Chemistry for Biologists 1

This first course unit focuses on the basic concepts of chemistry that are essential for understanding organic and inorganic chemistry, particularly in biologically relevant systems. Students will work through course materials (written and audio) in advance of certain lectures and tutorials, ensuring that in-person instruction during lectures and tutorials enables them to actively participate in the course, understand the concepts presented, and acquire the necessary skills. All concepts covered in this course are essential for understanding both chemistry and biology courses.

The objective of this course unit is to provide essential knowledge and skills in chemistry and biochemistry in the following areas

• Microscopic description of the structure of matter.

• Bonds and Interactions in a Chemical Compound.

• Chemical Reactions in Water

• Redox Reactions

• Acid-Base Reactions According to Brönsted and Lowry

• Precipitation Reactions

• International System units, conversion between units
• The Concept of the Mole

• The Atom: Chemical Symbol, Atomic Composition, Isotope, Atomic Mass
• Molecules, Ions
• Definition: Molecule, molecular ion
• Molecular formula
• Representations of a molecule: molecular formula, semi-molecular formula, topological formula
• Isomer: Definition, Chemical and Physical Properties
• Molar mass
• The Concepts of Solvent and Solute
• General Information on Chemical Reactions
• Balancing a Chemical Equation
• Total reaction, balanced reaction
• Stoichiometry and the Progress of a Reaction
• Progress Chart, Concepts of Excess and Deficiency Compounds
• Reaction speed: fast/slow
• The Concept of a Catalyst
• Main Functions of Organic Chemistry

For students who did not learn these concepts in high school, course materials—including videos and practice exercises—will be provided. Students will be expected to have mastered all of these concepts, and they will be assessed on them.

Recommended prerequisites*: High school Physics and Chemistry elective course

Assessment: Continuous, comprehensive assessment

1. Microscopic description of the structure of matter.

Quantum description of the atom: quantization of energy levels (basic concept in spectroscopy), wave nature of matter (concept of atomic orbitals), multi-electron atoms, electron configuration.

Periodic Table of the Elements: The concept of element groups; trends in atomic properties across the periodic table, particularly ionization energy, electronegativity, atomic radius, and ions. We will focus in particular on the metals and nonmetals most commonly encountered in biology.

1. Chemical bond.

Different types of interactions in chemistry: Strong bonds (ionic, metallic, covalent) and weak bonds (van der Waals, hydrogen bonding). When studying ionic compounds, we will cover the concept of salts and their solubility in water. We will focus in particular on salts involving nonmetals, alkali metals, and alkaline earth metals, as well as common ions (^NO₃⁻,^SO₄²⁻,^PO₄³⁻, ^NH₄⁺).Electronic structure and molecular geometry of molecules involving nonmetals: Lewis model of covalence. Concept of oxidation state; VSEPR model.

1. Chemical Reaction in Water

This section will help students consolidate their understanding of chemical reactions through reactions in aqueous solution—topics already covered in high school—which are essential for the remainder of the curriculum, particularly for those who will not take additional general chemistry courses in the second semester. These concepts may be covered, in particular, during tutorials. The law of mass action will be introduced, enabling students to derive the expression for a chemical equilibrium constant.

Redox reaction

Definition of a couple

Redox half-reactions and redox reactions in acidic and basic solutions

Note: We will introduce the concept of standard redox potential, but without justifying it through the study of batteries. Pairs involving organic or biochemical compounds will be considered.

This course will not cover: batteries, the physical meaning of a redox couple's potential, or Nernst's law.

Brønsted-Lowry Acid-Base Theory

Definition of an acid, a weak base, and a strong base. We will consider examples that are particularly important in biology (carboxylic acids, amines, amino acids, and phosphoric acid, among others).

Equilibrium constant (assumed without proof) and_pKa scale

Predominant range based on pH

Acid-Base Reaction

The concept of a buffer zone (this concept can be introduced through an exercise as an introduction to this important biological concept).

This course will not cover: titration curves

Precipitation reaction

Definition, equilibrium constant, range of precipitation

Hourly volumes*:

            CM : 16,5

            TD: 19.5

            Practical Work:

            Lot:

Recommended reading:

Reference 1: Chemistry: Molecules, Matter, and Metamorphoses. P. Atkins and L. Jones, DeBoeck Université, 1998.

Reference 2: Chemistry. Stéphane Perrio, Béatrice Roy, and Jean-Yves Winum, published by Dunod, 2017 

Reference 3: Visual Guide to General Chemistry. Series: Tout en fiches. Isabelle Bonnamour, Jean-Sébastien Filhol, Frédéric Lemoigno, Nathalie Perol, Jean-Yves Winum; published by Dunod, 2019.

Reference 4: Chemistry L1 - I Make Mistakes, So I Learn! Stéphane Perrio, Béatrice Roy, and Jean-Yves Winum, Dunod 2020.