describe how a mass spectrometer separates ions by mass-to-charge ratio
  3. S1.2.1Describe the electromagnetic spectrum and explain how atomic emission and absorption line spectra provide evidence for discrete electron energy levels
  4. S1.2.2Write electron configurations for elements and ions up to Z = 36 using sublevel (s, p, d) notation; apply the Aufbau principle, Hund's rule, and Pauli exclusion principle
  5. S1.3.1Apply the mole concept: use the Avogadro constant (6.022 × 10²³ mol⁻¹) to interconvert between amount of substance, number of particles, and molar mass
  6. S1.3.2Determine empirical and molecular formulae from percentage composition data and combustion analysis results

S2: Models of Bonding and Structure

7 outcomes

Open
  1. S2.1.1Describe ionic bonding as electrostatic attraction between oppositely charged ions; explain lattice structure and relate properties (melting point, conductivity) to ionic bonding
  2. S2.2.1Describe covalent bonding as the sharing of electron pairs; draw Lewis (electron dot) structures for molecules and polyatomic ions
  3. S2.2.2Predict and explain the shapes and bond angles of molecules and ions (linear, trigonal planar, tetrahedral, trigonal bipyramidal, octahedral) using VSEPR theory
  4. S2.2.3Distinguish between polar and non-polar bonds using electronegativity differences; determine the polarity of molecules from their geometry
  5. S2.3.1Describe metallic bonding as the electrostatic attraction between a lattice of cations and a sea of delocalised electrons; relate to physical properties of metals
  6. S2.4.1Compare the four types of solid structure (ionic, metallic, covalent network, molecular) and relate their structures to physical properties
  7. S2.4.2Describe London dispersion forces, dipole-dipole attractions, and hydrogen bonding; explain their influence on physical properties such as boiling points and solubility

S3: Classification of Matter

5 outcomes

Open
  1. S3.1.1Explain the organisation of the periodic table by increasing atomic number; identify patterns in physical and chemical properties across periods and down groups
  2. S3.1.2Explain trends in atomic radius, ionic radius, electronegativity, electron affinity, and ionisation energies across periods and down groups
  3. S3.2.1Name and draw structural formulae for the major homologous series: alkanes, alkenes, alkynes, arenes, halogenoalkanes, alcohols, aldehydes, ketones, carboxylic acids, esters, amines, and amides
  4. S3.2.2Identify structural isomers (chain, position, and functional group) and stereoisomers (cis/trans and optical) for organic compounds
  5. S3.2.3Predict physical and chemical properties of organic compounds from their functional groups and carbon skeleton

R1: What Drives Chemical Reactions?

6 outcomes

Open
  1. R1.1.1Define enthalpy change (ΔH) and distinguish between exothermic and endothermic reactions; calculate ΔH from calorimetric data using q = mcΔT
  2. R1.1.2Calculate standard enthalpy changes using Hess's law and standard enthalpies of formation (ΔfH°) or combustion (ΔcH°)
  3. R1.1.3Estimate enthalpy changes using average bond enthalpies and explain why calculated values differ from experimental values
  4. R1.3.1Compare energy density and combustion products of different fuels (hydrogen, hydrocarbons, biofuels) and evaluate their suitability as energy sources
  5. R1.4.1Define entropy (S) and explain how dispersal of energy and matter contribute to an increase in entropy in physical and chemical processes
  6. R1.4.2Calculate Gibbs free energy change (ΔG = ΔH − TΔS) and use its sign to predict whether a reaction is spontaneous under given conditions

R2: How Much, How Fast, and How Far?

8 outcomes

Open
  1. R2.1.1Balance chemical equations and use stoichiometric mole ratios to calculate masses, volumes, and amounts of reactants and products
  2. R2.1.2Identify the limiting reagent in a reaction; calculate theoretical yield, actual yield, and percentage yield
  3. R2.1.3Perform solution stoichiometry calculations involving concentration (mol dm⁻³), dilution, and acid-base titrations
  4. R2.2.1Define rate of reaction; describe experimental methods for monitoring reaction rate (gas volume, mass loss, colour change, conductivity)
  5. R2.2.2Explain collision theory and the effect of concentration, temperature, surface area, pressure (for gases), and catalysts on reaction rate using Maxwell-Boltzmann distributions
  6. R2.3.1Define dynamic equilibrium; describe the characteristics of a system at equilibrium in terms of equal forward and reverse rates
  7. R2.3.2Apply Le Chatelier's principle to predict the effect of changes in concentration, pressure/volume, temperature, and addition of a catalyst on the position of equilibrium
  8. R2.3.3Write the equilibrium constant expression Kc for homogeneous equilibria and calculate Kc from equilibrium concentrations

R3: What Are the Mechanisms of Chemical Change?

9 outcomes

Open
  1. R3.1.1Apply the Brønsted-Lowry theory to identify acids (proton donors), bases (proton acceptors), and conjugate acid-base pairs in reactions
  2. R3.1.2Distinguish between strong and weak acids/bases; calculate pH and pOH from [H⁺] and [OH⁻] concentrations using Kw = 1.0 × 10⁻¹⁴ at 25 °C
  3. R3.1.3Calculate pH of weak acids and bases using Ka and Kb values; derive the relationship pKa + pKb = pKw
  4. R3.1.4Describe acid-base titration curves for strong/weak acid and strong/weak base combinations; identify the equivalence point and choose an appropriate indicator
  5. R3.2.1Define oxidation and reduction in terms of electron transfer and changes in oxidation state; identify oxidising and reducing agents and balance redox equations
  6. R3.2.2Describe the operation of a voltaic (galvanic) cell including electrodes, salt bridge, and direction of electron and ion flow
  7. R3.2.3Calculate cell potential E°cell = E°cathode − E°anode using standard electrode potentials; predict spontaneity of redox reactions
  8. R3.3.1Describe free-radical reactions (homolytic bond cleavage), including the initiation, propagation, and termination steps of the halogenation of alkanes
  9. R3.4.1Describe electrophilic addition reactions of alkenes with H₂, X₂, HX (Markovnikov's rule), and H₂O; explain the mechanism using curly arrows