LEARNING OUTCOMES

The fundamentals of chemistry will be aquired (the matter and its atomic structure, chemical bonds, inorganic compounds, nomenclature, states of matter, principles of thermodynamics, solutions, chemical reactions, chemical equilibrium, electrochemistry, the main chemical properties of the most important elements and inorganic compounds).

AIMS AND LEARNING OUTCOMES

This course aims to provide the ground knowledge of the chemistry required for the next classes. 

The learning outcomes will be, together with the acquisition of the ground knowledge of chemistry, the ability to use the scientific language, and solve problems by applying the acquired notions to real cases.

TEACHING METHODS

Class lessons (80 hours) on the whole program (lessons and exercises) . 

During adverse situations (such as pandemic ot meteo alert), the lessons might be delivered online by following the University guidelines.

Further material on the class can be provided online (ex., Aulaweb or Teams).

SYLLABUS/CONTENT

• Introduction to Chemistry. Elements, compounds and mixtures. Solutions and concentration. Rules of chemical nomenclature. Chemical reactions. Stoichiometry.
• Gas state. The equation of state of ideal gas. Mixtures of gases and Dalton’s law of partial pressure. The real gases and Van der Waals equation.
• Thermodynamics. Heat of reaction and enthalpy. Enthropy. Gibbs free energy and spontaneous reactions.
• Atom. Atomic structure. Atomic orbitals. Electrons and orbitals. Periodic table.
• Chemical bond. Ionic bond. Covalent bound. Electronegativity. Lewis structures. The VSEPR theory. Hybrid orbitals. Intermolecular forces.
• Liquid state and solid state. Liquids. Solids. Metallic bond. Phase transitions and phase diagrams for single-component systems.
• Solutions. Solubility. Ideal solution and Raoult’s law. Colligative properties. Electrolytes. Degree of dissociation. Conductivity of electrolyte solutions.
• Chemical kynetics. Reaction rate. Collision theory. Factors affecting the rate of reactions. Kinetic equation. Catalysis.
• Chemical equilibrium. Law of mass action. Equilibrium constant. Le Chatelier’s principle. Homogeneous and heterogeneous equilibrium.
• Acids and bases. Theories of: Arrhenius, Brønsted-Lowry and Lewis. Strength of acids and bases. Acidity of aqueous solutions: pH. pH indicators. Hydrolysis. Buffer solutions. Solubility equilibrium. Complexes.
• Electrochemistry. Electrodes and galvanic cells. Reduction potentials and Nernst equation. Electrolysis. Faraday’s laws. Accumulators.
• Inorganic chemistry. Hydrogen. Main characteristics of the elements of 1, 2, 13, 14, 15, 16, 17, 18 Groups and their most representative compounds. Characteristics of the elements of d-block and representative compounds.

RECOMMENDED READING/BIBLIOGRAPHY

The recommended books are:

- Peter Atkins, Loretta Jones, “CHIMICA GENERALE”, Ed. Zanichelli.

- Peter Atkins, Loretta Jones, Leroy Laverman, “PRINCIPI DI CHIMICA” (4th edition), Zanichelli

Other books of General and Inorganic Chemistry at university level can be used, e.g.:

- Kotz, Treichel, Townsend, Treichel “CHIMICA”, VII ed., Ed. Edises

- Brown, Lemay, Bursten, Murphy, Woodward, “FONDAMENTI DI CHIMICA”, Ed. Edises

- Casarin, Casella, D'Agostino, Filippi, Grandinetti, Purrello, Re, Speranza, "CHIMICA GENERALE E INORGANICA" a cura di M. Speranza, Ed. Edi-ermes

- Petrucci, Herring, Madura, Bissonnette, “CHIMICA GENERALE. Principi ed applicazioni moderne" (+ complete solutions manual), Ed. Piccin