Learning outcomes of the course unit
The student must demonstrate knowledge of the basic concepts of general chemistry and know how to apply them in the resolution of exercises (stoichiometry, balance of reactions, calculations of thermodynamic quantities) as well as in the description of the phenomena studied in the teaching module.
It is required to be able to:
1. Be able to use the scientific language of the topics covered in the chemistry course. (knowledge and understanding)
2. demonstrate an adequate knowledge of the basic laws of general chemistry and to know their application in real cases ( applying knowledge and understanding)
3. express in a concise and precise form the basic concepts of general chemistry in the written test. (Communication skills )
4. to create links between the various chapters dealt with and apply the acquired knowledge to the solution of problems of stoichiometric calculation and to demonstrate the understanding of the basics of chemistry by illustrating some of the basic laws and by the formulation of some examples (making judgments)
5. to integrate the didactic material provided with textbooks is required in order to formulate a synthesis in order to construct a base of preparatory knowledge to face the comprehension of successive courses of chemistry. ( learning skills)
Course contents summary
Classification of the subject. Elements substances and mixtures. Mass conservation laws
Structure of the atom (neutron proton and electron) atomic number, atomic mass. Elements and Isotopes. Orbitals and rules of electron distribution. Periodic table and correlation with the electronic configuration. Periodic properties.
Chemical bond. Ionic and covalent bond. Oxidation number. Valence bond and octet rule. Lewis structures. Resonance formulas and formal charge. Orbitalic hybridization .Polarity in molecular bonds. Nomenclature of cations, anions and inorganic compounds.
Chemical reaction. Formula weight, molecular weight, size and use in the calculation of mass reactions. Stoichiometry. Balancing different types of chemical reactions. Ox-redox reactions.
Introduction to thermodynamics. First and second principles of thermodynamics. Reaction heat. Exothermic and endothermic reactions. Gibbs free energy, spontaneity of a process.
Chemical equilibrium. K equilibrium constant, Le Chậtelier's law. Factors that influence chemical balance.
States of the matter. Gaseous state: perfect gas state equation. Liquid state: vapor pressure, surface tension, boiling point, intermolecular forces (van der Waals forces, hydrogen bond). Notes on the solid state. Phase changes and phase diagrams, supercritical state.
Solutions. Solvent and solute, solubility. Colloidal solutions, emulsions. Methods to indicate the concentration (molarity, molality, normality, percentages). Henry's law. Colligative properties (cryoscopic lowering, ebullioscopic elevation, osmotic pressure).
Acids and Bases. Definition according to Brønsted. Conjugated acid and base. Ionic product of water, pH, calculation of Ka and Kb and their use in determining the strength of an acid or base. Strong acids and bases, weak acids and bases. Examples of hydrolysis of some salts, buffer solutions, pH of a buffer.
Overview of kinetics. Reaction speed, effect of concentration and temperature, Arrhenius's law, activation energy, catalysts (homogeneous, heterogeneous, enzymatic).
John C. Kotz,Paul M. Treichel,John R. Townsend
The course takes place in 48 hours of lectures. The lessons will be carried out through an oral explanation of the concepts summarized in slides. In some cases it will be possible to use more traditional tools (use of the blackboard). In addition to the illustration of the theoretical concepts, some sessions of exercises will be carried out. The slides will be made available to students on the Elly portal. The formulation of questions for the request for further clarification or the formulation of comments on the concepts expressed will be encouraged and stimulated.
Assessment methods and criteria
The access the exam is obtained by registering through the ESSE3 platform. The assessment procedure will be a written test that comprises ten questions including both the request to illustrate theoretical concepts and the stoichiometry exercises. Each question will be evaluated for a maximum of 3 points. For partial answers or partially completed exercises will be assigned scores from 1 to 2 points. The exam will last for 2 hours. The outcome will be communicated and recorded on the ESSE3 platform only after acceptance of the vote achieved. Students can view the exam by appointment with the teacher.