This course covers the fundamental principles of chemistry. It begins with the scientific method, precision in measurement, significant figures, and the classification of matter. The material then moves to the core concepts of elements and compounds, and provides an introduction to the different types of chemical reactions. A command of these foundational topics is non-negotiable for any scientific study. The principles of measurement and precision are the basis of all experimental science. Understanding the nature of matter and the classification of reactions is the essential vocabulary required to describe the chemical world. This is the starting point for all subsequent study in chemistry. By the end of this course, you will be able to perform calculations with the correct number of significant figures, identify the different states of matter, and classify various types of chemical reactions. You will also be able to apply the scientific method to solve problems and understand the importance of precision in quantitative measurements. This course is for students beginning their study of chemistry at the university foundation level. It is a mandatory prerequisite for any student intending to pursue a degree in chemistry, chemical engineering, medicine, or any of the biological sciences.

This course provides a complete guide to the modern theory of the atom. It traces the historical development of atomic models, from Dalton's foundational theory to the modern understanding of electronic structure. The material covers the discovery of subatomic particles, the contributions of Thomson and Rutherford, the Bohr model, and culminates in a full treatment of electronic configuration and its direct relationship to the periodic trends of the elements. A command of atomic theory is the absolute foundation of modern chemistry. The electronic structure of the atom dictates all chemical properties and bonding behaviour. This knowledge is essential for understanding the periodic table, predicting chemical reactions, and is the prerequisite for the study of spectroscopy, materials science, and quantum mechanics. By the end of this course, you will be able to describe the historical evolution of atomic theory. You will also be able to explain the structure of the atom, including the roles of protons, neutrons, and electrons, determine the electronic configuration of any element, and use periodic trends to predict and justify atomic properties like size, ionization potential, and electronegativity. This course is for students who have completed an introductory chemistry course. It is a mandatory prerequisite for any student pursuing a degree in chemistry, chemical engineering, materials science, or physics.

This course covers the principles that govern how atoms connect to form molecules. It provides a full treatment of ionic and covalent bonding, valence forces, and the various types of intermolecular forces, including hydrogen bonding. The core of the course is a practical guide to predicting the three-dimensional shape of molecules using VSEPR theory and the concept of orbital hybridization. A command of chemical bonding and molecular geometry is essential for understanding the properties and reactivity of all chemical substances. The shape of a molecule dictates its function, from the specificity of drug-receptor interactions in medicine to the properties of polymers in materials science. This is the foundational knowledge for designing new molecules and materials. By the end of this course, you will be able to draw Lewis structures for any molecule, predict its three-dimensional geometry and bond angles using VSEPR theory, and determine its polarity. You will also be able to explain the formation of sigma and pi bonds using the concept of orbital hybridization and identify the types of intermolecular forces present in a substance. This course is for students who have a complete understanding of atomic theory and electronic configuration. It is a mandatory course for all students of chemistry, biochemistry, and materials science, and a direct prerequisite for the study of organic chemistry.

This course covers the physical principles that govern the states of matter. It focuses on the behaviour of gases, providing a full treatment of the gas laws and the kinetic theory of matter that explains them. The material also includes an introduction to the structure of crystalline solids. The principles of kinetic theory and the gas laws are fundamental to chemistry, physics, and engineering. They are essential for understanding atmospheric science, designing chemical reactors, and for the engineering of engines and power systems. A command of this topic is required to predict how substances will behave under different conditions of temperature and pressure. By the end of this course, you will be able to apply the ideal gas law and other gas laws to solve for unknown pressures, volumes, or temperatures. You will also be able to explain the behaviour of gases using the postulates of the kinetic theory of matter and describe the basic structure of crystalline solids. This course is for students who have a complete understanding of chemical bonding and molecular geometry. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of physical chemistry and thermodynamics.

This course covers the foundational principles of chemical measurement. It provides a complete treatment of the mole concept, molar mass, and the determination of empirical and molecular formulae from gravimetric (mass-based) experimental data. The material also covers the essential skill of calculating solution concentrations, including molarity. A command of the mole concept is the absolute, non-negotiable foundation for all quantitative chemistry. These are the accounting principles used in every laboratory and industrial process to measure chemical substances. This knowledge is essential for preparing solutions of a known concentration and for determining the identity of an unknown compound. By the end of this course, you will be able to perform all calculations involving the mole, molar mass, and Avogadro's number. You will also be able to determine the empirical and molecular formula of any compound from its percentage composition or combustion data, and calculate the concentration of solutions in moles per dm³. This course is for students who have completed a course on atomic theory. It is the mandatory starting point for the study of stoichiometry and is a prerequisite for any further study in chemistry, chemical engineering, or the biomedical sciences.

This course focuses on the language of chemical transformations: the chemical equation. It covers the methods for writing and balancing a wide range of chemical equations, including simple, ionic, and complex oxidation-reduction (redox) reactions. The material provides a systematic guide to the rules of electron transfer and oxidation numbers. Correctly balanced chemical equations are the bedrock of all quantitative chemistry. They are essential for predicting reaction outcomes in industrial manufacturing, ensuring safety in laboratory procedures, and for all forms of chemical analysis. A command of redox reactions is specifically required for understanding electrochemistry, corrosion, and biological energy processes. By the end of this course, you will be able to write and balance any standard chemical equation. You will also be able to determine oxidation numbers, identify oxidizing and reducing agents, and use the electron transfer method to balance complex redox reactions. This course is for students who have mastered the mole concept and chemical formulae. It is a mandatory course for all students of chemistry, chemical engineering, and biochemistry, providing the essential procedural skills needed for both theoretical and practical work.

This course covers volumetric analysis, a major practical application of stoichiometry. The material focuses entirely on the theory and calculations behind titration. It covers the preparation of standard solutions and the detailed procedures for performing and calculating the results of neutralisation, precipitation, and complexometric titrations. Volumetric analysis is a fundamental quantitative technique in every analytical chemistry laboratory. It is the standard method used in industrial quality control, environmental testing, and medical diagnostics to determine the precise concentration of an unknown substance. A command of titration is a non-negotiable practical skill for any professional chemist. By the end of this course, you will be able to prepare a standard solution of a known concentration. You will also be able to perform all necessary calculations for any acid-base, precipitation, or complexometric titration to accurately determine the concentration of an unknown solution. This course is for students who have a complete mastery of the mole concept and balancing chemical equations. It is an essential course for any student of chemistry or chemical engineering and provides the foundational skills required for all quantitative laboratory work.

This course provides a complete guide to chemical equilibria, the state where the rates of forward and reverse reactions are equal. It covers the law of mass action, the definition and calculation of the equilibrium constant, and the factors that can cause a shift in the equilibrium position. The course then applies these principles to the study of aqueous equilibria, including the properties of acids, bases, and salts, and the calculation of pH. The principles of equilibrium govern the outcomes of all reversible reactions, from industrial synthesis to biological processes. A command of this topic is essential for chemists and chemical engineers to maximise the yield of a desired product, for environmental scientists to understand natural water systems, and for biochemists to analyse metabolic pathways. By the end of this course, you will be able to write the expression for the equilibrium constant for any reversible reaction, use Le Chatelier's principle to predict how a system at equilibrium will respond to changes in concentration, pressure, or temperature, and perform calculations involving the pH of acidic and basic solutions. This course is for students who have a solid foundation in stoichiometry. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of analytical chemistry, biochemistry, and environmental science.

This course provides a complete guide to chemical thermodynamics, the study of the energy changes and spontaneity of chemical reactions. It covers the fundamental concepts of enthalpy (heat of reaction), entropy (disorder), and Gibbs free energy. The material details the principles of calorimetry, Hess's law for calculating enthalpy changes, and the use of standard heats of formation. Chemical thermodynamics is essential for predicting the feasibility and energy efficiency of any chemical process. These principles are critical in chemical engineering for designing industrial reactors, in materials science for developing new energy sources and batteries, and in biochemistry for understanding the energy flow that drives metabolic pathways. By the end of this course, you will be able to differentiate between exothermic and endothermic reactions and calculate enthalpy changes using Hess's law and standard heats of formation. You will also be able to use the concepts of entropy and Gibbs free energy to predict whether a chemical reaction will be spontaneous under a given set of conditions. This course is for students who have a solid foundation in chemical equilibria. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of physical chemistry, materials science, and advanced thermodynamics.

This course provides a complete guide to chemical kinetics, the study of the rates and mechanisms of chemical reactions. It covers the formal definition of reaction rate, the concept of reaction order, and the determination of rate laws from experimental data. The material also introduces the collision theory, the role of activation energy, and the Arrhenius equation. Chemical kinetics is essential for controlling chemical reactions in industrial manufacturing, pharmaceutical development, and environmental science. The principles are used to optimise production yields by speeding up desired reactions, to develop catalysts that lower energy consumption, and to understand the complex reaction pathways in atmospheric and biological systems. By the end of this course, you will be able to define the rate of a reaction and determine the rate law and rate constant from experimental data. You will also be able to use the concept of activation energy to explain the effect of temperature on reaction rate and understand the basic principles of reaction mechanisms. This course is for students who have a solid foundation in stoichiometry and chemical equilibria. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of physical chemistry, industrial chemistry, and biochemistry.

This course provides a complete guide to electrochemistry, the study of the relationship between chemical reactions and electrical energy. It covers the principles of oxidation-reduction (redox) reactions and their application in electrochemical cells. The material details the structure and function of both galvanic (voltaic) cells, which produce electricity, and electrolytic cells, which use electricity to drive non-spontaneous reactions. Electrochemistry is the science behind all modern portable energy storage and industrial metal production. The principles covered are the basis for batteries, fuel cells, and rechargeable power sources. This knowledge is also critical for understanding corrosion, electroplating, and the industrial-scale electrolysis used to produce fundamental materials like aluminium and chlorine. By the end of this course, you will be able to identify the components of any electrochemical cell and predict the direction of electron flow. You will also be able to calculate standard cell potentials using a table of standard reduction potentials, apply Faraday's laws to electrolytic calculations, and use the Nernst equation to determine cell potential under non-standard conditions. This course is for students who have a solid foundation in stoichiometry and redox reactions. It is a mandatory course for all students of chemistry and chemical engineering and is a direct prerequisite for the study of analytical chemistry, materials science, and electrical engineering.

This course provides a complete introduction to radioactivity and nuclear chemistry. It covers the principles of radioactive disintegration, the different types of decay, and the concept of half-life. The material also introduces the powerful processes of nuclear fission and fusion, and explores the practical uses of radioisotopes. An understanding of radioactivity is essential in the modern world. These principles are the foundation of nuclear power generation, medical imaging techniques like PET scans, and carbon dating in archaeology and geology. This knowledge is critical for applications in medicine, energy production, and environmental science. By the end of this course, you will be able to describe the process of radioactive disintegration and identify the different types of nuclear radiation. You will also be able to explain the concepts of nuclear fission and fusion and describe the key applications of radioisotopes in medicine and industry. This course is for students who have a solid foundation in atomic theory. It is a mandatory course for any student of nuclear engineering or health physics and provides essential knowledge for students of chemistry, physics, and medicine.