GENERAL AND INORGANIC CHEMISTRY
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- Versione italiana
- Academic year
- 2022/2023
- Teacher
- SERENA BERARDI
- Credits
- 9
- Didactic period
- Primo Semestre
- 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.
- 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.
- 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 (40 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. Indicators. Titrations. 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. 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
- Written test plus oral examination.
The written test consists of 9 questions/numerical exercises on stoichiometry and/or application of theoretical principles. 4 of these questions deal with the First Part of the Course Programme, and will be evaluated with maximum 2.5 points each. The remaining 5 questions deal with the Second Part of the Course Programme, and will be evaluated with maximum 4 points each. The total test duration is 90 minutes. The use of periodic table, calculating machine and a list of formulae is allowed. To pass the exam, a score equal or higher than 18 points (at least 6 from the First Part and 12 from the Second) out of 30 must be reached. The passed writing test stays valid for 1 year, during which the student must pass also the oral examination. The latter will consist of one question on the “Chemical Bond” section and on the discussion of the possible wrong answers given in the written test. The oral exam will be separately evaluated, and a mark equal or higher than 18 points out of 30 is needed to pass it. The final mark will result from the averaged score of both the written test and the oral exam. In order to get the maximum mark (30 cum laude), both the written test and the oral examination must be perfect.
During the academic year, at least 6 exam sessions will be available for the students.
Furthermore, at the beginning of November 2022, students will be given the possibility to have a first partial written exam (not mandatory), dealing only with the topics of the First Part of the Couse. This partial test will consists of 4 questions/numerical exercises (maximum 2.5 points each) and will last 30 minutes. This test is passed with a score equal or higher than 6/10. In this latter case, the test will stay valid until July 31st 2023; by that time, the student must pass also the second partial test (dealing with the topics of the Second Part of the Couse), and then the oral examination. The second partial test will take place in January-February 2023, on the same dates of the total written examinations; it will consists of 5 questions/numerical exercises, scored with maximum 4 points each, and will last 60 minutes. The second partial test is passed with a score equal or higher than 12/20 and stays valid for 1 year. By that time, the student must pass also the oral examination. The second test will be available only for students having passed the first partial test.
The students who do not pass both the partial tests or who decide not to take this opportunity, must take the total written test, as described above. Also during the partial tests, the use of periodic table, calculating machine and a list of formulae is allowed. 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)
