First cycle
degree courses
Second cycle
degree courses
Single cycle
degree courses
School of Science
INDUSTRIAL CHEMISTRY
Course unit
GENERAL AND INORGANIC CHEMISTRY
SCN1035672, A.A. 2018/19

Information concerning the students who enrolled in A.Y. 2018/19

Information on the course unit
Degree course First cycle degree in
INDUSTRIAL CHEMISTRY
SC1157, Degree course structure A.Y. 2014/15, A.Y. 2018/19
N0
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Number of ECTS credits allocated 13.0
Type of assessment Mark
Course unit English denomination GENERAL AND INORGANIC CHEMISTRY
Website of the academic structure http://www.chimica.unipd.it/corsi/corsi-di-laurea/laurea-chimica-industriale
Department of reference Department of Chemical Sciences
E-Learning website https://elearning.unipd.it/chimica/course/view.php?idnumber=2018-SC1157-000ZZ-2018-SCN1035672-N0
Mandatory attendance No
Language of instruction Italian
Branch PADOVA
Single Course unit The Course unit can be attended under the option Single Course unit attendance
Optional Course unit The Course unit can be chosen as Optional Course unit

Lecturers
Teacher in charge MAURO SAMBI CHIM/03
Other lecturers FRANCESCO SEDONA CHIM/03

Mutuating
Course unit code Course unit name Teacher in charge Degree course code
SCN1035672 GENERAL AND INORGANIC CHEMISTRY MAURO SAMBI SC1156

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Basic courses CHIM/03 General and Inorganic Chemistry 11.0
Core courses CHIM/03 General and Inorganic Chemistry 2.0

Course unit organization
Period Annual
Year 1st Year
Teaching method frontal

Type of hours Credits Teaching
hours
Hours of
Individual study
Shifts
Practice 3.0 30 45.0 No turn
Laboratory 2.0 24 26.0 No turn
Lecture 8.0 64 136.0 No turn

Calendar
Start of activities 01/10/2018
End of activities 28/06/2019
Show course schedule 2019/20 Reg.2014 course timetable

Examination board
Examination board not defined

Syllabus
Prerequisites: None
Target skills and knowledge: Classroom lectures are meant to provide basic, yet rigorous foundations in chemical knowledge to undergraduate beginners. Exercises provide basic elements of stoichiometric calculations. Fundamental prevention and safety issues regarding chemical substances, workplace behavior and first aid norms, the correct use of chemical glassware and simple instrumentation, as well as and the most common experimental procedures are provided through several laboratory experiences.
Examination methods: The exam consists of three parts.
(a) A written test lasting three hours, which requires the resolution of three articulated exercises, each of which combines different knowledge and skills learned mainly in the part of exercises, and the answer to some questions of inorganic nomenclature. Within a calendar year after passing (with a score of at least 17/30), the written test gives access
(b) the oral test, in which the knowledge and skills mostly acquired by the student in the theoretical part of the course are assessed, typically through three questions, for a typical overall duration of 20-30 minutes. Two negative results of the oral test require the repetition of the written test.
(c) Finally, the laboratory activity is assessed on the basis of written reports produced by the student, compiled respecting a predetermined grid of questions.
The final grade is the weighted average of the evaluations obtained in the three tests, with weights of 38%, 46% and 16%, respectively.
Assessment criteria: The criteria for assessing the written test are the correctness of the numerical results, the traceability of procedures used to obtain them, the internal consistency between logically interdependent results and the rigorous usage of the correct units of measurement associated with the physical quantities. Criteria for assessing the oral test are rigorous quantitative demonstrations, the degree of detail in the answers, the ability to establish links between different aspects of a chemical phenomenon. The acquisition of the contents of the laboratory experiences is evaluated on the basis of the accuracy, completeness, conciseness and language quality in preparing the reports.
Course unit contents: CLASSROOM LECTURES: The scientific method. States of matter. Mixtures (homogeneous, heterogeneous) and pure substances. Elements and compounds; atoms and molecules. Atomistic theory. The atomic number and the mass number. Isotopes. Atomic mass units. Relative atomic mass. Mole. Percentages in mass, minimal formula, molecular formula. Oxidation numbers and their determination. Balancing chemical equations in molecular / ionic form. Mass and charge balance. Balancing non-redox reactions. Oxidation numbers method and half-reactions method of balancing redox reaction equations.
The chemical bond I: covalent, ionic and metallic bonds. Lewis structures. VSEPR method.
Atomic structure according to quantum mechanics. Bohr's atom and its limits. Uncertainty principle. Wave-particle duality. Wave function. Schrödinger equation and its solutions for the one-electron atom. Atomic orbitals. Electron spin. Introduction to polyelectronic atoms. Shell model of the atom. Aufbau principle. Pauli exclusion principle. Hund's rule.
Periodic properties: atomic and ionic radius, ionization energy, electron affinity, electronegativity. Stoichiometry of binary hydrides and oxides. Acid / base properties of oxides.
The chemical bond II. LCAO-MO theory for diatomic homonuclear and heteronuclear molecules.
Brief comparison of VB and the MO theories. Carbon hybrid orbitals.
Perfect gas law. Dalton's law. Kinetic theory of gases. Maxwell-Boltzmann distribution of molecular speeds. Effusion. Real gases. Van der Waals equation. Intermolecular interactions. Structure of solids.
Chemical equilibrium. Law of mass action. Le Chatelier's principle. Chemical thermodynamics. First and second laws of thermodynamics. Hess's law. Gibbs free energy. Criteria of spontaneity of a chemical reaction. Relationship between equilibrium constant and ΔG°.
Equilibria in solution. Strong and weak electrolytes. Acids and bases according to Aarhenius, Brønsted-Lowry, Lewis. Hydrolysis of salts. Buffer solutions. Slightly soluble salts.
Introduction to p, T phase diagrams for a single component. Phase rule. Phase diagrams for mixtures of two volatile components. Raoult's law. Distillation. Azeotropic mixtures. Colligative properties.
Electrochemistry. Standard reduction potentials. Nernst equation. Batteries. Corrosion and corrosion protection. Electrolysis. Faraday's laws. Overpotential.
Chemical kinetics. The speed and the order of reaction. Half-life. Activation energy. Arrhenius equation. Reaction mechanisms. Elementary processes. Rate-determining step. Catalysts.
NUMERICAL EXERCISES: exercises and demonstrations on topics covered in classroom lectures, with which they are closely matched.
LABORATORY: (1) Properties of some physical and chemical processes (acid / base reactions, salt formation, endo / exothermic processes); (2) Experiments in electrochemistry (redox reactions, Daniell cell, electrolysis of water); (3) Chemical equilibrium (effects of concentration, temperature and common ion) (4) acid-base titrations (strong / strong and weak / strong acid-base titrations); (5) Distillation of an aqueous solution of hydrochloric acid; (6) the cycle of copper (redox reactions, acid / base equilibria and precipitation applied to the chemistry copper in aqueous solution).
Planned learning activities and teaching methods: Classroom lectures, classroom numerical exercises, laboratory experiences. One or two hours a week are generally reserved for students' free questions, for the revision of complex concepts learned during the week, for optional in-depth discussions of selected topics.
Additional notes about suggested reading: Lecture notes, lecture slides available on the lecturer's website:

http://www.chimica.unipd.it/mauro.sambi/pubblica/didattica.html
Textbooks (and optional supplementary readings)
  • D. W. Oxtoby, H. P. Gillis, A. Campion, Principles of Modern Chemistry. --: Ed. Brooks/Cole, Cengage Learning, --. Cerca nel catalogo
  • S. S. Zumdahl, Chemical Principles. --: Ed. Brooks/Cole, Cengage Learning, --. Cerca nel catalogo
  • P. Michelin Lausarot , G. A. Vaglio, Fondamenti di stechiometria. --: Piccin, --. Cerca nel catalogo
  • P. Ferri, Calcoli stechiometrici. --: ETS, --. Cerca nel catalogo

Innovative teaching methods: Teaching and learning strategies
  • Lecturing
  • Laboratory
  • Problem based learning
  • Working in group
  • Questioning
  • Action learning
  • Video shooting made by the teacher/the students
  • Use of online videos

Sustainable Development Goals (SDGs)
Quality Education Responsible Consumption and Production Climate Action