PHYSICAL CHEMISTRY

Knowledge and understanding: the student acquires the knowledge of the basic laws of chemistry and physics necessary to understand the origin and evolution of chemical, biochemical and biological phenomena and their applications in the pharmaceutical field.

Ability to apply knowledge and understanding: the student acquires the principles of thermodynamics and how these allow or set limits in the various energy transformations.

Learning skills: the student becomes able to apply chemical-physical models for the rationalization of experiments.

Making judgments: after consolidating the basic concepts, the student develops his critical ability in evaluating and interpreting the data that allow him to independently undertake subsequent research in the chemical-pharmaceutical sector

Ability to solve numerical problems: the theoretical bases are applied by the student both to critically evaluate possible solutions to analytical problems and to support arguments in the chemical-biological field.

Lectures and numerical exercises on the basic concepts and on the many and applications in the chemical-pharmaceutical field.

If lectures are given in a mixed or remote way, some changes may be introduced from what has been stated above, in order to comply with the program and visaged and reported in the syllabus.

THERMODYNAMICS

The first law of thermodynamics. Work and Heat. State functions: internal energy, enthalpy, heat capacity at constant pressure and volume. Thermodynamic cycles, reversible and irreversible processes. Thermochemistry. Standard enthalpy, enthalpy of reaction, enthalpies of formation, bond energy endothermic and exothermic processes The Hess's law.

Experimental techniques: calorimetry, TGA, DTA, DSC and ITC. Energetic metabolism, caloric value of food, and respiratory quotient.

The second principle of thermodynamics. Entropy and spontaneous processes. Entropy changes with temperature and pressure and in the phase transitions.

The third principle of thermodynamics. Absolute entropy. Gibbs free energy. Gibbs energy dependence on pressure and temperature.

Chemical equilibrium. Thermodynamic equilibrium constants. Homogeneous, heterogeneous and combined equilibria. Effect of temperature on equilibrium. Efficiency and performance of biochemical cycles.

ELECTROCHEMISTRY

Conductivity of electrolyte solutions, conductometry and conductometric titrations. Electrodic potentials, half-cells, batteries, Nernst equation. Standard reduction potentials and its applications in chemistry and biochemistry. Electrolysis.

CHEMICAL KINETICS

Rates of chemical reactions, reaction order. Integrated form of the kinetic equations of zero, first and second order. Parallel-competitive reactions and consecutive reactions. Pharmacokinetics: intravenous and oral administration. Reaction mechanisms and reaction order: the model of the activated complex. Catalytic and autocatalytic processes, propagation of an epidemic. Enzyme-catalyzed reactions: Michaelis-Menten equation. Enzyme inhibitors: competitive, noncompetitive, uncompetitive and mixed. Inhibition by substrate and product. Effect of temperature on reaction rate: Arrhenius equation.

TECHNICAL INVESTIGATION OF MOLECULAR STRUCTURE

Brief introduction to quantum mechanics. Description of the different atomic motions and related spectroscopic techniques. Vibrational spectroscopies: infrared, Raman and resonant-Raman. Electron spectroscopy, molecular orbitals, chromophores. Photophysical and photochemical processes. Photosynthesis. Laser stimulated emission.

1. Lecture notes are available.

2. G.K. Vemulapalli “Chimica Fisica” Ed. EDISES

3. P.W. Atkins, J. De Paula "Chimica Fisica Biologica" Volume 1, Ed. Zanichelli

4. R. Chang "Chimica Fisica" Volume 1 Ed. Zanichelli

5. A Gambi "Esercizi di chimica fisica" Ed. Zanichelli