Duration
Theory : 30h Th
Practice : 20h Pr, 8h QA Sess.
Number of credits
| Bachelor in geology | 6 crédits |
Lecturer
Theory : Loïc Quinton
Practice : Loïc Quinton
Coordinator
Language(s) of instruction
French language
Organisation and examination
Teaching in the second semester
Schedule
Units courses prerequisite and corequisite
Prerequisite or corequisite units are presented within each program
Learning unit contents
Description of the teaching:
The general chemistry course is largelybased on an experimental approach. We are convinced that students will be more receptive to a chemistry described in a practical way, with a focus on the applications linked to the explored topics.
Table of contents:
Chapter 1: Matter and Atoms, Reminders
1.A Introduction: structure of the atom, isotopes, law of conservation of the matter.
1.B Periodicity of the elements.
1.C Key concepts: atomic and molecular masses, mole, molar mass and volume.
Chapter 2: Atoms and Electrons
2.A Light: electromagnetic wave, absorption spectroscopy, atomic emission, photoelectric effect.
2.B Atomic structure: planetary model of Bohr, wave-particle duality, ondulatory mechanics, model of the atom according to Schrödinger, quantum numbers and atomic orbitals.
2.C Electronic configuration of elements: spin quantum number, Pauli exclusion, Klechkowski and Hund rules.
Chapter 3: Molecules and Complexes
3.A Chemical binding: introduction and reminders
3.B Theory of the valence and of the molecular orbitals: chemical bond, LCAO model, electronegativity, electric dipole and dipolar moment.
3.C Molecular geometry: VSEPR model, hybridization of orbitals, metal complexes, organic molecules.
3.D Weak energy bonds: Van der Walls forces and hydrogen bonding.
Chapter 4A: Thermochemistry and 1st Principle of Thermodynamics
4A.A Introduction to thermodynamics: definitions and tools.
4A.B First Principle: Internal Energy, Enthalpy, Standard State, Molar Heat.
4A.C Enthalpy variation: Hess cycle, binding and formation enthalpies.
Chapter 4B: Chemical Thermodynamics
4B.A Introduction.
4B.B Entropy S, the state function of disorder: second and third principles.
4B.C Gibbs free entropy: definition, criterion of spontaneity, relation to equilibrium constant.
Chapter 5: The Chemical equilibrium.
5.A Introduction: equilibrium constant and quotient of reaction.
5.B Chemical equilibrium: dynamic equilibrium, homo / heterogeneous equilibria.
5.C Principle of Le Chatelier: effects of concentration, pressure and temperature.
Chapter 6: The Acido-Basic Balance
6.A Introduction: definition, polyprotic acids, dissociation of electrolytes, strength of acids and bases.
6.B phmetry: ionic product, pH calculations, acid-base properties of salts.
6.C Solution buffers and acid-base indicators.
6.D Sillen diagrams andfunction of species distributions.
6.E Acid-base titrations.
Chapter 7: Reactions of precipitation
7.A Introduction: Kps solubility product and solubility.
7.B Precipitation reactions.
7.C Solubility and effect of common ion.
7.D Solubility and effect of pH.
7.E Precipitation of metal hydroxides.
Chapter 8: Complex formation equilibrium
8.A Reactions of complexation.
8.B Equilibrium of complex formation.
8.C Distribution diagrams.
8.D Solubility and formation of complex ions.
8.E Basis of qualitative analysis.
Theory
Description of the teaching:
The general chemistry course is largelybased on an experimental approach. We are convinced that students will be more receptive to a chemistry described in a practical way, with a focus on the applications linked to the explored topics.
Table of contents:
Chapter 1: Matter and Atoms, Reminders
1.A Introduction: structure of the atom, isotopes, law of conservation of the matter.
1.B Periodicity of the elements.
1.C Key concepts: atomic and molecular masses, mole, molar mass and volume.
Chapter 2: Atoms and Electrons
2.A Light: electromagnetic wave, absorption spectroscopy, atomic emission, photoelectric effect.
2.B Atomic structure: planetary model of Bohr, wave-particle duality, ondulatory mechanics, model of the atom according to Schrödinger, quantum numbers and atomic orbitals.
2.C Electronic configuration of elements: spin quantum number, Pauli exclusion, Klechkowski and Hund rules.
Chapter 3: Molecules and Complexes
3.A Chemical binding: introduction and reminders
3.B Theory of the valence and of the molecular orbitals: chemical bond, LCAO model, electronegativity, electric dipole and dipolar moment.
3.C Molecular geometry: VSEPR model, hybridization of orbitals, metal complexes, organic molecules.
3.D Weak energy bonds: Van der Walls forces and hydrogen bonding.
Chapter 4A: Thermochemistry and 1st Principle of Thermodynamics
4A.A Introduction to thermodynamics: definitions and tools.
4A.B First Principle: Internal Energy, Enthalpy, Standard State, Molar Heat.
4A.C Enthalpy variation: Hess cycle, binding and formation enthalpies.
Chapter 4B: Chemical Thermodynamics
4B.A Introduction.
4B.B Entropy S, the state function of disorder: second and third principles.
4B.C Gibbs free entropy: definition, criterion of spontaneity, relation to equilibrium constant.
Chapter 5: The Chemical equilibrium.
5.A Introduction: equilibrium constant and quotient of reaction.
5.B Chemical equilibrium: dynamic equilibrium, homo / heterogeneous equilibria.
5.C Principle of Le Chatelier: effects of concentration, pressure and temperature.
Chapter 6: The Acido-Basic Balance
6.A Introduction: definition, polyprotic acids, dissociation of electrolytes, strength of acids and bases.
6.B phmetry: ionic product, pH calculations, acid-base properties of salts.
6.C Solution buffers and acid-base indicators.
6.D Sillen diagrams andfunction of species distributions.
6.E Acid-base titrations.
Chapter 7: Reactions of precipitation
7.A Introduction: Kps solubility product and solubility.
7.B Precipitation reactions.
7.C Solubility and effect of common ion.
7.D Solubility and effect of pH.
7.E Precipitation of metal hydroxides.
Chapter 8: Complex formation equilibrium
8.A Reactions of complexation.
8.B Equilibrium of complex formation.
8.C Distribution diagrams.
8.D Solubility and formation of complex ions.
8.E Basis of qualitative analysis.
Practice
This practical work aims to illustrate the main principles of chemistry detailed during the theoretical courses of the first and second quadrimesters. Laboratory sessions will be based on different teaching methods:
* The problem-based approach: in these sessions a chemical problem will be posed to the students. They will need to use their knowledge to establish a work strategy to answer the research question. They will be evaluated on the development work and application of their strategy, as well as on the communication of their results.
* The protocol approach: in these sessions the students will be asked to apply an analysis protocol to answer the research question. They will be assessed on their ability to follow the protocol and on the communication of their results.
* The concept-based approach: in these sessions, the students will be asked to do experiments illustrating chemistry concepts. They will be asked to identify this concept and explain its basics. They will be assessed on their understanding of the concept and on communicating their results.
Here are the nine practical sessions:
TP1-Session 0 : Introduction
TP2-Session 1 : Acid-Base - The bottles without labels
TP3-Session 2 : How to illustrate chemical equilibrium?
Learning outcomes of the learning unit
General chemistry teaching during the second period of the year aims to give to the students the basic theoretical and practical concepts in molecular chemistry, thermodynamics, kinetics, and solution chemistry (reactivity). These concepts are necessary in order to understand the phenomena studied in later parts of the curriculum.
Theoretical classes, practical work and tutorials allow students to learn the methods and basic techniques of solution chemistry while familiarising them with the formulae of the chemical products and understanding their evolution by change of phase or reaction. A special focus will be given to the chemical equilibrium conditions.
Theory
General chemistry teaching during the second period of the year aims to give to the students the basic theoretical and practical concepts in molecular chemistry, thermodynamics, kinetics, and solution chemistry (reactivity). These concepts are necessary in order to understand the phenomena studied in later parts of the curriculum.
Theoretical classes, practical work and tutorials allow students to learn the methods and basic techniques of solution chemistry while familiarising them with the formulae of the chemical products and understanding their evolution by change of phase or reaction. A special focus will be given to the chemical equilibrium conditions.
Practice
At the end of the course, the students:
* will have acquired a solid basis on the main principles of chemistry and their practical applications
* will have acquired problem-solving skills through the development of their critical thinking and analytical reasoning
* will be able to develop and perform simple scientific experiments on the basis of their knowledge
* will be able to correctly collect and analyze the data generated by these experiences
* be able to clearly communicate their results orally and in writing
* will be able to work in a team for the conduct of laboratory experiments
* will be able to work in the laboratory in complete safety, being aware of the associated risks, from a chemical and environmental point of view
Prerequisite knowledge and skills
For the entire course, the student is assumed to have very basic understanding of chemistry and in particular, to have knowledge of the basics of atomic and molecular theory as well as the elemental properties of the main types of chemical compounds (oxides, acids, bases and salts) and their principal reactions. These concepts will, however, be revised early on in the course. This course also makes use of a range of simple physical and mathematical tools.
Theory
For the entire course, the student is assumed to have very basic understanding of chemistry and in particular, to have knowledge of the basics of atomic and molecular theory as well as the elemental properties of the main types of chemical compounds (oxides, acids, bases and salts) and their principal reactions. These concepts will, however, be revised early on in the course. This course also makes use of a range of simple physical and mathematical tools.
Practice
Follow the course CHIM0738.
Planned learning activities and teaching methods
In addition to theoretical courses and sessions of exercices organized according to the established schedule, supervised laboratory work sessions will also enrich the teaching.
Organization. Practical lab sessions will be scheduled throughout the academic year. They will illustrate the important notions of reactivity in solution. A calendar will be distributed to students at the beginning of the year.
Security. Wearing the lab coat and glasses is mandatory. Any student who does not have his equipment will be excluded from the laboratory, and will automatically be sanctioned with a 00/20 at the session.
Attendance at practical sessions. TP sessions are mandatory and rated. An unjustified absence (eg medical certificate) will automatically be sanctioned by a 00/20 at the meeting.
Theory
In addition to theoretical courses and sessions of exercices organized according to the established schedule, supervised laboratory work sessions will also enrich the teaching.
Organization. Practical lab sessions will be scheduled throughout the academic year. They will illustrate the important notions of reactivity in solution. A calendar will be distributed to students at the beginning of the year.
Security. Wearing the lab coat and glasses is mandatory. Any student who does not have his equipment will be excluded from the laboratory, and will automatically be sanctioned with a 00/20 at the session.
Attendance at practical sessions. TP sessions are mandatory and rated. An unjustified absence (eg medical certificate) will automatically be sanctioned by a 00/20 at the meeting.
Practice
Three varied 4-hour laboratories, illustrating the theoretical material as much as possible.
Mode of delivery (face to face, distance learning, hybrid learning)
Each student will receive a personalised programme (log book) at the start of the year summarising all the information relating to the organisation of chemistry teaching (theory classes, practical sessions, revision, tutorials, tests).
An interactive online teaching platform is also available on eCampus, and offers to the students various learning tools such as course materials, TP and TD notes, solved problems or again a forum for asking questions.
Theory
Each student will receive a personalised programme (log book) at the start of the year summarising all the information relating to the organisation of chemistry teaching (theory classes, practical sessions, revision, tutorials, tests).
An interactive online teaching platform is also available on eCampus, and offers to the students various learning tools such as course materials, TP and TD notes, solved problems or again a forum for asking questions.
Organisational adjustments related to the current health context
During the most delicate periods of the health crisis, the theoretical course and the sessions of exercice will be proposed entirely online in the form of live videoconferences (exercices) or pre-recorded capsules (theoretical lessons).
Practices will be held face-to-face as much as possible. Additional laboratories will be requisitioned to allow students to carry out their own experiments, under optimal security conditions.
The discussion forum, created on eCampus will be a key tool for students to ask their questions. The teaching team is committed to doing its utmost to answer questions as quickly as possible.
The exam is held in person, unless prohibited by the authorities. In this extreme case, the exam would then be organized online via the eCampus platform.
Theory
During the most delicate periods of the health crisis, the theoretical course and the exercise sessions will be offered completely online in the form of live videoconferences (exercises) or pre-recorded capsules (theoretical courses).
Practices will be held face-to-face as much as possible. Additional laboratories will be requisitioned to allow students to carry out their own experiments, under optimal security conditions.
The discussion forum, created on eCampus will be a key tool for students to ask their questions. The teaching team is committed to doing its utmost to answer questions as quickly as possible.
The exam is held in person, unless prohibited by the authorities. In this extreme case, the exam would then be organized online via the eCampus platform.
Recommended or required readings
Leture notes and copies of the illustrations (pdf) will be available online following the course completion.
Theory
Leture notes and copies of the illustrations (pdf) will be available online following the course completion.
Practice
A handout, available in pdf, will be provided to guide students through their experiences.
Assessment methods and criteria
Below you will find information on the evaluation methods planned for in-person and remote exams as well as those planned for hybrid sessions. Depending on how the health crisis evolves, the chosen method will be communicated to you no later than one month before the start of the exam session.
Organization of exams.
An exam will be organized in May-June (first session), under the form of multiple choice questions combining both theoretical questions and exercises.
For students who have failed at the first session, a second exam will be prepared in May-September (second session).
Weighting of the notes:
The final grade of chemistry will be weighted like this:
Exam: 75%
Laboratories: 25%
Success criterion:
Success is awarded to any student with a final score equal to or greater than 10.00 / 20.
Theory
Organization of exams.
An exam will be organized in May-June (first session), under the form of multiple choice questions combining both theoretical questions and exercises.
For students who have failed at the first session, a second exam will be prepared in May-September (second session).
Weighting of the notes:
The final grade of chemistry will be weighted like this:
Exam: 75%
Laboratories: 25%
Success criterion:
Success is awarded to any student with a final score equal to or greater than 10.00 / 20.
Practice
During the practical work, students will be evaluated on their laboratory preparation, on the conduct of the experiment (their results) and the communication of results. The exact breakdown between these different levels is available for each session in the "evaluation criteria" section.
1. Concerning the preparation of each session, students will be assessed on the basis of their pre-report and / or a written question.
2. At the laboratory level, the students will be evaluated on the basis of the results obtained as well as on the communication thereof (report, graph, etc.).
The respect of safety rules is also strongly taken into account for the evaluation of the students.
Work placement(s)
Organizational remarks
Lecture notes and illustrations will be available online (myulg) after each lesson.
Theory
Lecture notes and illustrations will be available online (myulg) after each lesson.
Contacts
Prof. Loïc Quinton Laboratory of Mass Spectrometry - MolSys Research Unit Bat B6C, Local 0/R66 Tel: +0032 4 366 3679 Email: loic.quinton@uliege.be
Theory
Prof. Loïc Quinton Laboratory of Mass Spectrometry - MolSys Research Unit Bat B6C, Local 0/R66 Tel: +0032 4 366 3679 Email: loic.quinton@uliege.be
Practice
Prof. Loïc Quinton Laboratory of Mass Spectrometry - MolSys Research Unit Bat B6C, Local 0/R66 Tel: +0032 4 366 3679 Email: loic.quinton@uliege.be