First cycle
degree courses
Second cycle
degree courses
Single cycle
degree courses
School of Science
Course unit
SCO2045559, A.A. 2018/19

Information concerning the students who enrolled in A.Y. 2017/18

Information on the course unit
Degree course First cycle degree in
SC1157, Degree course structure A.Y. 2014/15, A.Y. 2018/19
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Number of ECTS credits allocated 6.0
Type of assessment Mark
Course unit English denomination LABORATORY OF PHYSICAL CHEMISTRY
Website of the academic structure
Department of reference Department of Chemical Sciences
Mandatory attendance No
Language of instruction Italian
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

Teacher in charge VINCENZO AMENDOLA CHIM/02

ECTS: details
Type Scientific-Disciplinary Sector Credits allocated
Core courses CHIM/02 Physical Chemistry 6.0

Course unit organization
Period Second semester
Year 2nd Year
Teaching method frontal

Type of hours Credits Teaching
Hours of
Individual study
Laboratory 4.0 48 52.0 2
Lecture 2.0 16 34.0 No turn

Start of activities 25/02/2019
End of activities 14/06/2019
Show course schedule 2019/20 Reg.2014 course timetable

Examination board
Board From To Members of the board
1 2019/20 20/01/2014 30/11/2020 AMENDOLA VINCENZO (Presidente)
ANTONELLO SABRINA (Membro Effettivo)
DURANTE CHRISTIAN (Membro Effettivo)

Prerequisites: Basic knowledge of mathematics, physics, physical chemistry and general chemistry and in particular:
The scientific method. State of aggregation of the matter. Mixtures (homogeneous, heterogeneous) and pure substances. The atomic number and the mass number. Isotopes. Atomic mass unit. Relative atomic mass. Mole. Minimum formula, molecular formula. Oxidation numbers. Chemical balancing. Balancing of non-redox, and redox reactions. The chemical bond: covalent, ionic and metallic. Structure of the atom according to quantum mechanics. Schrödinger equation. Pauli exclusion principle. Acid / base properties of oxides. LCAO-MO theory for homonuclear and heteronuclear diatomic molecules. Molecular orbitals and HOMO-LUMO states. Perfect gas law. Dalton's law. Kinetic theory of gases. Maxwell-Boltzmann distribution of molecular velocities. Real gases. Van der Waals equation. Intermolecular interactions. Solid structure.
Chemical equilibrium. Law of mass action. Le Chatelier's principle. Chemical thermodynamics. First and second law of thermodynamics. Gibbs free energy. Criteria for spontaneity of a chemical reaction. Relationship between equilibrium constant and ΔG °.
Equilibrium in solution. Strong and weak electrolytes. Acids and bases. Hydrolysis of salts. Buffer solutions. Introduction to phase diagrams p, T for a component. Phase rule. Phase diagrams for two-component volatile mixtures. Raoult's law. Distillation. Azeotropic mixtures. Colligative properties. Electrochemistry. Standard reduction potentials. Nernst's equation. The batteries. Electrolysis. Faraday's laws. Overvoltage. Chemical kinetics. The rate and the order of reaction. Activation energy. Arrhenius equation.
Basics. Real numbers. Inequalities. Elements of trigonometry. Exponentials and logarithms. Summations. Limitations. Continuous functions. Derivatives. A tangent line to the graph of a function. Fundamental theorems of differential calculus. Relative and absolute maxima and minima. Exponential and logarithmic trigonometric functions. Study of a function. Definite integrals. Solid volumes of rotation. Lengths of function graphs. Generalized integrals.
Numerical series. General notions. Taylor and Mac Laurin series.
Differential equations of the first linear order and separable variables. Models described by linear differential equations of the first order. Differential linear second-order equations with constant coefficients.
Functions of multiple variables. Limitations. Continuity. Partial derivatives. Differentiability. Tangent plans. Level curves. Directional derivative. Gradient vector. Maximum and minimum relative. Saddle points. Maximum and minimum limits.
Physical quantities and units of measurement. Work and energy: work of a force, power, kinetic energy, conservative forces, potential energy and conservation of mechanical energy.
inertia principle and force concept, Newton's laws, friction force.
Principles of thermodynamics. Thermodynamic potentials. Thermodynamic properties of pure substances. Phase equilibria of pure substances. Thermodynamic properties of multi-component systems. Ionic solutions. Galvanic cells and their thermodynamic description. Electricity and electric currents. Coulomb's law. Electric field. Electric potential of a charge and a distribution of charges. Electrostatic induction. Conductors. Insulators. Electric currents. Ohm's law. Joule's law. RC circuits. Semiconductors. Electromagnetism. Maxwell equations. Diffraction of light.
Target skills and knowledge: Learning of the "experimental method" for the measurement of physical quantities with relative uncertainties.
Direct and indirect measures.
Application of the experimental error propagation theory.
Verification and consolidation of concepts of Thermodynamics (Gibbs free energy, entropy, reaction enthalpy) and Spectroscopy (absorption and fluorescence).
Diffusion of molecular substances in fluid media.
Application of mathematical models for the interpretation of experimental results.
Ability to draw up scientific reports on the work performed.
Examination methods: Oral interview on the contents of the classroom lessons on the experiences carried out in the laboratory. The interview will consist of a minimum of two questions about general arguments about lessons, lab experiences and laboratory reports.
The final grade will take into account the results of the interview and the reports on the activity carried out in the laboratory.
Assessment criteria: Ability to expose the concepts introduced during the course during the oral examination.
Ability to explain the topics logically during the oral exam.
Ability to draw up scientific reports on laboratory experiences.
Ability to establish logical connections between the different topics covered during the course.
Course unit contents: - Lectures:
Introduction to the theory of errors in laboratory measurements.
Outline the use of IT tools for data analysis.
Theory of ionic conductivity in solution.
Diffusion processes in the liquid phase.
Reminder of the UV-Vis absorption spectroscopy and fluorescence emission.
Electrochemical systems and equilibrium thermodynamics, variation of G, H and S related to redox processes.
Illustration of experiences, methodology and instrumentation with particular regard to the processing of experimental data.
- Laboratory experiments:
6 experiences are planned:
Determination of the ionic conductivity of a strong electrolyte in the aqueous phase;
Determination of the diffusion coefficient of a dye molecule in the aqueous phase (via UV / VIS);
Study of phenomena of collisional quenching of fluorescence;
Nanosensor for the colorimetric quantification of a peptide;
Determination of thermodynamic quantities by measurements of emf of a stack;
Determination of thermodynamic quantities by cyclic voltammetry.
Planned learning activities and teaching methods: Introductory theoretical lectures in the classroom followed by laboratory experiences.
The laboratory experiences consist of both a practical part and a part of data processing carried out with the assistance of a teacher.
Additional notes about suggested reading: Lecture notes for teachers and specialized articles recommended in class.
Textbook as indicated below.
Textbooks (and optional supplementary readings)
  • Atkins, P. W.; De_Paula, Julio, Atkins' physical chemistryPeter Atkins, Julio De Paula. Oxford: Oxford university press, 2014. Cerca nel catalogo

Innovative teaching methods: Teaching and learning strategies
  • Laboratory
  • Problem solving

Innovative teaching methods: Software or applications used
  • SciDaVis

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