On successful completion of this module students should be able to:
1. Describe the current understanding of atomic theory and relate this to the formation and reaction of molecular systems.
2. Write balanced chemical equations and do stoichiometric calculations.
3. Understand the fundamental forces governing the state of a material and the properties of solutions.
4. Use the thermochemical laws to predicting the directions of physical/chemical changes and molar concentrations of species involved.
5. Use the laws of reactions and equilibria and the Arrhenius law in practical calculations for chemical reactions, to determine pH and pKa in buffers and during titration.

Introduction to General Chemistry: 1) Nature of elements and the Periodic Table; 2) Nature of atomic composition, atomic structure, electron configuration, energy of atoms, and valence electrons; 3) Nature of chemical compounds and Lewis dot symbols; 4) Nature of ionic bonding; 5) Nature of covalent bonding including coordinate bonding and molecular orbitals; 6)Nature of multiple covalent bonds; 7) Nature of polyatomic compounds; 8) Nature of polarized bonds; 9) Nature of molecular interactions; 10) Nature of van der Waals interactions; 11) Nature of hydrogen bond; 12) Nature of ionic forces; 13) Nature of hydrophobic forces;
14) Nature of molecular interactions and water solubility; 15) Nature of physical phases; 16) Apply the concept of moles to calculate concentrations and dilution ratios; 17) Understand how concentrations can be measured for different chemical solution; 18) Nature of the movement of electrons during chemical reactions; 19) Nature of heterolytic and homolytic reactions; 20) Nature of oxidation and reduction; 21) Nature of acids and bases, the strength of acids/bases, and apply dissociation constants; 22) Nature of ion products of water, the pH scale, and buffering solutions; and 23) Nature of acids and bases in biology

Introduction to Physical Chemistry: 1) Sources of energy and nature of energy transfer; 2) Nature of work and heat; 3) Nature of enthalpy and entropy; 4) Nature of spontaneous processes and relationship to Gibbs free energy; 5) Nature of equilibrium reactions and the equilibrium constant; 6) Nature of binding reactions; 7) Nature of the relationship between equilibria and Gibbs free energy; 8) Nature of rates of reaction and relationship to collision theory; 9) Nature of activation energy and Catalysis; and 10) Nature of enzymes, enzyme kinetics, and enzyme inhibition;

General university matriculation requirements.

Students that have completed CHEM 00010, CHEM 00020, CHEM 20100 or CHEM 20080 are not permitted to register for this module.

• Feedback individually to students, on an activity or draft prior to summative assessment
• Group/class feedback, post-assessment

1) Exam grades will be posted on Brightspace and you will be provided with a key to identify problems that you did not get correct. Please follow-up with your tutor or professor should you need explanations for the answers or deeper understanding. 2) Exercises will be assigned and answers will be available on Brightspace. Please follow-up with your tutor or professor should you need explanations for the answers or deeper understanding. 3) Laboratories will we managed by staff members and graduate students. They are there to help you do the experiments but also understand the concepts and complete any calculations that are required.