General and Inorganic Chemistry
A.Y. 2025/2026
Learning objectives
The primary goal of the course is to provide a solid foundation in the basic concepts and facts of general and inorganic chemistry, particularly those needed for a successful understanding of other subjects for which chemistry is a prerequisite. Basic laboratory skills will be also provided, which are fundamental to the student for properly facing the subsequent laboratory courses. Last but not least, the course aims to give the student an appreciation of the importance of chemistry to society in general and to daily life in particular.
Expected learning outcomes
At the end of the course, the student is expected to reach the following results:
- Knowledge, understanding and application: the student will acquire knowledge, understanding and critical application, even by the resolution of exercises of proper difficulty, over the basic chemical language with a particular focus on inorganic compounds nomenclature, atomic and electronic structure of the matter, chemico-physical properties of the elements and principal kinds of inorganic compounds, chemical bonds, Lewis structures, chemical reactions in particular redox reactions and their balancing, aqueous solutions and pH of acids, bases, salts, buffers, electrochemistry (i.e. batteries and electrolysis), basic thermodynamics and kinetics. Furthermore, the student will acquire elementary laboratory skills.
- Judgements and communication abilities: the student will be able to critically assess modes of interaction/transformation of inorganic molecules, even biologically interesting. Moreover, the student will acquire communication abilities using a specific language by employing proper chemical terms and expositive clearness.
- Knowledge, understanding and application: the student will acquire knowledge, understanding and critical application, even by the resolution of exercises of proper difficulty, over the basic chemical language with a particular focus on inorganic compounds nomenclature, atomic and electronic structure of the matter, chemico-physical properties of the elements and principal kinds of inorganic compounds, chemical bonds, Lewis structures, chemical reactions in particular redox reactions and their balancing, aqueous solutions and pH of acids, bases, salts, buffers, electrochemistry (i.e. batteries and electrolysis), basic thermodynamics and kinetics. Furthermore, the student will acquire elementary laboratory skills.
- Judgements and communication abilities: the student will be able to critically assess modes of interaction/transformation of inorganic molecules, even biologically interesting. Moreover, the student will acquire communication abilities using a specific language by employing proper chemical terms and expositive clearness.
Lesson period: First semester
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
Linea AK
Responsible
Lesson period
First semester
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 8
Practicals: 32 hours
Single bench laboratory practical: 16 hours
Lessons: 40 hours
Single bench laboratory practical: 16 hours
Lessons: 40 hours
Professors:
Colombo Valentina, Gallo Emma
Shifts:
Turno
Professor:
Gallo EmmaTurno 1
Professor:
Colombo ValentinaTurno 2
Professor:
Colombo ValentinaLinea LZ
Responsible
Lesson period
First semester
Course syllabus
Frontal teaching (40 hours):
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. Acid-Base reaction: Acids and bases (Arrhenius, Broensted, Lewis theories). pH. 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 compounds. 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. Chemical kinetics: Rates of chemical reactions, reaction order and the kinetic equation. Arrhenius's law. Catalysts.
Exercitations (48 h)
In the classroom: stoichiometry exercises (32 h)
In the laboratory: Elementary laboratory manipulations: weight, dissolution, precipitation, separation by filtration. Acid-base titrations with colourimetric indicators. (16 h).
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. Acid-Base reaction: Acids and bases (Arrhenius, Broensted, Lewis theories). pH. 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 compounds. 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. Chemical kinetics: Rates of chemical reactions, reaction order and the kinetic equation. Arrhenius's law. Catalysts.
Exercitations (48 h)
In the classroom: stoichiometry exercises (32 h)
In the laboratory: Elementary laboratory manipulations: weight, dissolution, precipitation, separation by filtration. Acid-base titrations with colourimetric indicators. (16 h).
Prerequisites for admission
The teaching of General and Inorganic Chemistry is the first course in Chemistry undertaken by students at the beginning of the degree course; therefore, it does not require prerequisites at the university level. The basic knowledge of Mathematics and Physics acquired in the secondary school second grade is enough for understanding the subjects.
Teaching methods
The lectures and frontal exercises take place in the classroom with the projection of 'slides' in PowerPoint format. Students have access to MyAriel platform, where various teaching materials are regularly published, including lecture slides, in-class exercises, and previous years' exams with solutions. Laboratory sessions are conducted at a single lab bench and involve performing basic laboratory operations and processing the resulting data.
Teaching Resources
Lesson slides are available at the teacher's MyAriel website.
Suggested Textbooks:
Tro, Chimica un Approccio Molecolare; Ed. EdiSES.
Petrucci, Herring, Madura, Bissonnette, Chimica Generale; Ed. Piccin.
Chang, Goldsby, Fondamenti di Chimica Generale; Ed. McGraw Hill
Atkins, Jones Chimica Generale; Ed. Zanichelli.
Suggested Textbooks:
Tro, Chimica un Approccio Molecolare; Ed. EdiSES.
Petrucci, Herring, Madura, Bissonnette, Chimica Generale; Ed. Piccin.
Chang, Goldsby, Fondamenti di Chimica Generale; Ed. McGraw Hill
Atkins, Jones Chimica Generale; Ed. Zanichelli.
Assessment methods and Criteria
The examination consists of a written test divided into two parts: the first part, consisting of 15 closed questions (theory), and the second part, consisting of 5 stoichiometric problems, for a total of 32/30 (corresponding to the grade). The written test lasts 2h 30'. To pass the exam, at least 3 out of 5 stoichiometric exercises must be carried out correctly, and a suitable number of theoretical questions must be answered correctly (the candidate must score a minimum of 18/30). There are no oral tests or restrictions on entry to the exam session. There are 2 partial exams ('prove in itinere') during the course itself, which, if both passed, will contribute to the final grade. For each academic year, a minimum of 7 exam sessions are fixed in ordinary and extraordinary examination sessions.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 8
Practicals: 32 hours
Single bench laboratory practical: 16 hours
Lessons: 40 hours
Single bench laboratory practical: 16 hours
Lessons: 40 hours
Professors:
Colombo Valentina, Maggioni Daniela
Shifts:
Turno
Professor:
Maggioni DanielaTurno 1
Professor:
Maggioni DanielaTurno 2
Professor:
Colombo ValentinaProfessor(s)
Reception:
By appointment
room 1053, first floor side B, building 5 (A), Department of Chemistry, Via Golgi 19 Milan