General and Inorganic Chemistry
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 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 can be attended as a single course.
Course syllabus and organization
Linea AK
Responsible
Lesson period
First semester
Synchronous lectures will not available on any web-conference platform.
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 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. Elettrochemistry: Cell potentials. Nernst's law. Electrolysis. Chemical kinetics: Rates of chemical reactions, reaction order and the kinetic equation. Arrhenius's law. Catalysts. Descriptive Inorganic Chemistry: The biologically relevant elements.
Laboratory activities and exercises (48 hours)
In Classroom: Stoichiometric Calculations (32 hours)
Laboratory activities: Weighing, precipitation, acid-base titrations. Preparation of buffer solutions. Typical reactions of inorganic cations and anions (16 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 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. Elettrochemistry: Cell potentials. Nernst's law. Electrolysis. Chemical kinetics: Rates of chemical reactions, reaction order and the kinetic equation. Arrhenius's law. Catalysts. Descriptive Inorganic Chemistry: The biologically relevant elements.
Laboratory activities and exercises (48 hours)
In Classroom: Stoichiometric Calculations (32 hours)
Laboratory activities: Weighing, precipitation, acid-base titrations. Preparation of buffer solutions. Typical reactions of inorganic cations and anions (16 hours)
Prerequisites for admission
The teaching of General and Inorganic Chemistry is the first course of Chemistry undertaken by the student at the beginning of the degree course; therefore it does not require prerequisites at university level. The basic knowledge of Mathematics and Physics acquired in the secondary school of second grade is enough for understanding the subjects.
Teaching methods
The lectures and frontal exercises take place in the classroom with projection of 'slides' in power point format. The students have at their disposal the Ariel and Teams site, where various teaching materials are regularly published, including: the slides of the lessons, the frontal exercises and the previous year exams with resolutions .
The laboratory experiences are carried out at a single laboratory bench and consist in the execution of elementary laboratory operations and processing of the obtained data. The laboratory experiences are: weighing, dissolving, precipitation, filtration separation. Acid-base titrations with use of indicators.
The laboratory experiences are carried out at a single laboratory bench and consist in the execution of elementary laboratory operations and processing of the obtained data. The laboratory experiences are: weighing, dissolving, precipitation, filtration separation. Acid-base titrations with use of indicators.
Teaching Resources
Lesson' slides available at the teacher's Ariel 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 exam consists of a written test divided into two parts: the first part consists of 15 multiple-choice questions (theory), and the second part consists of 5 stoichiometry exercises for a total score of 32/30 (equivalent to honors). The written test lasts 2 hours and 30 minutes. To pass the exam, it is necessary to correctly solve at least 3 out of 5 stoichiometry exercises and correctly answer a sufficient number of theoretical questions (the candidate must achieve a minimum score of 18/30). There are no oral exams or restrictions on exam registrations. There are 2 interim tests during the course, which, if both passed, will contribute to the final averaged grade and passing the exam. Each academic year, there are at least 7 exam dates scheduled in the regular and extraordinary exam 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, 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 of Chemistry undertaken by the student 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. The students have at their disposal the Ariel and Teams sites, where various teaching materials are regularly published, including the slides of the lessons, the frontal exercises, and the previous year's exams with resolutions. The laboratory experiences are carried out at a single laboratory bench and consist of the execution of elementary laboratory operations and processing of the obtained data.
Teaching Resources
Lesson' slides available at the teacher's Ariel 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 is a written test divided into two parts: the first one consisting of 15 closed questions (theory) and the second one consisting of 5 stoichiometric problems for a total of 32/30 (corresponding to the praise). The written test lasts 2h 30'. In order 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 and 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 number 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 ValentinaEducational website(s)
Professor(s)
Reception:
By appointment
room 1053, first floor side B, building 5 (A), Department of Chemistry, Via Golgi 19 Milan