65931 - Inorganic and General Chemistry

Learning outcomes

The objective of the course is to provide the essential notions relative to the structure and properties of the elements and inorganic chemical compounds. At the same time, the course is intended to give the necessary information for a critical analysis on the following topics:
- the composition of the material objects in the surrounding world;
- the dependence of the macroscopic properties of substances on their microscopic composition and structure;
- the ability of substances to combine together, or to decompose, giving rise to other substances.
At the end of the module, the student possesses a basic chemical culture and is capable of undertaking the study of the successive specialized parts of chemistry

Course contents

Chemical classification of matter
Composition of atoms, atomic symbols, atomic number and mass number, isotopes, ions; elements and compounds; periodic table and periodic behaviour of physical quantities.

Mole, concentration, chemical equations
Atomic mass, mole, molarity and other means of reporting concentration in solution, dilution, chemical reactions, chemical equations and their balancing.

Atomic structure
Wave-particle dualism and quantum-mechanical model of atom; orbital shells and sub-shells, quantum numbers and their meaning, Hund rule and Pauli principle, electronic configurations; dimensions of atoms and ions, ionization energy, and interpretation of their periodic behaviour.

The chemical bond
Valence electrons, covalent bond, Lewis structures, bond length and energy, electronegativity, partial and formal charge; shape of orbitals, shape of molecules, polarity; valence bond theory, hybrid atomic orbitals, double and triple bond; molecular orbitals theory; ionic bond, metallic bond (brief mention); oxidation numbers.

The gas state
Temperature as a property of matter, the states of matter; properties of gases, ideal gas law, Dalton law on partial pressures; molecular kinetics theory; deviations from the ideal behaviour.

Energy exchanges associated to the making and breaking of chemical bonds
Heat and energy; first principle of thermodynamics, state functions, enthalpy of reaction, standard states, Hess law, enthalpy of formation.

Liquids and solutions
Structure of liquids, intermolecular forces; kinetics theory of liquids, vapour tension, melting and boiling points; colligative properties, osmotic pressure, solubility.

The solid state
Brief mention to the solid state and the physical properties of solids.

Introduction to the chemical equilibrium
Complete and incomplete reactions, reaction rate, collision theory for reactions in the gas phase; expression of the equilibrium constant, reaction quotient, effect of temperature, Le Châtelier principle; calculation of the equilibrium constant.

Chemical thermodynamics
Spontaneous processes, entropy and its meaning, second and third principles of thermodynamics; standard entropy, Gibbs free energy, standard free energy; relationship between free energy and equilibrium constant, temperature dependence of the equilibrium constant.

Acids and bases
Properties of acids and bases, Brønsted-Lowry definition, acid-base conjugated pairs; dissociation of water, pH, strength of acids and bases; pH calculations for strong and weak acids and bases, anphoteric compounds, salts and pH of their solutions; buffer solutions and buffering ability, titration curves, indicators.

Redox reactions
Identification, stoichiometry, and balancing of redox reactions; oxidizing and reducing agents; voltaic cells, standard potentials, batteries, electrolytic cells, Faraday law, electrochemical cells in non-standard conditions, Nernst equation.

Chemical kinetics
Reaction rate, instantaneous rate, kinetic law and rate constant; relationship between kinetic law and reaction stoichiometry, order and molecularity; zero-, first- and second-order reactions; integrated form of first- and second-order kinetic laws; activation energy and its determination; catalysis.

Overview on the chemical properties of the principal elements
The periodic table and the periodic chemical characteristics; compounds of the elements with oxygen and hydrogen; brief mention to the properties of the main elements belonging to the s and p blocks (groups 1 through 3 and 14 through 18).

Readings/Bibliography

The topics dealt with in this course, which are fundamental for a first-level university grade, can all be found in any university textbook of general chemistry. For example, see:
A. M. Manotti Lanfredi, A. Tiripicchio, Fondamenti di Chimica, C.E.A, Milano, 2002.
I. Bertini, C. Luchinat, F. Mani, Chimica, C.E.A., Milano, 2004.
L. Moggi, M. Venturi, Chimica Generale ed Inorganica (2° ed.), Corso Ed., Ferrara, 2002.

Further reading:
M. Munowitz, Chimica, Zanichelli, Bologna, 2003
J.C. Kotz, P.M. Treichel, J.R. Townsend, Chimica-IV Ed., Edises, Napoli, 2010
P. Atkins, L. Jones, Chimica Generale, Zanichelli, Bologna, 1998

Teaching methods

The course is composed mainly of classroom lectures with the use of transparencies. Problem solving activities are also carried out. Subjects of high impact (e.g., under an applicative point of view), related to the topics treated in the course, are presented if time is available.

Assessment methods

The learning assessment takes place with the final exam. The acquisition of the learning outcomes is ascertained by means of a written test of 2 hours, to be undertaken without the support of notes or textbooks, followed by an oral exam.

The written test consists of 3 numerical problems, each related to a different topic of the program (atomic weight and mole, reaction stoichiometry, colligative properties, chemical equilibrium in the gas phase, acid-base solution equilibria, hydrolysis, buffer solutions, acid-base titrations, solubility equilibria, galvanic cells, chemical kinetics). A score comprised between 0 and 11 is assigned to each problem; the mark of the written test is calculated as the sum of the score obtained in the three problems.

A score of at least 18 in the written test is required to be admitted to the oral exam. Such an admission is valid for one solar year since the date of the positively evaluated written test; during this period the student can take the oral exam in any available session.

The oral exam has an average duration of 20 minutes and consists of 2 questions on the various topics of the course. If the oral exam is failed the written test does not have to be repeated; the student can try the oral exam again in a later session, within the term of validity of the written test. The final mark of the module is mainly determined from the outcome of the oral exam, taking into account, however, the score assigned to the written test.

The mark of the integrated course is calculated as the arithmetic mean of the marks obtained in the module of General and Inorganic Chemistry and in that of Organic Chemistry.

Teaching tools

The lecture slides are available on the internet (UniBo web site > Alberto Credi > Courses > General and Inorganic Chemistry > Teaching material). Numerical problems and exercises, some with solution, are available in the same site for training to the written test.

Links to further information

http://www.photonanolab.it

Office hours

See the website of Alberto Credi