Pharmacy

The structure of Matter: Atoms, atomic structure and atomic electron configurations. The elements and their compounds. Bonding and molecular structure: fundamental concepts. Hybridization. Intermolecular forces. The properties of gases, liquids and solids. Metals. Thermodynamics and its application to chemical process. Solutions. Chemical equations and stoichiometry. Chemical equilibrium reactions in aqueous solutions. Principles of reactivity. Chemistry of acids and bases equilibria. Strong and soft acids and bases. Solubility. Principles of electrochemistry;

Basics knowdges of Chemistry

Testi Consigliati N. J. Tro “Chemistry:a molecular approach” .

Experimental Measures. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole concept. Chemical formulas. Chemical equations and their quantitative significance. Balancing chemical equations. Oxidation number. Oxidation-Reduction and Balancing Reactions. Quantitative relationships between substances involved in a reaction. Solutions. Concentration and its units: molarity, molarity, molar fraction, percent by weight, percent by volume. Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. The laws of the ideal gas: the ideal gas state equation. Avogadro's Principle. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of Non-Electrolyte Solutions. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. (van't Hoff). Thermal dissociation. Degree of dissociation. Indirect analysis. Mass action law. Different forms of equilibrium constant and their relationships. Equilibria in a homogeneous and heterogeneous phase. Application of the Le Chatelier principle. Mass Action law on Electrolyte. Ostwald Law. Acid-base reactions. Ionic water product. Definition of pH and pOH. Acid solutions and strong bases; of weak monoprotic acids and bases. Dissolution of polyprotic acids. Buffer solutions. Acid-base equilibria in saline solutions: salts of strong acid and weak base and of weak acid and strong base. Salts of polyprotic acids and anfolites. Solubility equilibria. Solubility and solubility product. Common ion effect. Condition of formation of precipitates. Galvanic cell. Normal potential. Nernst's equation. Various types of electrodes and their applications. Tests of past exams are carried out during the lessons.

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first- and second-degree equations, and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions); • Elements of physics (mechanics, thermodynamics, electromagnetism).

Cacace, M. Schiavello “Stechiometria” Bulzoni Editore

The course is organized as follows: - resolution of numerical problems in the classroom -self-assessment tests The student can ask the teacher for additional explanations by appointment.

Attendance to the course is optional, but strongly recommended.

The purpose of the exam consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject. The exam consists of a written test for the resolution of numerical exercises after which, a few days later, there is the oral exam. The student also has the possibility to defer the oral exam up to two appeals after the one in which he/she passed the written exam. Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette “Chimica generale” Piccin

The course is organized as follows: - resolution of numerical problems in the classroom -self-assessment tests The student can ask the teacher for additional explanations by appointment.

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.

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

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

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.

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

Experimental measurements and Significant Digits. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole. Chemical formulas. Chemical equations and their quantitative relationship. Stoichiometry and Balancing Reactions. Oxidation number. Balancing Redox reactions. Equivalent weight in the neutralization and redox reactions. Quantitative relationships between substances involved in a reaction. (10 hours) Concentration of solutions: molarity, normality, molarity, mole fraction, percent composition (by mass and by volume). Dilution and mixing of solutions. Density. Volumetric analysis. Titrations. The gaseous state: units relative to volume, pressure and temperature. Ideal gas laws: Boyle's law, Charles's law, Gay-Lussac's law. Avogadro's law. Ideal gas equation. Density. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of non-electrolyte solutions. Vapor pressure depression (Raoult Law), Boiling point elevation and freezing point depression, Osmotic Pressure. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. Van't Hoff factor. Thermal dissociation. Degree of dissociation. Indirect analysis. (10 hours) Chemical equilibrium - The Law of Mass Action. Different forms of equilibrium constant and their relationships. Balances in a homogeneous and heterogeneous phase. Le Chatelier’s principle in the equilibrium law: applications. The law of mass action in the electrolytic dissociation reactions. Ostwald law. Acid-base equilibria. Acid-base equilibria. Ionic water product. pH. Strong acids and bases solutions. Weak monoprotic acid and bases solutions ands. Dissolution of polyprotic acids. Buffer solutions. Hydrolysis of salt and ph. Salts of polyprotic acids. Titrations. Indicators. Solubility. Solubility product expression. Common ion effect. Condition of formation of precipitates. Fractioned Precipitation. Cell. Half-cell and their representation. Normal potential. Nernst's equation. Various types of electrodes and their applications.(16 hours)

Although no prerequisites are explicitly requested, it is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations.

F. Cacace, M. Schiavello “Stechiometria” Bulzoni Editore P. Michelin Lausarot, G.A. Vaglio “Fondamenti di stechiometria” Piccin

Attendance is not mandatory but strongly recommended.

Refer to what described by Prof. Maria Elisa Crestoni

The course has the following organization: • resolution of numerical problems in the classroom The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher.

The structure of Matter: Atoms, atomic structure and atomic electron configurations. The elements and their compounds. Bonding and molecular structure: fundamental concepts. Hybridization. Intermolecular forces. The properties of gases, liquids and solids. Metals. Thermodynamics and its application to chemical process. Solutions. Chemical equations and stoichiometry. Chemical equilibrium reactions in aqueous solutions. Principles of reactivity. Chemistry of acids and bases equilibria. Strong and soft acids and bases. Solubility. Principles of electrochemistry;

Basics knowdges of Chemistry

Testi Consigliati N. J. Tro “Chemistry:a molecular approach” .

Elements, Materials, and stoichiometry Fundamental particles in an atom. Atomic number and mass number. Nuclides, isotopes and elements. Relative atomic mass of a nuclide and an item. Mole. Substances, molecular formulas and units of the formula. Molecular masses and masses on its formal. Elemental composition of a compound and its formula minimum. Amount of substance and Avogadro constant. Molar mass. Quantitative representation of a chemical reaction. Reagents in stoichiometric proportions, in the absence and in excess. Electronic Structure of Atoms and the Periodic Classification of Elements The discovery of the electron, proton and neutron and their characteristics. The wave - particle of light. Atomic spectra. Emission spectrum of black body. Photoelectric effect. The quantum model of Bohr's hydrogen atom. Heisenberg Uncertainty Principle. De Broglie's formula. -Wave quantum model of the hydrogen atom: orbital and their shape. Electronic structure of atoms Polielettronica: the Pauli exclusion principle and the maximum multiplicity (or Hund). Periodic classification of elements: ionization energy, electron affinity, and metallic character of an element. Elementary theory of chemical bonding - Structure and Molecular Geometry Atomic bond (or covalent). Atomic radius. Simple atomic bonds, double and triple. Atomic bonds dative (or coordination). Polarity in the atomic bonds. And non-polar molecules: dipole moment. Electronegativity of the elements. Lewis structures. Resonance. Linking to delocalized electrons. Ionic bond: lattice energy. Valence bond theory. Hybrid orbitals. VSEPR theory. Intermolecular forces: dipole-dipole, hydrogen bonding, London dispersion forces. States of matter Gaseous state. Macroscopic properties of gases. And ideal gas equation of state. Gaseous mixtures: mole fractions, partial pressures, molecular mass (average). Solid state. Macroscopic properties of solids. Liquid state. Macroscopic properties of liquids. Solution (liquid): passage of a species in solution gas, solid or liquid. Solute concentrations, dilution and mixing of solutions. Energy of the physico-chemical Thermodynamic systems: state of equilibrium, reversible and irreversible transformations. 1 st law of thermodynamics. The changes in heat at constant volume and constant pressure in those: the state function enthalpy. Thermal effect in chemical reactions: thermochemical equation. Standard states of substances. Standard molar enthalpy of formation. Additivity of thermochemical equations (Hess's Law). The state function entropy. The function of state free energy (or Gibbs function). Criteria of spontaneity and equilibrium in chemical reactions and phase transformations. Free energy and useful work. Equilibrium between different phases of chemically non-reactive Systems to a single component Equilibrium between different phases of the same substance, Clausius-Clapeyron. State diagram of water, carbon dioxide. Two-component systems Equilibrium liquid-vapor mixture: Raoult's law and related diagrams and isobaric-isothermal and non-ideal solutions (positive and negative deviations); distillation. Phase rule and its applications to systems with one or more chemically non-interacting components. Composition of solutions and their properties Expressions of concentration. Solubility and saturated solutions. Colligative properties: lowering of vapor pressure of a solvent, Cryoscopy, Ebullioscopy, Osmosis. Chemical Kinetics: general Reaction rate. Reaction Mechanism: elementary reactions, and reactions to multiple stages. Rate law. Influence of temperature on reaction rate: activation energy. Transition state theory and activated complex. Homogeneous and heterogeneous catalysis. Reaction equilibria in homogeneous and heterogeneous systems Generalities on homogeneous and heterogeneous chemical equilibria. Constant standard of balance of a homogeneous reaction and / or heterogeneous. Influence of variation in composition or the total pressure on 'equilibrium at constant temperature. Influence of temperature equilibrium: van't Hoff equation. Applications of phase rule to multi-component systems interacting chemically equilibrium. Ionic equilibria in aqueous solution The law of equilibrium chemical reactions in solution. Standard constant of a reaction in solution. The reaction of water and its constant autoionizzazione standards. Solutions neutral, acidic or basic pH. Electrolytes in non-ionic and ionic structure of acids and bases, salts and anfoliti. Composition of balance. Calculating the pH of dilute solutions of solutes consisting of salts, acids and bases monoprotiche and solutions obtained by mixing solutions acido-forte/base strong, weak acid / strong base and strong base / weak acid. Buffer solutions. Equilibria in saturated solutions of sparingly soluble compounds. Solubility product. To common ion effect. Oxidation States of Elements and Redox Reactions Oxidation state of an element in a compound. Variation of the oxidation state of an element: oxidation, reduction and redox reactions (aqueous solution). Balancing chemical equations with the redox ion-electronic method. Electrochemical and corrosion potential Redox half reactions and balance them with the ionic-electronic method. Possibility of conversion of "chemical energy" to "electricity" and vice versa in electrochemical devices. Potential and standard potential of a galvanic half cells. Table of standard reduction potentials of redox couples and its applications. electrolysis. Electrolysis of H2O and in molten salts. Electrolytic refining of metals (Cu). Corrosion of metals (galvanic mechanism and differential aeration) and passivation. Methods of corrosion protection

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first and second degree equations and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions) • Elements of physics (mechanics, thermodynamics, electromagnetism).

Teoria: M. SCHIAVELLO-L. PALMISANO: Fondamenti di Chimica (quinta Edizione) - Ed. EdiSES P. Atkins, L. Jones, L. Laverman: Fondamenti di Chimica Generale - Zanichelli II ed. P. Silvestroni, Fondamenti di Chimica - XI edizione - casa ed. ambrosiana (È comunque possibile utilizzare altrii testi di Chimica di livello universitario) Per le esercitazioni di Stechiometria: - R. Michelin, P. Sgarbossa, M. Mozzon, A. Munari; CHIMICA - TEST ED ESERCIZI - Casa Editrice Ambrosiana - Stechiometria; F. Cacace, M. Schiavello; Bulzoni Editore - Stechiometria - Un avvio allo studio della chimica -Bertini, Luchinat, Mani, Ravera - Casa Editrice Ambrosiana - Esercizi di Chimica Generale; Alessandro Del Zotto; ed. EdiSES

The course has the following organization: • explanation of the topics in the classroom • resolution of numerical problems in the classroom • self-assessment tests The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher. The student can ask the teacher additional explanation on appointment.

Recommended. Attendance aims to improve the quality of learning and to give a track record for the exam. Students who cannot attend the lessons can download the detailed program and the teaching materials from the e-learning website, and receive assistance from the teacher.

The exam consists of a written test with numerical exercises and theoretical questions. The exams take place during the exam periods provided for by the university teaching regulations, while ongoing tests are excluded in order not to interfere with the conduct and regular attendance of the semester's lessons. The written test consists in solving 3-4 stoichiometry problems and 4-5 theoretical questions. The duration of the test is between 1 hour and a half and two hours depending on the number of questions / exercises. It is possible to consult the Periodic Table of the Elements and a form provided by the teacher. The test is considered passed if the student correctly completes at least 50% of the exercises and if he answers at least 50% of the questions correctly. The weight of the exercises and theoretical questions for the purposes of the overall assessment are equivalent. Exercises and questions cover the entire study program and are designed to ensure that the student has acquired the basic concepts of General Chemistry and has also acquired the ability to apply them to the main topics covered in the course. The purpose of the exam also consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject.

- P. Silvestroni, Fondamenti di Chimica - XI edizione - casa ed. ambrosiana

The course has the following organization: • explanation of the topics in the classroom • resolution of numerical problems in the classroom • self-assessment tests The student will find on the e-learning platform the slides and teaching material (examination procedures, program, recommended texts) useful for the preparation of the exam. It is understood that the slides are a guide to the exam topics, but can never replace the recommended texts and lectures given by the teacher. The student can ask the teacher additional explanation on appointment.

Experimental Measures. Unit of measure. Weight ratios in chemical combinations. Atomic weight, isotopic abundance, molecular weight, formal weight. Mole concept. Chemical formulas. Chemical equations and their quantitative significance. Balancing chemical equations. Oxidation number. Oxidation-Reduction and Balancing Reactions. Quantitative relationships between substances involved in a reaction. Solutions. Concentration and its units: molarity, molarity, molar fraction, percent by weight, percent by volume. Dilution and mixing of solutions. Density. The gaseous state: units relative to volume, pressure and temperature. The laws of the ideal gas: the ideal gas state equation. Avogadro's Principle. Gas mixtures. Partial pressures. Dalton Law. Colligative properties. Colligative Properties of Non-Electrolyte Solutions. Electrolytic dissociation. Weak and strong electrolits. Degree of dissociation. Effect of electrolytic dissociation on colligative properties. (van't Hoff). Thermal dissociation. Degree of dissociation. Indirect analysis. Mass action law. Different forms of equilibrium constant and their relationships. Equilibria in a homogeneous and heterogeneous phase. Application of the Le Chatelier principle. Mass Action law on Electrolyte. Ostwald Law. Acid-base reactions. Ionic water product. Definition of pH and pOH. Acid solutions and strong bases; of weak monoprotic acids and bases. Dissolution of polyprotic acids. Buffer solutions. Acid-base equilibria in saline solutions: salts of strong acid and weak base and of weak acid and strong base. Salts of polyprotic acids and anfolites. Solubility equilibria. Solubility and solubility product. Common ion effect. Condition of formation of precipitates. Galvanic cell. Normal potential. Nernst's equation. Various types of electrodes and their applications. Tests of past exams are carried out during the lessons.

It is important to master the following preliminary knowledge: • Fundamental concepts of elementary algebra, use of powers and logarithms, methods for the resolution of first- and second-degree equations, and systems of linear equations. Elements of mathematical analysis (limits, derivatives, integrals, functions); • Elements of physics (mechanics, thermodynamics, electromagnetism).

Cacace, M. Schiavello “Stechiometria” Bulzoni Editore

The course is organized as follows: - resolution of numerical problems in the classroom -self-assessment tests The student can ask the teacher for additional explanations by appointment.

Attendance to the course is optional, but strongly recommended.

The purpose of the exam consists in verifying the level of understanding and deepening on the subject exposed during the course. It also intends to evaluate the student's reasoning skills and the ability to summarize the arguments carried out in the vision of an organic framework of the subject. The exam consists of a written test for the resolution of numerical exercises after which, a few days later, there is the oral exam. The student also has the possibility to defer the oral exam up to two appeals after the one in which he/she passed the written exam. Exams are held during the exam periods provided for in the university teaching regulations, while intermediate tests are not in progress so as not to interfere with the regular attendance of the semester lessons, as established by the study program board.

R. H. Petrucci, F. G. Herring, J. D. Madura, C. Bissonnette “Chimica generale” Piccin

The course is organized as follows: - resolution of numerical problems in the classroom -self-assessment tests The student can ask the teacher for additional explanations by appointment.