The global aim of Inorganic Chemistry is to develop basic principles concerning the structure and reactivity of chemical species in order that students can apply them in a systematic study of chemical compounds, in general, and inorganic compounds in particular. The objective is to emphasize the relationship and dependence between the bonding and the structure of compounds and their properties and chemical behaviour in such a way that studies can be extended to other species not been expressly described.
INORGANIC CHEMISTRY SUBJECT: CORE LINKING AREA: INORGANIC CHEMISTRY CORE AREA: INORGANIC CHEMISTRY DEPARTMENT: INORGANIC CHEMISTRY CREDITS: 5 theoretical, 2 practical, 0.5 of supervised work TEACHING SCHEDULE: 1st year, 1 st semester OBJECTIVES The global aim of Inorganic Chemistry is to develop basic principles concerning the structure and reactivity of chemical species in order that students can apply them in a systematic study of chemical compounds, in general, and inorganic compounds in particular. The objective is to emphasize the relationship and dependence between the bonding and the structure of compounds and their properties and chemical behaviour in such a way that studies can be extended to other species not been expressly described. THEORETICAL PROGRAM Chapter I. ATOMIC STRUCTURE AND PERIODICITY Unit 1. Atomic structure. Models for hydrogen-like atoms. Bohr model. Quantum numbers. Electron configurations. Unit 2. The wavefunction model. Heisenberg´s uncertainty principle. The Schrödinger equation: solutions for the hydrogen atom. Atomic orbitals. Unit 3. Many-electron atoms. Slater orbitals. Penetration and shielding of atomic orbitals. Radial and angular distribution functions. Unit 4. The periodic classification of the elements. The periodic table. Periodic and non-periodic properties. Chapter II. CHEMICAL BONDS Unit 5. The covalent bond. Valence-bond theory. Molecular topology: basic shapes of the valence shell electron pair repulsion model (VSEPR). Hybridization. Resonance. Unit 6. The covalent bond. Molecular orbital theory. Bonding and antibonding orbitals. Molecular orbital diagrams: homonuclear and heteronuclear diatomic molecules. Electronegativity. The dipole moment. Unit 7. The ionic bond. Close packing of spheres. Crystal lattices. Ionic radii. Lattice energy. The Born-Haber cycle. Properties of ionic compounds. Polarization and layered lattices. Lattice defects. Unit 8. Metallic bond: models. Interpretation of metallic properties. Structure of metals. Conductors, semiconductors and insulators. Unit 9. Intermolecular chemical forces. Van der Waals forces. Hydrogen bonding. Chapter III. REACTIVITY AND EQUILIBRIA IN INORGANIC COMPOUNDS IN SOLUTION. Unit 10. Acid-Base Concepts. Arrhenius, Brönsted and Lewis definitions. Hard and soft acids and bases: Pearson theory. Acid-Base strength: Drago and Wayland parameters. Unit 11. Oxidation and reduction reactions. Standard reduction potentials: relationship with atomic properties. The electrochemical series. Latimer and Frost diagrams. 1 Chapter IV. SYSTEMATIC CHEMISTRY OF NON-METALS AND THEIR COMPOUNDS. Unit 12. Hydrogen. Isotopes. Atomic and molecular hydrogen: properties and preparation. Hydrides: classification. Molecular and saline hydrides. Unit 13. The Halogens. Properties, preparation and uses. Halides of the elements. Classification. Interhalogen compounds. Unit 14. Oxygen and the elements of its group. Ozone: properties and uses. Hydrides: a particular study of water and hydrogen peroxide. Oxides. Sulfur, Selenium and Tellurium: properties and preparation. Hydrides: classification. Oxides and oxoacids. Contamination by sulfur oxides. Unit 15. Nitrogen and the elements of its group. Hydrides. Oxides and oxoacids. Environmental contamination by nitrogen oxides. The noble gases. Phosphorous, Arsenic, Antimony and Bismuth: properties and preparation. Hydrides. Oxides and oxoacids. Unit 16. Carbon and the elements of its group. Allotropic forms. Properties and uses. Preparation methods. Oxides and oxoacids of carbon: carbon monoxide and carbonates. Silica and silicate minerals. Silicones. Unit 17. Boron. Allotropic forms. Hydrides: a particular study of boranes. Oxides and oxoacids: boric acid. Chapter V. SYSTEMATIC CHEMISTRY OF METALS AND THEIR COMPOUNDS. COORDINATION CHEMISTRY. Unit 18. Introduction to coordination compounds. Coordination number. Types of ligands. Polydentate ligands and the chelation effect. Isomerism in coordination compounds. Types of isomerism: structural isomerism and stereoisomerism. Unit 19. Bonding in coordination compounds. Valence bond theory. Crystal field theory. Crystal field splitting orbitals diagrams. The Jahn-Teller effect. Molecular orbital theory. Unit 20. The s-block metals. Occurrence, preparation and uses of the elements. Representative compounds. Solution chemistry. Biological importance. Unit 21. The p-block metals. Occurrence, preparation and uses of the elements. Representative compounds. Solution chemistry. Unit 22. The d-block metals. Occurrence, preparation and uses of the elements. Oxidation numbers. Representative compounds. Solution chemistry. Unit 23. Metals of the 4f and 5f series. Occurrence, preparation and uses of the elements. Radionuclides. Representative compounds. Unit 24. Introduction to Bioinorganic Chemistry. Essential elements and trace elements. The role of inorganic elements in biological systems. PRACTICALS PROGRAM A broad range of laboratory experiments is proposed in order that the students, in rotation, carry out four of them, addressing the most important aspects of the program. Laboratory material: description and uses. Preparation of sodium bicarbonate by the Solvay method. Preparation and titration of hydrogen peroxide. Preparation of boric acid. Preparation of potassium permanganate. 2 Preparation of double salts: Mohr salt and iron alum. Preparation of the dichloro bis-ethylenediamine cobalt(II) chloride. Stoichiometric determination of the silver-ammonia complex. Vanadium and manganese complexes with acetylacetonate. Stability of nickel complexes. BIBLIOGRAPHY COTTON F.A. y WILKINSON G.-1986- "Química Inorgánica Avanzada", 4ª ed., Limusa, México. (There is a 5 th edition in English by Ed. John Wiley and Sons, New York, 1988. DOUGLAS B., McDANIEL D.H. y ALEXANDER J.J.-1987-"Conceptos y Modelos de Química Inorgánica", 2ª Ed., Reverté, Barcelona.( There is a 3rd edition in English by Ed.Wiley and Sons, New York, 1994.) GRAY, G.P.y HAIGHT, Jr.-1981- "Principios Básicos de Química", Reverté, Barcelona. GREENWOOD N.N. y EARNSHAW A.- 1984-"Chemistry of the Elements", Pergamon Press, Oxford. GUTIERREZ RIOS, E.- 1978- "Química Inorgánica", Reverté, Barcelona. HUHEEY, J.E.- 1981-"Química Inorgánica. Principios de Estructura y Reactividad", 2ª Ed., Harla, Méjico, (There is a 4th edition in English by Ed. Harper and Row, New York, 1993). MOELLER, T.- 1988- "Química Inorgánica", Reverté, Barcelona. PORTERFIELD W.W.-1984- "Inorganic Chemistry: A Unified Approach", Addison Wesley, London. RIVES V.R., SCHIAVELLO M, PALMISANO L.-2003-“Fundamentos de Química”, Ed. Ariel Ciencia, Barcelona PURCELL K.F. y KOTZ J.C.- 1979-"Química Inorgánica" Reverté, Barcelona. RODGERS G.E.-1994-"Química Inorgánica. Introducción a la Química de la Coordinación, del estado sólido y descriptiva", McGraww Hill, Madrid. SHRIVER D.F., ATKINS P.W. y LANGFORD C.H.-1998-"Química Inorgánica", Ed. Reverté, Barcelona. VALENZUELA C.-2002- “Química General e Inorgánica para estudiantes de Farmacia”, Ed. Univ. de Granada, Granada. 3 . INORGANIC CHEMISTRY SUBJECT: CORE LINKING AREA: INORGANIC CHEMISTRY CORE AREA: INORGANIC CHEMISTRY DEPARTMENT: INORGANIC CHEMISTRY CREDITS:. compounds. Unit 24. Introduction to Bioinorganic Chemistry. Essential elements and trace elements. The role of inorganic elements in biological systems.