GENERAL AND INORGANIC CHEMISTRY WITH LAB. I

This is a basic level course of the Bachelor degree in Technologies for the Conservation and the Restoration and its aim is to give the main concepts of General Chemistry and Stoichiometry that will be fundamental for the successive Chemistry courses
The formative objectives of this part of the course are: 1) to introduce to knowledge of chemical bonding, the main theories developed to describe it and its important involvements with the properties of the matter; 2) to develop the concept of chemical equilibrium and prove its importance for understanding chemical reactions; 3) to supply tools for describing acid-base equilibria, solubility and precipitation equilibria and electrochemical systems; 4) tohelp students to solve problems of stoichiometry that have to be regarded as applications of the theoretical part of the course

1. Knowledge and comprehension:
A) To know the main theories regarding the chemical bonding and the relationship between chemical bonding and the electronic structures of the involving elements.
B) To know the main features of acid-base equilibria, solubility and precipitation equilibria and electrochemical systems.

2. Ability to apply knowledge and comprehension:
A) To be able to utilize the different theories on chemical bonding to explain the manifold properties of the matter.
B) To use the concept of chemical equilibrium to predict the results of exchange and redox reactions;
C) To be able to solve stoichiometric problems regarding the chemical equilibrium

3. Ability of judgment:
A) To be able to assess consistence of the results obtained with the application of chemistry laws both in theoretical field and analysis of experimental results.
B) To be able to recognize possible errors by a critical analysis of the applied procedure

4. Ability of exposition:
A) To be able to communicate acquired knowledge and the results of its application utilizing an appropriate terminology both orally and in written form.
B) To be able to interact with the docent and other students during the lesson.

5. Ability of learning:
A) To be able to take notes, selecting information in order of importance and priority
B) To be sufficiently autonomous in the resolution of stoichiometric problems.

Being the first course of Chemistry of the Bachelor degree, no particular pre-requirements are required

The contents of the course can be divided in two main sections:
First section - Formative objectives: (1) Expected results of learning 1A, 2A, 3A,3B 4A, 4B, 5A, 5B).

- Chemical bonding: an introduction to the problem.
Atomic properties and chemical bonding; Electron pair bonds and Lewis representation of the molecules.
- Ionic bonding
A model for ionic bonding. Born-Haber cycle. Reticular energy. Periodic properties and reticular energy. Model of ionic bonding and properties of ionic compounds.
- Covalent bonding
A model for covalent bonding. Properties of covalent bonding. The model of covalent bonding and properties of covalent compounds. The concept of electronegativity.
- Metallic bonding
Models and properties of the metallic bonding. Properties of metallic crystals
- Molecular structures and shapes
Lewis diagrams for molecules. The octet rule; Electronic delocalization and the concept of resonance. Breakdown of the octet rule (odd-electron molecules; octet deficient molecules; valence shell expansion). Valence Shell Electron Pair Repulsion theory. The concept of electronic group. Geometry of electronic group and molecular shape. Molecular shapes, bond angles bond lengths and molecular polarity.
- Theory of covalent bonding
Valence Bond theory. The concept of hybrid orbital. Orbital hybridization and molecular shape. Single and multiple bond.
- Molecular orbital theory
Energy and shape of molecular orbitals. Description of thr Hydrogen molecule and of other bi-atomic molecules. Polarity and Molecular Orbital theory.
- The intermolecular forces
Phase-samples of matter and intermolecular forces. Ion-ion forces, dipole-dipole forces, ion-dipole forces, charge-induced dipole forces. The concept of polarizability. London dispersion forces. Hydrogen bonds.

Second section - Formative objectives: 2), 3), 4). 1) Expected results of learning: 1B, 2B, 3A, 4A, 4B, 5A, 5B).

- Chemical Equilibrium
An experimental approach to the problem of chemical equilibrium. Law of mass action and the equilibrium constants. Correlation between Kc and Kp. Le Chatelier priciple.
The kinetic approach to chemical equilibrium. The thermodynamic approach to chemical equilibrium. Spontaneous processes and chemical equilibrium. Free energy of Gibbs of reaction and its correlation with equilibrium constant. Resolutions of different typology of problems involving chemical equilibrium.
- Acid-base equilibria
Arrhenius acids and bases. Bronsted-Lowry acids and bases. Lewis acids and bases. Properties of acids and bases in aqueous solution. Autoionization of water and pH function. Acid and bases strength and week. Acid and base dissociation constant. Equilibria involving weak acids and weak bases. Hydrolysis. Calculation of buffer action. Acid-base indicators. Resolutions of different typology of problems involving acid-base equilibrium.
- Solubility and precipitation equilibria.
Strong and weak electrolytes. General features of solubility equilibria. Solubility and solubility product. The common-ion effect. The effect of pH on solubility. Complex ion and solubility. Resolutions of different typology of problems involving solubility and precipitation equilibria.
- Electrochemistry
Galvanic Cells. Preparation, mode of operation and schematic representation of galvanic cell. Nernst equation. Standard reduction potentials. Cell potentials and Gibbs free energy. Resolutions of different typology of problems involving galvanic cells. Electrolytic cells.

In addition to the lectures notes the following textbooks are recommended:
Petrucci,Harwood and Herring "Chimica Generale" Piccin Editore PadovaKotz and Treichel "Chimica" Edizioni EdiSES Napoli;
Kotz and Treichel "Chimica" Edizioni EdiSES Napoli;
Silberberg "Chimica: La natura molecolare della materia e delle sue trasformazioni" Mc Graw Hill Editore
Bandoli, Nicolini e Uguagliati, "Stechiometria con Complementi di Chimica" Edizioni Progetto Padova

For this module of the course the method for evaluating the learning ability includes an oral and a written exam. The final grade of these two proves will make average with the grade obtained by the student in the other module. The written exam consists in a series of numerical and not numerical exercises that have to be solved justifying the methods utilized for the solution. In this exam the student has to applied the concepts learned during the lessons with critical judgment. The time span for the written examination is two hours. During this prove the student can utilize only a scientific calculator and the periodic table. The written exam can be substituted by two intermediate written examinations at the half and at the end of the course.
The oral examination consists in a series of questions regarding the part of the program reported in the section “ Contents”. The student will be able to show both the learning of the program subjects and the ability to expose them in formal manner.

Frontal lesson with support of slides and exercitations with solution of numerical problems.
The slides will be provide to students in electronic format

Italian

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.

written and oral

This subject deals with topics related to the macro-area "Climate change and energy" and contributes to the achievement of one or more goals of U. N. Agenda for Sustainable Development