ITA | ENG
B000066 - CHEMISTRY
Main information
Teaching Language
Course Content
Suggested readings
Learning Objectives
Prerequisites
Teaching Methods
Further information
Type of Assessment
Course program
Academic Year 2018-19
Course year
First year - First Semester
Belonging Department
Industrial Engineering (DIEF)
Course Type
Single education field course
Scientific Area
CHIM/07 - PRINCIPLES OF CHEMISTRY FOR APPLIED TECHNOLOGIES
Credits
6
Teaching Hours
54
Teaching Term
17/09/2018 ⇒ 21/12/2018
Attendance required
No
Type of Evaluation
Final Grade
Course Content
show
Course program
show
Lectureship
- Last names A-D PAOLI PAOLA
- Last names E-N ROSSI PATRIZIA
- Last names O-Z ROSSI PATRIZIA
Teaching Language - Last names E-N
Italian
Teaching Language - Last names O-Z
Italian
Course Content - Last names A-D
Atoms, ions and molecules.
The electronic structure of atoms and the chemical periodicity.
Chemical bonding and molecular structure.
Intermolecular forces and states of matter.
The gaseous state.
Chemical equations and reaction stoichiometry.
Chemical thermodynamics.
Chemical equilibrium.
Electrochemistry.
Chemical kinetics.
The electronic structure of atoms and the chemical periodicity.
Chemical bonding and molecular structure.
Intermolecular forces and states of matter.
The gaseous state.
Chemical equations and reaction stoichiometry.
Chemical thermodynamics.
Chemical equilibrium.
Electrochemistry.
Chemical kinetics.
Course Content - Last names E-N
Atomic structure. Chemical bonds and their general characteristics. Intermolecular forces and states of matter. Solid state: structural characteristics of solids. Laws of Gases. Thermochemistry. Chemical equilibrium. Chemical reactions. Colligative properties. Electrochemistry: electrochemical processes; batteries and electrode potentials; the phenomenon of corrosion; electrolysis. Chemical kinetics.
Course Content - Last names O-Z
Atomic structure. Chemical bonds and their general characteristics. Intermolecular forces and states of matter. Solid state: structural characteristics of solids. Laws of Gases. Thermochemistry. Chemical equilibrium. Chemical reactions. Colligative properties. Electrochemistry: electrochemical processes; batteries and electrode potentials; the phenomenon of corrosion; electrolysis. Chemical kinetics.
Suggested readings - Last names E-N (Search our library's catalogue)
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- McQuarrie, Rock, Gallogly, Principi di Chimica, ed. Zanichelli
-Shultz, Chimica Generale, Ed. Zanichelli
-Silberberg, Chimica, ed. McGraw-Hill
- Dapporto, Paoli, Rossi, Lezioni di Chimica, ed. Progetto Leonardo
-Bertini, Luchinat, Mani, Stechiometria, ed. Casa Editrice Ambrosiana
-Ugozzoli, Come risolvere i problemi di chimica, Ed. Zanichelli
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- McQuarrie, Rock, Gallogly, Principi di Chimica, ed. Zanichelli
-Shultz, Chimica Generale, Ed. Zanichelli
-Silberberg, Chimica, ed. McGraw-Hill
- Dapporto, Paoli, Rossi, Lezioni di Chimica, ed. Progetto Leonardo
-Bertini, Luchinat, Mani, Stechiometria, ed. Casa Editrice Ambrosiana
-Ugozzoli, Come risolvere i problemi di chimica, Ed. Zanichelli
Suggested readings - Last names O-Z (Search our library's catalogue)
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- McQuarrie, Rock, Gallogly, Principi di Chimica, ed. Zanichelli
-Shultz, Chimica Generale, Ed. Zanichelli
-Silberberg, Chimica, ed. McGraw-Hill
- Dapporto, Paoli, Rossi, Lezioni di Chimica, ed. Progetto Leonardo
-Bertini, Luchinat, Mani, Stechiometria, ed. Casa Editrice Ambrosiana
-Ugozzoli, Come risolvere i problemi di chimica, Ed. Zanichelli
- Atkins, Jones, Fondamenti di chimica generale, Zanichelli
- McQuarrie, Rock, Gallogly, Principi di Chimica, ed. Zanichelli
-Shultz, Chimica Generale, Ed. Zanichelli
-Silberberg, Chimica, ed. McGraw-Hill
- Dapporto, Paoli, Rossi, Lezioni di Chimica, ed. Progetto Leonardo
-Bertini, Luchinat, Mani, Stechiometria, ed. Casa Editrice Ambrosiana
-Ugozzoli, Come risolvere i problemi di chimica, Ed. Zanichelli
Learning Objectives - Last names A-D
The course aims to provide students with the basic knowledge of chemistry essential for understanding the relationships between microscopic structure and macroscopic properties of materials, thus contributing to form a base of basic scientific knowledge to which to add the specific characteristics of the course of study. In particular, the course topics are selected in such a way as to enable students to face, understand and evaluate the chemical, thermodynamic, kinetic and catalytic aspects related to chemical processes and their optimal conduction.
Students will acquire:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and understanding of the role of these laws in the formulation of representative models of tangible reality.
Student will be able to:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basis for mechanical engineering problems.
Students will acquire:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and understanding of the role of these laws in the formulation of representative models of tangible reality.
Student will be able to:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basis for mechanical engineering problems.
Learning Objectives - Last names E-N
The aim of the course is to provide the student with the knowledge of chemistry that is essential to form the cultural background of the future engineer in view of the professional role she/he will play. In particular, those aspects of chemistry relevant in the field of industrial engineering will be privileged, among which for example: the study of chemical reactions and in particular of their spontaneity, the chemistry of metals, corrosion, electrochemistry, thermochemistry.
Knowledge Acquired:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and the understanding of the role of these laws in the formulation of representative models of tangible reality
Application Capacity:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basic for mechanical engineering problems.
Knowledge Acquired:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and the understanding of the role of these laws in the formulation of representative models of tangible reality
Application Capacity:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basic for mechanical engineering problems.
Learning Objectives - Last names O-Z
The aim of the course is to provide the student with the knowledge of chemistry that is essential to form the cultural background of the future engineer in view of the professional role she/he will play. In particular, those aspects of chemistry relevant in the field of industrial engineering will be privileged, among which for example: the study of chemical reactions and in particular of their spontaneity, the chemistry of metals, corrosion, electrochemistry, thermochemistry.
Knowledge Acquired:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and the understanding of the role of these laws in the formulation of representative models of tangible reality
Application Capacity:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basic for mechanical engineering problems.
Knowledge Acquired:
cc2: Knowledge and understanding of the relevant laws of chemistry and some laws of physics (thermodynamics) in the field of industrial engineering and the understanding of the role of these laws in the formulation of representative models of tangible reality
Application Capacity:
ca2: Applying knowledge and understanding related to the chemical field to solve mono-disciplinary problems of chemistry as a basic for mechanical engineering problems.
Prerequisites - Last names A-D
Not required
Prerequisites - Last names E-N
Prerequisites are not requested
Prerequisites - Last names O-Z
none
Teaching Methods - Last names A-D
The course includes lectures (approximately 70-80% of the total teaching hours) and exercises designed to prepare students to take the final exam.
Teaching Methods - Last names E-N
The course includes lectures (which will occupy approximately 70-80% of the total teaching hours) and exercises designed to prepare students to take the final exam.
Teaching Methods - Last names O-Z
The course includes lectures (which will occupy approximately 70-80% of the total teaching hours) and exercises designed to prepare students to take the final exam.
Further information - Last names A-D
Testing texts and teaching material related to particular topics will be provided by the teacher (available on the Moodle online platform).
Further information - Last names E-N
Testing texts and teaching material related to particular topics will be provided by the teacher.
Further information - Last names O-Z
Testing texts and teaching material related to particular topics will be provided by the teacher.
Type of Assessment - Last names A-D
The student evaluation includes a written test consisting of 4 open-ended theoretical questions and 4 exercises. In open-ended questions the student must demonstrate, in addition to a good knowledge of the topics covered (CC2 competence), to have sufficient exposure skills and to possess a specialized lexicon at least sufficient. In the exercises, the student will have to demonstrate a good ability to apply the acquired knowledge to solve problems in the chemical field (CA2 capacity). At the student's choice, if she/he has reached an evaluation of at least 18/30 in the written test, she/he can then take an oral test in which her/ his ability to organize her/his knowledge in the chemical field will be evaluated. This capacity must be at least sufficient.
Type of Assessment - Last names E-N
The student evaluation includes a written test consisting of 4 open-ended theoretical questions and 4 exercises. In open-ended questions the student must demonstrate, in addition to a good knowledge of the topics covered (CC2 competence), also to have sufficient exposure skills and to possess a specialized lexicon at least sufficient. In the exercises, the student will have to demonstrate a good ability to apply the acquired knowledge to solve problems in the chemical field (CA2 capacity). At the student's choice, if she/he has reached an evaluation of at least 18/30 in the written test, she/he can then take an oral test in which her/ his ability to organize her/his knowledge in the chemical field will be evaluated. This capacity must at least be sufficient
Type of Assessment - Last names O-Z
The student evaluation includes a written test consisting of 4 open-ended theoretical questions and 4 exercises. In open-ended questions the student must demonstrate, in addition to a good knowledge of the topics covered (CC2 competence), also to have sufficient exposure skills and to possess a specialized lexicon at least sufficient. In the exercises, the student will have to demonstrate a good ability to apply the acquired knowledge to solve problems in the chemical field (CA2 capacity). At the student's choice, if she/he has reached an evaluation of at least 18/30 in the written test, she/he can then take an oral test in which her/ his ability to organize her/his knowledge in the chemical field will be evaluated. This capacity must at least be sufficient
Course program - Last names A-D
Atomic structure of matter. Atoms, ions and molecules: the atomic model of matter; the subatomic particles; isotopes, atomic weight, molecular weight, mole.
Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; the Schrodinger equation; quantum numbers; atomic orbitals (s, p, d, f). Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
Periodic system. Periodic table of the elements; periodic quantities (ionization energy, electronic affinity, atomic radius, electronegativity).
Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory. Pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals and metallic bonding.
Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids.
Gaseous state. gas law equations. State diagram. Colligative properties.
Elements of thermodynamics. Thermochemistry. Chemical equilibrium. Law of mass action. Le Chatelier's principle. Spontaneity of a transformation.
Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. Oxidation number, balancing redox reactions.
Electrochemistry. Galvanic cells; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
Chemical kinetics.
Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; the Schrodinger equation; quantum numbers; atomic orbitals (s, p, d, f). Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
Periodic system. Periodic table of the elements; periodic quantities (ionization energy, electronic affinity, atomic radius, electronegativity).
Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory. Pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals and metallic bonding.
Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids.
Gaseous state. gas law equations. State diagram. Colligative properties.
Elements of thermodynamics. Thermochemistry. Chemical equilibrium. Law of mass action. Le Chatelier's principle. Spontaneity of a transformation.
Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. Oxidation number, balancing redox reactions.
Electrochemistry. Galvanic cells; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
Chemical kinetics.
Course program - Last names E-N
- Atomic structure of matter. Atoms, ions and molecules: the atomic model of matter; the subatomic particles; atomic weight, molecular weight, isotopes, mole.
-Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; wave mechanics; the Schrodinger equation; eigenfunctions and eigenvalues; quantum numbers; the wave function in polar coordinates, the physical meaning of the wave function. orbitals s, p, d, f; Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
- Periodic system. Periodic table of the elements; periodic quantities: ionization energy, electronic affinity, atomic radius.
- Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory, expansion of the octet; resonance; formal charge. Structural formulas; Electronegativity; pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals. Intrinsic and extrinsic semiconductors. Covalent bond model and energy band model.
- Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids. The solid state: amorphous solids and crystalline solids. Crystalline lattices and elementary cells (outline).
- Gaseous state. equation of state of perfect gases; van der Waals state equation.
- State diagram.
- Colligative properties: lowering of vapor pressure, elevation of boiling point, depression of freezing point, osmotic pressure.
-Elements of chemical thermodynamics. First principle. Thermochemistry (reaction enthalpy, Hess's law). - Chemical equilibrium. Law of mass action. Le Chatelier's principle. Criterion of spontaneity of a transformation.
- Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. The oxidation number. Balancing of an oxidation-reduction reaction.
-Elettcrochemistry. The batteries; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
- Chemical chemistry. Speed of chemical reactions; reaction order and reaction mechanisms; activation energy; catalysis.
-Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; wave mechanics; the Schrodinger equation; eigenfunctions and eigenvalues; quantum numbers; the wave function in polar coordinates, the physical meaning of the wave function. orbitals s, p, d, f; Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
- Periodic system. Periodic table of the elements; periodic quantities: ionization energy, electronic affinity, atomic radius.
- Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory, expansion of the octet; resonance; formal charge. Structural formulas; Electronegativity; pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals. Intrinsic and extrinsic semiconductors. Covalent bond model and energy band model.
- Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids. The solid state: amorphous solids and crystalline solids. Crystalline lattices and elementary cells (outline).
- Gaseous state. equation of state of perfect gases; van der Waals state equation.
- State diagram.
- Colligative properties: lowering of vapor pressure, elevation of boiling point, depression of freezing point, osmotic pressure.
-Elements of chemical thermodynamics. First principle. Thermochemistry (reaction enthalpy, Hess's law). - Chemical equilibrium. Law of mass action. Le Chatelier's principle. Criterion of spontaneity of a transformation.
- Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. The oxidation number. Balancing of an oxidation-reduction reaction.
-Elettcrochemistry. The batteries; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
- Chemical chemistry. Speed of chemical reactions; reaction order and reaction mechanisms; activation energy; catalysis.
Course program - Last names O-Z
- Atomic structure of matter. Atoms, ions and molecules: the atomic model of matter; the subatomic particles; atomic weight, molecular weight, isotopes, mole.
-Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; wave mechanics; the Schrodinger equation; eigenfunctions and eigenvalues; quantum numbers; the wave function in polar coordinates, the physical meaning of the wave function. orbitals s, p, d, f; Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
- Periodic system. Periodic table of the elements; periodic quantities: ionization energy, electronic affinity, atomic radius.
- Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory, expansion of the octet; resonance; formal charge. Structural formulas; Electronegativity; pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals. Intrinsic and extrinsic semiconductors. Covalent bond model and energy band model.
- Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids. The solid state: amorphous solids and crystalline solids. Crystalline lattices and elementary cells (outline).
- Gaseous state. equation of state of perfect gases; van der Waals state equation.
- State diagram.
- Colligative properties: lowering of vapor pressure, elevation of boiling point, depression of freezing point, osmotic pressure.
-Elements of chemical thermodynamics. First principle. Thermochemistry (reaction enthalpy, Hess's law). - Chemical equilibrium. Law of mass action. Le Chatelier's principle. Criterion of spontaneity of a transformation.
- Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. The oxidation number. Balancing of an oxidation-reduction reaction.
-Elettcrochemistry. The batteries; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
- Chemical chemistry. Speed of chemical reactions; reaction order and reaction mechanisms; activation energy; catalysis.
-Electronic structure of the atom. The Heisenberg uncertainty principle; electromagnetic radiation; light-matter interaction: absorption and emission spectra; the wave-particle duality and De Broglie's relationship; wave mechanics; the Schrodinger equation; eigenfunctions and eigenvalues; quantum numbers; the wave function in polar coordinates, the physical meaning of the wave function. orbitals s, p, d, f; Polyelectronic atoms; the quantum number of spin; the screen effect; energy flow of the orbitals as a function of Z; rules for filling the orbitals (minimum energy, Pauli, Hund).
- Periodic system. Periodic table of the elements; periodic quantities: ionization energy, electronic affinity, atomic radius.
- Chemical bonds. Introduction to chemical bonding. The covalent bond; hybridization and geometry of molecules; VSEPR theory, expansion of the octet; resonance; formal charge. Structural formulas; Electronegativity; pure and polar covalent bonds; dipole moment; polar and apolar molecules; the ionic bond. General characteristics of metals. Intrinsic and extrinsic semiconductors. Covalent bond model and energy band model.
- Intermolecular forces and solid state. The hydrogen bond. Intermolecular forces and states of aggregation of matter. Types of solids: metallic, ionic, covalent and molecular. Main properties of the different types of solids. The solid state: amorphous solids and crystalline solids. Crystalline lattices and elementary cells (outline).
- Gaseous state. equation of state of perfect gases; van der Waals state equation.
- State diagram.
- Colligative properties: lowering of vapor pressure, elevation of boiling point, depression of freezing point, osmotic pressure.
-Elements of chemical thermodynamics. First principle. Thermochemistry (reaction enthalpy, Hess's law). - Chemical equilibrium. Law of mass action. Le Chatelier's principle. Criterion of spontaneity of a transformation.
- Chemical reactions. Reactions in solution (molarity and pH). Oxidation-reduction and combustion reactions. The oxidation number. Balancing of an oxidation-reduction reaction.
-Elettcrochemistry. The batteries; the Nernst equation; spontaneity and displacement of redox reactions; oxidation-reduction reactions of water; electrolysis of molten salts and in aqueous solution; Faraday laws. The phenomenon of corrosion. Strategies for corrosion protection.
- Chemical chemistry. Speed of chemical reactions; reaction order and reaction mechanisms; activation energy; catalysis.