Learning objectives
The goal of the course is to provide a solid knowledge of the fundamental principles of chemistry and to develope in the students critical abilities through the solution of exercises.
Prerequisites
The module starts from the basic concepts of General Chemistry, although basic knowledge of General and Inorganic Chemistry can help for a faster assimilation.
Course unit content
Elementary substances and chemical compounds. Periodic Table. Chemical symbols of the elements. Chemical phenomena and physical phenomena. Chemically homogeneous and heterogeneous systems. The mixtures. Dalton's atomic theory. The atom as the fundamental unit of matter, through which chemical transformations occur. Lavoisier's law. The definition of mass and weight. The principle of Avogadro. Mass and atomic weight. The scale of atomic weights. Molecular Weight. Canizzaro rule. Chemical formulas: quality and quantity information. Atomic mass units. Chemical symbols and formulas. Fundamental subatomic particles: proton, neutron and electron. Atomic number (Z) and mass number.
Definition and application of oxidation number. The oxidation numbers of the elements. Nomenclature of inorganic compounds: oxides and hydroxides. Preparation of hydroxides. The peroxides, basic oxides and anhydrides. IUPAC nomenclature, Stock and traditional for oxides, hydroxides and anhydrides. Acids and hydracids (IUPAC and traditional nomenclature) and oxoacids (traditional nomenclature). The salts and the reactions of salification: reactions of simple exchange and double exchange.
Rules for balancing redox and not redox reactions. Acidic and Basic substances. Equations: molecular and ionic equations.
Structure: electrical nature of matter, particle nature of electricity. Atomic model of Thomson and Rutherford. Isotopes and isobars. Elettromegnetica radiation. Planck Theory. Bohr atom. Dualism of wave - particle (De Broglie). Uncertainty principle of Heisenberg. Wave mechanics. Atomic orbitals and quantum numbers. Polyelectronic atoms. Aufbau: Hund's Rule and the Pauli exclusion principle. Periodic Table. Periodic properties: first ionization energy and electron affinity. Electronegativity. Metals and non-metals.
The chemical bond. Ionic and covalent bonding. Lewis theory. Octet rule. Expansion of the sphere of valence. Polar and non-polar covalent bond. Dative covalent bond. Calculation of the percentage of ionic character of a bond. Molecular geometry. VB theory or valence bond. Hybridization (e.g. carbon: sp3, sp2, sp). Weak bonds. Van der Waals forces: dipole-dipole forces, dipole forces - induced dipole, dipole forces instant - instant dipole. Hydrogen bond. Paramagnetic and diamagnetic molecules.
States of matter. Gaseous state. Equation of state of an ideal gas. Ideal gas laws: Boyle's law, Gay-Lussac I °, II ° Gay-Lussac, the Law of Dalton on gas mixtures. Real gases. Liquid state: Properties. Surface tension, evaporation, vapor pressure, boiling point. Changes of state. The solutions: dilute and concentrated. Ways to express the composition of a solution (% weight / weight; % weight / volume; % volume / volume; molarity, molality, ppm; ppb; molar fraction). Density of a solution. Dissolution of a solid ion in water. Solubility. Factors affecting solubility.
Ideal solutions. Raoult's law. Colligative properties of solutions. Strong electrolytes and weak electrolytes. Osmotic pressure. Colligative properties of electrolyte solutions. Solid state: crystalline solids and amorphous solids. Polymorphism and isomorphism. Comparison between diamond and graphite. Types of chemical transformations. Chemical equilibrium: the equilibrium constant. Mobile principle of balance.
Effect of change of temperature on the equilibrium constant. Factors affecting the position of equilibrium. Heterogeneous equilibria and solubility equilibria (solubility product constant). Acids and bases: Arrhenius theory, theory of Bronsred-Lowry, Lewis theory. The strength of acids and bases. Leveling effect of the water. Henderson-Hasselbach equation. The ionic product of water. The pH of a solution. Indicators. The pH measurement. pH values for some solutions. Buffer solutions. Hydrolysis. Conjugate acid-base pair. Relationship between Ka, Kb, Kw a pair acid conjugate base. Electrochemistry: electrolytic and galvanic cells. Total electromotive force: the electrode potential. Electrochemical series of the elements. Kinetics. Reaction rate. Factors affecting the rate of a reaction. Collision theory. Activation energy. Effect of temperature on the rate of a reaction. Catalysts, enzyme catalysis.
EXERCISES
Nomenclature of inorganic compounds.
Reactions for the preparation of Salts, Acids and Hydroxides.
Stoichiometry and limiting reagent.
Ground state electronic configurations of the atoms of the elements.
Balancing redox reactions in molecular and ionic form.
Concentrations of the solutions; density of the solutions; dilutions of the solutions. Relations between solubility Salts and Kps.
pH and pOH of strong acids and weak.
Full programme
Elementary substances and chemical compounds. Periodic Table. Chemical symbols of the elements. Chemical phenomena and physical phenomena. Chemically homogeneous and heterogeneous systems. The mixtures. Dalton's atomic theory. The atom as the fundamental unit of matter, through which chemical transformations occur. Lavoisier's law. The definition of mass and weight. The principle of Avogadro. Mass and atomic weight. The scale of atomic weights. Molecular Weight. Canizzaro rule. Chemical formulas: quality and quantity information. Atomic mass units. Chemical symbols and formulas. Fundamental subatomic particles: proton, neutron and electron. Atomic number (Z) and mass number.
Definition and application of oxidation number. The oxidation numbers of the elements. Nomenclature of inorganic compounds: oxides and hydroxides. Preparation of hydroxides. The peroxides, basic oxides and anhydrides. IUPAC nomenclature, Stock and traditional for oxides, hydroxides and anhydrides. Acids and hydracids (IUPAC and traditional nomenclature) and oxoacids (traditional nomenclature). The salts and the reactions of salification: reactions of simple exchange and double exchange.
Rules for balancing redox and not redox reactions. Acidic and Basic substances. Equations: molecular and ionic equations.
Structure: electrical nature of matter, particle nature of electricity. Atomic model of Thomson and Rutherford. Isotopes and isobars. Elettromegnetica radiation. Planck Theory. Bohr atom. Dualism of wave - particle (De Broglie). Uncertainty principle of Heisenberg. Wave mechanics. Atomic orbitals and quantum numbers. Polyelectronic atoms. Aufbau: Hund's Rule and the Pauli exclusion principle. Periodic Table. Periodic properties: first ionization energy and electron affinity. Electronegativity. Metals and non-metals.
The chemical bond. Ionic and covalent bonding. Lewis theory. Octet rule. Expansion of the sphere of valence. Polar and non-polar covalent bond. Dative covalent bond. Calculation of the percentage of ionic character of a bond. Molecular geometry. VB theory or valence bond. Hybridization (e.g. carbon: sp3, sp2, sp). Weak bonds. Van der Waals forces: dipole-dipole forces, dipole forces - induced dipole, dipole forces instant - instant dipole. Hydrogen bond. Paramagnetic and diamagnetic molecules.
States of matter. Gaseous state. Equation of state of an ideal gas. Ideal gas laws: Boyle's law, Gay-Lussac I °, II ° Gay-Lussac, the Law of Dalton on gas mixtures. Real gases. Liquid state: Properties. Surface tension, evaporation, vapor pressure, boiling point. Changes of state. The solutions: dilute and concentrated. Ways to express the composition of a solution (% weight / weight; % weight / volume; % volume / volume; molarity, molality, ppm; ppb; molar fraction). Density of a solution. Dissolution of a solid ion in water. Solubility. Factors affecting solubility.
Ideal solutions. Raoult's law. Colligative properties of solutions. Strong electrolytes and weak electrolytes. Osmotic pressure. Colligative properties of electrolyte solutions. Solid state: crystalline solids and amorphous solids. Polymorphism and isomorphism. Comparison between diamond and graphite. Types of chemical transformations. Chemical equilibrium: the equilibrium constant. Mobile principle of balance.
Effect of change of temperature on the equilibrium constant. Factors affecting the position of equilibrium. Heterogeneous equilibria and solubility equilibria (solubility product constant). Acids and bases: Arrhenius theory, theory of Bronsred-Lowry, Lewis theory. The strength of acids and bases. Leveling effect of the water. Henderson-Hasselbach equation. The ionic product of water. The pH of a solution. Indicators. The pH measurement. pH values for some solutions. Buffer solutions. Hydrolysis. Conjugate acid-base pair. Relationship between Ka, Kb, Kw a pair acid conjugate base. Electrochemistry: electrolytic and galvanic cells. Total electromotive force: the electrode potential. Electrochemical series of the elements. Kinetics. Reaction rate. Factors affecting the rate of a reaction. Collision theory. Activation energy. Effect of temperature on the rate of a reaction. Catalysts, enzyme catalysis.
EXERCISES
Nomenclature of inorganic compounds.
Reactions for the preparation of Salts, Acids and Hydroxides.
Stoichiometry and limiting reagent.
Ground state electronic configurations of the atoms of the elements.
Balancing redox reactions in molecular and ionic form.
Concentrations of the solutions; density of the solutions; dilutions of the solutions. Relations between solubility Salts and Kps.
pH and pOH of strong acids and weak.
Bibliography
Franco Ugozzoli, LEZIONI DI CHIMICA, Edizioni Santa Croce.
Teaching methods
Classroom lectures
Assessment methods and criteria
Oral with written exercises
Other information
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2030 agenda goals for sustainable development
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