Examination arrangement

Course content

Introduction to basic concepts, chemical formulas and nomenclature. Atomic structure, basic orbital theory, quantum numbers and electron configuration. Periodicity, electronegativity and chemical bonding. Mol, concentrations (molar, mass percentage) and dilution. Chemical reactions, equations and stoichiometry. Gases and gas laws with the main emphasis on ideal gases. Chemical equilibrium, Le Chatelier's principle. Acids, bases, pH, buffer solutions, titration. Solubility, solubility product constant, precipitation reactions and complex ion equilibria. Basic thermochemistry. Oxidation and reduction reactions (oxidation numbers, balancing, electrochemical series).

Learning outcome

The student can explain basic atomic theory, orbital theory and the periodic system, and use this to specify elemental electron configurations for elements and ions. The student can describe relationships between electron structure, chemical properties and bonds for elements and chemical compounds. The student can apply nomenclature rules to name inorganic compounds. The student can explain basic chemical bonding theories, as well as use electronegativity to determine the type of bonding. The student can set up Lewis structures and use formal change. The student can demonstrate knowledge of some important main types of chemical reactions and draw up reaction equations based on this. The student can balance reaction equations and perform calculations on the basis of such equations (stoichiometry). The student can calculate mass, amount of substance and concentration. The student can apply the gas laws, perform calculations for chemical equilibria, and apply Le Chatelier's principle. The student can perform calculations of heat, internal energy and enthalpy and relate this to calorimetric experiments. The student can calculate change in enthalpy, entropy and Gibbs free energy for chemical reactions, and relate this to chemical equilibrium and spontaneity. The student can calculate pH, solubility and buffer capacity. The student can set up and balance oxidation and reduction reactions. The student can conduct simple chemical tests and document results in simple reports using standard methods. The candidate can handle chemicals properly and use safety data sheets.

Learning methods and activities

Lectures, theory exercises and laboratory work. Lectures: 80 hours Laboratory exercises: 40 hours Exercises: 40 hours Own effort: 130 hours

Further information about learning activities will be provided at the beginning of the semester.

Compulsory assignments

• Mandatory laboratory work
• Compulsory exercises

Further on evaluation

Required for the final examination: Approved exercises and laboratory course. 8 out of 12 theory excercises must be passed. 8 laboratory exercises with submission of 8 reports must be passed. Deferred examination: May / June. In case of postponed examination (continuation examination), written examination may be changed to oral examination. Permitted aids on the exam: Gordon Aylward and Tristan Findlay: SI Chemical Data, Wiley. Only simple calculators may be used during the examination. For applications for credentialing, approval and integration of courses from previous years or other institutions' equivalent education, each application will be dealt with individually and the applicant must be able to count credits for overlapping courses.

Specific conditions

Recommended previous knowledge

No

Required previous knowledge

Admission to the course requires admission at the Bachelor program in Chemical engineering of Engineering, NTNU, Trondheim or Bachelor program in Materials engineering, NTNU, Trondheim.

Course materials

Gordon Aylward and Tristan Findlay: SI Chemical Data, Wiley, 7th Edition, 2014. Nivaldo J. Tro: Chemistry. A Molecular Apporach, 5th edition, Pearson Prentice Hall, 2020. Reservations are made for some adjustments in literature. Any adjustments will be published on Blackboard before the start of the semester.

Credit reductions