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Politecnico di Torino
Anno Accademico 2015/16
06KWRLI, 06KWRJM, 06KWRLM, 06KWRLP, 06KWRLS, 06KWRLX, 06KWRLZ, 06KWRMA, 06KWRMB, 06KWRMC, 06KWRMH, 06KWRMK, 06KWRMO, 06KWRMQ, 06KWRNX, 06KWROD, 06KWRPC, 06KWRPI, 06KWRPL
Chemistry
Corso di Laurea in Ingegneria Dell'Autoveicolo (Automotive Engineering) - Torino
Corso di Laurea in Ingegneria Meccanica (Mechanical Engineering) - Torino
Corso di Laurea in Ingegneria Informatica (Computer Engineering) - Torino
Espandi...
Docente Qualifica Settore Lez Es Lab Tut Anni incarico
Bodoardo Silvia ORARIO RICEVIMENTO A2 CHIM/07 58.5 18 3 33 5
Saracco Guido ORARIO RICEVIMENTO PO CHIM/07 58.5 18 3 33 4
SSD CFU Attivita' formative Ambiti disciplinari
CHIM/07 8 A - Di base Fisica e chimica
Esclusioni:
16AHM
Risultati di apprendimento attesi
The course aims at providing the necessary background for the interpretation of chemical phenomena, for the understanding of the structure and properties of molecules and crystalline solids, and the comprehension and handling of energetic phenomena concerning chemical and electrochemical systems.
Prerequisiti / Conoscenze pregresse
To make profit of the course it is required to master the basic notions of general chemistry, the symbols of elements and compounds, the simplest nomenclature both organic and inorganic, the balancing of elementary stoichiometric reactions.
Programma
ATOM
Constitution of the nucleus, structure of the hydrogen atom and atomic models (Bohr and quantum-mechanical)
Quantum numbers, exclusion principle and Hundt rule
Spatial form of s,p and d orbitals

CLASSIFICATION OF THE ELEMENTS AND PERIODIC TABLE
Electronic configuration of the elements and periodicity in the chemical and physical properties
Atomic radius, ionization energy and electron affinity
Subdivision into metals, non-metals and semimetals.
Basics on the main groups of the periodic table and some transition metals.

THE CHEMICAL BOND
Bond: ionic, covalent, metallic. Intermolecular interactions.
Covalent bond: single, double and triple.
Molecular geometry, hybridisation and resonance.
Notes on the theory of molecular orbitals.

NOMENCLATURE, FORMULAS AND STOICHIOMETRY
Atomic and molecular mass, the mole, Avogadro's constant.
Acid-base reactions and formation of salts.
Oxidation state and balancing of redox reactions.
Mass relationships in a chemical reaction, limiting reagent.
Combustion reactions

GASEOUS STATE
Ideal gas laws. State equation of ideal gases.
Equilibrium distribution of kinetic energies in an ideal gas (Boltzmann).
Liquefaction of a gas.

LIQUID STATE
Vapour pressure of pure liquids.
Solutions: ways to express concentration. Dissociation and ionization degree. Colligate properties of solutions, both electrolytic and non. Definition of acid and base according to Arrhenius, Brønsted and Lewis. Ostwald dilution law.
Ionic product of water, pH and pOH.

SOLID STATE
Unit cell and structure of simplestcrystalline solids. Crystal lattices. Classification of solids.

CHEMICAL KINETICS AND CATALYSIS
Reaction rate and order. Arrhenius equation. Activation energy. Catalysis and catalysts.

CHEMICAL EQUILIBRIUM
Mass action law. Equilibrium constant. Homogeneous and heterogeneous chemical equilibria. Le Chatelier principle and influence of the temperature on the equilibrium.


CHEMICAL THERMODYNAMICS
First, second and third Principle. Reaction enthalpy and Hess law. Change in entropy and free energy of a reaction. Spontaneity criterion.

ELECTROCHEMISTRY
Normal and effective potential of an electrode. Electrochemical cells and Nernst equation. Electrochemical force of a cell. Reactivity of metals with ocids, oxidizing or not. Electrolysis and Faraday laws.

ORGANIC CHEMISTRY
Nomenclature and properties of the main organic compounds. Most common functional groups and their main reactions. Isomerism: structural, geometric, conformational.


Organizzazione dell'insegnamento
PRACTICAL
During practicals no new subject is dealt with, but only the numerical and computational of some subjects, among which:
' Survey of inorganic nomenclature
' Mole, gram-atom, molecular weight.
' Mass relationships in chemical reactions
' Redox reactions and their balancing.
' Ideal gases laws.
' Colligate properties of solutions.
' Chemical equilibria (homogeneous and heterogeneous)
' Reaction enthalpy (Hess law)
' pH and equilibria in aqueous solutions
' Nernst equation concerning an electrode or a cell.
' Faraday Laws

LABORATORY ACTIVITY
' Ideal gas laws
' Precipitation reactions
' Acid o-base titration
' Redox reactions
' pH measurement
' Daniell cell




Criteri, regole e procedure per l'esame (Prof. S. Bodoardo)
For students of last years (till a.a. 2014-2015) the exam consists in a written exam with 17 general questions (1 point per each correct answer) and 3 exercises (2,5 point per each correct exercises). !8/30 is requested to pass the exam. Oral is mandatory.

For new students (a.a 2015-2016):
-To get the access to the written exam  preliminary test @LAIB MANDATORY
- The validity of the pre-test is one year (4 exams)
- The pre-test is passed with 10 points over 15. Correct answer +1 point; not answered 0 points; wrong answer -0.25 points
- time: 30 minutes no mark

- Written exam: 3 exercises evaluated also on the procedure. Time: 1 hour. Highest mark 30

- Oral only if written exam is higher than 17. MANDATORY


Orario delle lezioni
Statistiche superamento esami

Programma definitivo per l'A.A.2015/16
Indietro



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