THREE-DIMENSIONAL MODELING

Course objectives

OBIETTIVI FORMATIVI A - Conoscenza e capacità di comprensione OF 1) Conoscere la struttura della tavola periodica OF 2) Conoscere il significato delle varie proprietà atomiche (raggio, elettronegatività, affinità elettronica, calore di atomizzazione) OF 3) Conoscere la struttura del nucleo atomico OF 4) Conoscere i principi degli equilibri in soluzione OF 5) Comprendere il significato di una costante condizionale di formazione OF 6) Conoscere la reattività in acqua di specie inorganiche OF7) Conoscere i concetti di radiofarmaco diagnostico e terapeutico B – Capacità applicative OF 8) Saper illustrare l’andamento periodico delle principali proprietà OF 9) Saper dedurre la stabilità di un nucleo atomico dal numero di protoni e neutroni OF 10) Saper calcolare il pH di acidi e basi forti e deboli per via algebrica OF 11) Saper calcolare il pH di acidi e basi forti e deboli e loro miscele per via grafica OF 12) Saper prevedere l’ordine di precipitazione tra più sali sia per via algebrica che via grafica OF 13) Saper calcolare la concentrazione di prodotti e reagenti di reazioni all’equilibrio C - Autonomia di giudizio OF 14) Essere in grado di valutare le principali proprietà di un elemento in base alla posizione sulla tavola periodica OF 15) Essere in grado di progettare la sintesi di un nucleo atomico di massa assegnata OF 16) Essere in grado di prevedere lo spostamento di una reazione ionica all’equilibrio D – Abilità nella comunicazione OF 17) Saper illustrare un diagramma di distribuzione. OF 18) Saper illustrare le proprietà degli elementi presenti nei vari gruppi OF 19) Saper descrivere la produzione e la ricostruzione di un radiofarmaco E - Capacità di apprendere OF 20) Avere la capacità di consultare la letteratura sugli argomenti trattati nel corso OF 21) Avere la capacità di comprendere una procedura analitica di laboratorio basata su equilibri ionici in soluzione A - Knowledge and understanding OF 1) Knowing the structure of the periodic table OF 2) Knowing the meaning of the different atomic properties (atomic radius, electronegativity, electron affinity, atomization heat) OF 3) Knowing the structure of the atomic nucleus OF 4) Knowing the principles of solution equilibria OF 5) Understanding the meaning of a conditional formation constant OF 6) Knowing the reactivity of inorganic species in water OF7) Knowing the meaning of diagnostic and therapeutic radiopharmaceuticals B - Application skills OF 8) Being able to illustrate the periodic behavior of the main atomic properties OF 9) Being able to deduce the stability of an atomic nucleus from the number of protons and neutrons OF 10) Being able to algebraically calculate the pH of strong and weak acids and bases OF 11) Being able to graphically calculate the pH of strong and weak acids and bases and their mixtures OF 12) Being able to predict both algebraically and graphically the precipitation order between different salts OF 13) Being able to calculate the concentration of products and reactants of equilibrium reactions C - Autonomy of judgment OF 14) Being able to evaluate the main properties of an element basing on its position on the periodic table OF 15) Being able to design the synthesis of an atomic nucleus of assigned mass OF 16) Be able to predict the displacement of an ionic equilibrium D - Communication skills OF 17) Being able to illustrate a distribution diagram OF 18) Being able to illustrate the properties of the elements belonging to the various groups OF 19) Being able to describe the production and reconstruction of a radiopharmaceutical E - Ability to learn OF 20) Having the ability to consult the literature on the topics covered in the course OF 21) Having the ability to understand an analytical laboratory procedure based on ionic equilibria in solution

Channel 1
BARBARA CHIAVARINO Lecturers' profile

Program - Frequency - Exams

Course program
Complements of General Chemistry. The Periodic Table. Radial and angular part of the electron wave function. Energy levels of atomic orbitals as a function of the atomic number. Characteristic electronic valence configurations. Electrons and valence orbitals of an atom. Electronic valence configurations of ions. Shielding effect and effective nuclear charge. Slater rules. Variation of Z* in the periodic table. Types of atomic radii. Periodicity of covalent radii. Scandide and Lanthanide Contraction. Periodic behavior of ionic radii. Effects of relativity on the orbital. Electronegativity of Pauling. Periodic behavior of Pauling electronegativity. Electronegativity of Allred-Rochow. Oxidation number. Periodic behavior of the most common oxidation numbers. Periodic behavior of the ionization energies and electronic affinity. Binding energies and single frequency. Periodic behavior of the heats of atomization of the elements. Physical properties of the elements, the main allotropes of non-metals. The metallic bond. Physical properties of metals. Standard reduction potentials. Periodic trends of stability of high oxidation states and acids. Stability of low oxidation states. The series of activity of metals. Systematic of Inorganic Chemistry. Hydrogen. Elements of the Group I. Properties and reactivity. Elements of Group II. Properties and reactivity. Elements of Group III. Properties and reactivity. Group IV elements. Properties and reactivity. Elements of the V Group. Properties and reactivity. Elements of Group VI. Properties and reactivity. Elements of Group VII. Properties and reactivity. Noble gases. Analytical Chemistry. Purpose of Analytical Chemistry. Steps of sample preparation. Classification of analytical methods. Evaluation of analytical data. Precision and Accuracy. Types of Errors. The statistical treatment of random. Effects and correction of systematic errors. Blunders. The chemical equilibrium. Effect of electrolytes on chemical equilibria. Ionic strength and activity coefficients. Debey-Huckel equation. Acid-base equilibria. Definition of acid and basic according to Arrhenius, Brønsted and Lowry, Lewis. The principle HSAB, Hard and soft acids and bases. Calculation of pH for strong, weak and polyprotic acids and bases. Graphical representation of acid base equlibrium: logarithmic charts. Graphical method in the calculation of the pH. Hydrolysis equilibria. Graphical method for the calculation of pH. Distribution diagrams. Hydration and hydrolysis of the cation. Hydroxides, oxides, oxoacids, Oxoanions. Anions hydrolysis. Buffer solutions. Buffering capacity. Coordination Compounds. Theoretical aspects. Reactions of complex formation. Role of coordination compounds in biochemistry. Application of Coordination Compounds in Analytical Chemistry. Stability and lability. Elements of Nuclear Chemistry. Properties of the nucleus, mass, radius, nuclear forces. Colomb nuclear barrier. Nuclear energy. Unit of measure. Nuclear energy per nucleon as a function of A. Factors determining the stability/instability of a nucleus. Stability of the nuclei as a function of A and Z. Semiempirical mass equation. Nuclear models: liduid drop and shells. Spontaneous nuclear reactions. Types of radioactive decay: positron emission (beta+ decay), Negatronic Emission (beta- decay), Electron Capture. Alpha decay. Gamma emission. Internal conversion. X-ray fluorescence Auger effect. Interaction of radiation with matter. Systems for detection of radiation. Counters: Ionization, Proportional, Geyger Muller, scintillation. Kinetics of decay. Decay constant, half-life time. Specific activity. Mixtures of nuclides. Kinetics of mixed decay, decay chain. Radioactive equilibrium, balance transient. Induced nuclear reactions. Notation and energy. Reactions induced by protons, alpha particles, neutrons. Summary of nuclides. Nuclear fission. Nuclear fusion. Natural and Artificial radioisotopes. Dating with Carbon 14.
Prerequisites
Basic concepts related to a general and inorganic chemistry course at the university level (atomic structure, electronic configuration, element symbols, stoichiometry and nomenclature of the main anions and cations, chemical bonds, equilibrium constant, thermodynamics and its application to chemical equilibria)
Frequency
Attendance is mandatory.
Exam mode
The purpose of the exam consists in verifying the level of understanding and deepening of 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 containing both exercises related to the resolution of stoichiometric calculations on chemical equilibria in aqueous solution and open-ended questions to verify the knowledge acquired. A few days later, for students who have obtained a grade equal to or greater than 18/30 there is the verbalization of the result obtained with possible integration with the oral 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.
Lesson mode
The course has the following organization: • theoretical lessons in the classroom • deepening of theoretical issues in the classroom • resolution of numerical problems in the classroom • eventually, at the end of the lessons, one (or more) simulation test of the exam (self-assessment test) will be made, following by relative correction 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.
Channel 2
FEDERICO PEPI Lecturers' profile

Program - Frequency - Exams

Course program
Physical and chemical properties of atoms in the periodic table. Principles of nuclear chemistry. The nuclear properties: mass, radius, nuclear forces. Factors affecting the stability/instability of a nucleus. Stability of nuclei as a function of A and Z. Semiempirical mass equation. Spontaneous nuclear reactions. Types of radioactive decay: alpha and beta decay, electron capture. Gamma emission. Internal conversion. X-ray fluorescence. Auger effect. Interaction of radiation with matter. Radiation Detection; Ionization, Proportional and Geyger-Muller counters. Kinetic aspects of the decay. Nuclear fission. Nuclear fusion. Natural and artificial radioactive elements. Dating with carbon 14. Use of the main radionuclides for diagnosis and treatment. Purposes of Analytical Chemistry. Sample Preparation. Classification of analytical methods. Evaluation of analytical data. Precision and Accuracy. Types of Errors. Effect of electrolytes on chemical equilibrium. Debey-Hückel equation Acid-base equilibria. Definition of acid and bases by Arrhenius, Brønsted-Lowry and Lewis. The HSAB principle. pH calculation. Graphic representation of acid-base equilibria: logarithmic plots. Distribution diagrams. Metal cations hydrolysis . Buffer solutions. Coordination compounds. Theoretical aspects. Classification of metals and ligands. Types of bonds, Crystal Field Theory. Distribution curves. Conditional constants. EDTA uses in analytical chemistry. Solubility. Solubility-product constant. Effect of ionic strength on solubility. Common-ion effect. Effect of side reactions on the solubility of slightly soluble ionic compounds. Solubility of metal hydroxides. Precipitation. Logarithmic plots Redox equilibria. Electrochemical cells. Redox potential. Nernst equation. Standards electrodes. Formal potential. Effect of the presence of ligands on the redox potential. Systematic Inorganic Chemistry: properties and preparation methods of the most common inorganic compounds.
Prerequisites
- structure and properties of matter and its chemical transformations - thermodynamics and its application to chemical equilibria - acid-base equilibria - basics of electrochemistry
Books
a) G. Wulfsberg: “La Moderna Chimica Inorganica: Previsioni di Reattività” - Ed. La Sorbona – Milano. b) Daniel C Harris: "Chimica analitica quantitativa”, Terza edizione italiana condotta sulla nona edizione americana - Ed. Zanichelli c) Skoog, West, Holler: “Fondamenti di Chimica Analitica” - EdiSES S.r.l. d) D.S. Hage, J.D. Carr: "Chimica Analitica e Analisi Quantitativa" Piccin Nuova Libraria. e) A. Liberti, A. Napoli: "Lezioni di Chimica Analitica" - Editrice Universitaria di Roma - La Goliardica. f) G. Saini, E. Mentasti: "Fondamenti di Chimica Analitica. Equilibri ionici e volumetria" - UTET Libreria
Lesson mode
The lessons are divided into theoretical lectures and exercises on stochoimetric calculations
  • Academic year2025/2026
  • CoursePharmacy
  • CurriculumCurriculum unico
  • Year2nd year
  • Semester1st semester
  • SSDCHIM/01
  • CFU4