GENERAL AND INORGANIC CHEMISTRY A - L

The goal of the course is to provide the general basics of chemistry as well as the understanding of issues related to it and developed in other teachings of the Degree Course.

Lectures and practical exercises

Course Content

1) Introduction - The 4 fundamental forces, matter and energy, states of aggregation of matter *, homogeneous and heterogeneous systems, the scientific method, elements *, compounds * and mixtures *.

2) Chemistry laws - Law of conservation of mass (Lavosier) *, law of definite proportions (Proust) *, atomic theory of Dalton, law of multiple proportions (Dalton) *, law of Avogadro *, generalities on atom, atomic number * and mass number *, isotopes *, mass defect, uma *, atomic mass *, molecular mass *, mole *, minimum formula *, molecular formula *, structural formula, isomers, percentages by weight.

3) Matter structure - Rutherford atomic model, Bohr-Sommerfield theory, quantum numbers *, wave mechanical model, atomic orbitals *, Pauli principle *, Hund rule *, Heisenberg uncertainty principle, ideal construction of atoms *.

4) Periodic system - periodicity and electron configurations *, ionization potential *, electron affinity *, electronegativity *, atomic radii.

5) Chemical bond* - Binding energy, ionic bond, covalent bond, dative bond, hydrogen bond, Lewis structures, valence, formal charge, valence bond theory, hybridization, resonance.

6) Chemical nomenclature* - Elements and their representation, valence and oxidation number, chemical reactions, representations and balancing, redox reactions and their balancing.

7) Thermodynamics - State functions*, first principle *, law of Hess, second principle *, entropy and disorder, free energy *.

8) The gaseous state - Partial pressures *, Dalton's law *, law of ideal gas *, real gas.

9) The liquid state - Properties, viscosity, surface tension, vapor pressure*.

10) Phase transitions - Phase diagram of H₂O* and CO₂.

11) Solutions* - Molarity, normality, molar fraction, molality, mass percentage, density, vapor pressure, Raoult's law, colligative properties, electrolytes, degree of dissociation, Van't Hoff coefficient.

12) Chemical equilibrium* - Law of mass action, equilibrium constant, relation between Kp and Kc, dependence of equilibrium constant on temperature, factors influencing equilibrium, relation between equilibrium constant and degree of dissociation.

13) Acids and bases* - Arrhenius acids a bases definition, Bronsted and Lowry acids a bases definition, Lewis acids a bases definition, strength of acids and bases, dissociation constant, amphoteric electrolytes, ionic product of water, pH calculations of acids and bases (strong and weak), pH indicators.

14) Salt hydrolysis - Hydrolysis constant, hydrolysis pH *, buffer solutions *, strong base strong acid titrations *, strong base weak acid titrations *, solubility product *, common ion effect on solubility.

15) Overview of Electrochemistry - cells and batteries, series of potential redox.

16) Overview of kinetics - Order and molecularity reaction, reaction rate.

17) Inorganic chemistry - Chemistry of the main elements from the first to the seventh group *, general properties of the groups and periods *, chemical-physical properties of the main elements and their most important compounds.

* indispensable topics for passing the exam

General and Inorganic Chemistry Books

1. Fondamenti di chimica P. Silvestroni, CEA
2. J.C. Kotz, P.M. Treichel, J.R. Townsed - Chimica
3. P.W. Atkins, L. Jones - Chimica Generale – Zanichelli
4. Lesson notes

Inorganic Chemistry

1. I. Bertini,C. Luchinat, F. Mani - Chimica Inorganica - Ambrosiana, (distribuzione Zanichelli)

Stoichiometry

1. P. M. Lausarot, G.A. Vaglio - Stechiometria Guida alla soluzione di problemi di chimica- Piccin

7. Exercises in class

Deepening books

8. P. Chiorboli, Fondamenti di Chimica, Brossura, UTET