The atoms. The mole. Electronic structure of atoms. The periodic table. Ionic bond. Covalent bond. Chemical formulas. Other chemical bonds. Ideal gas law. Change of state. Enthalpy, entropy and free energy. Spontaneity of reactions. The solutions. Chemical equilibrium. Redox reactions. Reduction potentials. Acid-base equilibria (pH, buffer solutions). Solubility product
I. Bertini, C. Luchinat, F. Mani, Chimica, editrice Ambrosiana
I. Bertini, F. Mani, Stechiometria, editrice Ambrosiana.
The course introduces the fundamental elements of the General Chemistry, which constitute the basic knowledge needed for the following courses of the Laurea degree. The concepts introduced in the course of General Chemistry are a requirement for the courses of Organic Chemistry, Enological Chemistry, Agricultural Biochemistry, Fermentation Biotechnology. The aim of the course is to introduce the student to basic principles of chemistry, providing information on the language of chemistry (symbols and formulas). The course aims at providing to the students the capability to understand the basic language of the chemistry, to be able to follow concepts requiring the basic knowledge of general chemistry, and to be able to solve elementary problems through the application of the introduced concepts.
Lectures and practicals on the topics covered by the program.
Total hours of the course: 150
Hours reserved to private study and other individual formative activities: 102
Contact hours for: Lectures (hours): 30
Contact hours for: practice (hours): 18
Frequency of lectures and practice, although non compulsory, is strongly recommended
Type of Assessment
Written tests and final oral examination
Atoms. Atomic mass, mole concept. Nomenclature of inorganic chemistry. Electronic structure of elements (orbitals, quantum number, aufbau, periodic properties). The periodic table. Covalent bond, Lewis structures. Bonding in solid state (ionic , molecular and covalent solids, metal). Hydrogen bond, van der Waals forces. Oxidation number. Gaseous state, ideal gas equation. Phase diagrams of one-component systems. Enthalpy, entropy, free energy, spontaneity of a chemical reaction. Concept of dynamic equilibrium. Redox reactions in aqueous solutions-electrochemical cells. Oxidation-reduction reactions. Acid-base reactions. Constants for acids and bases; pK; pH; buffers. Solubility product constants. Main properties of elements. Stoichiometry. Unit systems. Molecular structures. Determination of state variables from the ideal gas equation. Balancing of equations, redox reactions. Equilibrium in solution, calculation of pH.