00088 - Chemistry

Learning outcomes

The course is aimed to provide to the students a basic understanding of the structure of matter and of the thermodynamic and kinetic principles that rule its transformation. The students will also acquire the basic knowledge to understand the connections among the structure, the properties and the reactivity of the organic molecules with particular emphasis on their acid-base characteristics. The student will be able to critically analyze, from a molecular point of view, the chemical reactions that take place in the agro-environmental ecosphere.

Course contents

Introduction. What is Chemistry?

The atomic structure. The atomic theory; atomic composition; atomic and mass numbers. Isotopes and atomic weight. Bohr's atomic theory; energy quantization. Atomic structure and quantum theories ; orbitals, quantum numbers and spin. Orbitals in polyelectronic atoms, electronic configurations of elements. Periodic Table and relation with electronic configuration. Ionization energy, electron affinity, atomic and ionic radii.

Molecules and compounds. Minimum and molecular formula. Valence and oxidation degrees. Nomenclature. Lewis structures of molecule and polyatomic ions. Molecular geometry. Resonance, isomers, PM and PF. The mole and NA. Molar mass and numbers of moles.

Chemical bond. General concepts. Ionic bond: lattice energy, stoichiometry and geometry of ionic compounds. Covalent bonds: electronegativity and bond polarity; bond energy and distance. Valence bond theory and molecular orbital theory. Ibridization. Metallic bond. Intermolecular forces: Van der Waals, London and hydrogen bond.

The states of matter. Solid, liquid and gaseous states: general properties. Gas theoretic model. Equation of state for gases. Gas mixtures: partial pressure. Changes of state and phase diagrams.

Solutions and their properties. General properties of solutions. Concentration. Solubility. Solutions of electrolytes. Ideal, diluted or concentrated solutions. Changes of state in liquid solutions. Raoult and Henry laws. Osmosis. Colligative properties and determination of molecular weight.

Chemical reactions. Chemical reactions and equations; mass conservation law. Equation balancing. Redox reactions and their balancing. Reactions in solution and ionic equations; redox half-reactions. Mass relation in the reactions; equivalent weight.

Chemical thermodynamics. General aspects of thermodynamics; reactions and heat ( internal energy, enthalpy), spontaneous reactions (entropy, free energy), study of the free energy variation during a chemical reaction.

Chemical equilibria. Complete and uncompleted reactions. The equilibrium constants: Kc and Kp. Homogeneous and heterogeneous equilibria. Le Chatelier's principle. Solubility and Kps. Effects of P,V,T, concentrations of reagents and products on the position of the equilibria. Simultaneous equilibria. Stoichiometric calculations on equilibria.

Acids and bases. Protonic theory of acid and bases. Autoionization; Kw. Ka and Kb. Polyprotic acids and bases. Molecular structure and acid/base properties. Acidity of solutions: pH. Acid-base reactions. Buffers. pH and solubility.

Electrochemistry. Galvanic cells. Reduction potentials and cell e.m.f. Electrolysis

Kinetics. Generalities of Kinetic: rate of reaction, kinetic equation. Reaction mechanism. Activated complex and activation energy. Catalysis.

Organic Chemistry. Definition of hybrid and hybridation concepts. Organic acids and bases, nucleophilies and electrophiles. Description of the main functional groups and organic compounds classes with their nomenclature, and references to their structures and possible isomers and stereochemistry. Aminoacids, structures, acid-base properties, peptidic ligand and proteins. Lipids: fats and oils. Soaps. Phospholipids. Steroids. Biological membranes.

Readings/Bibliography

Slides of the lessons, examples of exercises with solutions are available on the internet.

Any book of General Chemistry for UNIVERSITY students is suitable for the preparation of the exams.

Some examples are the following

John C. Kotz “CHIMICA”, Ed. Edises

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette "CHIMICA GENERALE, Principi ed applicazioni moderne”, Ed. PICCIN.

Teaching methods

Class lessons and exercises discussed in class with the professor, power point presentations.

Assessment methods

The students will have to take a written test, they will have 2 hours minutes time to solve

3 numerical exercises (redox reactions, acid-base equilibria, colligative properties, etc.), each exercise will be evaluated with a maximum score of 11 points.

The students with an evaluation equal or higher than 18/30 will pass the exam.

The students that will pass the written test will have the possibility to take the oral part of the examination

NB: for the written test students will have to bring a valid identity document with picture, the periodic table of the elements and a scientific calculator. Mobile phones will be forbidden (even in the scientific calculator mode). Students will NOT be allowed to consult the chemistry book for numeric exercise resolution.

Teaching tools

PC connected projector, overhead projector for class lessons.

Distribution of copies of extra-materials when needed and possibility to download the files of the lessons from websites of the professors.

Office hours

See the website of Marco Montalti