| Chemistry
(objectives)
The course aims to enable students to acquire basic knowledge of general chemistry, in particular:
1) Knowledge and ability to understand the atomic theory of matter, the properties of elements and chemical substances), the ability of chemical substances to undergo transformations into other species, the ability to understand and evaluate the stoichiometric relationships, reactions and equilibria that occur in aqueous systems, the basic knowledge of organic chemistry with the study of the functional groups of organic molecules and biomolecules.
2) Knowledge and understanding applied to carrying out stoichiometry exercises typically used in a chemical laboratory.
3) Independent judgment in evaluating and solving questions of chemical interest.
4) Communication skills in the scientific language of theoretical and experimental chemistry.
5) Ability to learn new scientific topics starting from the acquired foundations of general and organic chemistry.
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Code
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119490 |
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Language
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ITA |
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Type of certificate
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Profit certificate
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Credits
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9
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Scientific Disciplinary Sector Code
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CHIM/03
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Contact Hours
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56
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Laboratory Hours
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16
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Type of Activity
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Basic compulsory activities
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Derived from
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118923 GENERAL AND INORGANIC CHEMISTRY in Natural and Environmental Sciences L-32 Sanna Nico
(syllabus)
1. Introduction
States of aggregation of matter. Homogeneous and heterogeneous systems. Chemical elements and substances. Main techniques of separation. Chemical and physical transformations. Energy and chemical transformations. Intensive and extensive properties of matter. Fundamental laws of physics.
The atom: protons, neutrons and electrons. Atomic number and mass number: isotopes. Atomic masses and relative atomic masses. Chemical symbols and their quantitative meaning. Molecular compounds and ionic compounds. Relative molecular mass. Avogadro number. The mole concept.
2. Chemical formulas and equations
Chemical equations and balance. Kind of reactions: combinations, decomposition and combustion. Chemical analysis by combustion. Balanced equations and quantitative information. The concept of limitant reagent. Chemical reaction in solution: acid-base and precipitation. Balancing redox equations. Concentration of solutions and corresponding units.
3. Atomic structure
Electromagnetic radiation. Bohr model of the hydrogen atom. Atomic spectra. De Broglie and the wave nature of matter. Heisenberg's uncertainty principle. Schrodinger equation. Wave-particle duality. Atomic orbitals. Quantum numbers. Pauli exclusion principle. Electronic configuration of the elements. Principle of Aufbau. The periodic system of the elements. Periodic properties: Dimensions of atoms and ions, ionization energy, electron affinity. Metals, non-metals and metalloids. Notes on coordination compounds and their biological significance.
4. The chemical bond
Ionic and covalent bonding. Bond properties: order, distance and energy. Electronegativity and Dipolar moment. Lewis's structures. VSEPR model and geometry of molecules. Chemical bond theory: hybrid orbitals and resonance theory in chemistry. Magnetic properties of matter. Intermolecular forces. Hydrogen bond.
5. The gaseous state
Ideal gas state equation. Dalton's Law for gaseous mixtures. Density and relative density of gases and gaseous mixtures. Average molecular mass of a gaseous mixture. Kinetic-molecular theory and velocity distribution. Graham's effusion law. Experimental methods for the determination of the molecular masses of gaseous substances. Real gases, Van der Waals equation.
6. Condensed states
The Liquid state
Intramolecular and intermolecular interactions. Intermolecular interactions of an electrostatic nature. Enthalpy of vaporization and its dependencies. Hydrogen bond. Phase's equilibria. Vapour pressure. Phase transitions and related enthalpies. Clausius-Clapeyron equation. One component phase diagram. Water Phase diagram of water.
The Solid state
Crystalline lattices and elementary cells. Molecular, ionic, covalent and metallic solids. Polymorphism and allotropy. X-ray diffraction. Definition of solids based on symmetry and intermolecular interactions.
7. Chemical thermodynamics
Definition of thermodynamic system. Status functions. Cyclic and open transformations. Reversible and irreversible transformations. Heat, work and internal energy. First principle of thermodynamics. Enthalpy and Hess's law. Entropy. Second principle of thermodynamics. Spontaneous processes. Free energy. Third principle of thermodynamics. Introduction to the concept of chemical equilibrium.
8. Solutions
Solubility and dissolving processes. Gas solutions in liquids. Enthalpy of dissolution and effect of temperature on solubilization processes. Ideal solutions and real solutions. Raoult's law. Ebullioscopic elevation and cryoscopic lowering. Colligative properties of the ideal solutions and determination of the molecular masses of compounds. Osmosis. Not ideal solutions. Fractional distillation. Azeotropic mixtures. Henry's law. Activity and ionic strength.
9. Chemical equilibrium
Spontaneous processes and thermodynamic equilibrium in chemical reactions. Mass action law. Isoterm and isochoric of van't Hoff. Homogeneous equilibria. The principle of Le Chatelier. Effect of the variation in concentration of a reagent or a product on equilibrium. Effect of variation of volume, pressure and temperature on homogeneous equilibria. Heterogeneous equilibria.
10. Equilibria in Solution
Acid-base equilibria: General definitions (Arrhenius, Broensted-Lowry, Lewis). Strength of acids and bases and equilibrium constants. Molecular structure and properties of acid-base. Water autoionization. The pH and the pOH. PH calculation of acidic, basic and saline solutions. Buffer solutions. Solubility and solubility product of salts.
11. Chemical Kinetics
Reaction rate. Kinetic laws and integrated kinetic laws. Order and molecularity of a reaction. Arrhenius equation. Activation energy. Kinetic mechanism of reactions. Collision theory and theory of activated complex. Catalysis.
12. Electrochemical
Galvanic cells. Electrode and electrode reaction. Standard potential. Thermodynamics of galvanic cells. Nerst equation.
Stoichiometry: Mole. Molecular and minimal formulas. Nomenclature of the main inorganic compounds. Chemical equations and ponderal ratios. Limiting reactive. Law of gases and gaseous species in chemical reactions. Indirect analysis. Solutions and volumetric analysis. Gaseous, homogeneous and heterogeneous chemical balances. Thermochemistry and thermodynamics of reactions. Colligative properties of non-electrolytes and electrolytes solutions. PH calculation of acid, base and salts solutions. Buffer solutions. Solubility and solubility product of salts.
Chimica Organica
13. General properties of organic compounds
Functional groups. Nomenclature. The bond in organic compounds and references to the theory of the molecular orbitals. Structure isomerism and stereoisomers. Chirality: compounds with multiple stereocenters and meso-forms, absolute and relative configuration, nomenclature of chiral compounds, optical activity of stereoisomers. Cis-trans geometric isomers. Conformational isomerism.
14. Reactivity of sp3 carbon compunds
General information on the reactivity of organic compounds. Nucleophilic substitution. Alcohols, ethers and sulfur analogues. Amines and alchil-ammonia salts.
15. Reactivity of sp2 carbon compunds
Alkenes and cycloalkenes. Aromatic compounds. Carbonyl compounds. Carboxylic acids and derivatives.
16. Compounds of significant biological interest
Carbohydrates. Lipids. Amino acids. Nucleotides. Biological polymers: polysaccharides or glycans, peptides and proteins, nucleic acids.
(reference books)
M. Speranza et al., General and inorganic chemistry, Edi-Ermes Editore (2013).
F. Cacace and M. Schiavello, Stoichiometry, Bulzoni Editore (1995).
A. Fiecchi et al. Chimica e propedeutica biochimica, Edi-ermes (2002).
NOTE: The teacher will communicate at the beginning of the course the link to the additional teaching material available to the students.
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Dates of beginning and end of teaching activities
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From to |
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Delivery mode
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Traditional
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Attendance
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not mandatory
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Evaluation methods
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Written test
Oral exam
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Teacher
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Sanna Nico
(syllabus)
1. Introduction
States of aggregation of matter. Homogeneous and heterogeneous systems. Chemical elements and substances. Main techniques of separation. Chemical and physical transformations. Energy and chemical transformations. Intensive and extensive properties of matter. Fundamental laws of physics.
The atom: protons, neutrons and electrons. Atomic number and mass number: isotopes. Atomic masses and relative atomic masses. Chemical symbols and their quantitative meaning. Molecular compounds and ionic compounds. Relative molecular mass. Avogadro number. The mole concept.
2. Chemical formulas and equations
Chemical equations and balance. Kind of reactions: combinations, decomposition and combustion. Chemical analysis by combustion. Balanced equations and quantitative information. The concept of limitant reagent. Chemical reaction in solution: acid-base and precipitation. Balancing redox equations. Concentration of solutions and corresponding units.
3. Atomic structure
Electromagnetic radiation. Bohr model of the hydrogen atom. Atomic spectra. De Broglie and the wave nature of matter. Heisenberg's uncertainty principle. Schrodinger equation. Wave-particle duality. Atomic orbitals. Quantum numbers. Pauli exclusion principle. Electronic configuration of the elements. Principle of Aufbau. The periodic system of the elements. Periodic properties: Dimensions of atoms and ions, ionization energy, electron affinity. Metals, non-metals and metalloids. Notes on coordination compounds and their biological significance.
4. The chemical bond
Ionic and covalent bonding. Bond properties: order, distance and energy. Electronegativity and Dipolar moment. Lewis's structures. VSEPR model and geometry of molecules. Chemical bond theory: hybrid orbitals and resonance theory in chemistry. Magnetic properties of matter. Intermolecular forces. Hydrogen bond.
5. The gaseous state
Ideal gas state equation. Dalton's Law for gaseous mixtures. Density and relative density of gases and gaseous mixtures. Average molecular mass of a gaseous mixture. Kinetic-molecular theory and velocity distribution. Graham's effusion law. Experimental methods for the determination of the molecular masses of gaseous substances. Real gases, Van der Waals equation.
6. Condensed states
The Liquid state
Intramolecular and intermolecular interactions. Intermolecular interactions of an electrostatic nature. Enthalpy of vaporization and its dependencies. Hydrogen bond. Phase's equilibria. Vapour pressure. Phase transitions and related enthalpies. Clausius-Clapeyron equation. One component phase diagram. Water Phase diagram of water.
The Solid state
Crystalline lattices and elementary cells. Molecular, ionic, covalent and metallic solids. Polymorphism and allotropy. X-ray diffraction. Definition of solids based on symmetry and intermolecular interactions.
7. Chemical thermodynamics
Definition of thermodynamic system. Status functions. Cyclic and open transformations. Reversible and irreversible transformations. Heat, work and internal energy. First principle of thermodynamics. Enthalpy and Hess's law. Entropy. Second principle of thermodynamics. Spontaneous processes. Free energy. Third principle of thermodynamics. Introduction to the concept of chemical equilibrium.
8. Solutions
Solubility and dissolving processes. Gas solutions in liquids. Enthalpy of dissolution and effect of temperature on solubilization processes. Ideal solutions and real solutions. Raoult's law. Ebullioscopic elevation and cryoscopic lowering. Colligative properties of the ideal solutions and determination of the molecular masses of compounds. Osmosis. Not ideal solutions. Fractional distillation. Azeotropic mixtures. Henry's law. Activity and ionic strength.
9. Chemical equilibrium
Spontaneous processes and thermodynamic equilibrium in chemical reactions. Mass action law. Isoterm and isochoric of van't Hoff. Homogeneous equilibria. The principle of Le Chatelier. Effect of the variation in concentration of a reagent or a product on equilibrium. Effect of variation of volume, pressure and temperature on homogeneous equilibria. Heterogeneous equilibria.
10. Equilibria in Solution
Acid-base equilibria: General definitions (Arrhenius, Broensted-Lowry, Lewis). Strength of acids and bases and equilibrium constants. Molecular structure and properties of acid-base. Water autoionization. The pH and the pOH. PH calculation of acidic, basic and saline solutions. Buffer solutions. Solubility and solubility product of salts.
11. Chemical Kinetics
Reaction rate. Kinetic laws and integrated kinetic laws. Order and molecularity of a reaction. Arrhenius equation. Activation energy. Kinetic mechanism of reactions. Collision theory and theory of activated complex. Catalysis.
12. Electrochemical
Galvanic cells. Electrode and electrode reaction. Standard potential. Thermodynamics of galvanic cells. Nerst equation.
Stoichiometry: Mole. Molecular and minimal formulas. Nomenclature of the main inorganic compounds. Chemical equations and ponderal ratios. Limiting reactive. Law of gases and gaseous species in chemical reactions. Indirect analysis. Solutions and volumetric analysis. Gaseous, homogeneous and heterogeneous chemical balances. Thermochemistry and thermodynamics of reactions. Colligative properties of non-electrolytes and electrolytes solutions. PH calculation of acid, base and salts solutions. Buffer solutions. Solubility and solubility product of salts.
Chimica Organica
13. General properties of organic compounds
Functional groups. Nomenclature. The bond in organic compounds and references to the theory of the molecular orbitals. Structure isomerism and stereoisomers. Chirality: compounds with multiple stereocenters and meso-forms, absolute and relative configuration, nomenclature of chiral compounds, optical activity of stereoisomers. Cis-trans geometric isomers. Conformational isomerism.
14. Reactivity of sp3 carbon compunds
General information on the reactivity of organic compounds. Nucleophilic substitution. Alcohols, ethers and sulfur analogues. Amines and alchil-ammonia salts.
15. Reactivity of sp2 carbon compunds
Alkenes and cycloalkenes. Aromatic compounds. Carbonyl compounds. Carboxylic acids and derivatives.
16. Compounds of significant biological interest
Carbohydrates. Lipids. Amino acids. Nucleotides. Biological polymers: polysaccharides or glycans, peptides and proteins, nucleic acids.
(reference books)
M. Speranza et al., General and inorganic chemistry, Edi-Ermes Editore (2013).
F. Cacace and M. Schiavello, Stoichiometry, Bulzoni Editore (1995).
A. Fiecchi et al. Chimica e propedeutica biochimica, Edi-ermes (2002).
NOTE: The teacher will communicate at the beginning of the course the link to the additional teaching material available to the students.
|
|
Dates of beginning and end of teaching activities
|
From to |
|
Delivery mode
|
Traditional
|
|
Attendance
|
not mandatory
|
|
Evaluation methods
|
Written test
Oral exam
|
|
|
