Chemistry

GENERAL CHEMISTRY

The General Chemistry teaching unit aims to provide students with the general basics of chemistry through the study of the nature of the elements and their compounds, the examination of the chemical reactions and the parameters associated with them. Starting from the atomic structure of matter, the course introduces the fundamental laws of stoichiometry also illustrated through exercises.
The course will allow the student to acquire the basic notions of chemistry necessary to understand processes, even complex, more specific than the degree course.


Atoms and atomic structure:
Nuclides, isotopes and chemical elements. Molecular formula and formula units. Unit of mass, atomic mass and molecular mass. Mole and Avogadro Number. Quantization of energy and photons. Emission spectrum of the hydrogen atom. Rutherford and Bohr's atomic models. Heisenberg's uncertainty principle. Charge density and probability. Orbitals and quantum numbers. Hybridization of carbon (sp, sp2 and sp3 hybrid orbitals). Diagram of energy levels and electronic configuration of the elements. Construction of the periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Oxidation numbers. Chemical formulas. Systematic nomenclature. Lewis symbols and structures. The ionic and the covalent bond. Electronegativity. Percentage of ionicity and polarity of bonds. Molecular geometry: VSEPR Theory and Valence Bond Theory. Intermolecular interactions.
Gases and their laws: pressure and absolute temperature. Ideal gases: Boyle's, Charles's, Gay-Lussac's and Avogadro's laws. Molar volume. Gas equation of state. Gaseous mixtures: definition of partial pressure and partial volume, Dalton's law and Amagat's law. Real gases.
Liquids and solutions: Concentration: percentage by weight, by volume, molarity and molality. Dilution. Mole fraction. The concept of equivalent. Equivalence number. Normality. Equivalent weight. Colligative properties: Vapor pressure, Raoult's law, boiling point elevation, freezing point depression and osmotic pressure.
Solids: amorphous and crystalline. Crystals: covalent, ionic and molecular. Elementary cells: types of packing and cubic cell. Metallic bond and band theory. Conductors, semiconductors and insulators. Allotropes of carbon and phosphorus.
Chemical reactions: Balancing. The principle of conservation of mass. Net ionic equation and charge conservation principle. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier's Principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions. Acids and Bases: Definition of acid and base (Arrhenius, Bronsted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Introductio to thermodynamics: State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. The second law of thermodynamics. Entropy. Gibbs free energy.


ORGANIC CHEMISTRY
For each functional groups we will discuss structures and reactivity. The programme is:
- Structure and properties or organic molecules
- Polarity
- Alcanes
- Alkyl halides: nucleophilic substitution reactions. Carbocations
- Alkenes: addition reactions
- Alkynes
- Alcohols and ethers
- Aldehydes and ketones
- Carboxylic acids and their derivatives
- Aromatic compounds
- Amines
- Carbohydrates
- Amino acids and proteins
- Nucleic acids
- Hints about organic chemical compounds of natural origin and their biological activity

General Chemistry teaching unit
The General Chemistry teaching unit aims to provide students with the general basics of chemistry through the study of the nature of the elements and their compounds, the examination of the chemical reactions and the parameters associated with them. Starting from the atomic structure of matter, the course introduces the fundamental laws of stoichiometry also illustrated through exercises.
The course will allow the student to acquire the basic notions of chemistry necessary to understand processes, even complex, more specific than the degree course.

Atoms and atomic structure:
Nuclides, isotopes and chemical elements. Molecular formula and formula units. Unit of mass, atomic mass and molecular mass. Mole and Avogadro Number. Quantization of energy and photons. Emission spectrum of the hydrogen atom. Rutherford and Bohr's atomic models. Heisenberg's uncertainty principle. Charge density and probability. Orbitals and quantum numbers. Hybridization of carbon (sp, sp2 and sp3 hybrid orbitals). Diagram of energy levels and electronic configuration of the elements. Construction of the periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Oxidation numbers. Chemical formulas. Systematic nomenclature. Lewis symbols and structures. The ionic and the covalent bond. Electronegativity. Percentage of ionicity and polarity of bonds. Molecular geometry: VSEPR Theory and Valence Bond Theory. Intermolecular interactions.
Gases and their laws: pressure and absolute temperature. Ideal gases: Boyle's, Charles's, Gay-Lussac's and Avogadro's laws. Molar volume. Gas equation of state. Gaseous mixtures: definition of partial pressure and partial volume, Dalton's law and Amagat's law. Real gases.
Liquids and solutions: Concentration: percentage by weight, by volume, molarity and molality. Dilution. Mole fraction. The concept of equivalent. Equivalence number. Normality. Equivalent weight. Colligative properties: Vapor pressure, Raoult's law, boiling point elevation, freezing point depression and osmotic pressure.
Solids: amorphous and crystalline. Crystals: covalent, ionic and molecular. Elementary cells: types of packing and cubic cell. Metallic bond and band theory. Conductors, semiconductors and insulators. Allotropes of carbon and phosphorus.
Chemical reactions: Balancing. The principle of conservation of mass. Net ionic equation and charge conservation principle. Equilibrium reactions: equilibrium constant and reaction quotient. Le Chatelier's Principle. Reactions in aqueous solution: electrolytes and non-electrolytes, precipitation reactions and solubility equilibria, acid-base reactions, oxidation-reduction reactions. Acids and Bases: Definition of acid and base (Arrhenius, Bronsted-Lowry and Lewis). Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Introductio to thermodynamics: State functions. First law of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. The second law of thermodynamics. Entropy. Gibbs free energy.


Organic Chemistry teaching unit
- Structure and properties or organic molecules
- Polarity
- Alcanes
- Alkyl halides: nucleophilic substitution reactions
Carbocations
- Alkenes: addition reactions
- Alkynes
- Alcohols and ethers
- Aldehydes and ketones
- Carboxylic acids and their derivatives
- Aromatic compounds
- Amines
- Carbohydrates
- Amino acids and proteins
- Nucleic acids
- Hints about organic chemical compounds of natural origin and their biological activity
- Application of basic concepts of organic chemistry to understanding of biochemistry topics.