Ateneo - UPO

The purpose of the course is to provide students the basic knowledge in general and inorganic chemistry. The connection with the various biological disciplines will be discussed, in particular with the use of examples and numerical exercises

The presentations will be available on the D.I.R. site. Suggested Reference Books:
-Kotz, Treichel, Townsend, “Chimica” Edises;
-Schiavello, Palmisano “Elementi di Chimica” Edises;
-Masterton, Hurley: "Chimica: Principi e Reazioni", Piccin;
-Tro: "Chimica: un approccio molecolare", Edises;
-Whitten, Davis, Peck, Stanley, Chimica (9 Ed.), Piccin.
Stoichiometry Reference Books:
-Giannoccaro, Doronzo: elementi di Stechiometria, EdiSES;
-Del Zotto: Esercizi di Chimica Generale, Edises;
-Breschi, Massagli: "Stechiometria", Edizioni ETS;
-Michelin-Lausarot, Vaglio: "Fondamenti di stechiometria", Piccin;
-Uguzzoli: "Come risolvere i problemi di chimica", Casa Editrice Ambrosiana

The course aims at introducing the students of the main understanding of chemical phenomena, with details of applicative aspects. A supplementary noteworthy effort will be set on the chemical behavior of aqueous solutions and related chemical reactions, to establish the necessary basis for supplementary chemistry courses and related biological courses.

None

Classroom lessons in which the main topics reported in the abovementioned program will be disseminated. Course is hereafter completed by practical classroom exercises to tackle a few of the exposed topics.

Learning Control: Interactive discussion of the explained topics will be stimulated. Students will be involved in the shared resolution of applicative exercises, to strengthen their knowledge and test actual progresses.

The final exam is a 2-hour written test, containing questions of both general chemistry (6 questions, each with a maximum score of 2 points) and applied stoichiometry exercises (6 numerical exercises, each one with a maximum score of 3 points). The sum of the points must be at least 18 to pass the examination.

The matter: physical states, definition of matter (elements, compounds and mixtures). The atomic structure. Atoms and isotopes. Compounds and molecular representations (the laws of definite proportions and of multiple proportions). Atomic and molecular weights. Definition of a.m.u. Avogadro's Number and the concept of mole. Chemical reactions (oxidation numbers, balance of redox and non-redox reactions). The quanto-mechanical description of the atom (orbital concept, quantum numbers, the Aufbau principle). The Periodic Table and its correspondence with the electronic structure of elements. Periodic properties. The chemical bond: the octet rule, ionic bonds, covalent bonds in the theory of valence bond. Hybrid orbitals. The concept of resonance. Bond order and bond lengths, multiple bonds. Electronegativity, polarity of bonds and molecules. Intermolecular forces (ion-dipole, dipole-dipole, hydrogen bonds, induced dipoles, dispersion forces). The aggregation states of matter. Gas: definition and the law of perfect gases. Liquid and solid states. State changes (state diagrams). Solutions: concentrations and colligative properties. Thermodynamics: definitions, the principles of thermodynamics, enthalpy, entropy, free energy. Chemical kinetics: definitions and integrated kinetic laws (zero order, 1st and 2nd order), activation energy and the control of a reaction rate (Arrhenius' law), catalysts. Chemical reactions: the law of the action of masses and Le Chatelier principle, influence of experimental parameters on the chemical constants. Reactions in aqueous solutions. Autoprotonation of water and the pH, acid-base concepts, strong and weak acids and bases (classification and their strength, the structure of most important acids containing N, P, S and halogen elements), hydrolysis, buffer solutions. Products of solubility: definition and applications. Electrochemistry: standard potentials and Nernst's equation, galvanic and electrolitic cells, corrosion. Descriptive Chemistry: metals, semimetals and non-metals. Principal properties of these groups. Stoichiometry exercises related to these issues.

Knowledge of the fundamental aspects of the matter at the elementary and compositional level, of the chemical laws underlying the formation, geometry, stability and reactivity of compounds. Knowledge of the aspects that correlate the structure at the atomic and molecular level with the physical states and its transformations. Ability to describe and determine the fundamental features of the chemistry in aqueous solution (concentration, colligative properties, pH). Knowledge of the main aspects of the equilibrium and of the thermodynamic variables related to the energetic aspects and to the spontaneity of the reactions, and of the rate of the chemical reactions. Capability to apply stoichiometric calculations on ponderal ratios in reactions, on pH determination for strong and weak acid and basic solutions, salt hydrolysis and buffer solutions