Inorganic chemistry
(objectives)
LEARNING OUTCOMES AND COMPETENCES The course aims to provide students with an introduction to the language and methodology of studying chemical phenomena of a general nature. The course, both through lectures and through exercises, intends to provide the student with the elements to be able to write the structural formulas of the main inorganic compounds and the related nomenclature, use the mole and molar ratios in chemical reactions, know the fundamental concepts of chemical thermodynamics for the study of the states of aggregation of matter, chemical solutions and equilibria with particular attention to acid-base and precipitation equilibria, also knowing the fundamental concepts of chemical kinetics. The knowledge of these concepts is essential to undertake the study of the subsequent courses that characterize the degree course.
Expected learning outcomes At the end of the course the student will have to show: 1) Knowledge and understanding: know the fundamental principles of General Chemistry to describe matter and its properties: the atomic structure, the properties of the elements and their ability to form compounds, molecular structures, chemical reactions, energy exchanges, states of matter, chemical kinetics, equilibria in solution, acid-base properties. 2) Ability to apply knowledge and understanding: having acquired application skills with reference to the balancing of reactions, stoichiometric calculations and problem solving on colligative properties, chemical equilibria, acid-base equilibria and the solubility product 3) Autonomy of judgment: to be able to independently evaluate and solve problems concerning the course contents. 4) Communication skills: having developed a good oral and written exposition capacity of the concepts acquired 5) Learning skills: being able to deepen the topics in different contexts and independently c)
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Teacher
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STORTI Roberta
(syllabus)
introduction States of aggregation of matter. Homogeneous and heterogeneous systems. Substances and chemical elements.
Atomic structure of matter Atomic properties: mass and dimensions. Avogadro number, mole concept. Chemical symbols and their quantitative meaning.
Structure of the atom Bohr model. Uncertainty principle. Wave nature electron. Atomic orbitals. Quantum numbers. Electronic configuration of the elements. Rules of the Aufbau. The periodic system of the elements. Periodic properties.
The chemical bond Ionic, covalent and coordination bonds. Bond properties: order, distance and energy. Electronegativity and dipole moment. Chemical bond theory: hybrid orbitals, resonance. Magnetic properties of molecules. Intermolecular bonds. Hydrogen bond.
Chemical formulas Nomenclature of inorganic compounds. Oxidation number. Typical molecules and ions structure.
Chemical reactions. The oxidoreductions
The gaseous state Read gases. State equation of ideal gases. Dalton's law for gaseous mixtures. Density and relative density of gases and mixtures gaseous. Average molecular mass of a gas mixture. Methods experimental for the determination of the molecular masses of substances gaseous. Real gases, Van der Waals equation. Kinetic theory of gases. The solid state Crystalline structures and their symmetries. Molecular, ionic solids, covalent and metallic. Polymorphism and allotropy. The liquid state Surface tension of a liquid. Viscosity and vapor pressure.
Thermodynamics Definition of thermodynamic system. State functions and variables of state. Cyclic and open transformations. Reversible transformations ed irreversible. Heat, work and internal energy. First principle of thermodynamics. Enthalpy and Hess's law. Entropy. Second principle of thermodynamics. Spontaneous processes. Free energy.
Chemical equilibrium Spontaneity and balance criteria in chemical reactions. Mass action law and its derivation. Homogeneous and heterogeneous equilibria.
Solutions Concentration and its units. Colligative properties of ideal solutions.
Acid-base equilibria General definitions. Strength of acids and bases. Acid-base structure and properties. Autoionization of water. The pH. Calculation of the pH of acidic, basic and saline solutions. Buffer solutions. Acid-base titrations and titration curves.
Solubility balances Solubility and factors that influence it. Solubility product. Common ion effect.
Elements of chemical kinetics Reaction speed. Arrhenius equation. Activation energy. Catalysis
(reference books)
SARANNO RESI DISPONIBILI DAL DOCENTE
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Dates of beginning and end of teaching activities
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From to |
Delivery mode
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Traditional
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Attendance
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not mandatory
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Evaluation methods
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Written test
Oral exam
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Note
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RINNOVO senza bando |
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