General and Inorganic Chemistry and Stoichiometry

A.Y. 2019/2020
10
Max ECTS
88
Overall hours
SSD
CHIM/03
Language
Italian
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. The general chemistry course must also give the student an appreciation of the importance of chemistry to society in general and to daily life in particular.
Expected learning outcomes
The expected learning outcomes for the students will be the achievement of the ability to correctly write the reactions, to identify the different reaction types, to evaluate the thermodynamic and kinetic reaction conditions and of the skillfulness to use friendly the methodologies for quantitative achievement of the chemical reactions.
Course syllabus and organization

Linea AK

Linea AK
Responsible
Lesson period
year
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.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.

[Program for not attending students with reference to descriptor 1 and 2]:
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.
Prerequisites, exams and assessment
The primary goal of the course is to provide a solid foundation in the basics concepts and facts of chemistry, particularly those needed for a successful understanding of other subjects for which chemistry is a prerequisite. The general chemistry course must also give the student an appreciation of the importance of chemistry to society in general and to daily life in particular.
Teaching methods
The teacher uses slides (PowerPoint) including both concepts and formulas of all the topics of the course program. Many exercises are also proposed to the students in order to test their understanding of the chemical concepts. Just before the "in itinere" test, an online simulation
of the exam is carried out.
Teaching resources and bibliography
Books:
» Tro Chimica. Un approccio molecolare. Ed. EDISES
» Whitten, Davis, Peck, Stanley Chimica. Ed. Piccin
» Atkins, Jones, Laverman Principi di chimica. Ed. ZANICHELLI
Schoolbooks:
» Demartin, Peloso Esercizi numerici di Chimica Generale, Ed. Progetto Libreria Padova.
» A. Caselli, S. Rizzato, F. Tessore Stechiometria dal testo di M. Freni e A. Sacco . Ed. EDISES
Teaching materials on Ariel site.
Exam
Written test in 2 h. The student must solve 16 questions, 14 multiple choices problems (10 stoichiometric exercises and 4 theoretical questions) and 2 open theoretical questions (1 of the 2 is necessary for bypassing the examination).
During the course, 3 ongoing tests are expected. Good results (≥18) in all the tests allow to pass the examination. The final mark could be the average of the 3 test results, on the basis of professor decision.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 10
Practicals: 16 hours
Lessons: 72 hours
Professor: Rimoldi Isabella

Linea LZ

Linea LZ
Responsible
Lesson period
year
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.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.

[Program for not attending students with reference to descriptor 1 and 2]:
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.
Prerequisites, exams and assessment
The primary goal of the course is to provide a solid foundation in the basics concepts and facts of chemistry, particularly those needed for a successful understanding of other subjects for which chemistry is a prerequisite. The general chemistry course must also give the student an appreciation of the importance of chemistry to society in general and to daily life in particular.
Teaching methods
The teacher uses slides (PowerPoint) including both concepts and formulas of all the topics of the course program. Many exercises are also proposed to the students in order to test their understanding of the chemical concepts. Just before the "in itinere" test, an online simulation of the exam is carried out.
Teaching resources and bibliography
Books:
» Tro Chimica. Un approccio molecolare. Ed. EDISES
» Whitten, Davis, Peck, Stanley Chimica. Ed. Piccin
» Atkins, Jones, Laverman Principi di chimica. Ed. ZANICHELLI
Schoolbooks:
» Demartin, Peloso Esercizi numerici di Chimica Generale, Ed. Progetto Libreria Padova.
» A. Caselli, S. Rizzato, F. Tessore Stechiometria dal testo di M. Freni e A. Sacco . Ed. EDISES
Teaching materials on Ariel site.
Exam
Written test in 2 h. The student must solve 16 questions, 14 multiple choices problems (10 stoichiometric exercises and 4 theoretical questions) and 2 open theoretical questions (1 of the 2 is necessary for bypassing the examination).
During the course, 3 ongoing tests are expected. Good results (≥18) in all the tests allow to pass the examination. The final mark could be the average of the 3 test results, on the basis of professor decision.
CHIM/03 - GENERAL AND INORGANIC CHEMISTRY - University credits: 10
Practicals: 16 hours
Lessons: 72 hours
Professor: Soave Raffaella