CHEMISTRY

Course objectives

The Chemistry course has an invaluable importance for its contents for any University Degree Course that deals with science and technology and aims to provide students with basic knowledge in Chemistry, applicable in both scientific and technological fields. In particular, the Chemistry Course will allow the students to understand and forecast the physico-chemical behaviour of matter, based on the atomic structure and on the rules which allow atoms to combine and react. 1) knowledge and understanding: the student will learn the basic knowledge of chemistry (nuclear and atomic structure) and the following rules for reactivity, useful for the understanding and forecast of the matter behavior, to solve problems which could arise in applied sciences. 2) Applying knowledge and understanding: Applying knowledge and understanding: the student will learn to apply the theoretical knowledge on atomic structure to simple forecast of matter behavior. 3) Making judgements: Making judgements: the student will learn to choose the right way to solve simple tests. 4) Communication skills: Communication skills: the student will learn to rigorously describe basic chemical concepts. 5) Learning skills: Learning skills: the student will learn: to use chemical basic methods; to forecast the chemical behavior; to solve simple applicative problems.

Channel 1
MARTA FEROCI Lecturers' profile

Program - Frequency - Exams

Course program
Electronic stucture of atoms. The Bohr theory. Heisemberg uncertainty principle. The nature of the light. Photoelectric effect. The de Broglie relation. Schrodinger equation. Atomic orbital shapes. Electron configurations and periodicity. Chemical bonds. Atomic weight and molecular weight. The mole concept. Electronegativity. Metals and nonmetals. Covalent, polar-covalent, ionic bond. Hybrid orbitals. The resonance concept. Delocalizated bonding. Metal bond. Inter-molecular bonds. Molecular geometry Chemical thermodynamics. The first low of thermodynamics. Hess’ law. Spontaneity of chemical reactions. Entropy. The second law of thermodynamic. Free energy and useful work. Free energies and equilibrium. States of matter. The ideal gas. The combined gas law. Dalton’s law of partial pressures. Kinetic molecular theory. The real gases Vapor pressures of liquids. Cristalline solids. Liquid crystals. Heating and cooling curves. Changes of states. Clausius-Clapeyron equation. Phase diagrams. Chemical Kinetics. Rate laws. Reaction orders. The Arrhenius equation. Reaction mechanism. Catalysts. Chemical equilibrium. The equilibrium constant. Thermodynamics and chemical equilibrium The pressure and the temperature in the chemical equilibrium. Acids and bases. Acid-base equilibria in aqueous solution. Ionization of water and pH. Dissociation of weak electrolites. Buffers. Hydrolysys. Acid-base indicators. Properties of the solutions. Concentration units. Rault’s law. Fractional distillation. Colligative properties of the solutions. Solubility product. Electrochemistry. Electrode reactions. Galvanic cell. The standard hydrogen electrode. The Nernst equation. The table of standard reduction potentials. Electrolysis. The lead storage battery. Corrosion.
Prerequisites
Basic notions of mathematics.
Books
a book on Stoichiometry - N. J. Tro, Chimica, Casa Editrice Edises (with exercises) - Chimica Generale – Petrucci, Herring, madura, Bissonnette – Piccin (2013) (with exercises) - T. L. Brown, H. E. LeMay, C. J. Murphy, P. Woodward, Fondamenti di Chimica, Casa Editrice Edises (with exercises)
Teaching mode
Lessons if possible in person, otherwise in blended or online mode.
Frequency
No obligation to attend
Exam mode
Written and oral ezam, if possible in person, otherwise online.
Lesson mode
Lessons in classroom
Channel 2
STEFANO VECCHIO CIPRIOTI Lecturers' profile
  • Lesson code101144
  • Academic year2024/2025
  • CourseManagement Engineering
  • CurriculumCurriculum unico
  • Year2nd year
  • Semester1st semester
  • SSDCHIM/07
  • CFU6
  • Subject areaFisica e chimica