Course content

Stoichiometry, gass law, chemical equilibria, aqueous ionic equilibria. Acid-base and redox equilibria. Basic chemical thermodynamics, energy, entropy, enthalpy, Gibbs energy. Calculations of equilibria from thermodynamical data. Electrochemistry: Reduction potential series, cell voltage, electrolysis and galvanic cells. Short introduction to batteries, fuel cells and corrosion of metals. Chemical bond. Basic organic chemistry and polymer chemistry. Important inorganic compounds and environmental issues related to them. Laboratory exercises give furthe insight into the following topics: Chemical principles: Stoichiometry, chemical equilibria, acids and bases, reduction and oxidation. Quantitative methods: Titration, instrumental methods: pH-electrode, redox-electrode, spectrophotometer. A compulsory safety course, including fire prevention and first aid has to be passed in order for admission to the laboratory course.

Learning outcome

The most important learning outcomes in this course is associated with quantitative treatment of aqueous equilibria and the relation between Gibbs free energy and equilibrium constants and electrode potentials. After successfully completing this course the student masters the theoretical and experimental foundation necessary for further courses in inorganic, organic and physical chemistry. The student can upon successful course completion: - Identify various chemical reactions and perform stoichiometric calculations - Carry out equilibrium calculations in gas mixtures and aqueous solutions, including calculation of pH and solubility. - Carry out simple thermodynamic calculations founded on knowledge on entropy, enthalpy and Gibbs free energy and be able to relate these to chemical equilibrium - Account for the relation between equilibrium constant, Gibbs' free energy, and electrode potential, and for a simplified derivation of these relations. - Principles for galvanic cells (batteries, fuel cells) and electrolysis and recognize industrial electrolysis processes. - Calculate cell potentials in electrochemical cells from Gibbs' free energy, from standard electrode potential and from the Nernst equation, including concentration cells. - Explain corrosion and corrosion protection. - Describe the various types of chemical bonds and why these come into being. - Explain the basic principles of organic and polymer chemistry, including rules for naming organic compounds. - Account for shape and name of the orbitals of the atom and assess the electron configuration of an element from its position in the periodic table. In the laboratory the students are supposed to obtain a deeper understanding of the principles through the experiments, and be trained in working accurately.

Learning methods and activities

Lectures, exercises and laboratory work. 2/3 of the written exercises have to be passed in order to take the final exam. All laboratory exercises must be performed satisfactorily. Up to two midterm exam(s) will be given where one must be passed in order to take the final exam. The exam may include topics that have been treated in the laboratory course. The assessment in the course is based on a final written exam.

Compulsory assignments

• Laboratory couse
• Midtermtests
• Exercises

Recommended previous knowledge

Knowledge of the more important elements and chemical compounds is expected. Also the understanding of chemical formulas and equations, the concepts of atoms, molecules, and moles. Calculations with logarithms and exponents should be mastered.

Course materials

R. H. Petrucci, G. G. Herring, J. D. Madura and C. Bissonnette, "General Chemistry. Principles and Modern Applications", 10. ed., Pearson, Toronto (2011). A. Blackman and L. R. Gahan, Aylward & Findlay's SI Chemical Data, 7. utg., Wiley, 2014. "TMT4110/TMT4115 Laboratoriekurs i generell kjemi" compendium will be made available to the students in the lab. Printed material and alternative text books are announced at the start of the course.

Credit reductions