Unit INORGANIC CHEMISTRY
- Course
- Chemistry
- Study-unit Code
- 55009912
- Curriculum
- In all curricula
- Teacher
- Alceo Macchioni
- CFU
- 12
- Course Regulation
- Coorte 2021
- Offered
- 2022/23
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa integrata
INORGANIC CHEMISTRY 1
| Code | A000799 |
|---|---|
| CFU | 6 |
| Teacher | Alceo Macchioni |
| Teachers |
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| Hours |
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| Learning activities | Caratterizzante |
| Area | Discipline chimiche inorganiche e chimico-fisiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | Chemical forces. Structures and energetics of metallic and ionic solids. Acids, bases and ions in aqueous and non-aqueous solutions. Reduction and oxidation reactions. Coordination chemistry. Chemistry of transition metals. Organometallic chemistry. Introduction to homogeneous and heterogeneous catalysis. |
| Reference texts | J. H. Huheey, E. A. Keiter, R. L. Keiter "Chimica Inorganica", 1999, Piccin. |
| Educational objectives | The course is a continuation and, at the same time, a deepening and an extension of the topics covered in the courses of General and Inorganic Chemistry and General Chemistry 2. In addition, the course provides the basis for studying the following topics: 1) structure of ionic solids; 2) coordination complexes of the transition metals; 3) organometallic compounds; 4) rection mechanisms for coordination complexes; 5) catalytic processes, both homogeneous and heterogeneous, mediated by coordination complexes or organometallic compounds. At the end of the course it is expected that students have acquired the ability to be capable to critically analyze and / or predict the structure of inorganic systems, both at the molecular level that supramolecular, based on their reactivity. |
| Prerequisites | It is necessary to have passed the examination of General and Inorganic Chemistry and General Chemistry 2. |
| Teaching methods | Face-to-face lessons on all subjects of the course, numeric exercises on the subjects of the course and laboratory experiences mainly related to the chemistry of coordination complexes. For the latter students are divided in group (max 3-5 students per group), which independently carry on the syntheses of coordination complexes, their characterization and kinetic studies. |
| Other information | |
| Learning verification modality | Oral exam (duration ca 1 hour) aimed at verifying that students have acquired the ability to be capable to critically analyze and / or predict the structure of inorganic systems, both at the molecular level that supramolecular, based on their reactivity. |
| Extended program | Chemical forces: internuclear distances and atomic radii, types of chemical forces, hydrogen bonding and effects of chemical forces. Energetics and structure of ionic and metallic solids: structures of complex solids, defects in crystals, ionic conductivity in solids, solids held together by covalent bonds, solid state materials with polar bonds. Acids, bases and ions in aqueous and non-aqueous acid-base concepts, measurement of acid-base strength, acids and bases "hard" and "soft" properties of water, non-aqueous solvents and molten salts. Redox reactions: standard reduction potentials in relation to thermodynamic properties, electrochemistry in aqueous and non-aqueous. Coordination chemistry: general considerations, structure, reactions, kinetics and reaction mechanisms. Descriptive chemistry of transition metals: periodic trends in general, the various states of oxidation chemistry, the chemistry of the elements potassium and zinc, the chemistry of the heavier transition metals, lanthanides and actinides on the signs. Organometallic Chemistry: the rule of the eighteen electron metal carbonyl complexes, nitrosyl complexes, dinitrogen complexes, metal-alkyl,-carbenes, Carbynes-and-carbydes, and olefin complexes acetylenes non-aromatic, metallocenes, reactions of organometallic complexes. Outline of homogeneous and heterogeneous catalysis: introduction and definitions, industrial applications of homogeneous catalysis, development of homogeneous catalysts, surfaces and interactions with adsorbed species in heterogeneous catalysis, commercial applications of heterogeneous catalysis. |
INORGANIC CHEMISTRY 2
| Code | 55078612 |
|---|---|
| CFU | 6 |
| Teacher | Paola Belanzoni |
| Teachers |
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| Hours |
|
| Learning activities | Caratterizzante |
| Area | Discipline chimiche inorganiche e chimico-fisiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | Introduction to inorganic chemistry. Electronic configurations of atoms. Bonding theories for molecules. Molecular symmetry. Coordination complexes and bonding. Electronic and magnetic properties of coordination complexes. |
| Reference texts | J.E. Huheey, E.A. Keiter, R.L. Keiter, "Chimica Inorganica - Principi, Strutture, Reattivita'", Ed. Piccin, Padova. D.F. Shriver, P.W. Atkins, C.H. Langford "Chimica Inorganica", Ed. Zanichelli, Bologna. C. E. Housecroft, A. G. Sharpe, "Inorganic Chemistry", Second Edition 2005, Pearson Prentice Hall, England. |
| Educational objectives | The course represents the extension of a learning process during which the student should have acquired preliminary and basic knowledge of the general chemistry. The main objective of this course is to provide the student with the knowledge of the fundamental physical principles and inorganic chemistry concepts which constitute the basis for approaching the in-depth study of many-electrons atom structure, chemical bond nature, electronic and magnetic properties of coordination compounds, molecular symmetry and its applications. The main knowledge acquired will be: many-electrons atom structure, through the use of basic concepts of quantum mechanics; relativistic effects in atoms; ionic and covalent chemical bond models; main theories of chemical bond, such as valence bond (VB) theory and molecular orbital (MO) theory, including the semi-empirical Huckel method, both simple and extended; basic concepts of symmetry and group theory; bonding in coordination complexes using crystal field theory and ligand field theory; basic notions for understanding electronic spectra and magnetic properties of coordination complexes. The main competence will be: analysis of the chemical bond in different systems, from simple molecules to coordination complexes; identification of the main symmetry elements in molecules, assigning them their point group, and utilizing the character tables to construct molecular orbital diagrams; application of the simple Huckel method to organic, planar and conjugate molecules and the extended Huckel method to more general molecules; use of the crystal field theory to predict the megnetic properties of the coordination complexes; application of the molecular orbital theory to coordination complexes in order to rationalize the ligand spectrochemical series; analysis of the electronic spectra of the coordination complexes to get important information on their electronic structure and bonding. |
| Prerequisites | In order to be able to understand and to know how to tackle the course, students must have the basic notions of general chemistry. |
| Teaching methods | The course is organized in lectures and exercises on all subjects of the course and experiments at the inorganic chemistry lab. |
| Learning verification modality | The exam includes two possible ways: i) midterm written tests; ii) oral test. During the course two midterm written tests will be performed. The two tests consist of resolving problems similar to those proposed in the reference textbooks and carried out in class and of theory questions. If the marks average of the two tests is less than 18/30 it is obligatory to take the oral test. If not, the oral test is optional. The oral test consists of an interview of about 40 minutes on the entire program of the course. |
| Extended program | Introduction to inorganic chemistry. Many-electron atoms and their electronic structure. Atomic states, term symbols and Hund's rules. Slater's rules for effective nuclear charge calculation. Electronegativity: Pauling, Mulliken and Allred-Rochow scales. Periodic anomalies and relativistic effects. Chemical bonding models: ionic bond and covalent bond. Valence Bond (VB) theory. Molecular Orbital (MO) theory. Application to some diatomic molecules (homonuclear and heteronuclear) and polyatomic molecules. Three center-two electrons bond: boranes and Xe compounds. Hückel's method. Fundamentals of symmetry and group theory. Chemistry of "d-block" elements: general considerations. Bonding in coordination complexes. Crystal field theory. Molecular orbital theory applied to coordination complexes. Ligand field theory. Spectrochemical series. Electronic spectra and magnetic properties of the coordination complexes. |