CFU: 6
Prerequisites
The student who accesses this course has a good preparation in the fundamentals of mathematics and physics. These prerequisites are provided by the teachings given in the High School.
Preliminary Courses
-
Learning Goals
Critical knowledge of the chemical and chemical-physical principles necessary to interpret the behavior and transformations of matter in relation to the main technologies and engineering problems: materials, production and accumulation of energy, pollution.
Identification and understanding of the analogies between the different processes and the interpretation of the thermodynamic and mechanistic models.
Expected Learning Outcomes
At the end of the course the student knows the structure of the atom, the properties of the elements and their ability to form compounds, the molecular structures, the chemical reactions, the states of matter, the equilibria in solution, the acid-base properties of the molecules. The student has the necessary skills to tackle the study of the subsequent topics of his course of study in which the knowledge of the chemical properties of matter will be fundamental.
Knowledge and understanding
The student must demonstrate knowledge and understanding of the problems relating to the transformation of chemical substances, stoichiometry, reactions and equilibria that occur in aqueous systems. The student must be able to illustrate examples relating to the transformation of chemical substances and the establishment of equilibria mainly in aqueous solutions.
Applying knowledge and understanding
The student will acquire the skills to interpret the properties, stoichiometry, and transformations of chemical species. The student, on the basis of the understanding of the structure of atoms and of the different chemical entities (molecules, ionic compounds) and of the periodic properties, will be able to understand and solve problems inserted in wider contexts connected to their field of study. He will be able to analyze the effects of acid-base equilibria on simple aqueous systems and then discriminate and solve problems related to more complex systems. The theoretical treatment of many topics is followed by stoichiometric calculations that facilitate understanding and deepening of the phenomena related to real systems.
Course Content - Syllabus
From the fundamental laws of chemistry to the atomic hypothesis. Atomic weight, molecular weight and mole. Chemical formulas and percentage composition. The equation of balanced chemical reaction and stoichiometric calculations. Atomic Theory. Experiences of Thomson, Millikan and Rutherford. Bohr atom. Atomic orbitals. Evidence of wave-particle duality. The Schrödinger equation. The orbitals. Pauli and Hund's principle. Aufbau's rule. The electronic structure of atoms. The Periodic Table of the Elements. The chemical bond. The covalent bond. The valence of atoms. Molecular geometry. Polar and apolar molecules. The ionic and metallic bond. The octet rule. Lewis structural formulas; resonance and formal charge. Nomenclature of the main inorganic compounds. The hydrogen bond, Van der Waals forces ion-dipole, dipole-dipole, ion-induced dipole, induced dipole-induced dipole.
Laws of ideal gases. Dalton's law of partial pressures. The Maxwell-Boltzmann distribution of the velocities and kinetic energies of molecules. Real gases. Liquid state. Solid state. Crystalline and amorphous solids. Types of solids: covalent, molecular, ionic, metallic. Elements of chemical thermodynamics. I and II principle of Thermodynamics - Criterion of spontaneity of transformations. Enthalpy/temperature diagram of pure substances. The phase transitions of pure substances. The solutions. The solubility. Henry's Law. Material balances in the operations of mixing and diluting the solutions. Phase equilibria in solution. Raoult's law. Cryoscopy and ebullioscopy. Concentration of a solution: molarity, molality, mole fraction, percent by weight. Colligative properties. Chemical reactions. Thermochemistry. Chemical equilibria. The law of mass action. Chatelier's principle. Acids and Bases. Classification of acids and bases: Arrhenius theory; Lowry – Bronsted theory; Lewis theory. Definition of pH. Weak acids and bases. Calculation of pH. Electrolytic solutions. Ionization of water. Acid and basic solutions. Hydrolysis. Neutralization.
Readings/Bibliography
- P. Atkins, L. Jones, PRINCIPI DI CHIMICA, Ed. Zanichelli –Bologna
- M.S. Silbeberg, CHIMICA, Ed McGraw-Hill
Slides of the lessons available on the teacher's website.
Teaching Methods
The teacher will use: a) lectures for about 70% of the total hours, b) exercises to practically deepen theoretical aspects for about 30% of the total hours. The student will have the slides of the lectures and the teaching material provided online during the course and available on the teacher's website.
Examination/Evaluation criteria
Exam type
Exam procedure: written test for access to the oral exam. The carrying out of each question is assessed from 0 to 10 points on the basis of the following indicators: completeness and relevance. Admitted material: calculator and periodic table. Maximum score achievable with the written test: 30, minimum score to pass the exam: 18.
The outcome of the written test is binding for the purposes of accessing the oral test. The written and oral tests each contribute 50% of the final evaluation, therefore passing the written test is not sufficient to pass the exam. Average time for the written test: 120 minutes.
Evaluation pattern
The student must be able to apply the knowledge acquired in order to independently solve problems and communicate the concepts learned with an adequate and rigorous chemical language.