CHEMISTRY
Academic year and teacher
If you can't find the course description that you're looking for in the above list,
please see the following instructions >>
- Versione italiana
- Academic year
- 2022/2023
- Teacher
- SERENA BERARDI
- Credits
- 9
- Didactic period
- Primo semestre (primi anni)
- SSD
- CHIM/03
Training objectives
- The course aims at presenting the theoretical and experimental basis of Chemical Sciences. Furthermore, it will provide the basic knowledge needed for the understanding and the description of phenomena and transformations concerning atoms and molecules.
At the end of the course, the students will be able to:
* understand and predict the properties of chemical elements
* identify and classify different chemical species
* correlate molecular structure with its chemical properties
* understand the qualitative, quantitative and energetic meaning of a chemical equation
* understand the basic principles of chemical reactivity
* solve simple stoichiometric problems
* use specific lexicon Prerequisites
- Previous knowledge of the fundamentals of algebra (first and second-degree equations, properties of the exponents, scientific notation), analysis (exponential and logarithmic functions, representation via the cartesian coordinate system) and physics (properties of matter and units of measurement).
Course programme
- FIRST PART: The structure of matter (32 hours)
- Introduction. Scientific method and basic notions of physics.
- Atoms, molecules and ions. Atomic structure and elementary particles. Atomic number and Mass number. Isotopes. Atomic weight. Periodic table of elements. Mole and Molar mass.
- Classification of chemical compounds. Ionic and molecular compounds: Formulae and chemical nomenclature. Oxidation states.
- Electronic structure of atoms. The electromagnetic radiation Quantization of energy. Bohr’s atomic model. Wave-particle duality. De Broglie hypothesis. Indetermination principle. Elements of quantum mechanics. Quantum probability. Quantum numbers. Atomic orbitals. Electronic spin. Pauli exclusion principle. Electronic configuration of multi-electronic atoms. Periodic properties.
- Chemical bond. Valence electrons and Lewis structures. Formal charges. Resonance. Exceptions to the octet rule. Molecular geometry. VSEPR theory. Electronegativity and bond polarity. Valence bond (VB) theory. Hybridization. Sigma and pi bonds. Elements of molecular orbital (MO) theory.
- States of matter. Gaseous state: Ideal gases. Boyle’s law. Charles’ law. Avogadro’s hypothesis. State equation of ideal gases. Mixtures of gases and partial pressure. Real gases. Van der Waals equation. Liquid state: Intermolecular interactions. Vapor pressure. Evaporation. Surface tension. Viscosity. Solid state: Fusion. Sublimation. Phase transitions. State diagram. Ionic, molecular, covalent and metallic solids. Insulators and conductors. Semiconductors. Superconductors.
- Solutions. Dissolution and solubility. Concentration. Different expressions for the concentration. Dilution. Ideal and non-ideal solutions. Henry’s law. Raoult’s law. Colligative properties.
SECOND PART: How matter transforms (42 hours)
- Chemical reactions. Chemical reactions and equations. Classification of chemical reactions. Law of mass conservation. Law of charge conservation. Balancing a chemical reaction. Stoichiometry. Limiting reagent. Chemical yield. Redox reactions and their balancing.
- Thermodynamics and thermochemistry. Energy. Heat. Work. Law of energy conservation. Internal energy. State function. First principle of thermodynamics. Enthalpy. Thermochemistry. Entropy. Spontaneity and irreversibility. Second principle of thermodynamics. Gibbs free energy.
- Chemical equilibrium. Concept of chemical equilibrium. Equilibrium constant and reaction quotient. Le Chatelier’s principles.
- Chemical equilibria in aqueous solution. Acids and bases. Arrhenius definition. Brønsted-Lowry definition. Ionic product of water. Strong acids and bases. pH and pOH. Weak acids and bases. Dissociation constant. Hydrolysis. Buffer solutions. Polyprotic acids. Lewis definition of Acids and Bases. Solubility of ionic compounds. Solubility product. Common ion effect.
- Electrochemistry. Electrochemical cells. Batteries. Electrochemical potential. Electrical work and Gibbs free energy. Nernst equation. Electrolysis. Faraday’s law.
- Chemical kinetics. Reactivity and kinetics. Rate of a chemical reaction. Reaction order. Activation Energy. Catalysis. Enzymes.
- Nuclear Chemistry. Natural radioactivity. Nuclear reactions. Radioactive decay and its kinetics. Nuclear fission and fusion. Applications of nuclear chemistry. Didactic methods
- The course consists of theoretical lectures using PowerPoint presentation slides. The commented resolution of numerical problems and exercises will be also provided.
Learning assessment procedures
- The final examination is based on a written test, consisting of 8 questions/exercises dealing with stoichiometry and applications of theoretical principles. Each answer will be evaluated with maximum 4 points. The test duration is 2 hours. The use of periodic table, calculating machine and a list of formulae is allowed. To pass the exam, a mark equal or higher than 18 points out of 30 must be reached.
Reference texts
- " General Chemistry: Principles and Modern Applications" R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette (PICCIN)
"Chemistry" J. R. Townsend, P. M. Treichel, J. C. Kotz (EdiSES)
