GENERAL AND INORGANIC CHEMISTRY
cod. 13482

Academic year 2016/17
1° year of course - First semester
Professor
- Giovanni PREDIERI
Academic discipline
Chimica generale e inorganica (CHIM/03)
Field
Discipline chimiche
Type of training activity
Basic
80 hours
of face-to-face activities
10 credits
hub: PARMA
course unit
in ITALIAN

Learning objectives

The student should obtain knowledge of the theoretical fundamentals and of the application of the modern general and inorganic chemistry

Prerequisites

Elemental knowledge of Mathematics and Physics

Course unit content

THE ATOMIC NATURE OF MATTER AND THE ATOMIC STRUCTURE
CHEMICAL BONDING
THE GASEOUS STATE
THE SOLID STATE
THE LIQUID STATE
STATES OF THE MATTER AND PHASE TRANSITION
SOLUTIONS
THERMODYNAMICS
CHEMICAL EQUILIBRIUM
ACID-BASE EQUILIBRIA AND DISSOLUTION AND PRECIPITATION EQUILIBRIA
ELECTROCHEMISTRY
CHEMICAL KINETICS
INORGANIC CHEMISTRY
STOICHIOMETRY

Full programme

GENERAL CHEMISTRY
THE ATOMIC NATURE OF MATTER AND THE ATOMIC STRUCTURE
Atomic masses. Mole and Avogadro’s number. Isotopes. Electromagnetic radiation. Quantum theory. The Bohr atom. Wave-particle duality. The indeterminacy principle. The Schroedinger equation. Atomic orbitals and quantum numbers. The aufbau principle. Electronic configuration. The periodic table and the main periodical properties.
CHEMICAL BONDING
The ionic bond. The covalent bond. Homonuclear and heteronuclear diatomic molecules. Lewis structures. Electronegativity. The shapes of molecules, the VSEPR theory. The valence bond theory. The molecular orbital theory. The metallic bond. The hydrogen bond.
THE GASEOUS STATE
Properties. Pressure. Ideal gas. Boyle’s and Charles’s laws. Absolute temperature. The ideal gas law. The kinetic theory of gases. Graham’s law. Real gases. Intermolecular forces. Liquefaction, critical temperature.
THE SOLID STATE
Structure and properties. Crystalline solids and amorphous solids. Crystal lattices and unit cells. Symmetry. The crystal systems. Ionic, covalent, molecular and metallic crystals. Polymorphism. X-ray diffraction and crystal structure.
THE LIQUID STATE
Structure and properties. Surface tension. Evaporation. Vapor pressure. Boiling. Liquid crystals.
STATES OF THE MATTER AND PHASE TRANSITION
Phase diagrams for one- and two-components systems. Phase rule.
SOLUTIONS
The composition of solutions. Intermolecular forces and solution enthalpy. Ideal solutions. Dissolution mechanism. Solubility; influence of temperature and pressure. Vapor pressure. Raoult’s law and deviations. Fractional distillation, azeotropic mixtures. Colligative properties; cryoscopy and ebullioscopy; osmosis and osmotic pressure. Colloidal sospensions.
THERMODYNAMICS
State functions. The first law. Work and heat. Heat capacities. Enthalpy. Termochemistry and applications. Degradation of energy and disorder. Entropy. The second law. The third law. Gibbs free energy. Criteria for spontaneity.
CHEMICAL EQUILIBRIUM
Reactions and chemical equilibrium. Law of mass action. Equilibrium constants. Le Chatelier’s principle. Heterogeneous equilibria. The Gibbs free energy and the equilibrium constant. The temperature dependence of the equilibrium constants.
ACID-BASE EQUILIBRIA AND DISSOLUTION AND PRECIPITATION EQUILIBRIA
Acids and bases. Bronsted-Lowry and Lewis theories. The strength of acids and bases. Ionization constants. Polyprotic acids. Acid-base properties as a function of molecular structure. Ionic product of water. pH. Hydrolysis. Acid-base indicators. Acid-base titration curves. Buffer solutions. Amphoterism. Solubility product constant, common-ion effect.
ELECTROCHEMISTRY
Electrical conductivity. Electrolytic dissociation. Electrolysis: processes, Faraday’s laws, applications. Galvanic cells. Electrodes. Reduction potentials and applications. Corrosion and its prevention.
CHEMICAL KINETICS
Rates of chemical reactions. Reaction rates and concentrations. Dependence of concentrations on time. First-order and second-order reactions. Activation energy. Effect of temperature on reaction rates. Reaction mechanisms. Catalysis.
INORGANIC CHEMISTRY
Description of all the groups of the periodical table. Preparation and properties of the following elements and their main compounds: hydrogen, alkali and alkaline-earth metals, aluminum, carbon, silicon, tin, lead, nitrogen, phosphorus, oxygen, sulphur, halogens, titanium, chromium, manganese, iron, copper, silver, zinc, mercury.

STOICHIOMETRY
Inorganic nomenclature. Oxidation number. Reaction types: salification, exchange and redox reactions. Chemical equations balancing. Empirical and molecular formula; percentage of elements present in the compounds. Weight ratios among reagents and products; mole; limiting reagent; reaction yield. Solutions: composition, dilution and mixing. Chemical equivalent.

Bibliography

J.C.KOTZ, P.TREICHEL, G.WEAVER: "Chimica", IV edizione, 2010, EdiSES, Napoli.

P.ATKINS, L.JONES: "Principi di chimica", III edizione, 2012, Zanichelli, Bologna.

G. PREDIERI, "Tracce delle lezioni", 2013, Libreria Editrice S. Croce, Parma

Teaching methods

Lessons and exercises

Assessment methods and criteria

Written test and oral examination

Other information

Classroom tutoring; educational material in the website