The course aims to provide students with the fundamental chemical knowledge essential for understanding the chemical aspects of the other subjects in the study program.
Course Prerequisites
Basic knowledge of mathematics and physics, as provided in upper secondary school. The course is designed so that no specific background in chemistry is required. However, students enrolled in the first year of Pharmacy and CTF programs may attend a preliminary chemistry course.
Teaching Methods
Classes with the support of presentations (PowerPoint, available on KIRO after the class) on screen and exercises at the blackboard. The course is completed by exercise classes with a tutor in classroom and by an online tutoring on a forum on Kiro.
Assessment Methods
The exam consists in a written test. During the course, the exam can be taken as two "in itinere" tests. Passing the first test (with a minimum of 16/30) is required to access to the second one. In alternative, the exam can be taken in a single final test, starting from the month of February. Both the partial and the final tests consist of theoretical questions and exercises. There will be no oral examination.
Texts
All the teaching material (power point slides and exercises) is available on KIRO (depending on the University's regulation on didactic material sharing) Suggested textbooks: Atkins, Jones, Laverman, Fondamenti di Chimica Generale, Zanichelli Petrucci, Herring, Madura, Bissonnette, Chimica Generale, Piccin Speranza, Casarin, Casella, etc, Chimica Generale e Inorganica, EdiErmes
Contents
Structure of the atom, periodic properties of the elements. Atomic and molecular masses, mole. Chemical reactions, reaction equations, stoichiometric calculations. Ionic and covalent bonds, structure and geometry of molecules. Polar bonds, the hydrogen bond. Nomenclature of ionic and covalent compounds, oxidation states. Interactions between molecules, states of aggregation. Solutions, properties of solutions, colloids. Chemical kinetics: rate law of a reaction, rate constant, catalysis, enzymes. Chemical equilibria: equilibrium constants; spontaneous and non-spontaneous reactions. Le Chatelier’s principle. Equilibria in aqueous solution: acid-base reactions, acidity and basicity constants, strength of acids and bases, buffer solutions. Lewis acid-base adducts; coordination compounds. Precipitation reactions: solubility product, common ion effect, dissolution of precipitates. Oxidation-reduction reactions: electrochemical cells, electrode potentials. Standard potentials series. Relationship between electrode potential and concentration, Nernst’s equation. Energy exchanges at the equilibrium: relationship between free energy change and equilibrium constant of a reaction.
