Chemistry 1
A.Y. 2024/2025
Learning objectives
The primary goal of the course is to provide a solid foundation in the basic concepts and facts of chemistry, particularly those needed for a successful understanding of other subjects for which chemistry is a prerequisite.
Expected learning outcomes
At the end of the course, students will be able to:
1. Recognize and name both the single chemical elements and the molecules formed by them;
2. Identify the bonds and chemical interactions underlying the formation of molecules;
3. Discuss the atomic structure, the electronic configuration of the elements and the periodic table;
4. Recognize and balance the chemical equation related to a given chemical reaction;
5. Calculate the pH, describe the properties of acids and bases, the acid-base equilibria, the constitution of buffer solutions and titration reactions;
6. Balance the oxidation-reduction reactions and calculate the potential and the electrode concentrations of an electrochemical cell by using the Nernst's law.
1. Recognize and name both the single chemical elements and the molecules formed by them;
2. Identify the bonds and chemical interactions underlying the formation of molecules;
3. Discuss the atomic structure, the electronic configuration of the elements and the periodic table;
4. Recognize and balance the chemical equation related to a given chemical reaction;
5. Calculate the pH, describe the properties of acids and bases, the acid-base equilibria, the constitution of buffer solutions and titration reactions;
6. Balance the oxidation-reduction reactions and calculate the potential and the electrode concentrations of an electrochemical cell by using the Nernst's law.
Lesson period: Second 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
CORSO A
Responsible
Lesson period
Second semester
Course syllabus
Structure of matter: Atomic structure. Atomic and molecular weights. Isotopes. Radioactivity. Mass defect.
Quantitative chemical relationships: Balancing redox reactions. Stoichiometric calculus. The chemical equilibrium. Le Chatelier's principle. Equilibrium constants. Colligative properties. Ionic strength and chemical activity.
Acid-Base reaction: Acids and bases (Arrhenius, Broensted, Lewis theories). pH. Buffer solutions. Hydrolysis. Acid-base titrations.
Atomic structure: Bohr's atomic model. De Broglie equation. Heisenberg's principle. On Schrödinger equation. Hydrogen atom. Many-electron atoms. The "aufbau" principle and the periodic table.
The Chemical bond: Ionic bonds. VSEPR Theory. The Covalent bond. The Hydrogen bond and the weak interactions. Bonding in coordination compound. Lattice energy and hydration energy. Ionic, molecular and van der Waals crystals.
Gases: Gas laws and the equation of state for ideal and real gases. Elements of the kinetic theory of gases. Solubility.
Thermodynamics: The first, the second and the third law of thermodynamics. Thermodynamic functions and chemical equilibrium.
Electrochemistry: Cell potentials. Nernst's law. Electrolysis.
Descriptive Inorganic Chemistry: The biologically relevant elements.
Quantitative chemical relationships: Balancing redox reactions. Stoichiometric calculus. The chemical equilibrium. Le Chatelier's principle. Equilibrium constants. Colligative properties. Ionic strength and chemical activity.
Acid-Base reaction: Acids and bases (Arrhenius, Broensted, Lewis theories). pH. Buffer solutions. Hydrolysis. Acid-base titrations.
Atomic structure: Bohr's atomic model. De Broglie equation. Heisenberg's principle. On Schrödinger equation. Hydrogen atom. Many-electron atoms. The "aufbau" principle and the periodic table.
The Chemical bond: Ionic bonds. VSEPR Theory. The Covalent bond. The Hydrogen bond and the weak interactions. Bonding in coordination compound. Lattice energy and hydration energy. Ionic, molecular and van der Waals crystals.
Gases: Gas laws and the equation of state for ideal and real gases. Elements of the kinetic theory of gases. Solubility.
Thermodynamics: The first, the second and the third law of thermodynamics. Thermodynamic functions and chemical equilibrium.
Electrochemistry: Cell potentials. Nernst's law. Electrolysis.
Descriptive Inorganic Chemistry: The biologically relevant elements.
Prerequisites for admission
1. Elements of Atomic Structure
2. Elements of Classical Thermodynamics (non-statistical)
3. Analysis 1 (differential equations, partial derivatives, Riemann integration)
2. Elements of Classical Thermodynamics (non-statistical)
3. Analysis 1 (differential equations, partial derivatives, Riemann integration)
Teaching methods
The teaching is provided in 32 hours of lessons and 24 of exercises, all frontal.
Teaching Resources
(1) F. Demartin, Fondamenti di Chimica generale, EDiSES.
(2) N. J. Tro, Chimica un approccio molecolare, EDiSES
(3) David W. Oxtoby, H. P. Gillis, Alan Campion, Chimica Moderna, EDiSES
(4) Petrucci, Herring, Madura, Bissonnette, Chimica Generale, Principi ed Applicazioni Moderne, Piccin Editore, Padova
(5) Tavola Periodica degli Elementi, versione IUPAC
(2) N. J. Tro, Chimica un approccio molecolare, EDiSES
(3) David W. Oxtoby, H. P. Gillis, Alan Campion, Chimica Moderna, EDiSES
(4) Petrucci, Herring, Madura, Bissonnette, Chimica Generale, Principi ed Applicazioni Moderne, Piccin Editore, Padova
(5) Tavola Periodica degli Elementi, versione IUPAC
Assessment methods and Criteria
The exam consists of a compulsory written test lasting 2 hours.
The written test focuses on the topics covered during the course and includes:
- the solution of 3 exercises, having contents and difficulties similar to those faced during the lessons.
- the answer to 3 theoretical questions.
For the purposes of the evaluation, the correctly carried out fractions of each exercise and theoretical question are calculated; if 1.5 exercises and 1.5 questions have been completed correctly, the student obtains a sufficient grade.
Any additional information on the assessment methods will be explained during the course.
The written test focuses on the topics covered during the course and includes:
- the solution of 3 exercises, having contents and difficulties similar to those faced during the lessons.
- the answer to 3 theoretical questions.
For the purposes of the evaluation, the correctly carried out fractions of each exercise and theoretical question are calculated; if 1.5 exercises and 1.5 questions have been completed correctly, the student obtains a sufficient grade.
Any additional information on the assessment methods will be explained during the course.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 6
Practicals: 24 hours
Lessons: 32 hours
Lessons: 32 hours
Professor:
Castellano Carlo
CORSO B
Responsible
Lesson period
Second semester
Course syllabus
Atoms and atomic structure - Nuclides, isotopes and chemical elements. Molecular formula. Atomic mass and molecular mass. Molecules and Avogadro's Number. Concentration: weight percentage and Molarity. Dilution. Molar fraction. Chemical reactions and Chemical equations. Balancing. The principle of conservation of mass.
Construction of the periodic table of elements and periodicity of the properties of elements. Chemical bonding and molecular geometry.
Oxidation number. Chemical formulae and systematic nomenclature.
Lewis symbols and structures. The ionic bond, the covalent bond, the metallic bond. Electronegativity. Polarity of covalent bonds and polarity of the molecules. Molecular geometry: VSEPR and Valence Bond Theory. Molecular Orbitals. Hydrogen bonding and weak interactions. Colligative properties.
Chemical thermodynamics - Recalls thermochemistry: internal energy, enthalpy, entropy and Gibbs free energy. State functions. First principle of thermodynamics. Spontaneity of a chemical reaction.
Equilibrium reactions: Equilibrium Constant and Reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria. Calculation of concentrations. Equilibrium in non-ideal solution: ionic strength and activity.
The gaseous state - Recalls on 'ideal' gases and their laws: Boyle's law, Charles and Gay-Lussac's law and Avogadro's law. Molar volume.
Equation of state of ideal gases. The universal gas constant. Gaseous mixtures - definition of partial pressure and partial volume, Dalton's law.
Acids and Bases - Definition of acid and base (Arrhenius, Broensted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions.
Titration curves. Acid-base reactions.
Balancing of oxidation-reduction reactions. Electrochemistry - Electrochemical cells. Reduction potentials. Nernst equation.
Construction of the periodic table of elements and periodicity of the properties of elements. Chemical bonding and molecular geometry.
Oxidation number. Chemical formulae and systematic nomenclature.
Lewis symbols and structures. The ionic bond, the covalent bond, the metallic bond. Electronegativity. Polarity of covalent bonds and polarity of the molecules. Molecular geometry: VSEPR and Valence Bond Theory. Molecular Orbitals. Hydrogen bonding and weak interactions. Colligative properties.
Chemical thermodynamics - Recalls thermochemistry: internal energy, enthalpy, entropy and Gibbs free energy. State functions. First principle of thermodynamics. Spontaneity of a chemical reaction.
Equilibrium reactions: Equilibrium Constant and Reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria. Calculation of concentrations. Equilibrium in non-ideal solution: ionic strength and activity.
The gaseous state - Recalls on 'ideal' gases and their laws: Boyle's law, Charles and Gay-Lussac's law and Avogadro's law. Molar volume.
Equation of state of ideal gases. The universal gas constant. Gaseous mixtures - definition of partial pressure and partial volume, Dalton's law.
Acids and Bases - Definition of acid and base (Arrhenius, Broensted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions.
Titration curves. Acid-base reactions.
Balancing of oxidation-reduction reactions. Electrochemistry - Electrochemical cells. Reduction potentials. Nernst equation.
Prerequisites for admission
1. Elements of Atomic Structure
2. Elements of Classical Thermodynamics (non-statistical)
3. Analysis 1 (differential equations, partial derivatives, Riemann integration)
2. Elements of Classical Thermodynamics (non-statistical)
3. Analysis 1 (differential equations, partial derivatives, Riemann integration)
Teaching methods
The teaching is provided in 32 hours of lessons and 24 of exercises, all frontal.
Teaching Resources
(1) All the slides of the course are available on Ariel website
(2) A. Credi, Viaggio nella Chimica, EDiSES
(3) A. Peloso, F. Demartin, Fondamenti ed esercizi di Chimica Generale ed Inorganica, Edizioni Progetto Padova
(4) I. Bertini, C. Luchinat, F. Mani, E. Ravera, Chimica struttura, proprietà e trasformazioni della materia. Zanichelli
(5) G.Rayner-Canham, T. Overton, Chimica Inorganica descrittiva, EdiSES
(6) Tavola Periodica degli Elementi, versione IUPAC
(2) A. Credi, Viaggio nella Chimica, EDiSES
(3) A. Peloso, F. Demartin, Fondamenti ed esercizi di Chimica Generale ed Inorganica, Edizioni Progetto Padova
(4) I. Bertini, C. Luchinat, F. Mani, E. Ravera, Chimica struttura, proprietà e trasformazioni della materia. Zanichelli
(5) G.Rayner-Canham, T. Overton, Chimica Inorganica descrittiva, EdiSES
(6) Tavola Periodica degli Elementi, versione IUPAC
Assessment methods and Criteria
The exam consists of a written test lasting 2 hours.
The written test focuses on the topics covered during the course and includes:
- the solution of 3 exercises, having contents and difficulties similar to those faced during the lessons.
- the answer to 3 theoretical questions.
For the purposes of the evaluation, the correctly carried out fractions of each exercise and theoretical question are calculated; if 1.5 exercises and
1.5 questions have been completed correctly, the student obtains a sufficient grade.
Any additional information on the assessment methods will be explained during the course.
The written test focuses on the topics covered during the course and includes:
- the solution of 3 exercises, having contents and difficulties similar to those faced during the lessons.
- the answer to 3 theoretical questions.
For the purposes of the evaluation, the correctly carried out fractions of each exercise and theoretical question are calculated; if 1.5 exercises and
1.5 questions have been completed correctly, the student obtains a sufficient grade.
Any additional information on the assessment methods will be explained during the course.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 6
Practicals: 24 hours
Lessons: 32 hours
Lessons: 32 hours
Professor:
Panigati Monica
Professor(s)
Reception:
Su appuntamento
Dipartimento di Chimica, Corpo A, piano rialzato, stanza R38