Physics

Brief introduction to atomic structure. Atomic mass. Electronic structure of the elements and their periodic properties. Nomenclature. Chemical reactions, redox. Introduction to chemical bond. Covalent, metallic and ionic bond. VB theory, VSEPR theory and Molecular orbitals. Weak bonds, H bond. Solid, liquid and gaseous states. Real gases. Solutions. Thermodynamics and thermochemistry: laws, entalpy, entropy, free energy, spontaneity of chemical reactions. Kinetics, homo-and heterogeneous catalysis. Homogeneous and heterogeneous chemical equilibria. Equilibrium constants, and their use. Le Chatelier principle. Effect of external parameters on equilibria. Equilibria in solution, acids and bases, pH, hidrolysis, buffered solutions. Solubility equilibrium, solubility product and common-ion effect.

The knowledge of basic concepts of mathematics is important.

1) Kotz, Treichel, Townsend “Chemistry and Chemical Reactivity” 2) Whitten, Davis, Peck, Stanley "Chimica" (Piccin) + Wendy Keeney-Kennicutt "Manuale delle soluzioni per Whitten, Davis, Peck, Stanley's Chimica" (Piccin) 3) Schiavello – Palmisano “Fondamenti di Chimica” (EdiSES)

Didactic activity consists of optional but strongly recommended traditional lessons and numerical excercises.

Classroom lessons and exercises.

The examination consists of a written test (duration: 3 hours; minimum score: 18/30) with numerical excersises and open questions concerning the program of the course. A compulsory exercise will concern nomenclature, chemical and structural formulae. Teacher or students can request a brief oral test in order to change the score obtained in the written test, but this oral test could also induce a failure in the exam. The aim of the tests is to check the knowledge of a student and his critical understanding of the subject. The student should be able to explain, in a simple but rigorous way, basic chemical processes, both in written and oral form.

Classroom lessons and exercises.

Brief introduction to atomic structure- Atomic mass- Electronic structure of the elements and their periodic properties. Nomenclature. Chemical reactions, redox, Introduction to chemical bond. Molecules- Molecular, covalent, metallic and ionic bond. VB, VSEPR theory and Molecular orbitals. Weak bonds, H bond. Solid, liquid and gaseous states. Real gases. Solutions. Thermodynamics and thermochemistry: laws, entalpy, entropy, free Energy, spontaneity of chemical reactions. Kinetics, homo-and heterogeneous catalysis. Homogeneous and heterogeneous chemical equilibria ᙦEquilibrium constants, and their use- Heterogeneous equilibrium- The le Chatelier principle. Equilibria in solution, acids and bases, pH, buffered solutions, hidrolysis. Effect of external parameters on equilibria.

The knowledge of basic concepts of mathematics is important.

Kotz, Trichel: Chimica (Edises) Whitten : Chimica (Piccin) Whitten: manuale delle soluzioni per Chimica (Piccin)

traditional lessons and numerical excercises.

Didactic activity consists of optional but strongly recommended traditional lessons and numerical excercises.

The examination consists of a written test (duration: 3 hours) with numerical excersises and open questions concerning the program of the course. A compulsory exercise will concern nomenclature, chemical and structural formulae. Teacher or students can request a brief oral test in order to change the score obtained in the written test, but this oral test could also induce a failure in the exam. The aim of the tests is to check the knowledge of a student and his critical understanding of the subject. The student should be able to explain, in a simple but rigorous way, basic chemical processes, both in written and oral form.

traditional lessons and numerical excercises.

Brief introduction to atomic structure. Atomic mass. Electronic structure of the elements and their periodic properties. Nomenclature. Chemical reactions, redox. Introduction to chemical bond. Covalent, metallic and ionic bond. VB theory, VSEPR theory and Molecular orbitals. Weak bonds, H bond. Solid, liquid and gaseous states. Real gases. Solutions. Thermodynamics and thermochemistry: laws, entalpy, entropy, free energy, spontaneity of chemical reactions. Kinetics, homo-and heterogeneous catalysis. Homogeneous and heterogeneous chemical equilibria. Equilibrium constants, and their use. Le Chatelier principle. Effect of external parameters on equilibria. Equilibria in solution, acids and bases, pH, hidrolysis, buffered solutions. Solubility equilibrium, solubility product and common-ion effect.

The knowledge of basic concepts of mathematics is required

1) Kotz, Treichel, Townsend “Chemistry and Chemical Reactivity” 2) Whitten, Davis, Peck, Stanley "Chimica" (Piccin) + Wendy Keeney-Kennicutt "Manuale delle soluzioni per Whitten, Davis, Peck, Stanley's Chimica" (Piccin) 3) Schiavello – Palmisano “Fondamenti di Chimica” (EdiSES) 4) Nivaldo Tro, Chemistry A molecular approach (Edises)

Classroom lessons and exercises.

The examination consists of a written test (duration: 3 hours; minimum score: 18/30) with numerical excersises and open questions concerning the program of the course. A compulsory exercise will concern nomenclature, chemical and structural formulae. Teacher or students can request a brief oral test in order to change the score obtained in the written test, but this oral test could also induce a failure in the exam. The aim of the tests is to check the knowledge of a student and his critical understanding of the subject. The student should be able to explain, in a simple but rigorous way, basic chemical processes, both in written and oral form.

Classroom lessons and exercises.

CHEMISTRY course program (Bachelor's degree in Physics) A.Y. 2024-25 • Fundamental principles of chemistry: scientific method, properties of matter, measurement and units of measurement, significant figures. Elements, compounds and mixtures, aggregation states of matter, Lavoisier's law, Proust's law, Dalton's atomic theory. Atoms and atomic mass. Concept of mole, Avogadro's number, Symbols of the elements. • Atomic nature of matter: elementary particles, mass and charge of elementary particles, atomic number, mass number, isotopes. Minimum, molecular and structural formula, atomic weight, molecular weight, stoichiometric calculations. • Chemical compounds, formulas and nomenclature: molecular and ionic compounds. Oxidation state. Acids, bases and salts, chemical formulas, traditional and Iupac nomenclature of the main organic and inorganic compounds. • Classes of chemical reactions: reactions in the gas phase and in aqueous solution, acid-base and redox reactions. Limiting reagent. Stoichiometric calculation, solutions and ways to express concentration. Balancing of redox reactions: ionic-electronic method. Numerical examples. • Gaseous state: pressure, ideal gas laws and ideal gas equation of state, gaseous mixtures, Dalton's law, real gases. Numerical examples. • Atomic structure: Thomson model, waves and electromagnetic spectrum, atomic spectra, Planck equation, photoelectric effect, energy quantization, Bohr atom, notes on wave mechanics, Schrodinger equation, quantum numbers, atomic orbitals, multielectronic systems. • Periodic table: electronic configurations of the elements. Aufbau, periodic properties of the elements. Sizes of atoms and ions. Ionization energy, electron affinity, electronegativity and their variation in the periodic table. • Chemical bond: Lewis theory, ionic bond. Covalent bond: order, length and bond energy; polar bonding and electronegativity. Resonance. Valence bond (VB) theory, hybrid orbitals and shape of molecules, VSEPR theory, resonance structures. Molecular orbital (MO) theory, LCAO methods, applications to homonuclear and heteronuclear diatomic molecules, bond order. Magnetic properties. Metallic bond. Band theory. • Thermochemistry: heat and work. First law of thermodynamics. Heat of reaction and enthalpy. Hess' law and its applications. • Liquids and solids: intermolecular forces and van der Waals bonds. Dipolar interactions. Hydrogen bonding Liquid state. Vapor pressure, Clausius Clapeyron equation. Ionic, covalent, metallic and molecular solids. Lattice energy, Born-Haber cycle. • Thermodynamics: spontaneous transformations, second and third law of thermodynamics. Entropy. Reversible and irreversible transformations. Gibbs free energy. • Chemical equilibrium: dynamic equilibrium, criteria of spontaneity in chemical processes, thermodynamic derivation of the equilibrium constant. Law of mass action, Kp, Kx and Kc. Homogeneous and heterogeneous equilibria. Le Chatelier's principle, dependence of equilibrium on pressure, volume, concentrations and temperature (van't Hoff's law). Numerical examples. • Equilibria in solution: solutions of electrolytes, strong and weak electrolytes, acids and bases according to Arrhenius, Brönsted-Lowry and Lewis; autoprotolysis of water, pH scale. Strength of acids and bases, structure-property correlation. Calculation of the pH of solutions of strong and weak acids (bases). Saline hydrolysis. Buffer solutions. Slightly soluble salts: solubility equilibria, Kps solubility product, effect of the common ion. Numerical examples. • Chemical kinetics: reaction rate. Kinetic law. Reaction order. Dependence of speed on temperature (Arrhenius equation), activation energy. Notes on collision theory. Homogeneous and heterogeneous catalysis.

Knowledge of basic mathematics is important.

1) Chimica, VII edizione (EdiSES); Kotz, Treichel, Townsend, Treichel. 2) Chimica, X edizione (Piccin); Whitten, Davis, Peck, Stanley 3) Chimica, V edizione, (McGraw-Hill) Silberberg, Amateis, Licoccia 

Attendance is optional although strongly recommended.

At the end of the course there will be a separate written test and a short oral (mandatory) test. The written test will last 3 hours and will contain numerical exercises and open questions on topics covered during the lessons, as per the course programme. The written test will contain a mandatory exercise for the purpose of passing the test itself, concerning nomenclature and structural formulas. At the discretion of the teacher and/or at the student's request, it will be possible to integrate the oral test with 1 or 2 additional questions, to confirm or modify the grade of the written test or even not allow the exam itself to be passed. The written test must be viewed by the student and discussed with the teacher on the day of the call for the oral test and the recording of the exam. The objective of the tests is to evaluate the knowledge and logical skills acquired by the student as well as his ability to present and explain concepts independently.

Classroom lessons and exercises.