Chemistry
A.Y. 2025/2026
Learning objectives
The student will be able to predict properties and the chemical reactivity of an element based on its position in the Periodic Table. He will know and be able to distinguish substances in acids and bases, to classify chemical reactions such as acid-base or redox reactions. The student will learn how to qualitatively and quantitatively assess the results of an equilibrium reaction; knowing how to solve simple stoichiometric exercises.
The students are also expected to acquire basic concepts of organic chemistry through identification of functional groups and understanding some organic transformations of interest to natural sciences. Emphasis on the importance of organic compounds in health, environment, and society will be highlighted.
The students are also expected to acquire basic concepts of organic chemistry through identification of functional groups and understanding some organic transformations of interest to natural sciences. Emphasis on the importance of organic compounds in health, environment, and society will be highlighted.
Expected learning outcomes
Students will acquire:
· Knowledge of the electronic structure and the chemical properties of the elements according to their position in the periodic system.
· Ability to evaluate the chemical reactivity of a chemical compound
· Basic concepts of electronic structure enabling them to solve problems from various areas of organic chemistry, including stereochemistry, reactivity patterns and synthesis.
· Knowledge of the electronic structure and the chemical properties of the elements according to their position in the periodic system.
· Ability to evaluate the chemical reactivity of a chemical compound
· Basic concepts of electronic structure enabling them to solve problems from various areas of organic chemistry, including stereochemistry, reactivity patterns and synthesis.
Lesson period: Activity scheduled over several sessions (see Course syllabus and organization section for more detailed information).
Assessment methods: Esame
Assessment result: voto verbalizzato in trentesimi
Single course
This course cannot be attended as a single course. Please check our list of single courses to find the ones available for enrolment.
Course syllabus and organization
A-L
Responsible
Lesson period
year
Course syllabus
GENERAL CHEMISTRY
The General Chemistry teaching unit aims to provide students with the general basics of chemistry through the study of the nature of the elements and their compounds, the examination of the chemical reactions and the parameters associated with them. Starting from the atomic structure of matter, the course introduces the fundamental laws of stoichiometry also illustrated through exercises.
The course will allow the student to acquire the basic notions of chemistry necessary to understand processes, even complex, more specific than the degree course.
Atoms and atomic structure:
Nuclides, isotopes and chemical elements. Molecular formula and formula units. Unit of mass, atomic mass and molecular mass. Mole and Avogadro Number. Quantization of energy and photons. Emission spectrum of the hydrogen atom. Rutherford and Bohr's atomic models. Heisenberg's uncertainty principle. Charge density and probability. Orbitals and quantum numbers. Hybridization of carbon (sp, sp2 and sp3 hybrid orbitals). Diagram of energy levels and electronic configuration of the elements. Construction of the periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Oxidation numbers. Chemical formulas. Systematic nomenclature. Lewis symbols and structures. The ionic and the covalent bond. Electronegativity. Percentage of ionicity and polarity of bonds. Molecular geometry: VSEPR Theory and Valence Bond Theory. Intermolecular interactions.
Gases and their laws: pressure and absolute temperature. Ideal gases: Boyle's, Charles's, Gay-Lussac's and Avogadro's laws. Molar volume. Gas equation of state. Gaseous mixtures: definition of partial pressure and partial volume, Dalton's law and Amagat's law. Real gases.
Liquids and solutions: Concentration: percentage by weight, by volume, molarity and molality. Dilution. Mole fraction. The concept of equivalent. Equivalence number. Normality. Equivalent weight. Colligative properties: Vapor pressure, Raoult's law, boiling point elevation, freezing point depression and osmotic pressure.
Solids: amorphous and crystalline. Crystals: covalent, ionic and molecular. Elementary cells: types of packing and cubic cell. Metallic bond and band theory. Conductors, semiconductors and insulators. Allotropes of carbon and phosphorus.
Chemical reactions: Balancing. The principle of conservation of mass. Net ionic equation and charge conservation principle. 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. Acids and Bases: Definition of acid and base (Arrhenius, Bronsted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Introductio to thermodynamics: State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. The second law of thermodynamics. Entropy. Gibbs free energy.
ORGANIC CHEMISTRY
For each functional groups we will discuss structures and reactivity. The programme is:
- Structure and properties or organic molecules
- Polarity
- Alcanes
- Alkyl halides: nucleophilic substitution reactions. Carbocations
- Alkenes: addition reactions
- Alkynes
- Alcohols and ethers
- Aldehydes and ketones
- Carboxylic acids and their derivatives
- Aromatic compounds
- Amines
- Carbohydrates
- Amino acids and proteins
- Nucleic acids
- Hints about organic chemical compounds of natural origin and their biological activity
The General Chemistry teaching unit aims to provide students with the general basics of chemistry through the study of the nature of the elements and their compounds, the examination of the chemical reactions and the parameters associated with them. Starting from the atomic structure of matter, the course introduces the fundamental laws of stoichiometry also illustrated through exercises.
The course will allow the student to acquire the basic notions of chemistry necessary to understand processes, even complex, more specific than the degree course.
Atoms and atomic structure:
Nuclides, isotopes and chemical elements. Molecular formula and formula units. Unit of mass, atomic mass and molecular mass. Mole and Avogadro Number. Quantization of energy and photons. Emission spectrum of the hydrogen atom. Rutherford and Bohr's atomic models. Heisenberg's uncertainty principle. Charge density and probability. Orbitals and quantum numbers. Hybridization of carbon (sp, sp2 and sp3 hybrid orbitals). Diagram of energy levels and electronic configuration of the elements. Construction of the periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Oxidation numbers. Chemical formulas. Systematic nomenclature. Lewis symbols and structures. The ionic and the covalent bond. Electronegativity. Percentage of ionicity and polarity of bonds. Molecular geometry: VSEPR Theory and Valence Bond Theory. Intermolecular interactions.
Gases and their laws: pressure and absolute temperature. Ideal gases: Boyle's, Charles's, Gay-Lussac's and Avogadro's laws. Molar volume. Gas equation of state. Gaseous mixtures: definition of partial pressure and partial volume, Dalton's law and Amagat's law. Real gases.
Liquids and solutions: Concentration: percentage by weight, by volume, molarity and molality. Dilution. Mole fraction. The concept of equivalent. Equivalence number. Normality. Equivalent weight. Colligative properties: Vapor pressure, Raoult's law, boiling point elevation, freezing point depression and osmotic pressure.
Solids: amorphous and crystalline. Crystals: covalent, ionic and molecular. Elementary cells: types of packing and cubic cell. Metallic bond and band theory. Conductors, semiconductors and insulators. Allotropes of carbon and phosphorus.
Chemical reactions: Balancing. The principle of conservation of mass. Net ionic equation and charge conservation principle. 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. Acids and Bases: Definition of acid and base (Arrhenius, Bronsted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Introductio to thermodynamics: State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. The second law of thermodynamics. Entropy. Gibbs free energy.
ORGANIC CHEMISTRY
For each functional groups we will discuss structures and reactivity. The programme is:
- Structure and properties or organic molecules
- Polarity
- Alcanes
- Alkyl halides: nucleophilic substitution reactions. Carbocations
- Alkenes: addition reactions
- Alkynes
- Alcohols and ethers
- Aldehydes and ketones
- Carboxylic acids and their derivatives
- Aromatic compounds
- Amines
- Carbohydrates
- Amino acids and proteins
- Nucleic acids
- Hints about organic chemical compounds of natural origin and their biological activity
Prerequisites for admission
It is strongly suggested to take the General Chemistry exam before Organic Chemistry.
Teaching methods
The exam is written and it is warmly suggested to participate to classes.
Traditional format with regularly scheduled class sessions on campus.
Traditional format with regularly scheduled class sessions on campus.
Teaching Resources
GENERAL CHEMISTRY
Raymond Chang, Kenneth Goldsby
FONDAMENTI DI CHIMICA GENERALE
Mc Graw Hill education
ISBN: 978-88-386-1513-9
ORGANIC CHEMISTRY
One of the following textbooks
- W. H. BROWN Introduzione alla Chimica Organica - EdiSES
- J. McMURRY Fondamenti di Chimica Organica - Zanichelli
- multiple authors Chimica Organica Essenziale - Edi-ermes
- L. G. WADE Fondamenti di Chimica Organica - Piccin
Supplementary material is available at the ARIEL websites
https://acolombocg.ariel.ctu.unimi.it
https://myariel.unimi.it/course/view.php?id=2097
Raymond Chang, Kenneth Goldsby
FONDAMENTI DI CHIMICA GENERALE
Mc Graw Hill education
ISBN: 978-88-386-1513-9
ORGANIC CHEMISTRY
One of the following textbooks
- W. H. BROWN Introduzione alla Chimica Organica - EdiSES
- J. McMURRY Fondamenti di Chimica Organica - Zanichelli
- multiple authors Chimica Organica Essenziale - Edi-ermes
- L. G. WADE Fondamenti di Chimica Organica - Piccin
Supplementary material is available at the ARIEL websites
https://acolombocg.ariel.ctu.unimi.it
https://myariel.unimi.it/course/view.php?id=2097
Assessment methods and Criteria
The final exam is made of two separate and independent written tests, one for the General Chemistry part and one for the Organic Chemistry part, for the evaluation of the acquired knowledge. The two tests has a mark expressed out of /30. The final mark is the average of the two tests: 4/10 for general chemistry and 6/10 for organic chemistry.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 4
CHIM/06 - ORGANIC CHEMISTRY - University credits: 6
CHIM/06 - ORGANIC CHEMISTRY - University credits: 6
Practicals: 24 hours
Lessons: 68 hours
Lessons: 68 hours
Professors:
Colombo Alessia, Puglisi Alessandra
Shifts:
M-Z
Responsible
Lesson period
year
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 4
CHIM/06 - ORGANIC CHEMISTRY - University credits: 6
CHIM/06 - ORGANIC CHEMISTRY - University credits: 6
Practicals: 24 hours
Lessons: 68 hours
Lessons: 68 hours
Professors:
Rossi Sergio, Stucchi Marta
Shifts:
Professor:
Stucchi Marta
Professor(s)
Reception:
By appointment
Office (Chemistry Department, room 3005)