GENERAL AND INORGANIC CHEMISTRY

Course objectives

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 1. 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. 2. 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. 3. 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. 4. 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. 5. 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.

Channel 1
SIMONETTA FORNARINI Lecturers' profile
MARIA ELISA CRESTONI Lecturers' profile

Program - Frequency - Exams

Course program
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.
Prerequisites
A basic knowledge of the main concepts learned during the course of Maths. There are no prerequisites.
Books
Per la teoria : - M. Schiavello, L. Palmisano “Fondamenti di Chimica” EdiSES - R. H. Petrucci et al. “ Chimica Generale” Piccin - F.Cacace, U. Croatto “Istituzioni di Chimica” La Sapienza Editrice - Paolo Silvestroni «Chimica generale», Quinta edizione, Zanichelli Per le esercitazioni: - F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore Roma
Frequency
Course attendance is recommended.
Exam mode
The final evaluation consists of a written test with 3 questions which, if passed, admits to the oral test.
Lesson mode
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).
DAVIDE CORINTI Lecturers' profile

Program - Frequency - Exams

Course program
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)
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.
Books
F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore P. Michelin Lausarot, G.A. Vaglio “Fondamenti di stechiometria” Piccin
Teaching mode
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
Course attendance is recommended.
Exam mode
Refer to what described by Prof. Maria Elisa Crestoni
Lesson mode
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.
Channel 2
ANTONELLO FILIPPI Lecturers' profile
CATERINA FRASCHETTI Lecturers' profile

Program - Frequency - Exams

Course program
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.
Prerequisites
Properties of exponents and logarithms Basic algebra concepts (first and second degree equations)
Books
"STECHIOMETRIA" di F. Cacace, M. Schiavello, Bulzoni Edition "CHIMICA GENERALE ed INORGANICA" di M. Speranza, EDI Ermes
Teaching mode
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
Classes will be held accordinf to the course calendar. Attending them is not mandatory but strongly suggested.
Exam mode
Refer to what described by Prof. Simonetta Fornarini
Lesson mode
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.
  • Lesson code10611082
  • Academic year2024/2025
  • CourseIndustrial pharmacy
  • CurriculumSingle curriculum
  • Year1st year
  • Semester2nd semester
  • SSDCHIM/03
  • CFU8
  • Subject areaDiscipline chimiche