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Chemistry I
Chemie I
Last Updated: 2026-02-05 16:16:23
Abstract
General Chemistry I: Chemical bond and molecular structure, chemical thermodynamics, chemical equilibrium.In the course "Chemistry I", the competencies of process understanding, system understanding, modeling, concept development and data analysis & interpretation are taught, applied and examined.
Objective
Introduction to general and inorganic chemistry. Basics of the composition and the change of the material world. Introduction to the thermodynamically controlled physico-chemical processes. Macroscopic phenomena and their explanation through atomic and molecular properties. Using the theories to solve qualitatively and quantitatively chemical and ecologically relevant problems.
Content
1. Stoichiometry Amount of substance and mass. Composition of chemical compounds. Reaction equation. Ideal gas law. 2. Atoms Elementary particles and atoms. Electron configuration of the elements. Periodic system. 3. Chemical bonding and its representation. Spatial arrangement of atoms in molecules. Molecular orbitals. 4. Basics of chemical thermodynamics System and surroundings. Description of state and change of state of chemical systems. 5. First law of thermodynamics Internal energy. Heat and Work. Enthalpy and reaction enthalpy. 6. Second law of thermodynamics Entropy. Change of entropy in chemical systems and universe. Reaction entropy. 7. Gibbs energy and chemical potential. Combination of laws of thermodynamics. Gibbs energy and chemical reactions. Activities of gases, condensed substances and species in solution. Equilibrium constant. 8. Chemical equilibrium Law of mass action. Reaction quotient and equilibrium constant. Phase transition equilibrium. 9. Acids and bases Properties of acids and bases. Dissociation of acids and bases. pH and the calculation of pH-values in acid-base systems. Acid-base diagrams. Buffers. Polyprotic acids and bases. 10. Dissolution and precipitation. Heterogeneous equilibrium. Dissolution and solubility product. Carbon dioxide-carbonic acid-carbonate equilibrium.
Resources
Lecture Notes
Online-Skript mit durchgerechneten Beispielen.
Literature
Charles E. Mortimer, CHEMIE - DAS BASISWISSEN DER CHEMIE. 12. Auflage, Georg Thieme Verlag Stuttgart, 2015. Weiterführende Literatur: Theodore L. Brown, H. Eugene LeMay, Bruce E. Bursten, CHEMIE. 10. Auflage, Pearson Studium, 2011. (deutsch) Catherine Housecroft, Edwin Constable, CHEMISTRY: AN INTRODUCTION TO ORGANIC, INORGANIC AND PHYSICAL CHEMISTRY, 3. Auflage, Prentice Hall, 2005.(englisch)
General Information
- Language
- German
- Levels
- BSC
- Frequency
- Yearly recurring
Examination
- Type
- session examination
- Mode
- written 90 minutes
- Aids
- Zusammenfassung: 3 A4-Seiten, einseitig, handgeschrieben (jegliche Art von Ausdrucken (z.B. von einem eingescannten Dokument oder von einem auf einem Tablet erstellten File) und jegliche Art von Fotokopien werden nicht akzeptiert), Periodensystem, einfacher Taschenrechner (die Liste mit den erlaubten Modellen wird in der Vorlesung verteilt), Periodensystem (Version PSE für Chemie I und II)
Course Components
| Type | Title | Time & Place | Hours |
|---|---|---|---|
| lecture |
Chemie I
Vorlesung im HG F1 mit Videoübertragung ins HG F3.
|
|
2 h weekly |
| exercise |
Chemie I
Übungen:
Mi 14-16 für Umweltingenieurwissenschaften
Do 10-12 für Agrar-, Lebensmittel-, Erdwissenschaften
Fr 8-10 für Umweltnaturwissenschaften
|
|
2 h weekly |