Basics of Chemistry

None

• Basic concepts; elements/compounds; atomic models; periodic table of the elements; electron configuration of the elements; electronegativity.
• Types of bonds: covalent, ionic, metallic. Intermolecular interactions; relationships between structure and properties. Water as molecule and dipole.
• States of aggregation; phase transformations; allotropy; ozone; ozone hole.
• Chemical formulae; Establishing reaction equations; Stoichiometry; Types of reactions; Oxidation numbers; Redox reactions; Photosynthesis.
• Concentration data; Reaction rate; The chemical equilibrium; Mass action law; The principle of Le Chatelier; Haber-Bosch method.
• Solubility products; Lime; Calcite; Gypsum.
• Dissociation of water; pH value; acid-base theories; strong and weak acids and bases: Titration; Buffer.
• Fundamentals of chemical thermodynamics: enthalpy. Entropy. Gibbs energy.
• Electrochemistry: Electrolysis; Galvanic cell; Electrochemical power generation: Battery, accumulator, fuel cell.

The students can:

• Name, understand and apply basic technical terms in chemistry.
• Identify relationships between molecular structure and properties of compounds.
• Establish chemical reaction equations, identify and explain possible problems in the reactivity of substances.
• Understand and apply the law of mass action.
• Independently analyse and solve fundamental problems in the fields of stoichiometry, pH calculations, solubility of substances and electrochemistry.
• Understand and apply the basic concepts of chemical thermodynamics. draw conclusions about the course of the reaction and confirm them with calculations.
• Describe the concept of redox reactions.
• Distinguish between the structure and functioning of electrochemical cells.
• Recognise and apply the above concepts, effects and phenomena in subsequent courses.
• Recognise and analyse basic chemical concepts in environmental engineering issues, and interpret the relationships between effects and phenomena.

Lecture and separate exrcise (2+1 SWH)

• Evaluation of performance in the exercises and home exercises (30 %)
• Final written examination (70 %)

For a positive grade, a minimum of 50% of the possible points must be achieved in each part of the examination.

None

• Blumenthal, Gert; Linke, Dietmar; Vieth, Siegfried (2006): Chemistry: Basic knowledge for engineers. 1st ed. Wiesbaden: Teubner (= chemistry in practice).
• Brown, Theodore L. et al. (2014): Basiswissen Chemie: Fundamentals of general, inorganic and organic chemistry. Hallbergmoos: Pearson (= Always learning).
• Bruice, Paula Yurkanis; Lazar, Thomas; Reiser, Oliver (2011): Organic Chemistry: Study compact. 2nd, German verb. and abbreviated editions]. = [5th, updated English edition Munich: Pearson Studies (= Pearson Studies - Chemistry).
• "Springer handbook of metrology and testing (2011): Springer handbook of metrology and testing. Second edition. Heidelberg: Springer.
•  Mortimer, Charles E.; Müller, Ulrich (2015) Chemistry: The basic knowledge of chemistry. 12th edition. Thieme.

• Presence event
• Lecture without compulsory attendance
• Exercises with compulsory attendance