CHEMISTRY - MODULE A
It is essential condition for addressing issues of Module A of the course the knowledge of concepts and basic fundamentals of mathematics (eg integral, exponential, logarithm, derivative, vector, tensor, matrix ...) and physical (eg the concepts of force, pressure, speed, potential energy, kinetic energy ...).
Module A of the course, implemented to be suitable for students of science-based degree programs, it offers a wide and timely introduction to the basic principles, theoretical and experimental of general chemistry, with frequent references to the real world. We expect, as learning results: i) understanding of the atomic model and its application to electronic configurations and the periodic table; ii) the thermochemical aspects and treated kinetic; iii) the theory of acids and bases; iv) chemical balance. Not to be neglected are the abilities in i) drawing Lewis structures; ii) predict the stereochemistry by VSEPR theory; iii) represent molecular orbital diagrams for simple diatomic molecules; iv) perform simple calculations in stoichiometry (including the reactions) balance. Finally, it is essential to learn to use periodic properties, intermolecular interactions, concepts of thermodynamics, kinetics and chemical equilibrium for the interpretation of wide phenomenology of general chemistry.
The main contents of the Module A are summarized as follows:
1. Definitions of matter, states of aggregation, element, compound, mixture, atom isotope.
2. Evolution of the atomic model. Elements of quantum mechanics: Schroedinger wave equation for hydrogen-like and electron atoms; atomic orbital; electron spin; Electronic configurations of the elements.
3. The periodic table and periodic properties: atomic radii, ionic, metallic, covalent; ionization energy, electron affinity, electronegativity.
4. The ionic bond: lattice energy, Born-Haber cycle. The covalent bond: Lewis formulas and their exceptions; partially polar covalent bond, dative and coordinative. Theory ''Valence Shell Electron Pair Repulsion''. Hybrid orbital bonding model. Molecular orbital model. The metallic bond: Sea theory of electrons; band theory for metals and semiconductors.
5. United liquid, solid and gaseous. Phase transitions and phase diagrams.
6. Chemical thermodynamics: enthalpy, entropy, Gibbs free energy; first, second and third law of thermodynamics.
7. Chemical equilibrium: thermodynamic equilibrium constants; Le Chatelier''s principle.
8. Chemical kinetics: reaction time; reaction of the first order, second, zero; Arrhenius equation; theory ''collisions'' and ''activated complex''.
9. Acids and bases: Arrhenius definitions, Broensted, Lewis; acid-base; ionization constant of the acid and base; pH scale. pH of aqueous solutions of strong acids, weak acids, strong bases, of weak bases; titrations.
10. Basics of radiochemistry and nuclear chemistry.
11. Solubility equilibria in water. Sparingly soluble salts: the effect common ion; effect of pH on the dissolution of a salt in aqueous solution.
12. Elements of electrochemistry.
13. Stoichiometry: the relationship between mass and mole; the balance of the reactions; preparing non-reactive or reactive solutions; conducting reactions in the absence or in the presence of limiting agent.
The Module A and Module B Course not provide for the adoption of a single reference text. Teachers recommend a set of books of general chemistry and organic chemistry (in Italian or English). Students can choose what suits them best. The set of suggested texts is not mentioned here because it can vary each academic year. In addition to the lessons, the teacher of Module B provides the projected slides, which are considered guidelines to the study, not substitute material of a textbook.
One of the text for the Form B could be:
John McMurry - Fundamentals of Organic Chemistry - 7th edition Brooks/Cole (4th edition from italian Zanichelli)
Each of the two teaching modules provides a final test and given a rating. The outcome of each trial is thirty: the test is deemed passed if the candidate gets a vote of at least 18/30. The final grade is the average, weighted on the number of credits, the outcome of the two tests.
Evidence relating to the items of the Form A is a written exam of 3 hours. It is multiple choice questions in sufficient numbers to cover all the topics of the lectures, including the stoichiometry. Each correct answer is awarded 1 point, while the incorrect answers are assigned zero score.
Evidence relating to the Form B is a written exam lasting approximately 2-2.5 hours when there are questions in an open form, short-answer questions, and also multiple-choice questions on the entire program carried out during the course. Each correct answer is awarded a score, while wrong answers is attributed to non-scoring.
The total score obtained by the candidate in each written test is normalized so as to be out of thirty. Following the publication of the votes, the teachers of Form A and Form B provide the opportunity very often disregarded, to view the writings by convening ad hoc candidates.