Atomic structure of the matter. Physics of the atoms. Chemical bond. Intermolecular interactions and properties of matter. Properties of gases, liquids and solids. Phase equilibria. Solutions. Chemical reactions. Chemical equilibrium. Termodynamics. Acid-base equilibria. Electrochemistry. Kinetics. Introduction to inorganic chemistry.
Course Content - Last names M-Z
Atomic structure of the matter. Physics of the atoms. Chemical bond. Intermolecular interactions and properties of matter. Properties of gases, liquids and solids. Phase equilibria. Solutions. Chemical reactions. Chemical equilibrium. Termodynamics. Acid-base equilibria. Electrochemistry. Kinetics. Introduction to inorganic chemistry.
Textbooks:
I. Bertini, C. Luchinat, F. Mani. Chimica. Casa Editrice Ambrosiana.
I. Bertini, C. Luchinat, F. Mani. Stechiometria. Casa Editrice Ambrosiana.
P. Atkins, L. Jones. Principi di Chimica. Zanichelli.
Textbooks:
I. Bertini, C. Luchinat, F. Mani. Chimica. Casa Editrice Ambrosiana.
I. Bertini, C. Luchinat, F. Mani. Stechiometria. Casa Editrice Ambrosiana.
P. Atkins, L. Jones. Principi di Chimica. Zanichelli.
Prerequisites - Last names A-L
Courses required: none
Courses recommmended: none
Prerequisites - Last names M-Z
none
Teaching Methods - Last names A-L
Total hours of the course (including the time spent in attending lectures, seminars, private study, examinations, etc...): 225
Hours reserved to private study and other indivual formative activities:
Contact hours for: Lectures (hours): 72
Contact hours for: Laboratory (hours): 0
Contact hours for: Laboratory-field/practice (hours): 0
Seminars (hours): 0
Stages: 0
Intermediate examinations: 0
Teaching Methods - Last names M-Z
CFU: 9
Total hours of the course (including the time spent in attending lectures, seminars, private study, examinations, etc...): 225
Hours reserved to private study and other indivual formative activities:
Contact hours for: Lectures (hours): 72
Contact hours for: Laboratory (hours): 0
Contact hours for: Laboratory-field/practice (hours): 0
Further information - Last names A-L
Office hours:
Thursday from 14 to 17 p.m.
Further information - Last names M-Z
Office hours:
Thursday from 14 to 17 p.m.
Type of Assessment - Last names A-L
Exam modality: written test
Type of Assessment - Last names M-Z
written test
Course program - Last names A-L
Course Contents (detailed programme):
Chemistry as an experimental scienze. Matter and its parameters. Phases. Components. Separation of components of an omogeneous system. Elements and compounds. Matter and energy. Law of conservation of energy and matter. Atoms. Subatomic particles. Atomic mass scale. Avogadro’s number. Radioactivity. Mass defect. Wave mechanics, Electron configurations and the periodic table. Electron affinity. Ionization energy. Chemical formulae. Ionic compounds. Lattice energy. Ionic radius. Covalent bond. Length and energy bond. Biatomic molecules. Sigma and p greek bonds. Polyatomic molecules. Valence shell electron pair repulsion theory. Octet rule. Lewis structures. Molecules with different geometry. Hybrid orbitals. Polar bonds. Electronegativity. Resonance. Intermolecular attractions and the properties of gas, liquids and solids. Dipole dipole attractions. Hydrogen bond. London forces. Parameters for the gases. Relationships between pressure, volume and temperature for a fixed amount of gas. The ideal gas law. Avogadro’s principle. Real gases: deviation from the ideal gas law. Van der Waals equation. Crystalline solids. Crystal lattices and unit cell. Molecular crystal, Covalent crystals and metallic crystals. Noncryastalline solids. Properties of liquids. Energy, internal energy of a system. Work and heat. The first law of thermodynamics. State functions. Hentalpy. Entropy. The second law of thermodynamics. The third principle of thermodynamics. The Gibbs free energy. Variation of free energy in chemical transformations. Changes of state and dynamic equilibrium. Vapor pressure. Solutions. Concentration units. Colligative properties. Raoult’s law. Freezing point depression and boiling point elevation. Osmotic pressure. Electrolytic dissociation. Colloidal solutions. Chemical equilibrium. Effects of temperature and pressure on the equilibrium. Le Chatelier principle. Thermodynamics of the equilibrium. Free energy and equilibrium constant. Heterogeneous equilibria. Solubility product constant. Rates of reactions. Factors that affect reaction rates. First and second order reactions. Theory of reaction rates. Collision theory and reaction mechanisms. Activation energy. Catalysis. Enzymes. Water dissociation. pH. Bronsted concept of acids and bases. Buffer solutions. Acid base titration. Acid base indicators. Lewis theory of acids and bases. Coordination compounds. Red ox reactions. Galvanic cells. Cell potentials and reduction potentials. Using standard reduction potentials. Hydrogen cell. The effect of concentration on cell potential. Potentiometric measurement of pH. Standard electrods. Electrolysis of fused salts and water solutions. Nomenclature od inorganic compounds. Chemical properties of hydrides and oxydes. Introduction to the chemical properties of the lighter elements of I, II, IV, V, VI and VII groups. General properties of the first transiton elements.
Course program - Last names M-Z
Course Contents (detailed programme):
Chemistry as an experimental scienze. Matter and its parameters. Phases. Components. Separation of components of an omogeneous system. Elements and compounds. Matter and energy. Law of conservation of energy and matter. Atoms. Subatomic particles. Atomic mass scale. Avogadro’s number. Radioactivity. Mass defect. Wave mechanics, Electron configurations and the periodic table. Electron affinity. Ionization energy. Chemical formulae. Ionic compounds. Lattice energy. Ionic radius. Covalent bond. Length and energy bond. Biatomic molecules. Sigma and p greek bonds. Polyatomic molecules. Valence shell electron pair repulsion theory. Octet rule. Lewis structures. Molecules with different geometry. Hybrid orbitals. Polar bonds. Electronegativity. Resonance. Intermolecular attractions and the properties of gas, liquids and solids. Dipole dipole attractions. Hydrogen bond. London forces. Parameters for the gases. Relationships between pressure, volume and temperature for a fixed amount of gas. The ideal gas law. Avogadro’s principle. Real gases: deviation from the ideal gas law. Van der Waals equation. Crystalline solids. Crystal lattices and unit cell. Molecular crystal, Covalent crystals and metallic crystals. Noncryastalline solids. Properties of liquids. Energy, internal energy of a system. Work and heat. The first law of thermodynamics. State functions. Hentalpy. Entropy. The second law of thermodynamics. The third principle of thermodynamics. The Gibbs free energy. Variation of free energy in chemical transformations. Changes of state and dynamic equilibrium. Vapor pressure. Solutions. Concentration units. Colligative properties. Raoult’s law. Freezing point depression and boiling point elevation. Osmotic pressure. Electrolytic dissociation. Colloidal solutions. Chemical equilibrium. Effects of temperature and pressure on the equilibrium. Le Chatelier principle. Thermodynamics of the equilibrium. Free energy and equilibrium constant. Heterogeneous equilibria. Solubility product constant. Rates of reactions. Factors that affect reaction rates. First and second order reactions. Theory of reaction rates. Collision theory and reaction mechanisms. Activation energy. Catalysis. Enzymes. Water dissociation. pH. Bronsted concept of acids and bases. Buffer solutions. Acid base titration. Acid base indicators. Lewis theory of acids and bases. Coordination compounds. Red ox reactions. Galvanic cells. Cell potentials and reduction potentials. Using standard reduction potentials. Hydrogen cell. The effect of concentration on cell potential. Potentiometric measurement of pH. Standard electrods. Electrolysis of fused salts and water solutions. Nomenclature od inorganic compounds. Chemical properties of hydrides and oxydes. Introduction to the chemical properties of the lighter elements of I, II, IV, V, VI and VII groups. General properties of the first transiton elements.