Fundamentals of Chemistry, 15 Credits

Contents

The course is divided into four modules: 

Module 1: Atoms, Molecules, and Matter (ATMO, 4.5 hp) 

This module covers the fundamental concepts of atomic structure, chemical bonding, and the states of matter.  

Atomic Structure: Explores the quantum mechanical model of the atom and how it explains periodicity. 

Chemical Bonding: Utilizes Pauling electronegativity, Lewis structures, valence shell electron pair repulsion (VSEPR) theory, valence bond theory, and molecular orbital theory to analyse chemical bonding. 

States of Matter: Examines gases, liquids, and solids through various theories and models, including gas laws, intermolecular bonding, and unit cells. 

Module 2: Thermodynamics and Equilibria (TEEQ, 4.5 hp) 

This module focuses on the principles of thermodynamics, and physical and chemical equilibrium. 

Thermodynamics: Introduces the concepts of work, heat, internal energy, enthalpy, entropy, and Gibbs free energy. Discusses spontaneous and non-spontaneous processes, exothermic and endothermic processes, system boundaries, and process reversibility. Explores the application of thermodynamic principles to predict the feasibility and direction of chemical processes, including how energy changes influence reaction pathways and the efficiency of reactions. 

Physical Equilibrium: Examines the concepts affecting phase changes in matter. Introduces solubility, molality, and colligative properties to understand the roles of solutes. 

Chemical Equilibrium: Explores the dynamic nature of equilibrium in chemical reactions, Le Chatelier's principle, and the calculation of equilibrium constants. 

Module 3: Reactions, Electrochemistry, Kinetics, and Nuclear Chemistry (REKN, 4.5 hp) 

This module covers various types of chemical reactions, electrochemistry, kinetics, and nuclear chemistry. 

Reactions and Electrochemistry: Investigates the principles of acid-base equilibria, solubility, and redox reactions and their applications in designing galvanic (batteries) and electrolytic cells. 

Chemical Kinetics: Analyses the factors affecting reaction rates, including the concentration of reactants/products, temperature, and catalysts. 

Nuclear Chemistry: Introduces the basic concepts of nuclear particles, nuclear reactions, radioactivity, and the different types of radiation along with their applications. 

Module 4: Laboratory Exercises (0001, 1.5 hp) 

This module involves hands-on laboratory work and the presentation of experimental results. 

Laboratory Work: Provides practical experience in conducting experiments and applying theoretical concepts. 

Presentation of Results: Teaches students how to effectively communicate their findings through formal lab reports and presentations. 

Expected learning outcomes

After completing the course, students should be able to: 

Knowledge and Understanding 

Chemical Foundations: 

• Understand chemical formulae and stoichiometric relationships. 
• Explain the physical and chemical properties of atoms and compounds using atomic and electronic structures, periodicity, and chemical bonding models. 

Phases of Matter: 

• Describe the differences between solids, liquids, and gases based on general properties, intermolecular forces, phase structures, and thermodynamics. 

Intermolecular Forces and Radioactivity: 

• Identify dominant intermolecular forces in chemical compounds by analysing atomic composition and molecular structures. 
• Describe fundamental aspects of radioactivity and differentiate between types of radiation. 

Thermodynamics and Equilibria: 

• Explain the principles of thermodynamics, including the concepts of enthalpy, entropy, Gibbs free energy, and their roles in determining the spontaneity of chemical processes. 
• Explain physical and chemical equilibrium, including Le Chatelier's principle, the calculation and significance of equilibrium constants, and the molality and molarity of solutions. 

Skills and Abilities 

Calculations and Applications: 

• Perform calculations using chemical formulae and stoichiometric relationships. 
• Apply different kinetic models to analyse chemical reactions. 
• Use integrated rate laws to predict concentrations of reactants or products over time. 

Thermodynamic Calculations: 

• Calculate changes in enthalpy, entropy, and Gibbs free energy for chemical reactions and processes. 
• Predict the direction and feasibility of reactions using thermodynamic data. 

Chemical Reactions: 

• Determine oxidation numbers, balance redox reactions, and design galvanic and electrolytic cells. 
• Use equilibrium constants and thermodynamic data to discuss acid-base characteristics, solubility, coordination chemistry, and redox properties. 

Laboratory Skills: 

• Plan and safely execute laboratory experiments.  
• Evaluate and present results both orally and in formal lab reports. 
• Maintain a detailed laboratory notebook. 

Evaluative Ability and Approach 

Chemical Analysis and Prediction: 

• Evaluate chemical structures using the appropriate models to predict physical properties and reactivities. 
• Evaluate and predict the direction of reactions using oxidation numbers and thermodynamic data. 
• Assess the effects of temperature and catalysts on the rate of reactions. 

Critical Evaluation: 

• Demonstrate an understanding of limitations inherent in different models, and the ability to select the appropriate model for a specific system. 
•  Critically evaluate their own chemical reasoning and that of others to ensure accuracy and validity. 

Required Knowledge

Form of instruction

The course includes lectures, problem-solving sessions, tutorials, demonstrations, and laboratory practicals. Attendance is mandatory for all laboratory practicals and safety sessions. 

Examination modes

Examinations consist of individual written exams, as well as written and oral presentations of laboratory work. 

For the written exam, engineering students receive one of the following grades: Fail (U), Pass (3), Pass with Merit (4), or Pass with Distinction (5). All other students receive one of these grades: Fail (U), Pass (G), or Pass with Distinction (VG). Laboratory work is graded as either Pass (3 or G) or Fail (U). To pass the course, students must pass all examinations and complete all compulsory modules. The final course grade is calculated as the average of the grades for the ATMO, TEEQ, and REKN modules. Grades of Pass (3 or G) or higher are only awarded if all laboratory practicals are passed. In cases of absence from any compulsory modules, the examiner will determine whether the student must complete compensation assignments or redo the missing parts at a later date. 

Students who pass the exam are not permitted to retake it to achieve a higher grade. 

A student who fails a course or part of a course twice is entitled to request the appointment of a different examiner, unless special reasons exist against it (HF Chap. 6 § 22). Requests for a new examiner should be submitted to the Head of the Department of Chemistry. 
 
The examiner may decide on deviations from the syllabus's examination form. Individual adaptation of the examination form should be considered based on the student's needs. The examination form is adapted within the framework of the syllabus's expected learning outcomes. A student who needs an adapted examination and who has received a decision on the right to support from the coordinator for students with disabilities at the Student Center must request adaptation from the responsible department no later than 10 working days before the examination. The examiner decides on the adapted examination, which is then communicated to the student. 

Other regulations

If the syllabus ceases to be valid or undergoes major changes, students are guaranteed at least three exam opportunities (including the regular exam opportunity) according to the regulations in the syllabus the student was originally registered under, for a maximum of two years from the date the previous syllabus ceased to be valid.