KNOWLEDGE AND UNDERSTANDING: Know and describe the atomic system. Describe the basis of the periodic system of elements. Know the naming conventions for the main inorganic compounds. Understand the concept of mole. Understand and describe atomic bonds forming molecules, the forces involved in their formation and their geometry. Understand chemical reactions and their description by chemical
equations. Understand and describe the gas phase, correlating physical and chemical quantities required to describe the system. Describe a system from the energetic point of view, using concepts of free energy, enthalpy and entropy. Know the basic concept about kinetics of reactions: reaction rate and activation energy. Understand the concept of chemical equilibrium. Know and understand Le Chatellier's principle and its application to chemical equilibria. Describe solutions and their properties. Understand the equilibria between chemical species in a solution. Know the concepts of pH, neutralization and buffer solution. Understand acid and basic hydrolysis equilibria and their relation. Know
the concept of solubility and ionic product applied to insoluble salts. Understand basic concepts of electrochemistry.
APPLYING KNOWLEDGE AND UNDERSTANDING: Describe a system from the chemical and physical point of view. Use concepts of mole and molar mass to solve stoichiometry exercises. Predict molecular geometry of the most common compounds. Balance chemical reactions, including simple redox reactions. Apply stoichiometry calculations to simple chemical systems. Solve exercises on quantities that describe a gas phase system.
Calculate chemical quantities that describe an equilibrium, applying the law of mass action. Predict the effects of external changes on an
equilibrium, considering Le Chatellier's principle. Calculate the pH of simple solutions of acids and bases. Determine the solubility of a salt from its ionic product.
MAKING JUDGMENTS: Identify strategies to solve simple chemical problems, applying concepts studied during the course. Acquire the ability to identify chemical reactions that can occur and the effects on the system of external changes. Considering the theory studied, understand the potential dangers connected with the use of chemicals and the precautions to apply in order to manage the risks.
COMMUNICATION SKILLS: Fully describe a chemical system using appropriate physical and chemical quantities and the specific terminology acquired during the course. Identify and describe energetic relations that determine the spontaneity and the outcome of a chemical process.
LEARNING SKILLS: Identify the possible sources to deepen the knowledge of the curriculum of the course. Acquire the ability of consult a chemical textbook, owning the basic ideas necessary to understand more complex concepts. Acquire the conceptual framework and the terminology helpful
for the continuation of the academic career of the student and its application in the professional field.

Basic mathematics. Basic physics. Concepts of mass and pressure.

Introduction: substances, elements and chemical compounds. Chemical formulae, phases, heterogeneous and homogeneous systems. Atomic
theory of matter. Atom and subatomic particles. Atomic number and mass number. Isotopes. Molecular mass. Periodic system. Electronegativity. Periodic properties of elements.Mole. Avogadro's constant. Molar mass. Isotopic abundance. Chemical bonds. Covalent bonds and ionic bonds. Dipole. Intermolecular forces. Hydrogen bonds. Oxidation number. Inorganic nomenclature: binary compounds and ternary compounds. Percentage composition. Chemical reactions. Chemical equations and stoichiometric coefficients. Redox reactions and stoichiometric coefficients. Ionic dissociation. Strong and weak electrolytes. Stoichiometry. Limiting reactant. Yield of a reaction. Gas phase. Pressure. Boyle's law, Charles' law, Gay-Lussac's law. Avogadro's law. Ideal gas and ideal gas law. Dalton's law. Gas mixtures. Partial pressure and volume. Non-ideal gas. Phase transitions. Phase diagram. Thermodynamics. Entropy and enthalpy. Reaction free energy. Exothermic and endothermic reactions. Exoergonic and endoergonic
reactions. Reaction rate. Activation energy. Gas phase reactions. Kc and Kp. Le Chatelier's principle. Effects of volume change, temperature change and pressure change on equilibrium. Solutions. Concentration measurement, molarity and molality. Dilutions. Colligative properties. Reactions in solution. Strong acids and bases. Weak acids and bases and equilibrium. Ionic product of water. pH, pKa and pKb. Titrations. Hydrolysis equilibrium.
Buffer solutions. Solubility. Saturated solution and unsolubilized residue. Soluble and insoluble salts. Solubility product. Effect of common ions and of pH on solubility equilibria. Electrochemistry. Electrochemical cell and half-cell. Nernst's equation. Electrolysis. Mode of operation of a pH-meter

Suggested textbooks:
- E. Santaniello, M. Coletta, F. Malatesta, G. Zanotti, S. Marini Chimica propedeutica alle scienze bio-mediche - Piccin.
- P. Michelin; Lausarot, G. A. Vaglio – Stechiometria per la Chimica generale – Piccin.
- Massimo Stefani, Niccolò Taddei, Chimica & Biochimica, 2017 (Zanichelli)
The slides of the each lecture will be available after each lecture itself.

- Introduction: substances, elements and chemical compounds. Chemical formulae, phases, heterogeneous and homogeneous systems.
- Atomic theory of matter. Atom, electron, proton, neutron, nucleus. Atomic number and mass number. Isotopes. Atomic mass units. Formulae and molecular mass.
- Mole. Avogadro's constant. Molar mass. Isotopic abundance.
- Periodic system. Electronegativity. Periodic properties of elements.
- Chemical bonds. Covalent bonds, ionic bonds, coordination bonds. Dipole. Intermolecular forces. Hydrogen bonds.
- Oxidation number. Inorganic nomenclature: binary compounds and ternary compounds. Percentage composition.
- Chemical reactions. Chemical equations and stoichiometric coefficients. Redox reactions and stoichiometric coefficients. Ionic dissociation. Strong and weak electrolytes. Stoichiometry. Limiting reactant. Yield of a reaction.
- Gas phase. Pressure. Boyle's law, Charles' law, Gay-Lussac's law. Avogadro's law. Ideal gas and ideal gas law. Dalton's law. Gas mixtures. Partial pressure and volume. Non-ideal gas. Phase transitions. Phase diagram.
- Thermodynamics. Entropy and enthalpy. Reaction free energy. Exothermic and endothermic reactions. Exoergic and endoergic reactions. Activation energy.
- Gas phase reactions. Kc and Kp. Le Chatelier's principle. Effects of volume change, temperature change and pressure change on equilibrium.
- Solutions. Concentration measurement, molarity and molality. Dilutions. Colligative properties.
- Reactions in solution. Strong acids and bases. Weak acids and bases and equilibrium. Ionic product of water. pH, pKa and pKb. Titrations. Hydrolysis equilibrium. Buffer solutions.
- Solubility. Saturated solution and unsolubilized residue. Soluble and insoluble salts. Solubility product. Effect of common ions and of pH on solubility equilibria.
- Electrochemistry. Electrochemical cell and half-cell. Nernst's equation. Electrolysis. Mode of operation of a pH-meter.

Lectures with exercises

Written test with a series of exercises and theoretical questions (final mark given in n/30).