Syllabus for The Basic Principles of Chemistry
Kemins grunder och principer
- 15 credits
- Course code: 1KB013
- Education cycle: First cycle
Main field(s) of study and in-depth level:
Explanation of codes
The code indicates the education cycle and in-depth level of the course in relation to other courses within the same main field of study according to the requirements for general degrees:
- G1N: has only upper-secondary level entry requirements
- G1F: has less than 60 credits in first-cycle course/s as entry requirements
- G1E: contains specially designed degree project for Higher Education Diploma
- G2F: has at least 60 credits in first-cycle course/s as entry requirements
- G2E: has at least 60 credits in first-cycle course/s as entry requirements, contains degree project for Bachelor of Arts/Bachelor of Science
- GXX: in-depth level of the course cannot be classified
- A1N: has only first-cycle course/s as entry requirements
- A1F: has second-cycle course/s as entry requirements
- A1E: contains degree project for Master of Arts/Master of Science (60 credits)
- A2E: contains degree project for Master of Arts/Master of Science (120 credits)
- AXX: in-depth level of the course cannot be classified
- Grading system: Fail (U), Pass (3), Pass with credit (4), Pass with distinction (5)
- Established: 2014-03-13
- Established by:
- Revised: 2023-02-08
- Revised by: The Faculty Board of Science and Technology
- Applies from: Autumn 2023
- Entry requirements: General entry requirements and Biology 2, Physics 1a or 1b1+1b2, Chemistry 2, Mathematics 4/Mathematics D
- Responsible department: Department of Chemistry - BMC
On completion of the course, the student should be able to:
- account for electronic structure in atoms and the quantum mechanical background to the periodic table, and relate these to the properties of elements
- account for chemical binding and interactions between particles (atoms, molecules, ions) in chemical systems, and relate these to the physical and chemical properties of matter.
- explain basic concepts of thermodynamics, kinetics and equilibria, and discuss links, similarities and differences between these fields.
- describe different types of transport processes in solution
- solve problems and perform basic calculations related to chemical and physical issues
- based on relevant theory and a scientific approach carry out basic laboratory work in a correct and safe manner, carry out risk and safety analyses, document laboratory work in a laboratory journal and report on the execution and results of the laboratory work.
- give examples of the implications of the course content for humans and the environment
Structure of atoms and molecules: Atomes, atomic orbitals and the periodical system. Lewis structures and molecular geometries. Molecular orbitals.
Inter- and intramolecular forces: Covalent bonding, ionic bonding, metallic bonding, coordinative bonding, as well as bonds between molecules and between ions and molecules. Surfactants. Phases and phase transformation. Interactions in gases, liquids and solids as well as in solutions and mixtures.
Physical forces: Surface tension, conductivity, diffusion, viscosity and sedimentation.
Thermodynamics: Energy conversion and energy transfer, especially for chemical reactions. Chemical driving forces. Enthalpy, entropy and free energy. Thermodynamic aspects of phase change, gases, liquids and solids as well as solutions and mixtures.
Kinetics: Reaction mechanisms. Dependence of the reaction rate on temperature, concentrations and catalysts.
Equilibria: Direction of reaction and position of equilibrium. Acids and bases. Solubility.
Laboratory methodology and basic risk assessment
Lectures, exercises, laboratory sessions, seminars and project.
Written examinations are organised during and at the end of the course and correspond to 5 and 4 credits respectively. The laboratory sessions with associated seminars and hand-in excercises correspond to 5 credits. The project with associated seminars and hand-in exercises corresponds to 1 credit. The final grade is a weighted average of the results of the different parts of the course.
If there are special reasons for doing so, an examiner may make an exception from the method of assessment indicated and allow a student to be assessed by another method. An example of special reasons might be a certificate regarding special pedagogical support from the disability coordinator of the university.
The course can not be included in higher education qualification together with 1KB001 Chemical Principles II and 1KB007 Basic Chemistry / 1KB000 Chemical Principles I.
Applies from: Autumn 2023
Some titles may be available electronically through the University library.
Aylward and Findlay's SI chemical data
Gahan, Lawrence R.
Aylward, Gordon Hillis;
Findlay, Tristan John Victor
7.ed.: Milton, Qld.: John Wiley & Sons, 2014
Silberberg, Martin S.;
Chemistry : the molecular nature of matter and change
9e.: New York, NY: McGraw-Hill Education,