Chemistry Pierluigi Stipa
KNOWLEDGE AND UNDERSTANDING:
The course aims to provide the foundation for a correct understanding and interpretation of chemical phenomena, upon which the technologies in use in engineering are based. The course is directed to the knowledge of the structure and properties of matter, creating a link between the microscopic and macroscopic world.CAPACITY TO APPLY KNOWLEDGE AND UNDERSTANDING:
The course provides the skills needed to apply the knowledge acquired to the analysis and to the comprehension of chemical problems in an engineering context, through the use of laws and methods which represent the foundation of the chemical phenomena. These capabilities will be acquired by the student with the development of suitable exercises requiring the use of models and methodologies described in the lectures. TRANSVERSAL SKILLS:
The course is designed to stimulate and emphasize connections with the other disciplines, with the aim to improve the learning and communication capacities through the mastery of the basic scientific terminology.
Matter and its structure: substances, properties, systems, phases and transformations. Symbols, formulas, equations. Mass conservation, relative atomic, molecular, and equivalent mass; mole. Avogadro's number. Atomic structure. Nuclides and radioactive decays. The Rutherford experiment. Heisenberg Uncertainty Principle and De Broglie equation. Quantization, wavefunction, Schroedinger equation and orbitals. Periodic table and properties. Valence bond theory: energy, angle and bond length. Hybridization and molecular geometry; dipole moment and polar molecules. Molecular orbitals (LCAO). Bonding in metals and electrical conductivity in materials: conductors, semiconductors and insulators; mentions on doping. Ionic bond and lattice energy. Intermolecular interacrions: hydrogen bonds, Van der Waals and London forces. The states of matter. Ionic, covalent, molecular and metallic solids. Crystals: properties and defects. Liquids: vapor pressure, ideal and real solutions. Concentrations: molarity, normality, mole fraction, percentages by volume and by weight, parts per million. Ideal and real gases: state equations and liquefaction. Chemical transformations. Thermodynamics: Reversible and irreversible transformations. First Principle and Thermochemistry: Internal Energy and Standard Enthalpy of Reaction, formation, combustion, solution and phase transition. Hess's Law. Second Principle and Entropy. Probability Thermodynamics State. Third Principle. Spontaneity and Gibbs Free Energy. Chemical equilibrium and equilibrium constant. Van't Hoff equation, Le Chatelier's principle and temperature dependence of the equilibrium constant. Gas phase and solution Equilibria. Aqueous solutions Ionic equilibria: acids, bases and pH. Salts: hydrolysis and solubility product. Phases Equilibria. Phase diagrams with one and two components with and without miscibility lacunae. Cooling curves, Clausius-Clapeyron Equation and Gibbs Rule. Electrochemical Thermodynamics: double layer, electromotive force and Nernst equation. The redox potentials scale. Corrosion in metals. Electrolysis and Faraday's laws: opposite electromotive force and overvoltage. Chemical kinetics: reaction rate and order. Reaction mechanism, transition state theory and activation energy. Arrhenius equation. Homogeneous and heterogeneous catalysis.
Development of the examination
LEARNING EVALUATION METHODS
The method consists in a written test and an oral exam.
In the written test, students must deal with stoichiometry problems and answer to selected theoretical questions.
In the oral exam students are asked to discuss their written test, and to present the main concepts of basic chemistry developed within the course.
LEARNING EVALUATION CRITERIA
In the course of the exams, students must demonstrate their basic chemical knowledge, and must be able to develop appropriate reasoning for their applications; they must also demonstrate sufficient capabilities to synthesize and clearly present ideas, concepts and possible solutions to basic chemical problems typical in engineering.
LEARNING MEASUREMENT CRITERIA
During the examinations is evaluated the student's ability to set and develop reasoning to interpret the basic chemical problems typical in engineering.
FINAL MARK ALLOCATION CRITERIA
The final mark arises from the average of the written and oral exams.
The maximum vote, equal to thirty points (cum laude) out of thirty, is assigned to students who demonstrate, in both exams, full capability in the interpretation of the basic chemical phenomena and to set logical processes for the understanding of basic chemical problems related to engineering.
The minimum mark, equal to eighteen points out of thirty, is assigned to students who demonstrate sufficient capability of interpretation of the basic chemical phenomena, and to set logical processes for the understanding of basic chemical problems related to engineering.
P. Chiorboli, Fondamenti di Chimica, Utet
M. Schiavello, L. Palmisano, Fondamenti di Chimica, Edises
P. Zanello, R. Gobetto, R. Zanoni, Conoscere la Chimica, Ambrosiana
M.S. Silberberg, Chimica, la natura molecolare della materia e delle sue trasformazioni, McGrawHill;
L. Laird, Chimica Generale, McGraw-Hill
D. W. Oxtoby, H. P. Gillis, Campion, H. H. Helal, K. P. Gaiter, Chimica Moderna, Edises
K. W. Whitten, R. E. Davis, M. L. Peck, G. G. Stanley, Chimica, Piccin
Slides from lessons download: lms.univpm.it
- Ingegneria Edile (Corso di Laurea Triennale (DM 270/04))