General Chemistry with Elements of Physical Chemistry

GOALS
The course is preparatory to the following chemistry courses: Chimica organica e laboratorio di chimica and Chimica biologica. Its purpose is to provide the minimum tools necessary to understand the chemical language and the basic topics (atoms, chemical bonds, chemical reactions, chemical equilibrium, thermodynamics and electrochemistry) essential for the study of biology.

PROGRAM
Atomic structure: Nuclides, isotopes and chemical elements. Molecular formula and formula unit. Unit of mass, atomic mass and molecular mass. Mole and Avogadro number. Quantization of energy and photons. Atomic models. Orbitals and quantum numbers. Electronic configuration of the elements. Periodic table of elements and periodic properties.
Chemical bond and molecular geometry: Lewis structures. Ionic and covalent bonds. Electronegativity. Bond polarity. Molecular geometry: VSEPR and valence bond theory. Intermolecular interactions.
Formulas and systematic nomenclature.
Solutions: Concentration. Dilution. Molar fraction. Colligative properties.
Chemical reactions: Chemical reactions and chemical equations. Balance. Principle of mass conservation. Net ionic equation and principle of charge conservation. Balance 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.
Gaseous state: Pressure and temperature. Ideal gas law. Molar volume. Ideal gas constant. Gaseous mixtures: partial pressure and partial volume, Dalton's law.
Acids and bases: Definitions of acid and base. Acid-base equilibria. Calculation of pH. Buffer solutions. Titration curves.
Chemical thermodynamics: State functions. First principle of thermodynamics. Enthalpy. Exothermic and endothermic reactions. Standard conditions. Second principle of thermodynamics. Entropy. Gibbs free energy.
Electrochemistry: Electrochemical cells and standard potentials. Cell potential and equilibrium constant. Nernst's equation.

REFERENCE MATERIAL
Raymond Chang, Kenneth Goldsby "Fondamenti di chimica generale (2a edizione)" McGraw-Hill, 2015.
Raymond Chang, Kenneth Goldsby "General chemistry. The essential concepts (7th edition)" McGraw-Hill, 2014.

PREREQUISITES AND EXAMINATION PROCEDURES
Examination consists of a written test including open questions and exercises similar to those presented in class and taken from the adopted textbook.

TEACHING METHODS
Teaching Methods: Traditional
Attendance: Recommended

LANGUAGE OF INSTRUCTION
Italian

RECOMMENDED PREREQUISITES
None

Electrons in Atoms:
Atomic particles and their properties. Chemical Elements. Atomic Weights, Formula Weights and Molecular Weights. The Avogadro Constant and the concept of the Mole. Quantum Theory. The Bohr Atom. The Uncertainty Principle. Quantum Numbers and Electron Orbitals. Electron Spin. Multielectron Atoms. Electron Configurations of the Elements.
The Periodic Law and the Periodic Table. Electron Configuration and the Periodic Table. Periodic properties: Metals and Nonmetals, Atomic Radius, Ionization Energy, Electron Affinity.

Chemical Bonding:
Lewis theory. Ionic and Covalent Bonding. Electronegativity. Lewis Structures. Resonance. Exceptions to the Octet Rule. VSEPR Theory and Molecular Shapes. Introduction to the Valence Bond Theory. Hybridization of Atomic Orbitals. Intermolecular forces.

Formulas and systematic nomenclature:
Oxidations States. Systematic Nomenclature of Inorganic Compounds.

Solutions:
Solution Concentration. Solution Dilution. Vapor Pressures of Solutions. Freezing Point. Depression and Boiling Point Elevation.

Chemical Reactions:
Chemical reactions and the Chemical Equation. Balancing. Determining the Limiting Reagent. Chemical Equilibrium. The Equilibrium Constant Expression. The reaction Quotient. Le Chatelier's Principle. Reactions in aqueous solutions: electrolytes and nonelectrolytes, Precipitation Reactions, Acid-Base Reactions, Oxidation-Reduction Reactions.

Gases:
The concept of Pressure and absolute Temperature. The Gas Laws: Boyle's law, Charles's Law and Avogadro's Law The Ideal Gas Equation. Mixtures of gases: partial pressure and partial volume. Dalton's Law and Amagat's Law. Real gas.

Acids and Bases:
Arrhenius Theory. Bronsted-Lowry Theory. Strong Acids and Strong Bases. Self-ionization of water. Definition of pH and pOH. Weak Acids and Weak Bases. Polyprotic Acids. Hydrolysis. Buffer Solutions. Neutralization reactions and Titration Curves.

Thermochemistry:
Functions of State. The First Law of Thermodynamics. Enthalpy. Entropy. The Second Law of Thermodynamics. Standard Free Energy Change. Free Energy Change and Equilibrium.

Electrochemistry:
Electrochemical cells, electromotive force, standard reduction potentials, electrolysis.


Recommended Book:
Petrucci; Herring; Madura; Bissonnette CHIMICA GENERALE PRINCIPI ED APPLICAZIONI MODERNE, Editore: Piccin
J. Kotz John, P. Treichel jr., G.C. Weaver, CHIMICA, Editore: Edises
Exercise book:
A. Caselli, S. Rizzato, F. Tessore "Stechiometria dal testo di M. Freni e A. Sacco" Editore: Eises


Teaching Mode:
Traditional Lectures. Iinteractive presentations partially supported by projected lecture slides. Attendance is highly recommended. Copies of the lecture slides, including the homework problems, will be made available on the Ariel web site.


Examination procedures:
Examination consists of two parts: a test (multiple-choice quiz) followed by a written examination. Test must be passed before taking the written exam. The written part of the exam involves two sections: Part A (stoichiometric problems; the exercises are of the same type as the ones solved in class and taken from the course book) and Part B: (open questions small exercises of general chemistry). In order to pass the exam, it is needed to obtain the sufficiency (18 over 30) in both parts.


Language of instruction:
Italian


WEB Page:
http://ariel.unimi.it