inorganic chemistry content

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, 1st 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.

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