Chemistry is an experimental science that combines academic study with the acquisition of practical and investigational skills.
It is often called the central science as chemical principles underpin both the physical environment in which we live and all biological systems. Apart from being a subject worthy of study in its own right, chemistry is often a prerequisite for many other courses in higher education, such as medicine, biological science and environmental science.
Through studying a science subject students should become aware of how scientists work and communicate with each other. While the scientific method may take on a wide variety of forms, the emphasis on a practical approach. In addition, through the overarching theme of the “Nature of Science” this knowledge and skills will be put into the context of way science and scientists work in the 21st century and the ethical debates and limitations of creative scientific endeavour.
The sciences are taught practically. Students have opportunities to design investigations, collect data, develop manipulative skills, analyse results, collaborate with peers and evaluate and communicate their findings. The investigations may be laboratory based or they may make use of simulations and data bases. Students develop the skills to work independently on their own design, but also collegiately, including collaboration with schools in different regions, to mirror the way in which scientific research is conducted in the wider community.
Chemistry syllabus outline:
- Higher level (240 hours)
- Internal assessment (individual investigation): 20%
- External assessment: 80%
- Standard level (150 hours)
- Internal assessment (individual investigation): 20%
- External assessment: 80%
Key features of the curriculum and assessment models –
- available at standard (SL) and higher levels (HL)
- The minimum prescribed number of hours is 150 for SL and 240 for HL
- Students are assessed both externally and internally
- Chemistry students at SL and HL undertake a common core syllabus and a common internal assessment (IA) scheme.
While there are core skills and activities common to both SL and HL, students at HL are required to study some topics in greater depth, to study additional topics and to study extension material of a more demanding nature in the options. The distinction between SL and HL is one of breadth and depth.
A practical approach to the course delivery is emphasised through the interdisciplinary group 4 project and a mixture of both short-term and long-term experiments and investigations.
Internal assessment accounts for 20% of the final assessment and this is assessed through a single individual investigation. This investigation may involve a hands-on approach, use of data-bases, modelling, simulation or a hybrid. Student work is internally assessed by the teacher and externally moderated by the IB.
The external assessment of chemistry consists of three written papers. In paper 1 there are 30 (at SL) or 40 (at HL) multiple-choice questions. Paper 2 contains short-answer and extended-response questions on the core (and Additional Higher Level (AHL) material at HL). Paper 3 has two sections; Section A contains one data-based question and several short-answer questions on experimental work on the core (and AHL material at HL). Section B contains short-answer and extended-response questions from each of the four options.
Please click on the arrow for a detailed breakdown:
THE LEARNING JOURNEY FOR CHEMISTRY | |||||
Unit | Subtopic | Key Episodes / Questions | Additional details | Length of time. | Learner Attribute(s) |
Unit 1 | Stoichiometry | Stoichiometric relationships | Formulae Particulate nature of matter Balancing equations | 8 Hours | Reflective |
The mole concept | The mole concept Empirical and molecular formula Reacting masses & volumes Gas Laws Concentration Titrations | ||||
Unit 2 & 12 | Atomic Structure | The nuclear atom | History of atomic theory Atomic structure Isotopes Calculating relative atomic mass | 8 Hours | Principled |
Electrons in atoms | Atomic orbitals Electron configurations Line spectra | ||||
Atomic structure (AHL) | Electrons in atoms | Calculating ionisation energies Successive ionisation energies | |||
Unit 3 & 13 | Periodicity | The periodic table | The structure of the periodic table Regions of the periodic table Electron configuration and the periodic table | 14 hours | Risk Taker |
Periodic trends | Atomic and ionic radii Effective nuclear charge and ionisation energy Electronegativity and electron affinity Metallic character and melting point Trends on oxide behaviour Trends within groups | ||||
The periodic table – Transition elements (AHL) | Properties of transition metals | Transition elements Variable oxidation states Structure of complex ions Magnetic and catalytic behaviour | |||
Coloured complexes | Colour of complex ions | ||||
Unit 4 & 14 | Chemical bonding & structure | Ionic bonding and structure | Ionic bonding Formulae of ionic compounds Physical properties of ionic compounds | 12 Hours | Communicator |
Covalent bonding | Nature of covalent bonding Polarity of covalent bonds | ||||
Covalent structures | The octet rule Lewis structures Resonance structures VSEPR theory Molecular polarity Giant covalent structures Allotropes of carbon | ||||
Intermolecular forces | Types of intermolecular forces | ||||
Metallic bonding | Metallic structure and bonding Alloys | ||||
Chemical bonding & structure (AHL) | Further aspects of covalent bonding | Sigma and pi bonds Formal charge Delocalised pi electrons Lewis structure and resonance Expanded octets and molecular geometry Catalytic destruction of ozone | |||
Hybridisation | Hybridisation of atomic orbitals | ||||
Unit 5 & 15 | Energetics/thermochemistry | Measuring energy changes | Measurement of heat energy Exothermic and endothermic reactions Experimental measurement of heat changes | 15 Hours | Balanced |
Hess’s Law | Hess’s Law | ||||
Bond enthalpies | Making and breaking bonds Ozone formation and destruction | ||||
Energetics/thermochemistry (AHL) | Energy cycles | Lattice enthalpy Born-Haber cycles The solubility of salts | |||
Entropy and spontaneity | Entropy Entropy and spontaneity Spontaneous reactions | ||||
Unit 6 & 16 | Chemical kinetics | Collision theory and rates of reaction | Collision theory and activation energy The Maxwell-Boltzmann distribution Rates of reaction Measuring rates of reaction experimentally Factors that rates of reaction The role of a catalyst | 10 Hours | Inquirer |
Chemical kinetics (AHL) | Rate expression and reaction mechanism | Rate expressions Determining the order of reaction graphically Reaction mechanisms | |||
Activation energy | The Arrhenius equation Graphical determination of activation energy | ||||
Unit 7 & 17 | Equilibrium | Equilibrium | Dynamic equilibrium The equilibrium constant Kc The reaction quotient Q La Chatellier’s principle Industrial equilibria | 10 Hours | Thinker |
Equilibrium (AHL) | The equilibrium law | Calculations involving homogenous equilibrium Gibbs free energy and equilibrium | |||
Unit 8 & 18 | Acids and bases | Theories of acids and bases | Brønsted-Lowry theory of acids and bases Conjugate acid-base pairs | 20 Hours | Knowledgeable |
Properties of acids and bases | Characteristic reactions of acids Neutralisation reactions | ||||
The pH scale | Definition of pH Acid-base indicators The ionic product of water | ||||
Strong and weak acids and bases | Ionisation of acids and bases Strength of conjugate acids and bases | ||||
Acid deposition | Acid deposition Effects and reduction of acid deposition | ||||
Acids and bases (AHL) | Lewis theories of acids and bases | Lewis theories of acids and bases | |||
Calculations involving acids and bases | Temperature dependence of Kw Acid and base dissociation constants Calculations of pH for weak acids and bases | ||||
pH curves | pH curves Acid-base indicators Buffer solutions Salt hydrolysis | ||||
Internal assessment | 10 Hours | Inquirer |
THE LEARNING JOURNEY FOR CHEMISTRY | |||||
Unit | Subtopic | Key Episodes / Questions | Additional details | Length of time. | Learner Attribute(s) |
Unit 9 & 19 | Redox processes | Oxidation and reduction | Definitions of oxidation and reduction Oxidation states The activity series Redox reactions | 12 Hours | Principled |
Electrochemical cells | Voltaic cells Electrolytic cells | ||||
Redox processes (AHL) | Electrochemical cells | Standard electrode potentials Electrolysis of aqueous solutions Calculations involving electrolysis | |||
Unit 10 & 20 | Organic chemistry | Fundamentals of organic chemistry | Homologous series Molecular and structural formula Structural isomerism Functional groups Naming organic compounds Trends in physical properties Classification of organic compounds Aromatic hydrocarbons | 15 Hours | Open minded |
Functional group chemistry | Alkanes Alkenes Alcohols Halogenoalkanes Benzene | ||||
Organic chemistry (AHL) | Types of organic reactions | Nucleophilic substitution reactions Electrophilic addition reactions Electrophilic substitution reactions Reduction reactions | |||
Synthetic routes | Devising synthetic routes and retrosynthesis | ||||
Stereoisomerism | Conformal isomerism Cis-trans and E/Z isomerism Optical isomerism | ||||
Unit 11 and 21 | Measurement and data processing | Uncertainties and errors in measurement and results | Qualitative and quantitative data Random and systematic errors Precision and accuracy Absolute and percentage uncertainties | 10 Hours | Balanced |
Graphical techniques | Graphical techniques | ||||
Spectroscopic identification of organic compounds | Index of hydrogen deficiency (IHD) Infrared (IR) spectroscopy Mass spectrometry (MS) Nuclear magnetic resonance spectroscopy (1H NMR) | ||||
Measurement and analysis (AHL) | Spectroscopic identification of organic compounds | High resolution 1H NMR Combining analytical techniques X-ray crystallography | |||
Option: Medicinal chemistry | Medicinal chemistry | Pharmaceutical products and drug action | Drug development Drug action and administration The therapeutic index | 25 Hours | Caring |
Aspirin and penicillin | The synthesis of aspirin How aspirin works Synthesis of penicillin How penicillin works | ||||
Opiates | Types of opiates How opiates work Use of opiates | ||||
pH regulation of the stomach | Neutralisation of stomach acid Decreasing acid secretion | ||||
Antiviral medications | How antiviral medicines work Influenza HIV | ||||
Environmental impact of some medications | Sources of medical waste Nuclear medical waste Green chemistry solutions | ||||
Medicinal chemistry (AHL) | Taxol – a chiral auxiliary case study | Chirality Taxol | |||
Nuclear medicine | What is nuclear medicine? Radiotherapy Targeted alpha therapy | ||||
Drug detection and analysis | Extraction and purification Spectroscopic methods Alcohol and steroid detection |