General Chemistry with Elements of Physical Chemistry
A.Y. 2024/2025
Learning objectives
The aim of the teaching is to provide a knowledge of basic chemistry, preparatory to the subsequent teachings of Organic Chemistry and Biological Chemistry. More specifically, the teaching will provide the minimum tools necessary for understanding the chemical language and basic topics (atoms, chemical bonds, chemical reactions, chemical, thermodynamic and electrochemical equilibrium). This basic knowledge constitutes the necessary tools for understanding the chemical language of life, an indispensable element for the future biological studies.
Expected learning outcomes
At the end of the teaching, the student will have to reach skills relating to the structure of matter and chemical bonds. The concepts learned will guide the graduate to work competently in all phases of the experimental and analytical management of chemical processes. In particular, the basic concepts of nomenclature, chemical formulas and stoichiometry, and the concepts concerning solutions, dissociations in solution, chemical and electrochemical equilibria, pH and buffer solutions must be applied.
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
A - L
Responsible
Lesson period
First semester
Course syllabus
Atomic structure. Nuclides, isotopes and chemical elements. Molecular formula and formula units. Atomic mass and molecular mass. Molecules and Avogadro's constant. Quantization of energy. Atomic models. Orbitals and quantum numbers. Electronic configuration of the elements.
Periodic table of the elements and periodic properties.
Chemical bonding and molecular geometry. Lewis structures. Ionic bonding and covalent bonding. Electronegativity and polarity of bonds. Molecular geometry: VSEPR model and valence bond theory. Intermolecular interactions.
Formulas and nomenclature of inorganic compounds.
Solutions. Units of concentration. Dilution. Colligative properties.
Chemical reactions and equations. Balance and principle of conservation of mass. Net ionic equation and charge conservation principle. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions.
Gaseous state. Pressure and temperature. Equation of state of gases. Molar volume. Universal gas constant. Gaseous mixtures: pressure and partial volume, Dalton's law.
Acids and bases. Definitions of acid and base. Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Chemical thermodynamics. State functions. First principle of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second principle of thermodynamics. Entropy. Gibbs free energy. Spontaneity of a reaction and equilibrium constant.
Electrochemistry. Electrochemical cells and standard potentials. Cell potential and Nernst equation.
Periodic table of the elements and periodic properties.
Chemical bonding and molecular geometry. Lewis structures. Ionic bonding and covalent bonding. Electronegativity and polarity of bonds. Molecular geometry: VSEPR model and valence bond theory. Intermolecular interactions.
Formulas and nomenclature of inorganic compounds.
Solutions. Units of concentration. Dilution. Colligative properties.
Chemical reactions and equations. Balance and principle of conservation of mass. Net ionic equation and charge conservation principle. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions.
Gaseous state. Pressure and temperature. Equation of state of gases. Molar volume. Universal gas constant. Gaseous mixtures: pressure and partial volume, Dalton's law.
Acids and bases. Definitions of acid and base. Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Chemical thermodynamics. State functions. First principle of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second principle of thermodynamics. Entropy. Gibbs free energy. Spontaneity of a reaction and equilibrium constant.
Electrochemistry. Electrochemical cells and standard potentials. Cell potential and Nernst equation.
Prerequisites for admission
The General Chemistry course is a basic course requiring no specific prerequisites. Basic knowledge in mathematics (algebra, algebraic equations of the first and second degree, logarithms) and physics, acquired during secondary school, is sufficient.
Teaching methods
Conventional delivery mode with lectures and classroom exercises. Lectures will be supported by the use of slides, which will be available on the myAriel portal. Where possible, the lectures and exercises will be supplemented with the use of digital technologies (Exam manager; Slido...)
Teaching Resources
Recommended Texts
- Alberto Credi et all. "Viaggio nella Chimica" Ed. EdiSES
- Tro, "Chimica un Approccio Molecolare" Ed. EdiSES.
- Chang, Goldsby, "Fondamenti di Chimica Generale" Ed. McGraw Hill
Reference texts for performing the exercises
- Caselli, Rizzato, Tessore "Stechiometria dal testo di M. Freni e A. Sacco" Ed. EdiSES.
- Del Zotto "Esercizi di chimica generale" Ed. EdiSES.
- Alberto Credi et all. "Viaggio nella Chimica" Ed. EdiSES
- Tro, "Chimica un Approccio Molecolare" Ed. EdiSES.
- Chang, Goldsby, "Fondamenti di Chimica Generale" Ed. McGraw Hill
Reference texts for performing the exercises
- Caselli, Rizzato, Tessore "Stechiometria dal testo di M. Freni e A. Sacco" Ed. EdiSES.
- Del Zotto "Esercizi di chimica generale" Ed. EdiSES.
Assessment methods and Criteria
The exam will consist of a written test divided into two parts: the first aimed at verifying the learning of the basic theoretical notions of general chemistry by means of 12 multiple-choice questions (12 points); the second aimed at verifying the ability to carry out and solve 4 exercises (20 points) for a total of 32/30 (corresponding to honours). The written test will last 3 hours. To pass the examination, the student must score a minimum of 18/30. There are no oral examinations and no restrictions on registration for the exam.
CHIM/02 - PHYSICAL CHEMISTRY - University credits: 1
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 5
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 5
Practicals: 16 hours
Lessons: 40 hours
Lessons: 40 hours
Professor:
Panigati Monica
M - Z
Responsible
Lesson period
First semester
Course syllabus
Atomic mass and molecular mass. Moles and Avogadro's constant. Energy quantization. Atomic models. Orbitals and quantum numbers. Electronic configuration of elements.
Periodic table of elements and periodic properties.
Chemical bonding and molecular geometry. Lewis structures. Ionic bond and covalent bond. Electronegativity and bond polarity. Molecular geometry: VSEPR model and valence bond theory. Intermolecular interactions.
Formulas and nomenclature of inorganic compounds.
Solutions. Units of concentration measurement. Dilution. Colligative properties.
Chemical reactions and equations. Balancing and principle of conservation of mass.
Net ionic equation and principle of conservation of charge. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier's principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions.
Gaseous state. Pressure and temperature. Gas state equation. Molar volume.
Universal gas constant. Gaseous mixtures: partial pressure and volume, Dalton's law. Acids and bases. Definitions of acid and base. Acid-base equilibria. pH calculation. Buffer solutions. Titration curves.
Chemical thermodynamics. State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second law of thermodynamics. Entropy. Gibbs free energy. Spontaneity of a reaction and equilibrium constant.
Electrochemistry. Electrochemical cells and standard potentials. Cell potential and Nernst equation.
Periodic table of elements and periodic properties.
Chemical bonding and molecular geometry. Lewis structures. Ionic bond and covalent bond. Electronegativity and bond polarity. Molecular geometry: VSEPR model and valence bond theory. Intermolecular interactions.
Formulas and nomenclature of inorganic compounds.
Solutions. Units of concentration measurement. Dilution. Colligative properties.
Chemical reactions and equations. Balancing and principle of conservation of mass.
Net ionic equation and principle of conservation of charge. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier's principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions.
Gaseous state. Pressure and temperature. Gas state equation. Molar volume.
Universal gas constant. Gaseous mixtures: partial pressure and volume, Dalton's law. Acids and bases. Definitions of acid and base. Acid-base equilibria. pH calculation. Buffer solutions. Titration curves.
Chemical thermodynamics. State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second law of thermodynamics. Entropy. Gibbs free energy. Spontaneity of a reaction and equilibrium constant.
Electrochemistry. Electrochemical cells and standard potentials. Cell potential and Nernst equation.
Prerequisites for admission
The course of General Chemistry with elements of Physical Chemistry is a basic course that does not require specific prerequisites. Basic knowledge in mathematics (algebra, first and second-degree algebraic equations, logarithms) and physics acquired during high school is sufficient.
Teaching methods
Traditional delivery mode with face-to-face lectures and classroom exercises. The lectures will be supported by the projection of slides, which will then be made available on the teacher's myAriel portal. Where possible, lectures and exercises will be integrated with the use of digital technologies (Exam manager; Slido...).
Teaching Resources
- Alberto Credi et all. "Viaggio nella Chimica" Ed. EdiSES
- Tro, "Chimica un Approccio Molecolare" Ed. EdiSES.
- Chang, Goldsby, "Fondamenti di Chimica Generale" Ed. McGraw Hill
- Caselli, Rizzato, Tessore "Stechiometria dal testo di M. Freni e A. Sacco" Ed. EdiSES.
- Del Zotto "Esercizi di chimica generale" Ed. EdiSES.
- Tro, "Chimica un Approccio Molecolare" Ed. EdiSES.
- Chang, Goldsby, "Fondamenti di Chimica Generale" Ed. McGraw Hill
- Caselli, Rizzato, Tessore "Stechiometria dal testo di M. Freni e A. Sacco" Ed. EdiSES.
- Del Zotto "Esercizi di chimica generale" Ed. EdiSES.
Assessment methods and Criteria
The exam will consist of a written test divided into two parts: the first aimed at assessing the learning of basic theoretical concepts of general chemistry through 12 multiple-choice questions (12 points); the second aimed at assessing the ability to perform and solve 4 exercises (20 points) for a total of 32/30 (which corresponds to the highest grade). The written test will have a duration of 3 hours. To pass the exam, the student must achieve a minimum score of 18/30. There are no oral exams scheduled, and there are no limitations on registration for exam sessions.
CHIM/02 - PHYSICAL CHEMISTRY - University credits: 1
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 5
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 5
Practicals: 16 hours
Lessons: 40 hours
Lessons: 40 hours
Professor:
Damiano Caterina
Professor(s)