Catalogo dei Corsi di studio

General expected learning outcomes.
The course aims to provide the student with a solid foundation in the fundamental concepts of chemistry, with particular reference to the chemistry of the elements, which will be the cultural heritage of the graduate in CTF. It deals with the indispensable topics for a correct understanding of matter and its transformations. On this basis it will be possible to found the skills that the student will have the opportunity to acquire in the courses of the following years. The course includes numerical exercises that make the student able to face the problems he/she will encounter in the various areas of chemistry, providing the essential tools for their analysis.

Specific expected learning outcomes.
Knowledge and understanding.
The student will have the opportunity to learn about general chemical structures and models, master the concepts underlying the properties and reactivity of matter, elements and chemical compounds, and understand the problems related to stoichiometry. He/she therefore knows the basic principles of general chemistry starting from the atomic structure, the periodic table and the chemical bond, up to chemical reactions (qualitative and quantitative aspects) with elements of kinetics and chemical thermodynamics and description of the aggregation states of matter. He/she is able to describe the equilibria (heterogeneous and homogeneous) and the fundamentals of electrochemistry. He/she will also have acquired a basic knowledge of the properties of the elements and their compounds.

Applying knowledge and understanding.
Upon completion of the course the student will be able to correlate the various topics developed in the program by relating the properties of matter with the properties of atoms and molecules. He/she will also become familiar with the correct and appropriate application of calculation tools, using the disciplinary methods of investigation, in order to solve application questions.

Making judgements.
The organization of the relevant exercises about the topics covered in the lectures will offer the student the opportunity to put to the test the knowledge acquired in relation to the various themes proposed. This allows to develop the ability to apply the concepts studied to practical cases and to critically evaluate the outcome and the method used in the procedures adopted.

Communication skills.
In addition to providing basic knowledge, the course aims to make the student acquire mastery of language and appropriate use of chemical terminology and scientific method, essential for communicating in the national and international scientific context. To this end, ample space is dedicated to informal interventions and discussions during the lessons and to the oral exam.

Learning skills.
The stimulus to use a correct scientific formalism and to formulate logically consistent deductions starting from the concepts and principles that underlie chemical science constitute a solid training towards cultural growth in the autonomy of future studies and professional activities.

Programme

Experimental measurements and Significant Digits. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole. Chemical formulas. Chemical equations and their quantitative relationship. Stoichiometry and Balancing Reactions. Oxidation number. Balancing Redox reactions. Equivalent weight in the neutralization and redox reactions. Quantitative relationships between substances involved in a reaction. (10 hours)
Concentration of solutions: molarity, normality, molarity, mole fraction, percent composition (by mass and by volume). Dilution and mixing of solutions. Density. Volumetric analysis. Titrations. The gaseous state: units relative to volume, pressure and temperature. Ideal gas laws: Boyle's law, Charles's law, Gay-Lussac's law. Avogadro's law. Ideal gas equation. Density. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of non-electrolyte solutions. Vapor pressure depression (Raoult Law), Boiling point elevation and freezing point depression, Osmotic Pressure. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. Van't Hoff factor. Thermal dissociation. Degree of dissociation. Indirect analysis. (10 hours)
Chemical equilibrium - The Law of Mass Action. Different forms of equilibrium constant and their relationships. Balances in a homogeneous and heterogeneous phase. Le Chatelier’s principle in the equilibrium law: applications. The law of mass action in the electrolytic dissociation reactions. Ostwald law. Acid-base equilibria. Acid-base equilibria. Ionic water product. pH. Strong acids and bases solutions. Weak monoprotic acid and bases solutions ands. Dissolution of polyprotic acids. Buffer solutions. Hydrolysis of salt and ph. Salts of polyprotic acids. Titrations. Indicators. Solubility. Solubility product expression. Common ion effect. Condition of formation of precipitates. Fractioned Precipitation. Cell. Half-cell and their representation. Normal potential. Nernst's equation. Various types of electrodes and their applications.(16 hours)

Adopted texts

F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore
P. Michelin Lausarot, G.A. Vaglio “Fondamenti di stechiometria” Piccin

Prerequisites

Although no prerequisites are explicitly requested, it is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations.

Study modes

The course has the following organization: • resolution of numerical problems in the classroom The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher.

Frequency modes

Course attendance is recommended.

Exam modes

Refer to what described by Prof. Maria Elisa Crestoni

Programme

Introductory notions. Subject of chemical research. Chemical phenomena. Fundamental laws of chemistry. Symbols and chemical notation. Amount. Atomic theory. Atoms and their properties. Mass and atomic weight. Avogadro's number. Atomic structure. Atomic spectra. Bohr model. Corpuscular and wave nature of the electron. Quantum numbers. Atomic orbitals. Electronic configuration. Chemical bond: concept of valence. The different types of bonds and their properties: order, energy, bond distance, dipolar moment. Valence bond theory and molecular orbitals. Hybrid orbitals, resonance. Structure of some typical molecules. Intermolecular bonds. States of aggregation and changes of state. Gaseous, liquid and solid state. Solutions and their colligative properties. Balance between phases and phase rules. Le Chatelier's principle. Basics of thermodynamics. Concept of balance. Principles of thermodynamics. Some thermodynamic functions. Thermochemistry. Chemical reactions and equilibria. Thermodynamic criteria for spontaneity and equilibrium in chemical transformations. Mass action law. Factors that influence the position of equilibrium. Electrolytic dissociation. Electrolytes and their properties in solution. Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Titulations. Indicators. Solubility. Solubility equilibria and factors that influence them. Partition equilibria. Electrochemical reactions. Redox reactions. Potentials, normal potentials, electromotive force, semi-elements, batteries, Nernst equation. Various types of electrolysis. Elements of kinetics. Speed, order, molecularity of a reaction, kinetic constant and its dependence on temperature. Arrhenius equation, activation energy. Basic notes on the theory of collisions and activated complexes. Catalysis. Outline of inorganic chemistry. Systematic nomenclature. Typical elements and their main compounds.
Stoichiometry exercises linked to the course. Notes on calculation methods. Exponential notation of numbers and relative elementary operations. Experimental measures and significant-figures. Logarithms. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Concept of mole. Chemical formulas. Law of definite proportions, law of multiple proportions, law of combination weights. Chemical equations and their quantitative significance. Balance of chemical equations. Oxidation number. Redox reactions and their balance. Equivalent weight of combination, neutralization and redox. Quantitative relationships between substances participating in a reaction. The solutions. Concentration and its units: molarity, normality, molality, mole fraction, weight percent, volume percent. Dilution and mixing of solutions. Density. Volumetric analysis. Titled solutions. The gaseous state: units relating to volume, pressure and temperature. The laws of ideal gases: Boyle's law, Charles's law, Gay-Lussac's law. Avogadro's principle. Equation of state of ideal gases. Density. Relative density. Gas mixtures. Partial pressures. Dalton's law. Colligative properties. Colligative properties of non-electrolyte solutions: vapor pressure, Raoult's law, ebullioscope rise and cryoscopic lowering, osmotic pressure. Electrolytic dissociation.

Adopted texts

For the theory:
- M. Schiavello, L. Palmisano “Fundamentals of Chemistry” EdiSES
- R. H. Petrucci et al. "General Chemistry" Piccin
- F.Cacace, U. Croatto “Chemistry Institutions” La Sapienza Editrice
- Paolo Silvestroni «General chemistry», Fifth edition, Zanichelli


For stoichiometry:

- F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore Rome

Prerequisites

A basic knowledge of the main concepts learned during the course of Maths. There are no prerequisites.

Study modes

The course has the following organization: • theoretical lessons in the classroom • deepening of theoretical issues in the classroom • resolution of numerical problems in the classroom The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher.

Frequency modes

The course is based on lectures and stoichiometry exercises in the presence; in-depth information, clarifications, review can also be carried out in mixed mode (in person and remotely).

Exam modes

The final evaluation consists of a written test with 3 questions which, if passed, admits to the oral test.

Exam reservation date start	Exam reservation date end	Exam date
18/01/2023	19/02/2023	21/02/2023
18/03/2023	17/04/2023	20/04/2023
20/05/2023	24/06/2023	26/06/2023
15/06/2023	15/07/2023	17/07/2023
20/08/2023	22/09/2023	25/09/2023
20/10/2023	21/11/2023	23/11/2023
15/12/2023	24/01/2024	26/01/2024

Programme

10 HOURS
Atomic weight, isotopic abundance, molecular weight. Mole. Chemical formulas. Chemical equations and their quantitative relationship. Stoichiometry and Balancing Reactions. Oxidation number. Balancing Redox reactions. Quantitative relationships between substances involved in a reaction. Concentration of solutions: molarity, molarity, mole fraction, percent composition (by mass and by volume). Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. Charles's law, Gay-Lussac's law. Avogadro's law. Ideal gas equation. Density.

10 HOURS
Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of non-electrolyte solutions. Vapor pressure depression (Raoult Law), Boiling point elevation and freezing point depression, Osmotic Pressure. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. Van't Hoff factor. Thermal dissociation. Degree of dissociation. Indirect analysis. Chemical equilibrium.

10 HOURS
The Law of Mass Action. Different forms of equilibrium constant and their relationships. Balances in a homogeneous and heterogeneous phase. Le Chatelier’s principle in the equilibrium law: applications. The law of mass action in the electrolytic dissociation reactions. Ostwald law. cid-base equilibria. Ionic water product. pH. Strong acids and bases solutions. Weak monoprotic acid and bases solutions ands. Dissolution of polyprotic acids. Buffer solutions. Hydrolysis of salts and pH. Salts of polyprotic acids. Solubility. Solubility product expression. Common ion effect. Condition of formation of precipitates. Cells. Half-cell and their representation. Normal potential. Nernst's equation. Various types of electrodes and their applications.

Adopted texts

"Stechiometria . Chimica generale attraverso gli esercizi" di A. Filippi, ALE Edition

"Stechiometria" di F. Cacace, M. Schiavello, Bulzoni Edition

Prerequisites

Properties of exponents and logarithms Basic algebra concepts (first and second degree equations)

Study modes

The course has the following organization: • resolution of numerical problems in the classroom The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher.

Frequency modes

in person

Exam modes

Refer to what described by Prof. Simonetta Fornarini

Exam reservation date start	Exam reservation date end	Exam date
14/02/2023	20/02/2023	21/02/2023
17/04/2023	19/04/2023	20/04/2023
20/06/2023	25/06/2023	26/06/2023
11/07/2023	16/07/2023	17/07/2023
19/09/2023	24/09/2023	25/09/2023
20/11/2023	22/11/2023	23/11/2023
19/01/2024	25/01/2024	26/01/2024