00130 - General Inorganic Chemistry

Learning outcomes

The General Chemistry course provides the basic knowledge required to study most of the other subjects of the degree. It deals with nature and atomic structure of chemical species as well as with their general properties, mainly in relation to the ability to undergo transformations into other species (chemical reactions). It also debates the general features of the reactions (stoichiometry, spontaneity, completeness, rate) and the main parameters which affect these properties. In this context, reference is commonly made to reactions in solution, acid-base and redox reactions in particular, because of their importance in many fields which will be studied in subsequent courses.

Course contents

1) Heterogeneous mixtures; homogeneous mixtures (solutions); chemical species: elements and compounds.

2) Atomic composition; atomic and mass numbers. Isotopes and atomic weight. Bohr's atomic theory; energy quantization. Quantum theory for H; orbitals and quantum numbers n, l and m. Spin. Orbitals in polyelectronic atoms, electronic configurations of elements. Periodic Table and relation with electronic configuration. Ionization energy, electron affinity, atomic and ionic radii.

3) Chemical bond: general concepts. Covalent bonds as sharing of electron pairs: number of bonds, molecules and infinite networks; electronegativity and bond polarity; bond energy and distance. Covalent bond and electronic configuration: electron promotion. Lewis structures of polyatomic molecules and ions. Dative bond: electron acceptors and donors. Molecular geometry. Ibridization. MO theory: sigma and pai orbitals; application to biatomic and polyatomic molecules. MO theory for infinite networks: band theory. Resonance.

4) Ionic bond: lattice energy. Stoichiometry and geometry of ionic compounds. Metallic bond: electrical conductivity; semiconductors. Intermolecular forces: Van der Waals, London and hydrogen bond. Nature of bond and position in the Periodic Table: metals and non-metals.

5) Empirical and molecular formula. Isomerism, polymorphism and allotropism. Molecular and formula weight. Mole and NA, molar mass. Determination of chemical formula.

6) Valence, oxidation state, coordination number. Binary compounds of oxygen. Classification and nomenclature of oxides and their derivatives. Binary conpound of hydrogen. Other binary compounds. Salts. Coordination and organometallic compounds.

7) Solid, liquid and gaseous states: general properties. Equation of state for gases. Gas mixtures: partial pressure. Changes of state and phase diagrams.

8) General properties of solutions. Concentration. Solubility. Solutions of electrolites. Ideal, diluted or concentrated solutions. Changes of state in liquid solutions. Osmosis. Colligative properties and determination of molecular weight. Colloidal systems; lyophilic and lyophobic colloids. Amphiphilic species: micelles and bilayers.

9) Chemical reactions and equations; mass conservation law. Equation balancing. Redox reactions and their balancing. Reactions in solution and ionic equations; redox half-reactions. Mass relation in the reactions; equivalent weight.

10) Thermochemistry: internal energy and enthalpy of reaction. Hess's law; enthalpy of formation. Spontaneity of reactions: entropy and free energy. Change of G during a reaction: reversible and irreversible reactions. Free energy and useful work.

11) Rate of reaction, kinetic equation. Reaction mechanism. Activated complex and activation energy. Catalysis. Chain reactions.

12) Chemical equilibrium: Kc and Kp. Dependence of K on T. Homogeneous and heterogeneous equilibria. Le Chatelier's  principle. Solubility and Kps. Simultaneous equilibria. Stoichiometric calculations on equilibria.

13) Protonic theory of acid and bases. Autoionization; Kw. Ka and Kb. Polyprotic acids and bases. Molecular structure and acid/base properties. Acidity of solutions: pH. Acid-base reactions. Buffers. pH and solubility.

14) Galvanic cells. Reduction potentials and cell e.m.f. Electrolysis.

15) Position in the Periodic Table, electronic configuration, main oxidation states, acid/base and redox properties of: H, Li, Na, K, Be, Mg, Ca, Ba, B, Al, C, Si, Sn, Pb, N, P, As, Sb, Bi, O, S, F, Cl, Br, I, Cr, Mn, Fe, Co, Ni, Cu, Zn, Ag, Hg.

Readings/Bibliography

L. MOGGI e M. VENTURI - Chimica Generale ed Inorganica - Corso Editore, Ferrara

I. Bertini, C. Luchinat, F. Mani - Chimica -Casa Editrice Ambrosiana 

Kotz, Treichel, Weaver, Chimica, EdiSES

trasparencies used during the class

Slides that can be downloaded at https://campus.cib.unibo.it/

Information on Elements, that can be downloaded at https://campus.cib.unibo.it/

Teaching methods

Class lessons: theory and stoichiometric exercises

Assessment methods

Final written (5 stoichiometric problems) and oral examination. Admission to oral depends on the result of the written test (> 18/30).

The validity of the written text is extended to the next April 30.

For being admitted to the written test, the student should register at Almaesami three working days in advance.

Teaching tools

During the course slides will be projected. These slides can be downloaded from the indicated internet page(https://campus.cib.unibo.it/)

Links to further information

https://campus.cib.unibo.it/

Office hours

See the website of Luca Prodi