Pharmacy

MARIA ELISA CRESTONI
CHIARA SALVITTI

The main objectives are the knowledge of the fundamental concepts of general chemistry and the skill to address numerical exercises relevant to the application of these concepts.
More specific objectives are the knowledge and application of fundamental concepts concerning the atomic structure, the chemical bond, the geometry and structure of molecules, the states of matter and their properties, the transitions phase, the main laws of thermodynamics and kinetics, the equilibria in solution and in the gas phase, the acids, bases and titration, the solubility equilibria, the electrochemistry and its application.
Further objectives are the ability to connect the acquired knowledge, the ability to communicate what the student has learnt, the ability to understand the contents of the following chemistry courses.

The main objective of the course is to: - provide principles and applications of general and inorganic chemistry, preparatory to various disciplines and necessary to describe and understand the structure and reactivity of matter; - to educate in an adequate scientific method and language; - transmit the ability to study in a critical and reasoned way.

A basic knowledge of the main concepts learned during the course of Maths.
There are no prerequisites.

Introductory notions. Subject of chemical research. Chemical phenomena. Fundamental laws of chemistry. Symbols and chemical notation. Amount. Atomic theory. Atoms and their properties. Mass and atomic weight. Avogadro's number. Atomic structure. Atomic spectra. Bohr model. Corpuscular and wave nature of the electron. Quantum numbers. Atomic orbitals. Electronic configuration. Chemical bond: concept of valence. The different types of bonds and their properties: order, energy, bond distance, dipolar moment. Valence bond theory and molecular orbitals. Hybrid orbitals, resonance. Structure of some typical molecules. Intermolecular bonds. States of aggregation and changes of state. Gaseous, liquid and solid state. Solutions and their colligative properties. Balance between phases and phase rules. Le Chatelier's principle. Basics of thermodynamics. Concept of balance. Principles of thermodynamics. Some thermodynamic functions. Thermochemistry. Chemical reactions and equilibria. Thermodynamic criteria for spontaneity and equilibrium in chemical transformations. Mass action law. Factors that influence the position of equilibrium. Electrolytic dissociation. Electrolytes and their properties in solution. Acids and bases. Definition and theories on acid-base equilibria. Relations between molecular structure and acid-base properties. Acid-base equilibria in aqueous solutions. Titulations. Indicators. Solubility. Solubility equilibria and factors that influence them. Partition equilibria. Electrochemical reactions. Redox reactions. Potentials, normal potentials, electromotive force, semi-elements, batteries, Nernst equation. Various types of electrolysis. Elements of kinetics. Speed, order, molecularity of a reaction, kinetic constant and its dependence on temperature. Arrhenius equation, activation energy. Basic notes on the theory of collisions and activated complexes. Catalysis. Outline of inorganic chemistry. Systematic nomenclature. Typical elements and their main compounds.
Stoichiometry exercises linked to the course. Notes on calculation methods. Exponential notation of numbers and relative elementary operations. Experimental measures and significant-figures. Logarithms. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Concept of mole. Chemical formulas. Law of definite proportions, law of multiple proportions, law of combination weights. Chemical equations and their quantitative significance. Balance of chemical equations. Oxidation number. Redox reactions and their balance. Equivalent weight of combination, neutralization and redox. Quantitative relationships between substances participating in a reaction. The solutions. Concentration and its units: molarity, normality, molality, mole fraction, weight percent, volume percent. Dilution and mixing of solutions. Density. Volumetric analysis. Titled solutions. The gaseous state: units relating to volume, pressure and temperature. The laws of ideal gases: Boyle's law, Charles's law, Gay-Lussac's law. Avogadro's principle. Equation of state of ideal gases. Density. Relative density. Gas mixtures. Partial pressures. Dalton's law. Colligative properties. Colligative properties of non-electrolyte solutions: vapor pressure, Raoult's law, ebullioscope rise and cryoscopic lowering, osmotic pressure. Electrolytic dissociation.

For the theory:
- M. Schiavello, L. Palmisano “Fundamentals of Chemistry” EdiSES
- R. H. Petrucci et al. "General Chemistry" Piccin
- F.Cacace, U. Croatto “Chemistry Institutions” La Sapienza Editrice
- Paolo Silvestroni «General chemistry», Fifth edition, Zanichelli
For stoichiometry:
- F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore Rome

F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore Rome

The development of the course includes lessons related to the topics listed in the program; analysis and discussion of recent scientific publications on inorganic chemistry topics

The course is based on lectures and stoichiometry exercises in the presence; in-depth information, clarifications, review can also be carried out in mixed mode (in person and remotely).

The final evaluation consists of a written test with 3 questions which, if passed, admits to the oral test.

Stoichiometry exercises related to the program carried out.
Questions on the lesson topics developed.