Chemical Sciences

Content of the course The course includes 6 CFU of frontal teaching, divided into four general topics: atomic structure (8 h), covalent chemical bond, ionic, metallic (16 h), chemical bond in coordination complexes (8 h), study of systematic elements of the periodic table, with particular attention to the block if block p (16 h). General description: Basic course in which the chemical bond is treated. In general, the course includes: concepts and applications of chemical bonding for simple molecules and for coordination compounds, by illustrating the main models for the interpretation of the link. Covalent bond (VSEPR methods, valence bond VB, molecular orbitals MO), ionic, metallic. Hydrogen bond and weak interactions. Introduction to coordination compounds VB theory, crystalline field theory, MO theory. Systematic treatment of the main elements of block s and block p, according to their location in the periodic table. Detailed program of the course: in the following section the program with the relative articulation over time is illustrated in detail. The course includes 6 credits and develops in 48 hours of frontal teaching with constant involvement of the students present. Topic 1, Structure of the atom (8 h): role of inorganic chemistry, origin and distribution of the elements, Law of Lavoisier, Proust law, atomic theory of Dalton. Atoms and atomic mass. Gay Lussac's law and Cannizzaro experiments. Avogadro number, Elementary particles, mass and charge of elementary particles, Thomson, Mullikan and Rutherford experiments. Atomic number, mass number, isotopes. Waves and electromagnetic spectrum, atomic spectra, Planck equation, photoelectric effect, energy quantization, Bohr atom. Atomic models. Particle-wave dualism, De Broglie's principle. Elements of wave mechanics, uncertainty principle, Schrodinger equation, quantum numbers, atomic orbitals, representation of radial and angular wave functions. Multielectronic systems, effective nuclear charge, atomic orbital energy, electronic configurations of the elements. Aufbau, principle of maximum multiplicity of Hund and Pauli's escaping principle, periodic properties of the elements. Dimensions of atoms and ions. Ionization energy, electronic affinity, electronegativity and their variation in the periodic table. Metallic character, polarizability. Topic 2, Chemical bond (16 h): ionic bond, crystalline structure, packing of spheres, rules of the radial relationship, reticular energy. Born Haber cycle and Born Landè equation. Covalent bond: order, length, geometry and bonding energy; Lewis theory, polar link and electronegativity. Valence bond theory (VB), model VSEPR. hybrid orbitals and molecule form, resonance structures, electronic delocalization. Characteristics of covalent bonding, sigma and p-greek bonds, examples, correlation between structure and reactivity in simple inorganic molecules. Molecular orbital theory (MO), LCAO methods, applications to homonuclear biatomic molecules. Molecular orbitals for heteronuclear and polynuclear molecules, binding order. Magnetic properties. Metal bond, metals and alloys, band theory, Fermi level, electrical conductivity, insulators, intrinsic semiconductors and band gap, semiconductors. Electrostatic bonds, hydrogen bonding. Intermolecular forces, interactions between permanent, induced and instantaneous dipoles. Ionic, covalent, metallic and molecular solids. Topic 3, Binding in coordination compounds (8 h): general characteristics of transition metals. Structure and isomerism in the complexes. VB treatment of the bond in transition metal complexes. Retrodonation and examples. Crystalline field theory, octahedral complexes, planar and tetrahedral squares, examples, spectrochemical series of ligands. Field theory of binders and MO method applied to complexes. Sigma and p-greek bonds. Electronic spectra and magnetic properties of the complexes, examples Topic 4, Structural characteristics and properties of the elements of block s and block p and their compounds (16 h): Hydrogen and its compounds: isotopic effects, metal, ionic and covalent hydrides. First and second groups: properties, compounds and bonding structures, alkaline and alkaline earth metals, main compounds, hydrides, halides, carbides, organometallic compounds (Grignard) crown complexes, cryptands, biological importance. Group XIII: elemental boron and bond in its compounds, hydrides, halides, oxides and ossoanions, BN, borazine, borax, borane, carboran, aluminum and its compounds. Group XIV: elemental carbon, allotropic forms and its compounds, fullerenes, oxides, halides, alkanes, alkenes, aromatic compounds, carbides and intercalation compounds. Elementary silicon, silicates, molecular sieves and zeolites, silanes, halides, silicon organ compounds, silicones. Hydrides and halides. Group XV: nitrogen, hydrides, ammonia, oxides and bone anions, acids; Elemental phosphorus and its compounds, hydrides, oxides, oxyacids, phosphates and polyphosphates, halides, phosphazens, phosphines, arsenic, antimony and bismuth, main compounds, hydrides and halides. Group XVI: oxygen, ozone, acid, basic and neutral oxides, oxides, peroxides and superoxides, elemental sulfur, sulfur oxides and oxides, sulfuric, sulfuric, sulfuric acids, hydrides. Group XVII: Halogens, properties of halogens, oxides, acids, oxyacids and ossoanions, interhalogenic compounds, polyhalides. Group XVIII: compounds of noble gases, xenon compounds, oxides and halides.

This course is in the Bachelor Degree of Chemistry, in the first year, second semester and it is included in the basic courses. Some basic preliminary knowledge are indispensable, in particular those deriving from the General and Inorganic Chemistry course, for which the prerequisites are required (first semester course of the first year) such as the ability to write and balance chemical reactions, basic nomenclature, definition of acids and bases, redox reactions, laws of thermodynamics. Furthermore, the basic skills of mathematical analysis, which are acquired during the first year of the first semester, are useful and important.

The frequency of teaching classes is not mandatory but recommended.

The modalities through which the achievement of the learning outcomes are ascertained consist in an oral exam, in which the student is asked to describe, also with examples and simple exercises, what has been learned in the course. During the lesson, tests for the evaluation will be also provided in order to help the learning process of the students The exam is aimed at verifying the level of knowledge and in-depth examination of the topics of the teaching program and the reasoning skills developed by the student. The evaluation is expressed in thirtieths (minimum grade 18/30, maximum mark 30/30 with honors). The evaluation consists of an oral test. The overall exam allows to verify the achievement of the objectives in terms of knowledge and skills acquired as well as communication skills. The timing of the exam will be at the end of the course and in the sessions provided by the CAD (June-July, September, January-February). The oral exam includes open-ended questions on the topics covered in the course, accompanied by examples and exercises. The answers are evaluated for completeness of content, ability to synthesize and links between the different themes developed during the course. The examples are useful for verifying the ability to interpret the link. In the assessment of the examination the determination of the final grade takes into account the following elements: the theoretical basis followed by the student for the exposure of the question, the capacity for reasoning, the ownership of language, the clarity of exposition and the critical capacity. To pass the exam, the student must demonstrate that he has acquired sufficient knowledge of the topics related to the chemical bond by applying it to examples of inorganic chemistry. To achieve the maximum score (30/30 cum laude), the student must demonstrate that he has acquired an excellent knowledge of all the topics covered during the course, being able to link them in a logical and coherent way, with a correlation capacity between the chemical structure and properties.

This course is structured in frontal lectures with the development of numerous examples to demonstrate and apply the models on display to simple molecular systems. In particular, a total of 48 hours of frontal teaching (6 CFU) are planned to acquire the knowledge highlighted in the training objectives. In order to develop the ability to apply knowledge, examples and exercises are expected. The lessons are held weekly in the classroom, with two lessons each two hours, for a total of 4 hours per week and the exposure is done using the blackboard and / or slides on power-point.

Content of the course The course includes 6 CFU of frontal teaching, divided into four general topics: atomic structure (14 h), covalent chemical bond, ionic, metallic (16 h), chemical bond in coordination complexes (8 h), study of systematic elements of the periodic table, with particular attention to the block if block p (10 h). General description: Basic course in which the chemical bond is treated. In general, the course includes: concepts and applications of chemical bonding for simple molecules and for coordination compounds, by illustrating the main models for the interpretation of the link. Covalent bond (VSEPR methods, valence bond VB, molecular orbitals MO), ionic, metallic. Hydrogen bond and weak interactions. Introduction to coordination compounds VB theory, crystalline field theory, MO theory. Systematic treatment of the main elements of block s and block p, according to their location in the periodic table. Detailed program of the course: in the following section the program with the relative articulation over time is illustrated in detail. The course includes 6 credits and develops in 48 hours of frontal teaching with constant involvement of the students present. Topic 1, Structure of the atom (14 h): role of inorganic chemistry, origin and distribution of the elements, Law of Lavoisier, Proust law, atomic theory of Dalton. Atoms and atomic mass. Gay Lussac's law and Cannizzaro experiments. Avogadro number, Elementary particles, mass and charge of elementary particles, Thomson, Mullikan and Rutherford experiments. Atomic number, mass number, isotopes. Waves and electromagnetic spectrum, atomic spectra, Planck equation, photoelectric effect, energy quantization, Bohr atom. Atomic models. Particle-wave dualism, De Broglie's principle. Elements of wave mechanics, uncertainty principle, Schrodinger equation, quantum numbers, atomic orbitals, representation of radial and angular wave functions. Multielectronic systems, effective nuclear charge, atomic orbital energy, electronic configurations of the elements. Aufbau, principle of maximum multiplicity of Hund and Pauli's escaping principle, periodic properties of the elements. Dimensions of atoms and ions. Hard-soft theory, Ionization energy, electronic affinity, electronegativity and their variation in the periodic table. Metallic character, polarizability. Topic 2, Chemical bond (16 h): ionic bond, crystalline structure, packing of spheres, rules of the radial relationship, reticular energy. Born Haber cycle and Born Landè equation. Covalent bond: order, length, geometry and bonding energy; Lewis theory, polar link and electronegativity. Valence bond theory (VB), model VSEPR. hybrid orbitals and molecule form, resonance structures, electronic delocalization. Characteristics of covalent bonding, sigma and p-greek bonds, examples, correlation between structure and reactivity in simple inorganic molecules. Molecular orbital theory (MO), LCAO methods, applications to homonuclear biatomic molecules. Molecular orbitals for heteronuclear and polynuclear molecules, binding order. Magnetic properties. Metal bond, metals and alloys, band theory, Fermi level, electrical conductivity, insulators, intrinsic semiconductors and band gap, semiconductors. Electrostatic bonds, hydrogen bonding. Intermolecular forces, interactions between permanent, induced and instantaneous dipoles. Ionic, covalent, metallic and molecular solids. Topic 3, Binding in coordination compounds (8 h): general characteristics of transition metals. Structure and isomerism in the complexes. VB treatment of the bond in transition metal complexes. Retrodonation and examples. Crystalline field theory, octahedral complexes, planar and tetrahedral squares, examples, spectrochemical series of ligands. Field theory of binders and MO method applied to complexes. Sigma and p-greek bonds. Electronic spectra and magnetic properties of the complexes, examples Topic 4, Structural characteristics and properties of the elements of block s and block p and their compounds (10 h): Hydrogen and its compounds: isotopic effects, metal, ionic and covalent hydrides. First and second groups: properties, compounds and bonding structures, alkaline and alkaline earth metals, main compounds, hydrides, halides, carbides, organometallic compounds (Grignard) crown complexes, cryptands, biological importance. Group XIII: elemental boron and bond in its compounds, hydrides, halides, oxides and ossoanions, BN, borazine, borax, borane, carboran, aluminum and its compounds. Group XIV: elemental carbon, allotropic forms and its compounds, fullerenes, oxides, halides, alkanes, alkenes, aromatic compounds, carbides and intercalation compounds. Elementary silicon, silicates, molecular sieves and zeolites, silanes, halides, silicon organ compounds, silicones. Hydrides and halides. Group XV: nitrogen, hydrides, ammonia, oxides and bone anions, acids; Elemental phosphorus and its compounds, hydrides, oxides, oxyacids, phosphates and polyphosphates, halides, phosphazens, phosphines, arsenic, antimony and bismuth, main compounds, hydrides and halides. Group XVI: oxygen, ozone, acid, basic and neutral oxides, oxides, peroxides and superoxides, elemental sulfur, sulfur oxides and oxides, sulfuric, sulfuric, sulfuric acids, hydrides. Group XVII: Halogens, properties of halogens, oxides, acids, oxyacids and ossoanions, interhalogenic compounds, polyhalides. Group XVIII: compounds of noble gases, xenon compounds, oxides and halides.

This course is in the Bachelor Degree of Chemistry, in the second semester of the first year, and it’s included in the basic courses. Some basic preliminary knowledge is indispensable, especially that deriving from the General and Inorganic Chemistry course, for which the prerequisites are fundamental (first semester course of the first year) such as the ability to write and balance chemical reactions, basic nomenclature, definition of acids and bases, redox reactions, laws of thermodynamics. Furthermore, the basic skills of mathematical analysis, which are acquired during the first year of the first semester, are useful and important.

One between the following: 1) J.D.Lee “Chimica Inorganica”, Piccin Editore, 2) J.E.Huheey, E.A. KEttter, R.L. Keiter “Chimica Inorganica Principi, Strutture, Reattività”, Piccin Editore, 3) P. Atkins, T. Overton, J. Rourke, M. Weller, F.Armstrong “Chimica Inorganica”, Zanichelli Editore. didactic material is also available on elearning Moodle 2 Sapienza.

The frequency of teaching classes is not mandatory but strongly recommended.

The modalities through which the achievement of the learning outcomes is ascertained consist of an oral exam, in which the student is asked to describe, through examples and simple exercises, what has been learned in the course. During the lesson, informal tests for the evaluation will be also provided in order to help the learning process of the students. The exam is aimed at verifying the level of knowledge and in-depth examination of the topics of the teaching program and the reasoning skills developed by the student. The evaluation is expressed in thirtieths (minimum grade 18/30, maximum mark 30/30 with honors). The evaluation consists of an oral test. The overall exam allows to verify the achievement of the objectives in terms of knowledge and skills acquired as well as communication skills. The timing of the exam will be at the end of the course and in the sessions provided by the CAD (June-July, September, January-February). The oral exam includes open-ended questions on the topics covered in the course, accompanied by examples and exercises. The answers are evaluated for completeness of content, ability to synthesize and links between the different themes developed during the course. The examples are useful for verifying the ability to interpret the chemical bond. In the assessment of the examination, the determination of the final grade takes into account the following elements: the theoretical basis followed by the student in answering the question, ability for reasoning, ownership of language, clarity of exposition and critical ability. To pass the exam, the student must demonstrate that they have acquired sufficient knowledge of the topics related to the chemical bond by applying it to examples of inorganic chemistry. To achieve the maximum score (30/30 cum laude), the student must demonstrate that they have acquired an excellent knowledge of all the topics covered during the course, being able to link them in a logical and coherent way, with an ability to correlate between the chemical structure and properties.

This course is structured in frontal lectures with the development of numerous examples to demonstrate and apply the models on display to simple molecular systems. In particular, a total of 48 hours of frontal teaching (6 CFU) are planned in order to acquire the knowledge highlighted in the training objectives. To develop the ability to apply knowledge, examples and exercises are expected. The lessons are held weekly in the classroom, with two lessons each two hours, for a total of 4 hours per week using the blackboard and / or slides on power-point.

Electromagnetic radiation. The origins of the atomic theory: Faraday's, Thomson's and Millikan's experiments. Black body radiation and Plank's quantum hypothesis; photoelectric effect and emission spectra of the hydrogen atom. Thomson's and Bohr's atomic models. Eisenberg's uncertainty principle and De Broglie's hypothesis. Bragg's law and Davisson and Germer's experiment. Wave properties of the electron, origins of the time-dependent and time-independent Schroedinger's equation. Properties of the wave function. Solution of the Schroedinger's equation for some simple systems: the electron in the box, mono- and tridimensional cases; separation of variables, energy quantization and wave function normalization. The hydrogen atom: definition of the Schroedinger equation, separation of the electron motion from that of the mass center, change to polar coordinates and final form of the Hamiltonian operator; separation of variables and definition of the related differential equations. Solution of the φ equation, final result for the r and ϑ equations, quantum numbers. Shape of the p and d orbitals expressed by real functions. Radial distribution functions. Filling of atomic orbitals throughout the periodic table. Schroedinger equation for poli-electronic systems, introduction to approximated methods. Variational theorem and linear variations method. The covalent bond, the H2+ molecule-ion and introduction to molecular orbital theory; H2 molecule and introduction to the valence bond theory. Hybrid orbitals and their formulation; a practical method to write the related wave functions for the most common geometries (linear, triangular, tetrahedral, octahedral, triangular bi-pyramidal). Molecular orbital diagrams for the main diatomic molecules: B2, C2, N2, O2, F2, HF, CO, NO. Application of the valence bond theory and of the VSEPR method to the most representative molecules of the main elements: BF3, B(OH)3, CO2, CH4, C2H4, C2H2, CO32-, NH3, N2O, NO2, NO2-, NO3-, O3, PH3, PCl3, PCl5, PO43-, HPO32-, H2PO2-, SO2, SO3, SF6, SO32-, SO42-, S2O32-, ClO-, ClO2-, ClO3-, ClO4-, IF3, IF5, IF7, XeF4. Main classes of solids. Ionic solids: ionic bond model, lattice energy, Madelung's constant, Born-Haber's cycle. Metallic solids: free electron theory and band theory. Covalent solids: insulators and semiconductors according to the band theory; geometric and electronic structures of diamond, graphite, silicon, IV and III-V group semiconductors. P and n-type semiconductors; the structures of tin and lead. Transition metal complexes, Pauli's and Syrkin and Diatkina's theories. Crystal field theory: energy splitting of the d orbitals in octahedral, tetrahedral and square planar complexes; high- and low-spin electron configurations. Crystal Field Stabilization Energy (CFSE), magnetic properties of transition metal complexes. Periodic properties, ionization energy, electron affinity, electronegativity, atomic radii, oxidation states. Chemical properties of the main group's elements.

Basic mathematical skills from high school teaching programs. Elements of differential calculus (derivatives, integrals, simple differential equations) known at least at a basic level. It is recommended, but not mandatory, that students have already passed the exam of "Chimica Generale ed Inorganica con Laboratorio" (General and Inorganic Chemistry with Laboratory).

One of the following two textbooks (the choice is left to the student): 1. G. L. Miessler, D. A. Tarr: Inorganic Chemistry, Ed. Piccin. 2. J. E. Huheey, E. A. Keiter, R. L. Keiter: Inorganic Chemistry, Ed. Piccin 3. L. Pauling, E.B. Wilson: Introduction to Quantum Mechanics with applications to Chemistry, Ed. McGraw-Hill To be used as a reference for some quantum chemical problems. Free download is allowed from the home page of the teacher in the web site of the Chemistry Department. 4. For the treatment of transition metal complexes according to Pauling's e di Sirkin e Diatkina's theories, see the following text, available in the library of our Department: Belluco, Cattalini, Croatto, Furlani, Sartori: Chimica Inorganica, pag. 132-145. 5. A consistent part of the program is covered by notes written by the course teacher. Free download is allowed from the home page of the teacher in the E-learning site of the University of Rome “La Sapienza”.

Lecture-based classroom. Educational media: blackboard. If needed, lectures can be made available through the internet.

Attendance is recommended, but not mandatory.

Oral examination at university or, if needed, through the internet.

Journal articles are not employed.

Lecture-based classroom. Educational media: blackboard. If needed, lectures can be made available through the internet.

Content of the course The course includes 6 CFU of frontal teaching, divided into four general topics: atomic structure (8 h), covalent chemical bond, ionic, metallic (16 h), chemical bond in coordination complexes (8 h), study of systematic elements of the periodic table, with particular attention to the block if block p (16 h). General description: Basic course in which the chemical bond is treated. In general, the course includes: concepts and applications of chemical bonding for simple molecules and for coordination compounds, by illustrating the main models for the interpretation of the link. Covalent bond (VSEPR methods, valence bond VB, molecular orbitals MO), ionic, metallic. Hydrogen bond and weak interactions. Introduction to coordination compounds VB theory, crystalline field theory, MO theory. Systematic treatment of the main elements of block s and block p, according to their location in the periodic table. Detailed program of the course: in the following section the program is illustrated in detail. The course includes 6 credits and develops in 48 hours of frontal teaching. Topic 1, Structure of the atom: role of inorganic chemistry, origin and distribution of the elements. Atoms and atomic mass. Elementary particles, mass and charge of elementary particles. Atomic number, mass number, isotopes. Waves and electromagnetic spectrum, atomic spectra, Planck equation, photoelectric effect, energy quantization, Bohr atom. Atomic models. Particle-wave dualism, De Broglie's principle. Elements of wave mechanics, uncertainty principle, Schrodinger equation, quantum numbers, atomic orbitals, representation of radial and angular wave functions. Multielectronic systems, effective nuclear charge, atomic orbital energy, electronic configurations of the elements. Aufbau, principle of maximum multiplicity of Hund and Pauli's escaping principle, periodic properties of the elements. Dimensions of atoms and ions. Ionization energy, electronic affinity, electronegativity and their variation in the periodic table. Metallic character, polarizability. Topic 2, Chemical bond: ionic bond, crystalline structure, packing of spheres, rules of the radial relationship, reticular energy. Born Haber cycle and Born Landè equation. Covalent bond: order, length, geometry and bonding energy; Lewis theory, polar link and electronegativity. Valence bond theory (VB), model VSEPR. hybrid orbitals and molecule form, resonance structures, electronic delocalization. Characteristics of covalent bonding, sigma and p-greek bonds, examples, correlation between structure and reactivity in simple inorganic molecules. Molecular orbital theory (MO), LCAO methods, applications to homonuclear biatomic molecules. Molecular orbitals for heteronuclear and polynuclear molecules, binding order. Magnetic properties. Metal bond, metals and alloys, band theory, Fermi level, electrical conductivity, insulators, intrinsic semiconductors and band gap, semiconductors. Electrostatic bonds, hydrogen bonding. Intermolecular forces, interactions between permanent, induced and instantaneous dipoles. Ionic, covalent, metallic and molecular solids. Topic 3, Binding in coordination compounds: general characteristics of transition metals. Structure and isomerism in the complexes. VB treatment of the bond in transition metal complexes. Retrodonation and examples. Crystalline field theory, octahedral complexes, planar and tetrahedral squares, examples, spectrochemical series of ligands. Field theory of binders and MO method applied to complexes. Sigma and p-greek bonds. Electronic spectra and magnetic properties of the complexes, examples. Topic 4, Structural characteristics and properties of the elements of block s and block p and their compounds: Hydrogen and its compounds: isotopic effects, metal, ionic and covalent hydrides. First and second groups: properties, compounds and bonding structures, alkaline and alkaline earth metals, main compounds, hydrides, halides, carbides, organometallic compounds (Grignard) crown complexes, cryptands, biological importance. Group XIII: elemental boron and bond in its compounds, hydrides, halides, oxides and ossoanions, BN, borazine, borax, borane, carboran, aluminum and its compounds. Group XIV: elemental carbon, allotropic forms and its compounds, fullerenes, oxides, halides, alkanes, alkenes, aromatic compounds, carbides and intercalation compounds. Elementary silicon, silicates, molecular sieves and zeolites, silanes, halides, silicon organ compounds, silicones. Hydrides and halides. Group XV: nitrogen, hydrides, ammonia, oxides and bone anions, acids; Elemental phosphorus and its compounds, hydrides, oxides, oxyacids, phosphates and polyphosphates, halides, phosphazens, phosphines, arsenic, antimony and bismuth, main compounds, hydrides and halides. Group XVI: oxygen, ozone, acid, basic and neutral oxides, oxides, peroxides and superoxides, elemental sulfur, sulfur oxides and oxides, sulfuric, sulfuric, sulfuric acids, hydrides. Group XVII: Halogens, properties of halogens, oxides, acids, oxyacids and ossoanions, interhalogenic compounds, polyhalides. Group XVIII: compounds of noble gases, xenon compounds, oxides and halides.

This course is in the Bachelor Degree of Chemistry, in the first year, second semester and it is included in the basic courses. Some basic preliminary knowledge are indispensable, in particular those deriving from the General and Inorganic Chemistry course, for which the prerequisites are required (first semester course of the first year) such as the ability to write and balance chemical reactions, basic nomenclature, definition of acids and bases, redox reactions, laws of thermodynamics. Furthermore, the basic skills of mathematical analysis, which are acquired during the first year of the first semester, are useful and important.

1) Weller, Overton, Rourke, M.Weller, Armstrong "La Chimica Inorganica di Atkins", Zanichelli Editore. 2) Huheey - Keiter - Keiter "Chimica Inorganica", Piccin Editore. 3) Miessler - Tarr "Chimica Inorganica", Piccin Editore.

This course is structured in frontal lectures with the development of numerous examples to demonstrate and apply the models on display to simple molecular systems. In particular, a total of 48 hours of frontal teaching (6 CFU) are planned to acquire the knowledge highlighted in the training objectives. In order to develop the ability to apply knowledge, examples and exercises are expected. The lessons are held weekly in the classroom, with two lessons each two hours, for a total of 4 hours per week and the exposure is done using the blackboard and / or slides on power-point. The frequency of teaching classes is not mandatory but recommended.

The lessons are held weekly in the classroom, with two lessons each two hours, for a total of 4 hours per week and the exposure is done using the blackboard and / or slides on power-point. The frequency of teaching classes is not mandatory but recommended.

The modalities through which the achievement of the learning outcomes are ascertained consist in an oral exam, in which the student is asked to describe, also with examples and simple exercises, what has been learned in the course. During the lesson, tests for the evaluation will be also provided in order to help the learning process of the students The exam is aimed at verifying the level of knowledge and in-depth examination of the topics of the teaching program and the reasoning skills developed by the student. The evaluation is expressed in thirtieths (minimum grade 18/30, maximum mark 30/30 with honors). The evaluation consists of an oral test. The overall exam allows to verify the achievement of the objectives in terms of knowledge and skills acquired as well as communication skills. The timing of the exam will be at the end of the course and in the sessions provided by the CAD (June-July, September, January-February). The oral exam includes open-ended questions on the topics covered in the course, accompanied by examples and exercises. The answers are evaluated for completeness of content, ability to synthesize and links between the different themes developed during the course. The examples are useful for verifying the ability to interpret the link. In the assessment of the examination the determination of the final grade takes into account the following elements: the theoretical basis followed by the student for the exposure of the question, the capacity for reasoning, the ownership of language, the clarity of exposition and the critical capacity. To pass the exam, the student must demonstrate that he has acquired sufficient knowledge of the topics related to the chemical bond by applying it to examples of inorganic chemistry. To achieve the maximum score (30/30 cum laude), the student must demonstrate that he has acquired an excellent knowledge of all the topics covered during the course, being able to link them in a logical and coherent way, with a correlation capacity between the chemical structure and properties.

This course is structured in frontal lectures with the development of numerous examples to demonstrate and apply the models on display to simple molecular systems. In particular, a total of 48 hours of frontal teaching (6 CFU) are planned to acquire the knowledge highlighted in the training objectives. In order to develop the ability to apply knowledge, examples and exercises are expected.