The Chemistry Course aims to provide students with basic knowledge of the structure of the matter, chemical bonding and the principles that govern the chemical equilibrium in homogeneous and heterogeneous systems with particular attention to reactions in aqueous solvent. It also gives some basic knowledge about the chemical properties of the main elements of the periodic table and their most important compounds. The course thus aims to give students the tools to know the matter and the chemical transformations as well as to transmit the ability to describe chemical phenomena through scientific language appropriately. The course includes numerous practical sessions related to the stoichiometry of the processes on the topics discussed in the theoretical part of the course.
Elements of elementary math.
Atomic structure; The chemical bond; Chemical reactions; Matter aggregation states (16 hours + 14 exercise):The matter and its property- Classification of matter: elements, atoms, molecules, compounds; Electromagnetic radiation. Atomic models. Electronic configuration of atoms and chemical periodical. Periodic trends in the size of atoms, of the ionization energy, electronic affinity and electronegativity. Atoms and elements- The molar mass. The balanced chemical equation: stoichiometric relationships. Valence electrons. The ionic bond. The covalent bonds and Lewis structures. Molecular geometry. Hybridization. VSEPR theory. Nomenclature of inorganic compounds. Metallic bond. The gaseous state- pressure and temperature. The ideal gas law. Gaseous mixtures. The distribution of molecular speed. Condensate phases- Intermolecular Forces: forces of Van der Waals, hydrogen bond. Liquid state. Solid state: solid ionic, covalent solids, metallic solids, molecular solids. Solutions- The chemical equilibrium (16 hours + 18 exercise):Solutions; Factors affecting solubility: pressure and temperature. Quantitative expressions of concentration. The law of mass action: the equilibrium constant. Le Chatelier's principle.Equilibria in acqueous solution. Monoprotic acids and bases in water. The pH. The neutralization. Hydrolysis reactions.
Thermodynamics, kinetics, Electrochemistry (8 hours).The principles of thermodynamics. Standard enthalpy of reaction. Calculation of the entropy change. Free energy and spontaneity of reactions. Chemical kinetics. Electrochemistry- Galvanic cells. Electrolytic cells.
Part Work from the website: www.ingegneria.uniparthenope.it.
-Brown, Lemay, Bursten, Murphy ‘Fondamenti di Chimica’ TerzaEdizione Casa Editrice: EdiSES.
-P. Giannoccaro, S. Doronzo, Elementi di Stechiometria, seconda edizione-EDISES
The exam consist of a written test and a final oral discussion. The written test deals with the resolution of 5 stoichiometry problems in two hours. The use of PC or smartphone is not allowed while a periodic table and a scientific calculator can be used. The oral test provides a discussion on the theoretical aspects of general and inorganic chemistry. The full understanding of the topics dealt in the course and the capability of properly using an appropriate scientific language will be evaluated. The final vote comes from the verification of those abilities.