• Introduction: States of aggregation of matter. Homogeneous and heterogeneous systems. Chemical substances and elements
• Atomic structure of matter: Atomic theory and laws of Lavoisier and Dalton. Properties of the atom. Nuclear structure and isotopes. Atomic weights. Chemical symbols and their quantitative meaning
• Nomenclature of the main chemical substances: Molecular and ionic chemical substances, chemical formulas of simple compounds.
• Chemical reactions: Writing and balancing of chemical reactions. • Calculations with chemical formulas and equations: Avogadro number, concept of mole. Determination of chemical formulas. Stoichiometry.
• The gaseous state: gaseous pressure and its measurement. Empirical laws of gases. Law of ideal gases. Gas mixtures and partial pressures. Overview of the kinetic theory of gases. Distribution of velocities, diffusion and effusion.
• Thermochemistry: Energy and unit of measurement. Reaction heat. Enthalpy and enthalpy variation. Thermochemical equations. Law of Hess.
• Atom structure: First models. Atomic spectra and their interpretation. Bohr model. Principles of quantum mechanics: wave nature of the electron, De Broglie's relation, indetermination principle. Quantum numbers and atomic orbitals. Electronic spin and Pauli exclusion principle. Principle of Aufbau. Electronic configuration of atoms. Hund rule. The periodic system of the elements. Periodic properties of the elements: ionization potential, electronic affinity.
• The chemical bond: Ionic bond. Electronic ion configurations. Covalent bond: general information, rule of the octet. Lewis formulas. Delocalized links and resonance. Distance, order and binding energy. Molecular geometry and dipolar moment. Theory of repulsion between electron pairs (VSEPR). Valence bond theory: hybrid orbitals, resonance, multiple bonds, examples (methane, boron trifluoride, ethylene). Magnetic properties of molecules. Molecular orbital theory: hydrogen molecule, electronic configurations of diatomic molecules, binding order.
• Phase transitions. Equilibrium between phases in one-component systems. Liquid-vapor equilibrium, vapor pressure. Boiling point. State diagrams.
• The liquid state: Main properties of liquids. Intermolecular forces. Hydrogen bond.
• Solid state: Crystalline structures. Molecular, covalent, ionic solids. Metallic solids.
• Solutions: Types of solutions. Solubility and factors that influence it. Henry's law. Concentration and its units. Ideal solutions. Raoult's law. Mixtures of totally miscible liquids: liquid-vapor equilibria. Colligative properties of solutions: cryoscopic lowering, ebullioscopic elevation, osmosis.
• Chemical kinetics: reaction speed. Dependency of the reaction rate from the concentration. Collision theory and activated status. Arrhenius equation. Activation energy. Catalysis.
• Chemical reactions and equilibria: reaction equations and their quantitative meaning. Classification of the different types of reaction. Chemical equilibrium. Balance constant. Heterogeneous equilibria. Balance shift: Le Chatelier's principle. Effect of temperature on equilibrium: Van't Hoff equation.
• Acid-base equilibria: Definitions of acids and bases according to Arrhenius, Brønsted and Lewis. Molecular structure and strength of acids. Ionisation of water. Solution of an acid or strong base. The pH of a solution. Equilibrium of ionization of an acid or a weak base. Hydrolysis. Buffer solutions. Acid-base titrations. Indicators
• Solubility equilibria: Solubility product. Effect of common ions. Precipitation criteria. Effect of pH on solubility.
• Thermodynamics and equilibrium: First principle of thermodynamics. Entropy and the second principle of thermodynamics. Standard entropies and the third law of thermodynamics. Free energy and spontaneity. Relationship between free energy and equilibrium constants
• Oxidoreduction Reactions: Oxidation numbers. Balancing of redox reactions.
• Electrochemistry: Electrical work by redox reactions. Batteries and their electromotive force. Normal potentials and their meaning. Nernst's equation. Common types of electrodes. Concentration batteries.
• Electrolysis: Electrolysis of molten salts. Solutions electrolysis. Stoichiometry of electrolysis.
• Description of the elements of the main groups: Periodic chemical properties. Structure, properties and nomenclature of the main compounds of the elements of the blocks s and p.
