1. Bonding Periodic Table Stuff & Redox

3. Bonding in Ionic Compounds

4. Ionic Bonds (Salts) Between a metal (usually) and a non-metal (usually). The metal gives up its electron to the non-metal. Giving up electrons turns the metal into a positively charged ion called a cation. Gaining the electrons turns the non-metal into a negtatively charged ion called an anion. The positive and negative charges attract each other. This is the ionic bond. Ionic compounds are crystals – the formula shows the ratio of the elements in the compound. It is known as a formula unit. They have high melting points. They are more likely to be soluble in water, the universal solvent. They are electrolytes.

5. CsCl CaF 2

6. Experienced chemists can often predict the structure that a given ionic species will adopt, based on the nature of the ions involved. This means that it is often possible to design ionic compounds having certain well-defined and desirable properties. As an example, chemists have been able to make high-temperature superconductors, such as the complicated ionic compound, YBa 2 Cu 3 O 4. This solid conducts electricity with no resistance at all at low temperature (below ca. -100 degrees centigrade). Previous superconductors only had this property at much lower temperatures. The lack of resistance makes superconductors very useful in a number of technological applications - e.g. in designing high-speed trains that levitate above the track! The repeating structure of this solid is shown below (oxygen is large and red, barium large and yellow-ish, yttrium small and pink, and copper small and blue). Notice how many oxygen ions surround each barium and yttrium ion.

7. Covalent Bonds (Not-Salts) The electrons are shared between compounds. This allows each atom to have a full outer shell for stability. Covalent compounds are represented by true molecules. The formula represents how many of each atom there are in the molecule. 1 electron each shared is a single bond, 2 electrons each is a double bond and 3 electrons each is a triple bond. They have low melting points. They don’t usually dissolve well in water. They are not electrolytes.

8. Bonding in Covalent Compounds Plot of region where e- sit. Not localized.

9. Bonding in Metals

10. Bonding in Covalent Compounds – VSEPR shapes

11. Bonding in Covalent Compounds – Polarities of Molecules

12. Bonding between Molecules – Intermolecular Bonding: Hydrogen Bonding

13. Bonding between Molecules – Intermolecular Bonding: Dipole - Dipole Bonding & Induced Dipole Bonding (london dispersion) Collectively: van der waals forces http://chemsite.lsrhs.net/bonding/LondonDispersion.html

14. Families/Groups; Periodic Law; Ionization energy & Electronegativity

16. Assigning Oxidation Numbers: PO 4 -3 H 2 SO 4

17. OIL RIG