CHEMISTRY
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- Versione italiana
- Academic year
- 2022/2023
- Teacher
- SIMONE MELONI
- Credits
- 6
- Didactic period
- Secondo Semestre
- SSD
- CHIM/03
Training objectives
- The course aims at presenting the theoretical and experimental foundations of the chemical sciences and provide an elementary introduction to the description of atomic and molecular phenomena.
The main knowledge acquired during the course are:
•fundamentals of atomic and molecular theory,
•elementary introduction to quantum mechanics and to quantum-mechanical description of atoms and molecules and nuclei,
•phenomenological theory of ideal gases,
•elementary introduction to the description of solids, liquids and solutions,
•fundamentals of classical thermodynamics,
•elementary thermodynamic description of chemical reactions,
•fundamentals of electrochemistry,
•introduction of chemistry of materials.
The main skills acquired during the course are:
•interpretation of fundamental properties of the elements,
•interpretation of structure and properties of atoms and molecules,
•calculation of stoichiometric quantities,
•calculation of properties of chemical reactions in solution,
•calculation of thermodynamic potentials. Prerequisites
- Although no preparatory learning is required, Students are strongly encouraged to achieve the following preliminary knowledge:
•basic mathematical concepts of linear and vector algebra, differential analysis, integral calculus, powers and logarithms, trigonometric functions, methods for solving first and second order equations,
•basic concepts of classical mechanics and electromagnetism. Course programme
- Atomic and molecular theory:
(1) Chemical elements and compounds, Proust's law, Daltons atomic theory, Relative atomic weights of elements.
(2) Atoms and molecules, Empirical formula, Molecular formula, Molecular weight (mass), Avogadro's number, Mole, Molar weight (mass).
(3) Rutherfords atomic model, Elementary particles, Proton, Neutron, Electron, Atomic number Mass number, Isotopes, Isotopic mixtures, Average atomic weight, Atomic and molecular ions, Ionic and molecular compounds.
(4) Types of chemical compounds, Oxidation states (numbers).
(5) Chemical reactions, Law of mass conservation, Law of charge conservation, Balance of a chemical reaction.
(6) Black-body radiation, Planck's hypothesis, Energy quantization, Bohr's atomic model, Photoelectric effect.
(7) Elementary introduction to basic concepts in quantum mechanics, Electron diffraction, Particles and waves, Quantum interference, Quantum probability, Base states, Probability amplitude and probability density, Operator and observables, Eigenvalues, Copenhagen interpretation, Energy base states, Hamiltonian operator, Two-base quantum systems.
(8) Base states of position, Schrödinger equation, Atomic orbitals, Electronic probability distribution, Quantum numbers, Electronic configuration of hydrogen atom, Electron spin, Multi-electron atomic configurations.
(9) Outer-shell electronic configuration and chemical properties of elements, Periodic Table.
(10) Chemical bond, Valence, Covalent bond.
(11) Molecular geometry, Valence-shell electron pair repulsion (VSEPR) model, Electronegativity.
(12) Symmetry and invariance, Noether theorem, Molecular geometry, Symmetry groups, Linear combination of atomic orbitals, Fundamentals of valence bond theory, Molecular orbital theory.
Sates of matter (8 hours)
(13) Gaseous state, The variables PVT, Ideal gases, Avogadro's hypothesis, State equation of ideal gases.
(14) Solid state, Ionic, molecular, covalent and metallic solids, Elementary introduction to the theory of solids, Periodic symmetry, Bravais' lattices, Insulators and conductors, Semiconductors, Structure of solid water, Hydrogen bond, Allotropy of elementary carbon, Silicon and silicate minerals, Quasi-crystals.
(15) Liquid state, Solutions, Concentration of solutions, Evaporation, Vapor pressure, Ideal solutions. Colligative properties
Chemical reactions:
(16) Oxidation-reduction reactions, Acids and bases, Dissociation constants, Ionic product of water, Acidic and basic solutions, Buffer solutions.
Thermodynamic and electrochemistry:
(17) Introduction to thermodynamic theory, Thermodynamic systems, Conversion of mechanical work into heat, Conservation of energy, Reversible and irreversible transformations, First principle of thermodynamic, State functions, Internal energy, Isothermal and adiabatic processes, Enthalpy, Carnot's cycle, Entropy, Time-reversible and -irreversible processes, Second principle of thermodynamics, Molecular interpretation of entropy, Boltzmann's equation.
(18) Gibbs free energy, Van't Hoff equation, Standard free energy, Free energy of chemical reactions, Free energy and equilibrium constant, Arrhenius equation, Spontaneous reactions.
(19) Free energy and electrical work, Electrochemical cells, Electrochemical potential, Nernst equation, Type of electrochemical cells, Electrolysis. Batteries and electrical energy storage. Didactic methods
- The course has the following organization:
•theoretical lessons,
•deepening of theoretical issues in the classroom,
•resolution of numerical problems in the classroom. Learning assessment procedures
- The purpose of the examination is to ascertain the level of understanding and deepening of the arguments developed during the course. The numerical and theoretical exercises are aimed at verifying Student's ability to achieve the goals stated in the section 'Educational Objectives'. It is also intended to evaluate the Student's ability to correctly employ the scientific language, to draw logically consistent conclusions from abstract concepts and general principles underlying the chemical theory, and to develop a critical approach to the interpretation of the theoretical and experimental foundations of chemical sciences.
The exam consists of a written test and an oral examination to be held on different days. The written exam requires the resolution of 10 theoretical and numerical problems, which are scored up to a maximum of 5/30. The outcome of the written examination determines the final grade. To pass the exam the student must achieve a minimum score of 18 out of 30. Reference texts
- Modern chemistry
David W. Oxtoby, H. P. Gillis, Alan Campion
(Thomson Brook/Cole)
General chemistry
Ralph H. Petrucci,
(Piccin-Nuova Libraria)
Inrìtroductory Chemistry Essentials
Nivalo J. Tro
(Pearson)
Chemistry and Chemical Reactivity
John C. Kotz, Paul M. Treichel, John R. Towsend
(EdiSES)
Chemical principles - the quest for insights
Peter Atkins, Loretta Jones
(W. H. Freeman and Co.)
Lecture notes distributed by the teacher on the various arguments of the course.
Slides utilized during the lessons.
