Unit GENERAL AND INORGANIC CHEMISTRY
- Course
- Quality control of healthcare products
- Study-unit Code
- GP002982
- Curriculum
- In all curricula
- Teacher
- Morena Nocchetti
- Teachers
-
- Morena Nocchetti
- Riccardo Vivani (Codocenza)
- Hours
- 21 ore - Morena Nocchetti
- 21 ore (Codocenza) - Riccardo Vivani
- CFU
- 6
- Course Regulation
- Coorte 2025
- Offered
- 2025/26
- Learning activities
- Base
- Area
- Discipline chimiche
- Academic discipline
- CHIM/03
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa monodisciplinare
- Language of instruction
- Italian
- Contents
- Periodic table of elements, Electronic structure and reactivity of elements. Compounds and stoichiometric relationships. Bases of chemical reactivity. Principia of chemical equilibrium
- Reference texts
- L. Palmisano, et al., Elementi di Chimica, EdiSES, Napoli 2020. Additional didactic material (slides, exercises and examples, and other material) available on-line at the web site http://www.unistudium.unipg.it.
- Educational objectives
- Teaching is the first approach to general and inorganic chemistry. The main objective of the course is to provide students with the basic concepts of general chemistry as a description of nature, an appropriate scientific language and the ability to study in a critical and rational way. The main knowledge gained will be: - Atomic theory and electronic structure of atoms. - Chemical bond and molecular geometries. - Intermolecular forces. - Chemical reactions. - Chemical equilibrium in the gas phase and in aqueous solution. The main skills (ability to apply knowledge acquired): - Identify and be able to write formulas of inorganic compounds; - Represent molecules or molecular ions inorganic highlighting the orientation of the atoms and the links between them; - Predict the polarity and the physical state of molecules; - Predict the reactivity of inorganic compounds both in redox reactions and that of non-redox; - Write and describe the qualitative and quantitative aspects (stoichiometric) of a chemical reaction in relation to chemical equilibrium homogeneous and heterogeneous
- Prerequisites
- In order to understand and achieve the intended learning is necessary that the student possesses skills in mathematics and physics. In particular, the student should know and be able to use some basic mathematical tools (equivalence, equation of first and second degree, logarithmic, exponential, inequalities, derivatives, integrals) and concepts of basic physics (units, force, energy).
- Teaching methods
- The course is organized as follows: - Lectures on all the topics of the course. The lessons will be conducted with the help of the blackboard and through slide shows. - Numerical exercises in the classroom for the solution of numerical exercises guided with the aid of the blackboard. The teaching material (slides, exercises during numerical exercises, texts of previous written tests, other material) are made available to students on the e-studium platform after registration.
- Other information
- At the exam the students are advised to bring student card and proof of identity. - Essentials allowed for the written exam: periodic table, traditional calculator (scientific), pen. - Not Allowed: mini computers or PDAs, cell phones, notebooks, books, notes or other information. - The test must be written in non-erasable pen. - The student who had not passed a test, can access any of the subsequent tests.
- Learning verification modality
- The exam consists of a written test lasting about three hours. It consists of 10-15 open-ended questions of both theoretical and numerical type, in which case the procedure followed to obtain the result must be reported. Theoretical questions require a clear, concise and comprehensive answer, according to the knowledge transmitted during the lectures. The exam is designed to ascertain the knowledge, understanding, language acquisition own discipline and the ability to display and summary about the theoretical aspects, and ensure the ability to apply the acquired skills to solve numerical problems related to practical cases. In the event that, for any reason, it is not possible to complete the written exam session in person, this will be supported electronically through the LibreEOL platform (www.libreeol.org) with rules similar to those described above. For information on support services for students with disabilities and/or DSA visit http://www.unipg.it/disabilita-e-dsa.
- Extended program
- Generalities: Intensive and extensive properties of matter. Physical quantities. System of measurement S.I. Conversion factors. Definition of systems. Fundamentals of atomic theory and electronic structure of atoms: Concept of mole. Nuclides, isotopes, elements. The hydrogen atom and quantum numbers. Electronic configurations. Aufbau. Periodic table. Ionisation energy, electronic affinity, atomic and ionic radii. The chemical bond Ionic bonding. Binary ionic compounds. Description of the covalent bond using the valence bond method. V.S.E.P.R. method and molecular geometry. Hybridisation. Multiple bonds. Resonance. Electronegativity and oxidation number. Structure formulas of the most common molecules and oxanions. Chemical nomenclature. Minimum formulas and molecular formulas. Chemical reactions: Rules for balancing chemical reactions. Acid-base reactions. Oxidation-reduction reactions using the electronic ion method. Intermolecular bonds Ion-dipole interaction, dipole-dipole, instantaneous dipole-induced dipole, hydrogen bonding. States of aggregation of matter: Ideal gas laws. Partial pressures. Liquids. Vapour pressure. Liquid-vapour, solid-liquid, solid-vapour equilibrium. State diagrams. Properties of solutions: Solutions. Units of concentration (% by weight, mole fraction, molarity, molality). Colligative properties, cryoscopy, ebulloscopy, osmotic pressure, electrolytic dissociation. Concepts of chemical thermodynamics: Functions of state. First principle. Internal energy. Enthalpy. Standard enthalpy of formation. Thermochemistry. Second principle. Entropy and temperature. Third principle. Absolute entropies. Free energy. Spontaneity criteria. Chemical, electrochemical equilibrium: homogeneous and heterogeneous equilibria. Equilibrium constant. Le Chatelier principle. Effects of temperature, pressure and concentration on chemical equilibria. Acid-base equilibria. Brönsted theory. Acid-base conjugate pairs. Autoprotonation of water. Strength of acids and bases. Ka, Kb, strong acids. Calculation of pH in simple systems. Strong acids (or bases). Weak acids (or bases). Buffer solutions. Acid-base indicators. Redox balances. Notes on galvanic cells. Electromotive force and electrode potential. Series of normal potentials and its use. Concentration cells and pH measurements. Elements of Chemical Kinetics: Kinetic laws. Specific rate constant, reaction order. Effect of reactant concentration. Integration of kinetic laws: 1st and 2nd order reactions. Reaction mechanism. Reaction intermediates. Effect of temperature. Arrhenius equation. Activation energy. Activated complex. Effect of light. Notes on catalysis.