Unit GENERAL AND INORGANIC CHEMISTRY
- Course
- Chemistry
- Study-unit Code
- 50170105
- Curriculum
- In all curricula
- Teacher
- Nadia Balucani
- CFU
- 12
- Course Regulation
- Coorte 2022
- Offered
- 2022/23
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa integrata
GENERAL AND INORGANIC CHEMISTRY 1
| Code | GP000256 |
|---|---|
| CFU | 6 |
| Teacher | Nadia Balucani |
| Teachers |
|
| Hours |
|
| Learning activities | Base |
| Area | Discipline chimiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | Introductory topics to the laws of chemistry: Stoichiometry and stoichiometric calculations. The gas laws. Thermodynamics and thermochemistry. The solutions and their properties. Phase transitions and equilibria, phase diagrams. The principles of chemical equilibrium. Solutions of acids and bases , neutralization reactions, pH calculation, acid-base indicators, titrations. Solubility. |
| Reference texts | Peter William Atkins, Loretta Jones, Leroy Laverman, Principi di chimica, Zanichelli, 4° edizione (2018) ISBN: 8808320979 BERTINI, LUCHINAT, MANI, Stechiometria, Un avvio allo studio della chimica; CEA MIlano 2009 A copy of the lecture slides will be available at the Unistudium webpage. |
| Educational objectives | In this course we will offer a first overview of the general laws of chemistry and will provide the basis of the knowledge / skills of chemistry necessary for a fruitful study of the subjects of the entire degree course. Particular attention will be paid to the quantitative aspects of empirical disciplines. At the end of the course, students will be able to perform complex stoichiometry exercises, to apply the laws of gases, to perform thermochemical calculations, to understand and apply the laws of chemical equilibrium, to calculate the pH of solutions containing one or more species able to modify the pH, to determine the concentration of less soluble species and to predict in which conditions the precipitates are formed. |
| Prerequisites | Understanding of simple mathematical equations and some principles of physics at secondary school level. |
| Teaching methods | Lectures, numerical exercises in the classroom, tutoring |
| Other information | |
| Learning verification modality | The exam consists of a written test followed by (if judged to be sufficient) an oral test. The written test consists in solving numerical problems and is aimed at verifying the ability to correctly apply the acquired knowledge and the ability to understand the topics covered in class. The oral test consists of a discussion lasting about 20 minutes aimed at ascertaining the level of knowledge and understanding achieved by the student on the contents indicated in the program. The oral exam will also enable students to verify their communication skills with language properties and autonomous organization of the topics. |
| Extended program | Introduction to Chemistry Atoms and atomic mass. Isotopes. Symbols of the elements. Quantitative aspects: mass, chemical reactions, balance and mass conservation. Reduction oxide reactions. Elementary analysis. Minimal molecular and structural formula. Isomers. The gas The empirical laws of gases. The equation of state of ideal gases. Gas mixtures. Deviations from ideal behavior. Thermodynamics and thermochemistry Introduction to Thermodynamics. First law of thermodynamics. Reaction heat and enthalpy. Bonding energy. Entropy, second and third principle. Free energy and criteria of spontaneity and balance. Physical equilibria State changes and physical balances. Vapor tension and temperature trend. State diagrams. Mixtures of volatile liquids and Raoult's law. Henry's law. Mixtures with non-volatile solutes. State diagrams of solutions. The principles of chemical equilibrium Equilibrium in homogeneous and heterogeneous systems. The equilibrium constant and the reaction quotient. The principle of Le Chatelier. Homogeneous reactions in liquid and gas phase. Acids and bases Theories compared to Arrhenius, Brønsted-Lowry and Lewis. Acid-base equilibria and conjugate species. Water autoionization. PH and pOH scale. Calculation of the pH of strong and weak solutions of acids (bases). Saline hydrolysis and buffer solutions. PH indicators and acid-base titrations. Other balances in aqueous solution Solubility equilibria. Selective precipitation. Complexation equilibria. |
GENERAL AND INORGANIC CHEMISTRY 2
| Code | GP000250 |
|---|---|
| CFU | 6 |
| Teacher | Filippo De Angelis |
| Teachers |
|
| Hours |
|
| Learning activities | Caratterizzante |
| Area | Discipline chimiche inorganiche e chimico-fisiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | The course introduces the basic concepts underlying the electronic properties of atoms and their interactions in constituting molecules and materials. The topics include: nucleus structure and atomic models; basic elements of quantum mechanics; periodicity of atomic properties; chemical bond and molecular structures; intermolecular forces and states of matter; introduction to chemical kinetics; elements of electrochemistry. Such topics are introduced and discussed in direct connection to inorganic chemistry applications in the framework of energy production and storage. |
| Reference texts | Peter William Atkins, Loretta Jones, Leroy Laverman, Principi di chimica, Zanichelli, 4° edizione (2018) ISBN: 8808320979. |
| Educational objectives | The course topics provide the interpretative and predictive bases to deal and be familiar with atomic, molecular and materials properties, in relation to the chemical and physical properties and the macroscopic behavior of matter. A target of the course is to allow students to master the basic laws and interpretative models of chemistry, in connection the topics directly discussed in the course. In particular, the following objectives will be pursued: to assign atomic electronic configurations; to use the periodic table to rationalize the periodic behavior of atomic properties; to predict molecular geometries in simple cases; to analyze the chemical bond of diatomic molecules in terms of sigma and pi contributions; to provide elements to assess the aggregation state of different chemical species; to illustrate the factors influencing the velocity of chemical reactions; to be able to balance redox reactions and to understand the factors influencing redox potentials. A general objective of the course is also to connect the theoretical lessons learnt to actual technologies in the energy field, such as batteries and solar cells. |
| Prerequisites | For an effective understanding of the topics dealt by the course it is important for students to be familiar with mathematics (linear and quadratic equations, sine and cosine functions, exponential functions and logarithms, derivatives) and physics (concepts of work and kinetic and potential energy) basic notions at the high school level. |
| Teaching methods | Classroom lectures on the course topics: the classes hours will be devoted to presenting and discussing the main concepts that will be employed for the solution of problems, including numerical ones, selected to deepen and enhance the students’ understanding of the main discussed topics. |
| Other information | Further Information available at http://www.dcbb.unipg.it/chimtriennale |
| Learning verification modality | The exam consists of a written test followed by (if judged to be sufficient) an oral test. The written test consists in solving numerical problems and is aimed at verifying the ability to correctly apply the acquired knowledge and the ability to understand the topics covered in class. The oral test consists of a discussion lasting about 20 minutes aimed at ascertaining the level of knowledge and understanding achieved by the student on the contents indicated in the program. The oral exam will also enable students to verify their communication skills with language properties and autonomous organization of the topics. For information on support services for disabled students and other issues please visit http://www.unipg.it/disabilita-e-dsa |
| Extended program | - Atomic structure: atomic models; energy quantization and quantum mechanics; energy levels and atomic orbitals; the Aufbau principle; electronic configurations. - Periodic table of the elements: periodicity in atomic properties; ionization energy and electron affinity; atomic and ionic radii; oxidation numbers. - Molecular structure and chemical bond: covalent and ionic bonds; electronegativity; Lewis structures of chemical bonds; molecular structures by the VSEPR model; valence bond theory; molecular orbitals; electronic configuration of homo-nuclear diatomic molecules; band structures in solids. - Intermolecular interactions: solid state and crystal lattices; liquid state; hydrogen bonds and weak interactions. - Chemical kinetics: reaction velocity and factors affecting it. - Basic electrochemistry: definition of redox potentials; Galvanic cells; redox processes and standard potentials; the Nernst equation; lead acid and lithium batteries; electrochemical cells and Faraday laws; photo-electrochemical solar cells. |