Facoltà di Ingegneria - Guida degli insegnamenti (Syllabus)


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Chimica per Bioingegneria
Chemistry for Bioengineering
Michela Pisani

Seat Ingegneria
A.A. 2016/2017
Credits 9
Hours 72
Period II
Language ENG


Learning outcomes
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.
The course will furnish 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 and thermodynamic phenomena, with particular reference to the biological ones. 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.
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. To this end, the course aims to encourage students to develop an aptitude for logical reasoning, based on the scientific method.

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
The method consists in a written test and an oral exam. In the written test, the students must solve 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 during the course.

During the exams, the 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.

During the examinations the student's ability is evaluated in order to set and develop reasoning to interpret the basic chemical problems typical in engineering.

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 in the logical processes setting 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 in the interpretation of the basic chemical phenomena, and in the t logical processes setting for the understanding of basic chemical problems related to engineering.

Recommended reading
M. Schiavello, L. Palmisano, “Fondamenti di Chimica”, Edises; L. Laird, “Chimica Generale”, McGraw-Hill; R. Michelin, A. Munari, “Fondamenti di Chimica”, CEDAM Stechiometria: A. Caselli, S. Rizzato, F. Tessore, “Stechiometria”, EdiSES

  • Ingegneria Biomedica (Corso di Laurea Triennale (DM 270/04))

Università Politecnica delle Marche
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