Course content

This course introduces the fundamental concepts, models, and calculations that form the foundation of the field of chemistry. You will develop an understanding of how substances are structured, how they react with each other, and what properties they have. You will also learn about the principles of green chemistry for the responsible use of resources and minimal environmental impact.

Knowledge of basic chemistry is important for understanding many phenomena in nature and society and forms the basis for further studies in science, medicine, technology, and engineering.

The course covers the following areas of chemistry:

• Atoms, molecules and structure: atoms and molecules; elements, atomic and electronic structure; the periodic table; chemical bonding; molecular structure and properties of molecules.
• The language of chemistry: nomenclature; chemical formulas; reaction equations and stoichiometry.
• States and properties of matter: intra- and intermolecular forces; properties of gases, liquids, solutions and solids; gas laws; solubility and concentration.
• Chemical reactions and changes: chemical equilibrium; acids, bases and buffer properties; redox reactions; electrochemistry; thermodynamics; spontaneity and kinetics.

In addition, you will gain practical laboratory experience with basic chemical techniques and analyses and learn to conduct experiments safely and responsibly.

Learning outcome

Knowledge

After completing the course, the student can:

• Identify different chemical reactions and name common chemical compounds.
• Describe atomic, molecular, and electronic structure and how this forms the basis for the periodic table.
• Describe different types of inter- and intramolecular chemical bonds and how these affect the properties of substances such as boiling point, melting point, and solubility.
• Describe chemical equilibrium and how it is affected by changes, e.g., in concentration, pressure, and temperature.
• Describe how a dissolved substance changes the vapor pressure, freezing point, boiling point, and osmotic pressure of the solvent.
• Define reaction rate and describe factors (including catalysis) that affect reaction rate.
• State the laws of thermodynamics and describe how these are used to study energy changes in chemical reactions and physical processes.
• Describe the principles of galvanic cells/batteries and electrolysis.

Skills

After completing the course, the student can:

• Perform stoichiometric calculations and balance different chemical equations, including redox reactions.
• Perform calculations for equilibria in gas mixtures and in aqueous solutions, especially for calculating pH and solubility.
• Predict molecular geometry using the VSEPR method and recognize polar and nonpolar compounds.
• Derive the rate law from experimental data.
• Calculate entropy, enthalpy, and Gibbs energy changes for reactions and relate this to equilibrium and spontaneity.
• Draw cell diagrams, calculate voltage for galvanic cells using standard reduction potentials and the Nernst equation, and relate this to equilibrium and spontaneity.
• Plan and conduct simple chemical experiments in a safe and responsible manner, including the use of basic laboratory techniques such as weighing, measuring volume, filtration, and titration.

General knowledge

After completing the course, the student can:

• Explain results from simple chemistry experiments using chemical concepts and principles.
• Follow applicable HSE routines for safety in the laboratory, including using protective equipment, handling chemicals, and waste management.
• Give examples of sustainability challenges in chemistry and possible solutions considering the principles of green chemistry.

Learning methods and activities

Lectures, exercises, laboratory exercises, and self-study. The course workload is estimated at 210 hours per semester, including 60 hours of lectures, 40 hours for exercises, 60 hours for laboratory work, and 50 hours for self-study.

The course has compulsory assignments consisting of both theoretical exercises and laboratory work. A compulsory HSE module (HMS0001) and a course-specific digital HSE lecture must be completed before admission to the laboratory.

Specific requirements for the approval of compulsory activities will be announced at the start of the course.

Compulsory assignments

• Approved laboratory course
• Approved exercises

Specific conditions

Recommended previous knowledge

Chemistry and mathematics from high school/upper secondary school. Students without Chemistry 1 or 2 should consider taking a preparatory chemistry course.

Course materials

• Raymond Chang, Kenneth E. Goldsby, General Chemistry: The Essential Concepts, 7th edn, McGrawHill.

Course materials for completing the compulsory activities will be announced at the start of the course.

Credit reductions