Learning outcomes of the course unit
Give a chemical insight for the understanding of natural phenomena. Teach the students the importance of chemistry in every days life. Give a basic and solid knowledge of fundamental chemistry, presenting clearly lots of topics of interest. Teach the students to critically think and solve problems.
Solid knowledge in basic mathematics and physics.
Course contents summary
Fundamental laws of chemistry. Chemical reactions. Mass relationships in chemical reactions. Reactions in water solution. Atomic structure. Basics of atomic theory. Electromagnetic waves. Atomic spectra. Quantized energy. The Bohr atom. Protons, neutrons and electrons. The quantomechanic atom. Orbitals and their energies. Electronic configurations of elements. Pauli’s principle. Hund’s rule. The aufbau principle. Periodic system of the elements. Periodic properties. Electronegativity. Metals, non metals, metalloids. Inorganic nomenclature. Chemical bond. Ionic bond. Covalent bond. Molecular geometry. Structural formulas. Exceptions to the octet rule. VSEPR theory. Bond in aliphatic hydrocarbons. Valence Bond theory (VB). LCAO-MO theory. Intermolecular forces. Hydrogen bond. The behaviour of gases. The ideal gas law. Gaseous mixtures. Real gases. Liquefaction of gases. The properties of liquids. Vapor pressure of liquids. Phase diagram of one component systems. Phases rule. Boiling and melting points. The properties of solids. Crystal packing. Ionic crystals. Covalent crystals. Molecular crystals. Metal crystals and metal bond. Solutions. Concentration. Raoult's law. Colligative properties. Chemical thermodynamics. First principle of thermodynamics. Thermochemistry. Hess's law. Standard enthalpy of formation. Enthalpy of reaction. Combustions. Second principle of thermodynamics. Third principle and absolute entropy. Entropy variation in chemical reactions. Spontaneity of the reactions. Gibbs free energy and equilibrium constant. Chemical equilibrium. Homogeneous equilibria. Le Chatelier-Brown principle. Dependence of equilibrium constants from temperature. Ionic equilibria. Acids and bases. Broensted-Lowry theory. Ionic product of water. pH. Strength of acids and bases. Polyprotic acids. Hydrolysis. Solubility product. Electrochemistry. Electrical and chemical energy. Galvanic cells. Daniel cell. Cell potential. Electrode potential. Standard electrode potentials and their applications. Redox reactions. Nernst equation. Corrosion of metals. Common galvanic cells. Accumulators. Electrolysis. Faraday's law. Chemical kinetics. Reaction rate. Influence of temperature. Introduction to catalysis. Nomenclature of principal organic compounds.
B. Laird, Chimica Generale, McGraw-Hill
Theorical lessons using Power Point slides
Assessment methods and criteria
Written questions and oral examination
Attendance strongly recommended