GENERAL AND INORGANIC CHEMISTRY WITH LAB. I

The course is one of the core training activities of the Degree Course, and allows the student to gain knowledge and understanding on the main concepts of Chemistry.
Educational objectives of the course are:
1) knowing the laws that govern general chemistry and chemical reactions;
2) knowing the chemical nomenclature;
3) developing the ability to solve problems of general chemistry (stoichiometry);
4) favoring and stimulating the use of a logical and deductive reasoning in the resolution of these problems, an approach of fundamental importance to face any problem in the scientific field;
5) developing the ability to expose scientific concepts and reasoning in a formal way, both orally and by writing.

1. Knowledge and understanding
i) to know the chemical nomenclature.
ii) Knowing the main laws and the main concepts of general chemistry.
iii) Knowing the approach methodologies to solve chemical problems.
2. Ability to apply knowledge and understanding
i) Knowing how to write the chemical formula of an inorganic material and/or assign the name to a chemical compound starting from the chemical formula.
ii) Knowing how to use the laws and concepts learned to solve theoretical and practical problems.
3. Judgment skills
i) To be able to evaluate the logical consistency of the results to which the application of the learned laws takes place, both from a theoretical point of view and in the resolution of stoichiometry problems.
4. Communication skills
i) Knowing how to communicate the knowledge learned and the result of their application using an appropriate terminology, both in oral and written.
ii) Knowing how to interact with the teacher and with the classmates in a respectful and constructive way.
5. Learning skills
i) Knowing how to take notes, selecting and collecting information according to their importance and priority.
ii) Knowing how to integrate the concepts and examples collected by the personal notes with the files provided by the teacher and the reference texts.
iii) Knowing how to critically consult the reference texts and the bibliography they contain.

The students should have a basic knowledge of mathematics and algebra (first and second degree equations, logarithms and exponentials).

-The atomic structure of matter. Electron, proton, neutron. Atomic and mass number. Isotopes. The atomic mass unit. Molecular mass. Mole and Avogadro number. Molar mass.
- Chemical reactions. Elements and compounds. Symbols and chemical formulas. Oxidation number. Chemical reactions. Laws of conservation of mass and charge. Balance of reactions. Redox reactions.
-Inorganic chemical nomenclature (IUPAC and traditional nomenclature).
-The atomic nucleus. Stable and radio nuclide. The processes of radioactive decay.
-The electronic structure of atoms. Photoelectric effect. Ondulatory and corpuscular nature of electromagnetic radiation. Schrödinger equation for the H atom. Quantum numbers. Atomic orbitals. Energy levels in polyelectronic atoms. The Pauli exclusion principle and the Hund rule. The electronic configurations of atoms in the ground state (Aufbau principle).
- The periodic classification of the elements. Periodic table. Periods and groups. Periodic properties of the elements. Effective nuclear charge. Atomic and ionic rays. Ionization energy. Electronic affinity. Electronegativity.
- The chemical bond. Bonding energy, length and bonding angle. Ionic and covalent bond. The VB theory. σ and π bonds. Valence state of some elements of the second and third periods. Hybridization: hybrid orbitals. Molecular geometry. Resonance. MO theory. LCAO method: formation of molecular binding orbital boundaries from the combination of atomic orbitals. Binding order. Polarity of the chemical bond. Dipolar moment. Polar and apolar molecules. Ionic character of the bond. Hydrogen bond. Ion-dipole and Van der Waals interactions. London forces.
-The aggregation states of the matter. Solid, liquid and gaseous state. The gas laws: Boyle's law, Gay Lussac's laws and Avogadro's law. The equation of state of ideal gases. Dalton's law for gaseous mixtures. Definition of partial pressure. Real gases. Overview of kinetic gas theory. Average kinetic energy of a gas. Solutions: molarity, molality, molar fraction.
- Principles of thermodynamics. System definition. State variables. The first principle of thermodynamics. Internal energy (E). Enthalpy (H). Exothermic and endothermic reactions. The second principle of thermodynamics. Gibbs free energy (G). Criteria for spontaneity of a reaction.
- Chemical equilibrium. Chemical balance. Kc and Kp homogeneous equilibrium constants in gaseous and heterogeneous phase. The principle of mobile equilibrium or Le Chatelier law. Factors that influence chemical equilibrium.
-Ionic equilibria in aqueous solution. Self-ionization of water. Acid, basic and neutral solutions; pH. Acids and bases and their strength. Strong acids. Weak acids: Ka. Strong bases. Weak bases: Kb. Hydrolysis of salts. Calculation of pH: solutions of a strong acid and strong base; of a weak acid and weak monoprotic base and salts. The neutralization reactions of a strong acid with a strong base. Buffer solutions: Henderson-Hasselbalch equation. Solubility equilibrium. Common ion effect.
- Balance between different phases. Vapor pressure. H2O and CO2 status diagrams. Ideal two-component solutions. Vapor pressure of a solution. Raoult's law. Real solutions, azeotrope. Solubility of gas in liquids: Henry's law. Colligative properties.
-Electrochemistry. Galvanic and electrolytic cells. Batteries. Electromotive force and potential of a semi-element: Nernst equation. Potential reduction standards. Oxidizing/reducing power of redox couples.

- R.Chang, K.Goldsby - Fondamenti di Chimica Generale - McGraw Hill Education - Milano.
- P. Silvestroni - Fondamenti di Chimica - Veschi Roma.
- A. Peloso - Problemi di Chimica Generale - Libreria Cortina Padova.
- Lesson notes
- Lesson slides provided by the teacher.

The assessment of learning takes place through a written test. The test, to be performed in two hours, consists of questions of theory and exercises of stoichiometry. During the exam the use of books, notes, electronic media is not allowed.

Teaching is organized in lectures including problem solving exercises.
In the Ca' Foscari "Moodle" platform, the teaching material projected in the classroom during the lessons and some model exercises for the preparation of the written exam are available.

Italian

STRUCTURE AND CONTENT OF THE COURSE COULD CHANGE AS A RESULT OF THE COVID-19 PANDEMIC.


Accessibility, Disability and Inclusion

Accommodation and support services for students with disabilities and students with specific learning impairments:
Ca’ Foscari abides by Italian Law (Law 17/1999; Law 170/2010) regarding support services and accommodation available to students with disabilities. This includes students with mobility, visual, hearing and other disabilities (Law 17/1999), and specific learning impairments (Law 170/2010). In the case of disability or impairment that requires accommodations (i.e., alternate testing, readers, note takers or interpreters) please contact the Disability and Accessibility Offices in Student Services: disabilita@unive.it.

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This subject deals with topics related to the macro-area "Natural capital and environmental quality" and contributes to the achievement of one or more goals of U. N. Agenda for Sustainable Development