Chemistry and Laboratory
A.Y. 2023/2024
Learning objectives
General Aims and Learning Objectives of the course: The course is a prerequisite for subsequent courses of Mineralogy and Geochemistry. Its purpose is to provide the tools needed to understand chemical language and the foundation of chemistry (atom, chemical bonding, chemical reactions, chemical equilibrium, thermodynamics, knowledge of the principal inorganic species of metals and non-metals), the learning of which is essential to proceed in the earth science study.
Expected learning outcomes
Knowledge and understanding : Students are expected to understand the basis of chemical language and to know the foundation of chemistry in order to be able to operate in working contexts related to mineralogy and geochemistry.
Applying knowledge and understanding: Students are expected to apply their knowledge and understanding, and problem solving abilities in new or unfamiliar environments within broader (or multidisciplinary) contexts related to their field of study: mineralogy and geochemistry.
Making judgements: Students are expected to have the ability to integrate knowledge and handle complexity, and formulate judgements with incomplete or limited information, but that include reflecting on social and ethical responsibilities linked to the application of their knowledge and judgements.
Communication skills: Students should be able to communicate their conclusions, and the knowledge and rationale underpinning these, to specialist and non-specialist audiences clearly and unambiguously.
Learning skills: Students are expected to have the learning skills to allow them to continue to study in a manner that may be largely self-directed or autonomous.
Applying knowledge and understanding: Students are expected to apply their knowledge and understanding, and problem solving abilities in new or unfamiliar environments within broader (or multidisciplinary) contexts related to their field of study: mineralogy and geochemistry.
Making judgements: Students are expected to have the ability to integrate knowledge and handle complexity, and formulate judgements with incomplete or limited information, but that include reflecting on social and ethical responsibilities linked to the application of their knowledge and judgements.
Communication skills: Students should be able to communicate their conclusions, and the knowledge and rationale underpinning these, to specialist and non-specialist audiences clearly and unambiguously.
Learning skills: Students are expected to have the learning skills to allow them to continue to study in a manner that may be largely self-directed or autonomous.
Lesson period: First semester
Assessment methods: Esame
Assessment result: voto verbalizzato in trentesimi
Single course
This course can be attended as a single course.
Course syllabus and organization
Single session
Responsible
Lesson period
First semester
Course syllabus
Measurement and units: Measurement of Matter and Metric Units. Scientific notation. Significant Figures in Measurements. Accuracy and Precision. Dimensional analysis.
Electrons in Atoms: Atomic particles and their properties. Chemical Elements. Atomic Weights, Formula Weights and Molecular Weights. The Avogadro Constant and the concept of the Mole. Quantum Theory. The Bohr Atom. The Uncertainty Principle. Quantum Numbers and Electron Orbitals. Electron Spin. Multielectron Atoms. Electron Configurations of the Elements.
The Periodic Law and the Periodic Table. Electron Configuration and the Periodic Table. Periodic properties: Metals and Nonmetals, Atomic Radius, Ionization Energy, Electron Affinity.
Chemical Bonding: Lewis theory. Ionic and Covalent Bonding. Electronegativity. Lewis Structures. Resonance. Exceptions to the Octet Rule. VSEPR Theory and Molecular Shapes. Introduction to the Valence Bond Theory. Hybridization of Atomic Orbitals. Intermolecular forces.
Formulas and systematic nomenclature: Oxidations States. Systematic Nomenclature of Inorganic Compounds.
Solutions: Solution Concentration. Solution Dilution. Vapour Pressures of Solutions. Freezing Point. Depression and Boiling Point Elevation.
Chemical Reactions: Chemical reactions and the Chemical Equation. Balancing. Determining the Limiting Reagent. Chemical Equilibrium. The Equilibrium Constant Expression. The reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solutions: electrolytes and nonelectrolytes, Precipitation Reactions, Acid-Base Reactions, Oxidation-Reduction Reactions.
Gases: The concept of Pressure and absolute Temperature. The Gas Laws: Boyle's law, Charles's Law and Avogadro's Law. The Ideal Gas Equation. Mixtures of gases: partial pressure and partial volume. Dalton's Law and Amagat's Law.
Acids and Bases: Arrhenius Theory. Bronsted-Lowry Theory. Strong Acids and Strong Bases. Self-ionization of water. Definition of pH and pOH. Weak Acids and Weak Bases. Polyprotic Acids. Hydrolysis. Buffer Solutions. Neutralization reactions and Titration Curves.
Transition metal complexes: Lewis Acids and Bases. Ligands. Isomers. Geometry of Complex Ions. Complex-Ion Equilibria.
Thermochemistry: State functions. The First Law of Thermodynamics. Enthalpy. Entropy. The Second Law of Thermodynamics. Standard Free Energy Change. Gibbs Energy Change and Equilibrium.
Electrons in Atoms: Atomic particles and their properties. Chemical Elements. Atomic Weights, Formula Weights and Molecular Weights. The Avogadro Constant and the concept of the Mole. Quantum Theory. The Bohr Atom. The Uncertainty Principle. Quantum Numbers and Electron Orbitals. Electron Spin. Multielectron Atoms. Electron Configurations of the Elements.
The Periodic Law and the Periodic Table. Electron Configuration and the Periodic Table. Periodic properties: Metals and Nonmetals, Atomic Radius, Ionization Energy, Electron Affinity.
Chemical Bonding: Lewis theory. Ionic and Covalent Bonding. Electronegativity. Lewis Structures. Resonance. Exceptions to the Octet Rule. VSEPR Theory and Molecular Shapes. Introduction to the Valence Bond Theory. Hybridization of Atomic Orbitals. Intermolecular forces.
Formulas and systematic nomenclature: Oxidations States. Systematic Nomenclature of Inorganic Compounds.
Solutions: Solution Concentration. Solution Dilution. Vapour Pressures of Solutions. Freezing Point. Depression and Boiling Point Elevation.
Chemical Reactions: Chemical reactions and the Chemical Equation. Balancing. Determining the Limiting Reagent. Chemical Equilibrium. The Equilibrium Constant Expression. The reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solutions: electrolytes and nonelectrolytes, Precipitation Reactions, Acid-Base Reactions, Oxidation-Reduction Reactions.
Gases: The concept of Pressure and absolute Temperature. The Gas Laws: Boyle's law, Charles's Law and Avogadro's Law. The Ideal Gas Equation. Mixtures of gases: partial pressure and partial volume. Dalton's Law and Amagat's Law.
Acids and Bases: Arrhenius Theory. Bronsted-Lowry Theory. Strong Acids and Strong Bases. Self-ionization of water. Definition of pH and pOH. Weak Acids and Weak Bases. Polyprotic Acids. Hydrolysis. Buffer Solutions. Neutralization reactions and Titration Curves.
Transition metal complexes: Lewis Acids and Bases. Ligands. Isomers. Geometry of Complex Ions. Complex-Ion Equilibria.
Thermochemistry: State functions. The First Law of Thermodynamics. Enthalpy. Entropy. The Second Law of Thermodynamics. Standard Free Energy Change. Gibbs Energy Change and Equilibrium.
Prerequisites for admission
Elementary notions of mathematics and knowledge of the main physical quantities, their mutual relationships and main unit measurements.
Teaching methods
Teaching Mode: Traditional Lectures. Interactive presentations partially supported by projected lecture slides. Attendance is strongly recommended.
Teaching Resources
RECOMMENDED BOOK:
CHIMICA
J. Kotz, P.Treichel jr., G. C. Weaver
Editore: EDISES
ISBN: 9788879599665
CHIMICA GENERALE
PRINCIPI ED APPLICAZIONI MODERNE
R. H. Petrucci; F. G. Herring; J. D. Madura; C. Bissonnette
Editore: PICCIN
ISBN: 978-88-299-2933-7
FONDAMENTI DI CHIMICA GENERALE
Raymond Chang, Jason Overby, Alberto Costanzo, Roberta Galeazzi, Paola Turano
Editore: McGraw-Hill Education
ISBN-10: 8838696292
ISBN-13: 9788838696299
EXERCISE BOOK:
CHIMICA. ESERCIZI E CASI PRATICI
P. D'Arrigo, A. Famulari, C. Gambarotti, M. Scotti
Editore: EDISES
ISBN: 9788879599634
CHIMICA
J. Kotz, P.Treichel jr., G. C. Weaver
Editore: EDISES
ISBN: 9788879599665
CHIMICA GENERALE
PRINCIPI ED APPLICAZIONI MODERNE
R. H. Petrucci; F. G. Herring; J. D. Madura; C. Bissonnette
Editore: PICCIN
ISBN: 978-88-299-2933-7
FONDAMENTI DI CHIMICA GENERALE
Raymond Chang, Jason Overby, Alberto Costanzo, Roberta Galeazzi, Paola Turano
Editore: McGraw-Hill Education
ISBN-10: 8838696292
ISBN-13: 9788838696299
EXERCISE BOOK:
CHIMICA. ESERCIZI E CASI PRATICI
P. D'Arrigo, A. Famulari, C. Gambarotti, M. Scotti
Editore: EDISES
ISBN: 9788879599634
Assessment methods and Criteria
The exam is written and divided into two parts: Part A (stoichiometric problems) and Part B: (test and questions). In order to pass the exam, it is needed to obtain the sufficiency in each of the two parts.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 9
Practicals: 36 hours
Lessons: 48 hours
Lessons: 48 hours
Professor:
Rizzato Silvia
Educational website(s)
Professor(s)
Reception:
Wednesday and Friday 16:00-17:00. Please send an e-mail.
Dipartimento di Chimica, Corpo A, stanza 1402