• Introduction: Physical States of Matter, Homogeneous and Heterogeneous Systems. Chemical Substances and Elements.
• Atomic Structure of Matter: the law of mass conservation and Dalton’s Atomic Theory. Atomic properties. Nuclear Structure and Isotopes. Atomic weights. Chemical Symbols and their quantitative meaning.
• Names and formulas of chemical compounds: Molecular and ionic compounds.
• Chemical Reactions: writing and balancing chemical equations. Calculations involving chemical formulas and equations. Avogadro’s number, the mole concept. Determination of chemical formulas, Stoichiometry.
• Gas Phase: Gas pressure and its measurement. The gas laws and their experimental foundation. The ideal gas law. Gas mixtures and partial pressure. The kinetic-molecular theory. Molecular speed distribution, diffusion and effusion.
• Thermochemistry: Energy and its units. Heat and work. Enthalpy and heats of reaction. Thermochemical equations. Hess’s law
• Atomic Structure: First Models. Atomic spectra and their interpretation. The Bohr model of hydrogen atom. Principles of quantum theory: wave nature of electrons, de Broglie equation, the Heisemberg uncertainty principle. Atomic Orbitals and Quantum Numbers. Electron Spin and Pauli exclusion principle. Aufbau principle. Electron configurations of atoms. Hund’s rule. The periodic system of elements. Periodic trends of elements: Ionization Energy, Electron Affinity.
• Chemical bonding: Ionic bonding model, Electron configuration of ions. Covalent bonding model: properties, octet rule, Lewis dot structures. Delocalized bonds and resonance a dell'ottetto. Bond length, bond order and bond Energy. Valence-Shell Electron-Pair Repulsion Theory and molecular shape. Molecular Geometry and molecular polarity. Valence Bond Theory and Orbital Ibridization, resonance, multiple bonds. Examples (methane, boron fluoride, ethene). Magnetic properties of molecules. Molecular orbital theory: hydrogen molecule, molecular electron configuration ofdiatomic molecole, bond order.
• Phase changes: Equilibrium nature of phase changes. Liquid-gas equilibrium, Vapor pressure. Boiling point. Phase diagrams
• Liquids: Main properties of the liquid state, Intermolecular forces. Hydrogen bonding.
• The solid state: Structure, Properties and Bonding. Crystilline solids, Ionic solids, Molecular and covalent solids, Metals
• Solutions: Types of solutions, Solubility: effect of temperature and of pressure. Henry’s law. Quantitative ways to express concentration. Ideal solutions. Raoult’s law. Mixtures of totally miscible liquids: liquid-vapor equilibrium. Colligative properties: boiling point elevation, freezing point depression, osmotic pressure.
• Chemical Kinetics: Reaction Rates, Factors that influence reaction rate, The rate law. Collision Theory and Transition State Theory. Arrhenius equativo. Catalysis.
• Reactions and chemical equilibria: equilibrium state. Chemical equilibrium. Equilibrium constant. Heterogeneous equilibria. Reaction conditions and the equilibrium state: Le Chatelier’s principle. Effect of temperature on the equilibrium state: van’t Hoff equation.
• Acid-base equilibria: Acid and base definitions according to Arrhenius, Brønsted-Lowry and Lewis. Molecular structure and acid strength. Autoionization of water. Solution of strong acids or strong bases. The pH scale. Ionization equilibria of a weak acid or a weak base. Hydrolysis. Buffer solutions. Acid-base titrations. Acid-base indicators.
• Equilibria of slightly soluble ionic compounds. Solubility Product constant. The effect of a common ion on solubility. Precipitation. The effect of pH on solubility.
• Thermodynamics and Equilibrium: First principle of thermodynamics. Entropy and second principle of thermodynamics. Standard entropies and third principle of thermodynamics. Gibbs free energy and spontaneous reactions. Relationship between free energy and equilibrium constant.
• Redox reactions: oxidation states. Balancing redox reactions.
• Electrochemistry: electrical work from redox reactions. Voltaic cells. Cell potential and electromotive force. Standard cell potentials. Nernst equation. Types of Electrodes.. Concentration Cells.
• Electrolysis: Electrolysis of molten salts. Electrolysis of aqueous ionic solutions. The stoichiometry of electrolysis.
• Description of the chemical elements in main groups. Periodic chemical properties Structure and properties of compounds of main groups elements.• Introduction: Physical States of Matter, Homogeneous and Heterogeneous Systems. Chemical Substances and Elements.
• Atomic Structure of Matter: the law of mass conservation and Dalton’s Atomic Theory. Atomic properties. Nuclear Structure and Isotopes. Atomic weights. Chemical Symbols and their quantitative meaning.
• Names and formulas of chemical compounds: Molecular and ionic compounds.
• Chemical Reactions: writing and balancing chemical equations. Calculations involving chemical formulas and equations. Avogadro’s number, the mole concept. Determination of chemical formulas, Stoichiometry.
• Gas Phase: Gas pressure and its measurement. The gas laws and their experimental foundation. The ideal gas law. Gas mixtures and partial pressure. The kinetic-molecular theory. Molecular speed distribution, diffusion and effusion.
• Thermochemistry: Energy and its units. Heat and work. Enthalpy and heats of reaction. Thermochemical equations. Hess’s law
• Atomic Structure: First Models. Atomic spectra and their interpretation. The Bohr model of hydrogen atom. Principles of quantum theory: wave nature of electrons, de Broglie equation, the Heisemberg uncertainty principle. Atomic Orbitals and Quantum Numbers. Electron Spin and Pauli exclusion principle. Aufbau principle. Electron configurations of atoms. Hund’s rule. The periodic system of elements. Periodic trends of elements: Ionization Energy, Electron Affinity.
• Chemical bonding: Ionic bonding model, Electron configuration of ions. Covalent bonding model: properties, octet rule, Lewis dot structures. Delocalized bonds and resonance a dell'ottetto. Bond length, bond order and bond Energy. Valence-Shell Electron-Pair Repulsion Theory and molecular shape. Molecular Geometry and molecular polarity. Valence Bond Theory and Orbital Ibridization, resonance, multiple bonds. Examples (methane, boron fluoride, ethene). Magnetic properties of molecules. Molecular orbital theory: hydrogen molecule, molecular electron configuration ofdiatomic molecole, bond order.
• Phase changes: Equilibrium nature of phase changes. Liquid-gas equilibrium, Vapor pressure. Boiling point. Phase diagrams
• Liquids: Main properties of the liquid state, Intermolecular forces. Hydrogen bonding.
• The solid state: Structure, Properties and Bonding. Crystilline solids, Ionic solids, Molecular and covalent solids, Metals
• Solutions: Types of solutions, Solubility: effect of temperature and of pressure. Henry’s law. Quantitative ways to express concentration. Ideal solutions. Raoult’s law. Mixtures of totally miscible liquids: liquid-vapor equilibrium. Colligative properties: boiling point elevation, freezing point depression, osmotic pressure.
• Chemical Kinetics: Reaction Rates, Factors that influence reaction rate, The rate law. Collision Theory and Transition State Theory. Arrhenius equativo. Catalysis.
• Reactions and chemical equilibria: equilibrium state. Chemical equilibrium. Equilibrium constant. Heterogeneous equilibria. Reaction conditions and the equilibrium state: Le Chatelier’s principle. Effect of temperature on the equilibrium state: van’t Hoff equation.
• Acid-base equilibria: Acid and base definitions according to Arrhenius, Brønsted-Lowry and Lewis. Molecular structure and acid strength. Autoionization of water. Solution of strong acids or strong bases. The pH scale. Ionization equilibria of a weak acid or a weak base. Hydrolysis. Buffer solutions. Acid-base titrations. Acid-base indicators.
• Equilibria of slightly soluble ionic compounds. Solubility Product constant. The effect of a common ion on solubility. Precipitation. The effect of pH on solubility.
• Thermodynamics and Equilibrium: First principle of thermodynamics. Entropy and second principle of thermodynamics. Standard entropies and third principle of thermodynamics. Gibbs free energy and spontaneous reactions. Relationship between free energy and equilibrium constant.
• Redox reactions: oxidation states. Balancing redox reactions.
• Electrochemistry: electrical work from redox reactions. Voltaic cells. Cell potential and electromotive force. Standard cell potentials. Nernst equation. Types of Electrodes.. Concentration Cells.
• Electrolysis: Electrolysis of molten salts. Electrolysis of aqueous ionic solutions. The stoichiometry of electrolysis.
• Description of the chemical elements in main groups. Periodic chemical properties Structure and properties of compounds of main groups elements.
