Introduction
Aggregation states of matter. Homogeneous and heterogeneous systems. Compounds and chemical elements. Separation techniques (filtration, centrifugation, distillation). Physical and chemical changes. Energy and chemical changes. Intensive and extensive properties of matter. Atomic structure: protons, electrons and neutrons. Atomic number and mass number: isotopes. Atomic mass and relative atomic mass. Symbols of chemical elements. Molecular compounds and ionic compounds. Relative molecular mass. Mole and Avogadro’s number.

Atomic structure
The Bohr model of the hydrogen atom. Atomic spectra. De Broglie and the wave nature of matter The Heisenberg indeterminacy principle. Particle-wave duality. Atomic orbitals. Quantum numbers. The Pauli exclusion principle. Electron configuration of the elements: aufbau principle. The periodic system of the elements. Periodic properties.

Chemical Bond
Ionic and covalent bond. Bond properties: order, energy and length. Electronegativity and dipole moment of molecules. Lewis structures. The VSEPR model and the shape of molecules. Theories of chemical bonding: hybridization of atomic orbitals, resonance theory in chemistry. Magnetic properties of molecules. Intermolecular forces. Hydrogen bonding.

Chemical Formulas
Nomenclature of inorganic compounds. Oxidation number. Oxidation-reduction reactions.

The gaseous state
The ideal gas law. Dalton’s law and mixtures of gases. The density of gases. Relative density of gas and mixture of gases. The average molecular mass of a mixture of gases. Real gases; the Van der Waals equation of real gases. Boyle’s temperature. The critical state of gases.

The solid state
Crystal lattices and unit cells. Molecular, ionic and covalent solids. Metals. Allotropy and polymorphism. Molecular orbital theory. The band theory of solids: metals, semiconductors and insulators. Doped semiconductors: n and p-type semiconductors.

The liquid state
Surface tension of liquids. Viscosity. Vapor pressure. Thermotropic and lyotropic liquid crystals: properties and technological applications.

Thermodynamics
Thermodynamic system. State functions. Cyclic and non-cyclic processes. Reversible and irreversible processes. Heat, work and internal energy. The first law of thermodynamics. Enthalpy and Hess’s law. Entropy. The second law of thermodynamics. Spontaneous processes. Free energy. The third law of thermodynamics.

Physical equilibria
Phase transitions: Clapeyron and Claussius-Clapeyron equations. Phase diagram of water and carbon dioxide.

Solutions
Units of concentration. Solubility and dissolution processes. Solutions of gases in liquids. Entalpy of solution and the effect of the temperature on solubility. Ideal and real solutions. Roult’s law. Colligative properties of ideal solutions. Colligative properties and molar mass determination. Miscible, immiscible and partially miscible liquids.

Chemical Equilibrium
Spontaneous processes and thermodynamic equilibrium in chemical reactions. Law of mass action. The equilibrium constant. van't Hoff equations: isotherm and isochore equation. Equilibri omogenei. Le Chathelier’s principle. Effect of the addition or removal of a reagent or product. Effect of volume, pressure and temperature changes on the homogeneous equilibria. Heterogeneous equilibria.

Electrolytic solutions
Arrhenius theory of electrolytic dissociation. Ions and molecules in aqueous solutions: strong electrolytes and weak electrolytes. Colligative properties of solutions containing ions: van't Hoff factor.

Chimical equilibria in solutions
Acid-base equilibria. Classifications of acids and bases (Arrhenius, Broensted-Lowry, Lewis). Acid and base strength: the ionization constant. Molecular structure and acid strength. Autoionization of water. The pH scale. Calculation of pH of a strong/weak acid/base solutions. Acid-base properties of salt solutions. Buffer solutions. Solubility of salts and the solubility product constant.

Chemical Kinetics
Rates of chemical reactions. Rate laws and integrated rate laws. Order of chemical reactions The Arrhenius equation and the temperature dependence of reaction rate. Activation energy. Collision theory and transition state theory of chemical reactions. Reaction mechanisms, molecularity of a chemical reaction. Catalysis.

Electrochemistry
Semielement potential and the Nernst equation. Standard reduction potentials. Electrochemical cells: chemical cells and concentration cells. Electrolysis: Faraday’s laws. Application: storage battery and corrosion.

Stoichiometry: Mole. Empirical and molecular formulas. Chemical equations and mass relationships in chemical reactions. Limiting reactant. Gas law and chemical reactions. Quantitative analysis of a mixture. Solutions and volumetric analysis. Gas-phase equilibium; homogeneous and heterogeneous equilibria. Thermochemistry and thermodynamics of chemical reactions. Colligative properties of solutions. Calculation of pH of aqueous solutions: strong/weak acid and base solutions, salt solutions and buffer solutions. Electrochemistry: Electrochemical cells and cell potential.

1) M. Casarin, L. Casella, R. D'Agostino, A. Filippi, F. Grandinetti, R. Purrello, N. Re, M. Speranza, "Chimica Generale e Inorganica", Edi Ermes
2) M. Silberberg, P. Amateis "Chimica", McGraw-Hill 4 Ed.
3) T. L. Brown, H. E. LeMay, B. E. Bursten, C. J. Murphy, P. M. Woodward, M. W. Stoltzfus “Fondamenti di Chimica”, IV Edizione, Ed. Edises
4) P. Atkins, L. Jones "Principi di Chimica", Ed. Zanichelli

Stechiometria:
F. Cacace, M. Schiavello, "Stechiometria", ed Bulzoni.
I. Bertini, F. Mani, C. Luchinat "Stechiometria" ed. CEA