For the course unit "General Chemistry 1", at the end of the course, the student will be able to :
describe the microscopic structure of matter (at the atomic and molecular levels);
master nomenclature;
to predict the properties of molecular structures (geometry, polarity);
to model chemical reactions;
to apply the ideal gas theory;
to carry out stoichiometric calculations;
to define the properties of solutions (concentration, cryoscopic depression, osmosis, etc.);
to define the basic concepts of thermodynamics;
to explain the states of matter using thermodynamic concepts;
to describe the state of dynamic equilibrium and its displacement;
to calculate the values of equilibrium constants;
to derive some thermodynamic formulae;
to use chemistry equipment correctly to carry out laboratory experiments;
to use theoretical concepts to analyse, interpret and comment on experimental results;
to write simple mesomeric forms;
to apply the concepts and rules of stereochemistry.
The objectives of this course are to • to give the student a rigorous basic training in certain aspects of general chemistry (structure of matter, reactivity and stoichiometry); • describe matter (pure bodies or mixtures) in the three levels of knowledge (macroscopic, microscopic and symbolic); • explain and predict chemical transformations using different theoretical concepts; • to carry out an experimental approach; • solve problems using mathematical reasoning and tools; • interpret data presented in different forms (table, graph, text, etc.)
This module focuses on the fundamental theories of chemistry. The description of the atom and the study of the nature of bonds and interactions lead to an understanding of the structure and geometry of molecules, as well as the different states of matter and changes of state. The classification of different molecules according to their function leads to the nomenclature of these various compounds. The presentation of basic concepts and the main thermodynamic variables provides an introduction to physico-chemical equilibria.
Chapter 1: Atoms and molecules: 1.1. Matter: mixtures, pure substances 1.2. The atom 1.3. Atomic mass 1.3.1. Atomic mass of a nuclide 1.3.2. Atomic mass of an element 1.3.3. Mass defect 1.4. The concept of the mole 1.5. Atomic structure.
Chapter 2: Electronic structure of atoms 2.1. Hydrogen emission spectrum 3.2. Bohr’s atomic model 2.3. Limitations of the Bohr model 2.4. Schrödinger’s atomic model 2.5. Electronic structure and the periodic table 2.6. Mendeleev’s classification.
Chapter 3: Electronic structure and reactivity 3.1. Ionisation energy 3.2. Electroaffinity 3.3. Electronegativity 3.4. Acid-base character 3.5. Formation of ions 3.6. Oxidation state.
Chapter 4: Structure and Nomenclature of Molecules 4.1. Chemical bonds 4.2. Nomenclature and structural formulae of planar molecules 4.3. Molecular geometry.
Chapter 5: Intermolecular Forces and the Laws of Gases 5.1. States of matter 5.2 Van der Waals interactions 5.3. Hydrogen bonding 5.4. Intermolecular forces and physicochemical properties 5.5 Gas laws. 5.5.1. Ideal gas law 5.5.2. Units of pressure 5.5.3. Partial pressures 5.5.4. Solubility of gases 5.5.5. Density of gases.
Chapter 6: Stoichiometric quantities 6.1. The fundamental laws of chemistry 6.2. Molecular mass, molar mass 6.3. Calculating the amount of substance (n) 6.4. Solutions and concentration 6.5. Dilution 6.6. Stoichiometric problems
Chapter 7: Molar mass and molecular formulae 7.A. Experimental determination of molar masses 7.A.1. Colligative properties 7.A.2. Mass spectrometry 7.B. Experimental determination of molecular formulae 7.B.1. Elemental analysis 7.B.2. Combustion furnace.
Chapter 8: Thermochemistry: First Law: Energy Exchanges. 8.1. Basic Concepts of Thermochemistry. 8.2. Forms of Energy. 8.3. Conservation of Energy: First Law of Thermodynamics. 8.4. Determination of ΔH (ΔU) for a Reaction.
Chapter 9: Thermochemistry: Second Law: criterion of spontaneity. 9.1. Criterion of spontaneity for a reaction. 9.2. Equilibrium criterion. 9.3. Determining the spontaneity of a reaction. 9.4. Second Law of Thermodynamics. 9.5. Influence of temperature, pressure and concentration
Chapter 10: Equilibria. 10.1. Equilibrium and thermodynamics. 10.2. Equilibrium shift, Le Chatelier’s principle. 10.3. Phase diagram of pure substances.
Chapter 11: Structure of carbon compounds 11.1. Representation of molecules 11.2. Classification of carbon molecules 11.3. Hybridisation and molecular geometry 11.4. Stereochemistry 11.5. Mesomerism 11.6. Characterisation of carbon molecules.
Different approaches are used in this teaching unit: • The theoretical concepts are presented in the form of a lecture based on a powerpoint. The latter is made available to students on the university's website "webcampus"; • Exercises in small groups (about 30 students), supervised by an assistant, allow the theoretical concepts to be applied and deepened; • Practical laboratory work, carried out individually under the supervision of an assistant, allows the theoretical concepts to be illustrated and manipulated. They also allow students to learn the correct use of the basic equipment of a chemistry laboratory and the protocols to be followed to carry out simple manipulations. • Teaching methods may be adapted to comply with health requirements.
The teaching unit "General Chemistry I" consists of three learning activities: - the theoretical course - tutorials (exercises) (TD) - practical work (laboratories) (TP) Each of these learning activities is assessed. In the course of the term, the student • The student will be tested on exercises (TD), the average of which will count for 20% of the final grade of the course. The student must bring a simple, non-programmable calculator without a cover to the tests. If the student is absent during a test, and if this absence is justified by a medical certificate, submitted to the secretariat of the Faculty of Science at the end of the certificate, the student must retake the test at the end of the term, on a date to be communicated to him/her in due course. If the absence is not justified by a medical certificate, the student will receive a mark of 0/20 for this test. • must carry out practical work. Each practical session is evaluated by an entry test (1/4 of the points) and a laboratory report (3/4 of the points) which must be handed in to the assistant within the time limit specified by the latter during each practical session. The average of the TP evaluations constitutes 10% of the final grade of the teaching unit. In the event of absence, if justified by a medical certificate submitted to the secretariat of the Faculty of Science at the end of the certificate, the student must send an e-mail to "didactique.chimie@unamur.be" within three days of the beginning of the absence to inform the secretariat of the absence and the date on which the student will be able to collect the practical work. If the student fails to do this, a mark of 0/20 will be awarded for the practical course concerned. Any absence not justified by a medical certificate will result in a mark of 0/20 for the practical course concerned. The final marks of the practical and practical courses are definitively acquired at the end of the corresponding activities.
During the examination session at the end of the first semester (January), the student has a written examination on the whole subject of the course unit. This is an open-ended written examination (3 hours) with many exercises. During the examination, the student may not have access to any documents other than the questionnaire and answer form provided by the teacher. The student must bring a simple, non-programmable, uncovered calculator to the examination. The student may not carry or have within reach any connectable object. To validate the credits of the teaching unit, the student must obtain a weighted average mark of at least 10/20. The weighted average for the teaching unit is calculated as follows: written examination in session (70%), final mark acquired during the year for TD (20%), final mark acquired during the year for TP (10%). The assessment of the different learning activities may be adapted to comply with the health requirements, which could lead to a modification of the weighting of the different activities (lectures, tutorials, practical work) in the calculation of the final mark of the course. All changes imposed by the health requirements will be communicated to students via the SCHIB118: General Chemistry I website.
During the examination session at the end of the second semester (May-June), the student has a written examination on the whole subject of the course unit, if he/she has not validated the credits corresponding to this course unit during the January session. The examination is an open-ended written examination (3 hours) with numerous exercises. During the examination, the student may not have access to any documents other than the questionnaire and answer form provided by the teacher. The student must bring a simple, non-programmable calculator without a cover to the examination. The student may not carry or have within reach any connectable object. To validate the credits of the course unit, the student must obtain a weighted average mark of at least 10/20. The calculation of the weighted average mark is the same as in January. The TD and TP marks acquired during the year are retained.
During the summer examination session (August) the student has a written examination on the whole subject of the course unit, if he/she has not validated the credits corresponding to this course unit during one of the two previous sessions. The examination is an open-ended written examination (3 hours) with numerous exercises. During the examination, the student may not have access to any documents other than the questionnaire and answer form provided by the teacher. The student must bring a simple, non-programmable calculator without a cover to the examination. The student may not carry or have within reach any connectable objects. To validate the credits of the course unit, the student must obtain a weighted average mark of at least 10/20. The calculation of the weighted average mark is the same as in January and June. The TD and TP marks acquired during the year are retained.
Chemistry concentrate, J.Wouters, PUN
| Training | Block | Credits | Mandatory |
|---|---|---|---|
| Bachelor in Biology | 1 | 7 | Yes |