|esercitazioni||1||I sem.||Adolfo Speghini|
|laboratorio [laboratorio I]||2||I sem.||Adolfo Speghini|
|laboratorio [laboratorio II]||2||I sem.||Adolfo Speghini|
|teoria||6||I sem.||Adolfo Speghini|
|laboratorio [laboratorio I]||Monday||1:30 PM - 5:30 PM||laboratorio||Laboratory Laboratorio Didattica (Lebrecht)||from Oct 20, 2014 to Jan 30, 2015|
|laboratorio [laboratorio I]||Wednesday||1:30 PM - 5:30 PM||laboratorio||Laboratory Laboratorio Didattica (Lebrecht)||from Nov 19, 2014 to Jan 30, 2015|
|teoria||Monday||8:30 AM - 12:30 PM||lesson||Lecture Hall Berni (Lebrecht)|
|teoria||Wednesday||8:30 AM - 12:30 PM||lesson||Lecture Hall Berni (Lebrecht)|
The course provides the fundamental concepts of General Chemistry and some basics of Inorganic Chemistry. In particular:
- models and general concepts as means of justification and prediction of physical and chemical properties of systems of increasing degree of complexity: atoms, molecules, substances, multi-component systems (homogeneous and heterogeneous).
- concepts and methods for predicting qualitative and quantitative changes of intensive and extensive properties of chemical systems in transformation.
Numerical exercises integrate the knowledge acquired by the student in the theoretical part of the course. They are essential for the student in order to improve the skills to solve real problems of chemical interest.
The experiments in the General Chemistry laboratory integrate the knowledge acquired by the student in the theoretical part of the Course. The student learns how to manage problems of chemical interest, obtains information about the common equipment present in a chemical laboratory and how to work in safe conditions.
Introduction. Chemical and physical properties of matter and their measurements.
Elements, atoms and compounds.
Nomenclature of inorganic compounds.
Types of chemical reactions. Reaction stoichiometry.
Ideal and real gases.
Thermochemistry. Internal energy and enthalpy. Standard enthalpy of reaction and formation.
Atomic structure. Atomic orbitals. Electronic configuration, Aufbau principle.
Periodic properties: atomic and ionic radii, ionization energy, electron affinity, electronegativity.
Elementary notions on the ionic bond. Ionic compounds.
Covalent bond. Lewis formula. Resonance. Molecular geometry and polarity. Orbital hybridisation. Single and multiple bonds.
Properties of liquids. Solutions. Colligative properties. Binary liquid mixtures. Distillation.
Properties of solids.
Chemical kinetics. Arrhenius equation. Reaction mechanisms.
Chemical equilibrium. Equilibrium constant.
Acid-base equilibrium. Acid, base and salt solutions. Acid-base titration. Buffer solutions.
Entropy. Spontaneous processes. Gibbs free energy. Standard free energy of reaction and formation.
Electrochemical cells. Electrolysis.
Stoichiometry problems solving.
- determination of the hydrogen peroxide concentration in a commercial sample for pharmaceutical use
- determination of the number of water molecules in hydrate copper sulphate
- spectrophotometric determination of the concentration of a potassium permanganate solution
- weak base-strong acid titration
- strong base-strong acid titration
- determination of tap and commercial water hardness
The final exam consists of a written part, with solving of stoichiometry problems and general questions and of an oral part.
|esercitazioni||Maurizio Bruschi||Stechiometria e Laboratorio di Chimica Generale||Pearson Italia, Milano, Torino||2011||978-88-7192-576-9|
|teoria||Martin S. Silberberg||CHIMICA - La natura molecolare della materia e delle sue trasformazioni (Edizione 3)||McGraw-Hill Education, Italy||2016||978-88-386-1542-9|