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Teacher
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Tundo Grazia Raffaella
(syllabus)
Introduction remarks. Periodic table of elements and inorganic nomenclature. Atom: atom models, atomic particles: proton, neutron, electron. Isotopes. Electrons and atom electronic configuration. The quantum-mechanical model of the atom. Quantum numbers and orbitals. Auf-bau. Chemical bonds.
Matter states. Gas: ideal gas law. Absolute temperature and its relation with mean molecular speed. Mixture of gases; Dalton law. Liquids: vapor pressure of a liquid. Solids: structural characteristics of covalent, ionic, molecular and metallic solids.
Thermodynamics. Thermodynamic potentials; enthalpy, Hess law, entropy. Free energy: relationship with enthalpy and entropy.
Solutions. Concentrations of solutions: dilution and mixing of solutions. Vapor pressure of a solution (Raoult law). Solubility of gases in liquids: Henry law.
Chemical equilibrium. Equilibrium in gaseous phase. Expression of equilibrium constant. Kp and Kc relationship. Equilibrium influencing factors. Homogeneus and hetherogeneus equilibrium.
Solutions of electrolytes. Strong and weak electrolytes: dissociation grade. Colligative properties of electrolyte solutions. Van't Hoff binomial. Acid and bases following Arrhenius, Bronsted and Lowry definitions. Strong and weak acid and bases. Dilution law of Ostwald. pH in strong and weak acid and base solutions. Buffers. Dissociation of polyprotic acids and bases. Acid-base titrations.
Heterogeneous systems. Equilibria of slightly soluble ionic compounds. The solubility-product constant. The effect of a common ion.
Kinetic. Kinetic introduction, activated complex theory, activation energy. Kinetic equations and reaction order. Relationship between kinetic constant and activation energy (Arrhenius energy). Relationship between kinetic constants and equilibrium constants.
Electrochemistry. Redox reactions and chemical potentials. Oxidation number. Redox reactions and their balance. Redox standard potentials. Nernst equation. Electromotive force potential of a cell. Half-cell. Chemical and concentration cells.
Carbon atom hybridization. Sp3, sp2, sp hybridization and their geometry.
Hydrocarbons. Saturated hydrocarbons (arenes): alkanes, cicloalkanes. Nomenclature. Conformational isomerism and geometric isomerism (cis-trans). A Unsaturated hydrocarbons: alkenes and alkynes. Nomenclature. Addiction reactions to alkenes. Markovnikov rule.
Aromatic compounds. Benzene structure: resonance model. Aromatic compounds nomenclature. Polycyclic aromatic hydrocarbons.
Alcohols, phenols, thiols. Nomenclature. Acidity and alkalinity of alcohols and phenols. Alcohol with more than an unique alcoholic group. Alcohols and phenols in comparison. Thiols. Aldehydes and ketones. Nomenclature. Carbonylic group. N Acetals and hemiacetals formation. Oxidation of carbonylic compounds.
Carboxylic acids and their derivatives. Nomenclature. Carboxylate ion resonance. Effects of acid structure: inductive effect. Carboxylic acid derivatives: esters, anhydrides, amides.
Difunctional acids. Dicarboxylic acids. Unsaturated acids. Ketoacids. Esterification mechanisms. Glycerol triesters. Ammines and other nitrogen compounds. Classification and nomenclature of ammines. Ammines reactions: heterocycles, pyrrole, pyridine, imidazole, pyrimidine, purines.
Stereoisomerism. Chirality. Enantiomers. Polarized light. Diastereoisomers. Meso compounds. Carbohydrates. Definition, classification and nomenclature. Monosaccharides. Monosaccharides chirality. Fisher projections.
(reference books)
Peter Atkins , Loretta Jones, Leroy Laverman Chemical Principles: The Quest for Insight
Chemistry by M.S. Silderberg, McGraw-Hill International Edition.
Katherine J Denniston, Joseph J Topping and Robert L Caret. General, Organic & Biochemistry. 7th Ed. 2010. McGraw-Hill Higher Education.
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