GENERAL AND INORGANIC CHEMISTRY
Academic year and teacher
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- Versione italiana
- Academic year
- 2016/2017
- Teacher
- VALERIO BERTOLASI
- Credits
- 9
- Didactic period
- Primo Semestre
- SSD
- CHIM/03
Training objectives
- KNOWING.
The student will learn basic knowledges with respect to:
- the fundamental theory of matter;
- the properties of chemical substances;
- the ability of substances to undergo transformations into other species (chemical reactions).
SKILLS.
The student will acquire the ability to:
- read into the properties and transformations of matter basing on the structure of atoms and molecules;
- apply the known knowledges to understand all chemical aspects related to pharmaceutical and health products. Prerequisites
- For achieving a correct and successful understanding of all the arguments proposed during the Course, the following basic knowledge is required:
- Elementary Chemistry
- Elementary classical physics,
- Elementary algebra,
- Exponential and logarithmic calculus,
- First and second degree equations,
- Single-variable functions,
- Diagrams and two-dimensional representation of a
single-variable function. Course programme
- -States of matter. Compounds and elements. Chemical and physical changes.
-Atoms and molecules. The atomic structure. The atomic number and atomic weight. The isotopes. The Periodic Table. Molecules, compounds and chemical formulas. The mole.
-Chemical reactions. Lavoisier's law of conservation of matter. Balancing chemical equations. The oxidation number. The limiting reactant concept. Percent yields.
-Heat changes and thermochemistry. The first law of thermodynamics. Heat capacity. Calorimetry. Enthalpy. Hess's law.
-The atomic structure. The quantum numbers and atomic orbitals. The shape of atomic orbitals: s, p, d, f. The electron spin. The Pauli exclusion principle. Aufbau. The electronic configurations of the elements of the fundamental groups. Ionization energy and electron affinity.
-The chemical bonding and molecular structure. Covalent bonding and Lewis structures. Resonance. Octet rule and limitations of the rule. VSEPR model and molecular geometry. Multiple bonds. Electronegativity. Valence bond theory. Hybridization of atomic orbitals. Sigma and pi-bonds.
-Gases. The ideal gases. The combined gas law. The Avogadro's law. The gas mixtures. The Dalton's law. The kinetic theory of gases. The diffusion of gases and Graham's law. The real gases.
-The intermolecular forces. The liquid state. Evaporation and condensation. Vapor pressure. Boiling point.
-The solid state. The structure of Ionic and molecular solids. Phase diagrams of water and CO2
The solutions and their behavior. Concentrations: molarity, molality, weight %, mole fraction. Enthalpy of solution. Solubility of gases in liquids: Henry's law.
-The colligative properties. The Raoult's law. Lowering of vapor pressure. Freezing point depression, boiling point elevation and osmotic pressure. The van't Hoff coefficient.
-Chemical kinetics. Concentration versus time. The integrate rate equations. The transition state theory. Activation energy. The Arrhenius equation. Catalysts.
-The chemical equilibrium. The equilibrium constants Kc and Kp.. The principle of Le Chatelier. The Haber-Bosch process for the production of ammonia
Acids and bases and other equilibria in solution. The Brønsted-Lowry concept of acid-base. Kw. The pH. Ka and Kb. Hydrolysis. The buffer solutions. The equivalent weight and normality. Acid-base titrations. Titrations curves. Indicators. Solubility. The solubility product Kps. The common ion effect.
-Thermodynamics. The two aspects of spontaneity. The second law of thermodynamics. The third law of thermodynamics. Entropy. Gibbs free energy G.
-Electrochemistry. The standard electrical potentials E°. Potential of Voltaic cells The Nernst equation. Electrolysis of molten salts and of aqueous solutions. Faraday's laws.
The batteries. Didactic methods
- Theoretical lessons and numerical exercises on the solution of chemical problems using occasional PDF slides to show particular structures, instruments and graphics.
Learning assessment procedures
- The final exam can consist of two written partial tests (the former by the middle of the semester and the latter after the end of the course) OR in a single written total test.
Each partial test consists of 6 exercises concerning stoichiometric problems and applications of theoretical principles. Each exercise has a maximum score of 5 when is completely and correctly carried out. In order to take the latter partial test it is necessary to obtain a score of at least 18/30 in the former partial test. The final score of the exam will be the result of the arithmetic mean of the scores of the partial tests, which must be both sufficient (with score of at least 18/30). In the case the minimum target is not reached, even in a single partial test, the student has to repeat the written exam in the total way.The total written exam will consist of a single test containing 6 exercises regarding all the arguments of the course including stoichiometric problems and applications of theoretical principles. Each exercise has a maximum score of 5 when is completely and correctly carried out. A score of at least 18/30 is necessary to consider the examination to be positive and acceptable.
A time of 2 h is given both for partial and total exams. During the test it is allowed to use only the periodic table and the calculating machine. Reference texts
- -J.C. Kotz, P.M. Treichel, J.R. Townsend, CHIMICA (V. Ed.) - EdiSES (NA)
-M.Giomini, E. Balestrieri, M. Giustini, FONDAMENTI DI STECHIOMETRIA - EdiSES (NA)
-F. Ugozzoli, COME RISOLVERE I PROBLEMI DI CHIMICA - CEA (MI)
On request:
-PDF slides of the course
-Previous exam tests with the solutions of the problems.
