Portale di Ateneo - En.Unibs.it

Fundamentals and Reaction stoichiometry
Introduction. Atoms, ions, molecules. Atomic and molecular interactions. The aggregation states of matter. Chemical and physical transformations.
Chemical formulas. Chemical reactions, law of conservation of mass. Main chemical reactions. Atomic mass and molecular mass. The mole. Concentration expression for solutions. Unit of measurement. Fundamentals of error theory and significant digits.

The property of gases
Temperature and pressure. Ideal gases: the ideal gas law, the Dalton law of partial pressures, the kinetic model, the Maxwell-Boltzman distribution of speeds, interpretation of the gas laws through the kinetic model. The real gases: compression factor and the Van der Waals equation.

Atomic structure and periodic properties
Historic introduction. Atomic models. Bohr model. Energy quanta: the photoelectric effect, emission spectra of atoms. Wave-Particle duality. Fundamentals of quantum mechanics. Quantum-mechanic model. Electron orbitals. Aufbau principle and the electronic configuration of elements. Periodic table. Periodic properties of elements: ionization energy, atomic radius, mean energy of valence electrons.

Chemical Bonds
The three models for the chemical bond. Lewis theory. The ionic bond. The covalent bond. Polar covalent bonds. Electron affinity. Formal charge, partial charge, oxidation number. The VSEPR model for molecular geometry. Molecular polarity. Valence bond theory. Fundamentals of molecular orbitals theory.

Cohesion and structure
Intermolecular forces: Van der Waals forces, Hydrogen bonding. Phase changes. Connections between interaction forces and boiling (melting). Phase diagrams. Solid state properties and connection between structure and mechanical properties of solids. Liquid state: definition, surface tension, viscosity, vapor pressure. Amorphous solids and liquid crystals. Solutions. Solubility. Electrolytic solutions. Colligative properties: Raoult law, freezing-point depression and boiling point elevation, osmosis.

Chemical Thermodynamics
First and second thermodynamics laws. Calorimetry: thermal capacity, specific heat. State properties: enthalpy. Standard enthalpy of reaction. Hess’s laws. Thermal yield of reactions.

Kinetics and chemical equilibria
Reaction rate and collision theory. The equilibrium constant for reaction in solutions and in gas phase. The reaction quotient. Le Chatelier’s Principle.

Acids and Bases
Arrhenius and Bronsted-Lowry definitions of acids and bases. The strength of acids and bases. Ionization grades. Connection between strength and molecular structure of acids and bases. Polyprotic acids. Amphoteric substances. Amphiprotic solvents. Autoprotolysis of water. pH, pOH e pK scales. pH calculation for: monoprotic strong acids, monoprotic weak acids and polyprotic acids (diluted and very diluted). Experimental measurement of pH through indicators. Saline hydrolysis. Buffer solutions. Acid/base titration. Acid rain.

Electrochemistry
Redox equations. Voltaic cell and Daniell pile. The electrochemical potential. The electrochemical series. Standard cell potential. Nerst equation. Pb/acid cells. Fuel cells. Corrosion. Electrolytic cell. Faraday’s Law.