Examination arrangement

Course content

Basic chemical terminology: amount of substance, concentration and stoichiometry. Rules for naming chemical compounds. Fundamental results from quantum mechanics: atomic orbitals and the principle behind the construction of the periodic table. Properties of gases: units of pressure, vapour pressure of liquids, the ideal gas law, Dalton's law. Chemical equilibrium: the law of mass action, acid-base equilibria, buffer solutions, titration, solubility and precipitation, complex formation. Basic thermochemistry and chemical thermodynamics: work, heat, internal energy, enthalpy, entropy and Gibbs energy.

The course introduces general aspects of the field of chemistry, and creates a foundation for further specialization within organic, inorganic and biological chemistry, as well as electrochemistry, thermodynamics and materials science. The laboratory part provides an introduction to basic chemical laboratory techniques and precision work, as well as a practical demonstration of selected parts of the subject matter.

Learning outcome

After completing the course, the candidate will be able to:

1. Write balanced chemical reactions and perform stoichiometric calculations for acid-base reactions, redox reactions, and solubility reactions
2. Explain what chemical equilibrium is, and use the law of mass action to calculate equilibrium constants and composition at equilibrium for various types of chemical reactions, including calculations of solubility and solubility products, and pH calculations for buffer solutions
3. Calculate change in enthalpy, entropy and Gibbs energy for a chemical reaction, and connect this with chemical equilibrium and spontaneity
4. Conduct simple chemical experiments, explain the theoretical foundation of the experimental methods through calculations, and document and report experimental results through written reports
5. Use the gas laws and tabulated values of vapour pressure to perform calculations related to the properties of gases, both theoretically and in connection with experimental work
6. Read and understand safety data sheets and handle chemicals accordingly
7. Explain electronic configurations for atoms and ions, and how atomic orbitals form the basis for the construction of the periodic table
8. Explain the main differences between the covalent, ionic and metallic models for chemical bonding, and use the difference in electronegativity between atoms to describe the character of the chemical bond that is formed
9. Use rules for chemical nomenclature to name inorganic compounds

Learning methods and activities

Lectures, problem sets, laboratory assignments and self-study. An estimate of the time required for the course during a semester is 60 hours for lectures, 40 hours for problem sets, 40 hours for laboratory assignments (including preparation and report writing), and 70 hours self-study (sum: 210 hours).

Compulsory assignments

• Laboratory assignments
• Problem sets

Further on evaluation

Both laboratory assignments and problem sets need to be approved in order to access the final exam. Participation and an approved written report is required for all laboratory assignments. Specific requirements for approval of problem sets will be given at the start of the semester.

In the case of a re-sit exam or a re-take of the ordinary exam in an attempt to improve the final grade, it is not required to complete the laboratory assignments and/or problems sets again if these have been approved in a previous semester.

Re-sit exams are held in the end of the spring semester (May or June). For the re-sit exam, the examination form may be changed from written to oral.

Specific conditions

Recommended previous knowledge

The first part of the course corresponds to basic chemistry on the level of Kjemi 1 in Norwegian upper secondary education, and the remainder of the course builds on this fundament. The pre-course in chemistry offered by NTNU is strongly recommended for candidates without this or an equivalent background in chemistry.

Course materials

Nivaldo J. Tro, Chemistry: A Molecular Approach, Fifth Edition, Pearson, 2021. (Lectures are based on this book, but other university-level general chemistry textbooks may be used at your own discretion.)

Allan G. Blackman and Lawrence R. Gahan, Aylward and Findlay’s SI Chemical Data, 7th Edition, Wiley, 2014. (Indispensable both for problem sets and laboratory assignments, and is also a permitted aid during the final exam.)

Credit reductions