Inorganic Chemistry

The course covers electronic structure of atoms; The Pauli principle, Hunds rule, Aufbau, quantum numbers, hypervalence. Covalent bonding, Lewis-theory, Valence shell electron repulsion theory (VSEPR), Valence band/hybridisation. MO-theory for diatomic molecules. Bond triangle, polar covalant bonds and dispersion forces. Ionic compounds, lattice entalphy. Metallic bonding, band-theory. Explanation of periodic trends of physical and chemical properties. Transition metal complexes, crystal field theory. Introduction to catalytic processes and properties of Group 14 network structures. The laboratory course gives practical knowledge concerning simple catalytic processes and propertis of zeolites, complex reactions and red-ox reactions for elements in the d-block also including introduction to UV-vis spectroscopy.

After finishing the course, the student is expected to:

• Know the rules governing electron structure build-up including the electron quantum numbers
• Apply the bond theories Lewis, VSEPR, VB and MO to covalent compounds in the p-block
• Utilise VSEPR in stereochemistry of p-block compounds
• Sketch MO-diagrams for diatomic molecules
• Explain the difference between ionic, covalent and metallic bonding
• Calculate lattice entalphy for ionic compounds using the Born-Haber cycle
• Explain chemical and physical properties and periodic trends based on bonding, structure and electron configuration
• Explain properties of transition metal complexes from crystal field theory
• Be able to set up balanced equations for precipitation-, complex exchange- and red-ox reactions

Lectures (4 hours per week), exercises (2 hours per week) and laboratory work (ca. 7 hours per week). Attendance on 8 out of 10 exercises is required. 75 hours of laboratory work. Written examinaton 5 Hours (100%). For extraordinary examinations, written examination may be changed to oral examination.