Unit GENERAL CHEMISTRY
- Course
- Biotechnology
- Study-unit Code
- GP004014
- Curriculum
- In all curricula
- Teacher
- Cristiano Zuccaccia
- CFU
- 6
- Course Regulation
- Coorte 2019
- Offered
- 2019/20
- Learning activities
- Base
- Area
- Discipline chimiche
- Academic discipline
- CHIM/03
- Type of study-unit
- Obbligatorio (Required)
- Type of learning activities
- Attività formativa monodisciplinare
GENERAL CHEMISTRY - Canale A
| Code | GP004014 |
|---|---|
| CFU | 6 |
| Teacher | Cristiano Zuccaccia |
| Teachers |
|
| Hours |
|
| Learning activities | Base |
| Area | Discipline chimiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | Atomic theory of matter. Mole and Avogadro number. Chemical formulas and chemical equations. Electronic structure of atoms. Periodic properties. Chemical bond. Chemical reactions. States of matter: gases, liquids and solids. Introduction to thermodynamics. Nature and properties of solutions. Physical and chemical equilibria.Equlibria in solution and acid-base equilibria. |
| Reference texts | University level textbooks recommended by the teacher. |
| Educational objectives | The course aims at providing students with the general knowledge of the fundamental principles of general and inorganic chemical chemistry with the final goal of deliver the basic understanding of more complex systems and processes at the molecular level, including biological and biochemical processes. The topics will be addressed so that the student, by deepening the scientific method, can tackle chemical problems and apply the acquired knowledge and understanding to synthetic procedures and analytical methodologies characteristic of chemical disciplines. Numerical exercises relevant to the topics discussed during lessons will offer the student the opportunity to evaluate and verify the acquired knowledge. |
| Prerequisites | Basic knowledge of mathematics. Equivalence relation; linear and quadratic equations; etc. |
| Teaching methods | - lectures; - classroom numerical exercises; - virtual lab - lab. |
| Other information | Two written test and the two oral examination sessions will be scheduled for each examination periods. Students are required to enroll in the written test following the procedures of the University. In case of problems and difficulties students are encouraged to contact teachers. In case of positive result of the written examination, the student can take the oral exam in the same call, or may decide to postpone the oral examination to one of the subsequent sessions (up to the beginning of the next academic year). |
| Learning verification modality | The final evaluation consists of a written test (mandatory) and an oral exam (mandatory). The written test consists of a total of 10 questions, divided as follows: 5 questions (10 points) and 5 problems of stoichiometry (20 points). The positive result of this test allows access to the oral exam. The grade is valid until the beginning of the next academic year. The oral exam consists of an interview with the student. |
| Extended program | Atomic theory of matter: History of atomic theory. Fundamental laws. Fundamental particles of the atom. Atomic number, mass number. Isotopes. Atomic weights and atomic mass units. The concept of mole. Avogadro's number. Chemical formulas and chemical equations. ¿Electronic structure of atoms: Bohr's atomic model. Uncertainty principle. Quantum mechanics and wave. Description of atomic orbitals. Pauli exclusion principle. Periodic table of elements. Periodic properties. Ionization energies. Electron affinity. ¿Chemical Bonding: Ionic bond, covalent and metallic. Theory of valence bond and molecular orbital. Binding energy. Number of oxidation and chemical reactions. Acid-base reactions, exchange, oxidation-reduction. The bond in coordination compounds. ¿Gaseous state: ideal gas equation of state. Meaning of the constant R and temperature. Kinetic theory of gases. Real gases. Equation of van der Waals forces. ¿Liquid state: Properties General. Changes of state. ¿Solid state: Types of solids and their properties. Ionic crystals, covalent, molecular and metallic. ¿Thermodynamics: overview. State functions, internal energy, enthalpy, entropy, Gibbs energy liner. 1 st and 2 nd law of thermodynamics. ¿Solutions: The nature of the solutions. Colligative properties of solutions. ¿Chemical equilibria: homogeneous and heterogeneous equilibria. Equilibrium constant. Of laws? Balance. Equilibria in solution. Acid-base equilibria. Strength of acids and bases. Ionic product of water. PH and pH Determination of POH. Buffer solutions. Acid-base titration. Indicators. |
GENERAL CHEMISTRY - Canale B
| Code | GP004014 |
|---|---|
| CFU | 6 |
| Teacher | Cristiano Zuccaccia |
| Teachers |
|
| Hours |
|
| Learning activities | Base |
| Area | Discipline chimiche |
| Academic discipline | CHIM/03 |
| Type of study-unit | Obbligatorio (Required) |
| Language of instruction | Italian |
| Contents | Atomic theory of matter. Mole and Avogadro number. Chemical formulas and chemical equations. Electronic structure of atoms. Periodic properties. Chemical bond. Chemical reactions. States of matter: gases, liquids and solids. Introduction to thermodynamics. Nature and properties of solutions. Physical and chemical equilibria.Equlibria in solution and acid-base equilibria. |
| Reference texts | University level textbooks recommended by the teacher. |
| Educational objectives | The course aims at providing students with the general knowledge of the fundamental principles of general and inorganic chemical chemistry with the final goal of deliver the basic understanding of more complex systems and processes at the molecular level, including biological and biochemical processes. The topics will be addressed so that the student, by deepening the scientific method, can tackle chemical problems and apply the acquired knowledge and understanding to synthetic procedures and analytical methodologies characteristic of chemical disciplines. Numerical exercises relevant to the topics discussed during lessons will offer the student the opportunity to evaluate and verify the acquired knowledge. |
| Prerequisites | Basic knowledge of mathematics. Equivalence relation; linear and quadratic equations; etc. |
| Teaching methods | - lectures; - classroom numerical exercises; - virtual lab - lab. |
| Other information | Two written test and the two oral examination sessions will be scheduled for each examination periods. Students are required to enroll in the written test following the procedures of the University. In case of problems and difficulties students are encouraged to contact teachers. In case of positive result of the written examination, the student can take the oral exam in the same call, or may decide to postpone the oral examination to one of the subsequent sessions (up to the beginning of the next academic year). |
| Learning verification modality | The final evaluation consists of a written test (mandatory) and an oral exam (mandatory). The written test consists of a total of 10 questions, divided as follows: 5 questions (10 points) and 5 problems of stoichiometry (20 points). The positive result of this test allows access to the oral exam. The grade is valid until the beginning of the next academic year. The oral exam consists of an interview with the student. |
| Extended program | Atomic theory of matter: History of atomic theory. Fundamental laws. Fundamental particles of the atom. Atomic number, mass number. Isotopes. Atomic weights and atomic mass units. The concept of mole. Avogadro's number. Chemical formulas and chemical equations. ¿Electronic structure of atoms: Bohr's atomic model. Uncertainty principle. Quantum mechanics and wave. Description of atomic orbitals. Pauli exclusion principle. Periodic table of elements. Periodic properties. Ionization energies. Electron affinity. ¿Chemical Bonding: Ionic bond, covalent and metallic. Theory of valence bond and molecular orbital. Binding energy. Number of oxidation and chemical reactions. Acid-base reactions, exchange, oxidation-reduction. The bond in coordination compounds. ¿Gaseous state: ideal gas equation of state. Meaning of the constant R and temperature. Kinetic theory of gases. Real gases. Equation of van der Waals forces. ¿Liquid state: Properties General. Changes of state. ¿Solid state: Types of solids and their properties. Ionic crystals, covalent, molecular and metallic. ¿Thermodynamics: overview. State functions, internal energy, enthalpy, entropy, Gibbs energy liner. 1 st and 2 nd law of thermodynamics. ¿Solutions: The nature of the solutions. Colligative properties of solutions. ¿Chemical equilibria: homogeneous and heterogeneous equilibria. Equilibrium constant. Of laws? Balance. Equilibria in solution. Acid-base equilibria. Strength of acids and bases. Ionic product of water. PH and pH Determination of POH. Buffer solutions. Acid-base titration. Indicators. |