08 Ionic Compounds
The lecture introduces the concept of an ionic compound, i.e. one where one or more electrons is transferred completely from one atom to another. The Born-Haber cycle is detailed, which helps us understand some of the properties of ionic compounds such as high melting point and brittleness.
ppt-08     Chap.6    A-04 tut-03

09 Grp. 1A Chemistry
The lecture starts with a statement of the octet rule, and shows how this rule can be applied to simple compounds. The rules for determining the stoichiometry of simple compounds are explained. Some group 1A chemistry (specifically that of hydrogen) is described. The concept of electronegativity and covalent bonds is introduced.
ppt-09     Chap.6    A-04

10 Grp. 2A Chemistry, Lewis Diagrams
Group 2A chemistry is described, including the production and uses of Mg and Ca. The method for drawing correct Lewis structures is detailed. Note that it is necessary to be able to do this in order to predict molecular shapes via the VSEPR theory (in a subsequent lecture). The idea of formal charges is explained, which helps to predict the most likely arrangements of bonds in some molecules. Some molecules have several equivalent structures, so-called resonance structures. Some examples of these are given.
ppt-10     Chap.7    A-04

11 VSEPR Theory, Molecular Shapes
The case is made that molecular shape determines molecular properties, i.e. chemistry of all species. Valence Shell Electron Pair Repulsion Theory (VSEPR) is a simple tool for predicting the shapes of molecules. Once the Lewis structure is established, the molecular shape is predicted from the number of bonding and non-bonding electrons in the molecule. Note that you must be able to figure out the Lewis structure in order to use VSEPR theory. Review yesterday's lecture!

ppt-11     Chap.7    A-05 tut-04 VSEPR

12 Hybrid Orbitals
So far, the only orbitals we have examined are atomic orbitals (s, p, d and f). What happens when we combine atomic orbitals to make a molecule? One way to predict the outcome is by the use of hybrid orbitals. As the name suggests, the resulting bonds between atoms are hybrids of the participating atomic orbitals.
ppt-12     Chap.7    A-05 Hybrid Orbitals

13 Molecular Orbitals
Hybrid orbitals are good at predicting some aspects of bonding, including shape. However, molecular orbital (MO) theory is quantitatively correct, and is capable of predicting such things as the bond order and paramagnetism. MO theory also has its roots in wavw functions, which were used to predict the shapes of atomic orbitals.
ppt-13     Chap.7    A-05 Molecular Orbitals