Atomic Structure. Mole. Chemical reactions. Atomic Orbitals. Periodic Properties. Covalent Bond. Lewis formulae. Ionic bonds. H-bond. Intermocular interactions. Aggregation states. Solutions. Thermodynamics. Chemical equilibria. Acid-Base equilibra. pH. Complexation equilibria. Solublity product. Kinetics. Electrochemistry. Reduction Potentials. Nuclear Chemistry. Basic concepts in Inorganic Chemistry
Learning Objectives - Last names N-Z
Knowledge and Understanding: students will acquire base knowledge on structure of matter, on chemical equilibria, on factors driving the reactivity.
Applying knowledge and Understanding:
Provide quantitative solutions of chemical problems, and apply then to the daily pratice in a chemical/biochemical/biotech labortory.
Using the acquired knowledge as base backgroudn knowledge for future courses of each individual track.
Teaching Methods - Last names N-Z
In-front Teachings, numerical exercises, in class supervised work
Type of Assessment - Last names A-M
Written and oral exams.
Type of Assessment - Last names N-Z
6 examinations dates throughout the year. Detalied schedule availabe at: https://sol.unifi.it/docprenot/docprenot
Examination. written + oral (compulsory). Content and duration: written part (2 hours) consisted in two parts; A: lewis formulae, redox reaction, nunclature; B: stechiometry, questions. Oral part (about 30-45 min): assessment of the individual knowldege and understanding level.
Course program - Last names N-Z
Atomic structure: atom, nucleus, molecular and atomic mass, the molecule, the mole. The elctromagnetic waves, photons, Schoredinger equations, the hydrogen atom problem. Wave functions and atomic orbitals. Quantum number. Aubfau principles. Covalent bond, sigma and pi bonds, bond energy and distances, examples. VSEPR model, Lewis formulae, concepts examples and applciations. Electronegativity, polar bonds, oxidation numbers and dipole moment, coordination compounds, ionic bonds, metallic bonds. H-bonds. and intermolecular interactions. Solutions: concentration measurements. Aggregation states and state diagrams. Collgiative properties. Thermodynamics. Chemical equilibrium. Equilibrium constant . Equilibrium in heterogeneous systems. Le Chatelier principle. Acid and base definitions, solution equilibirum, pH. Strong and weak acide and bases. Kw. Titration, buffers, poliprotic substances. Chemical reactions: oxidation numbers and redox reactions. Kinetics: order reaction, activation energy, first order kinetics, Epot vs reaction coordinate, catalyzers. Electrochemistry: Reduction potential, spontaneous reactions, Daniel Battery, Nerst Equation. Nuclear reactions, mass defects, stable isotopes, radioactivity, nuclear fission, nuclear fusion. Inorganic chemistry: elements, oxides, peroxides, hydroxides, acids, alogenide, salts.