1. CHEMISTRY PART 6 Ionic Compounds

2. 1+ 2+ 3+ 3- 2- 1- Charges of transition metals will be given in the periodic table as their formation is complicated.

3. Ionic Compounds  A compound made up of oppositely charged ions held together by ionic bonds.  Ionic bonds are very strong.

4. Ionic Compounds  For an atom to gain electrons, a different atom must lose them.  Example:  Table Salt  sodium chloride.  NaCl  Sodium loses 1e- and chlorine gains the 1e-.

6. Ionic Compounds  Example:  Calcium Chloride  CaCl 2  Calcium loses 2 e-  Chloride needs to gain 1e-  So need two chlorines to take from calcium.

8. Binary Ionic Compounds  A compound composed of ions of one metal element and ions of one non-metal element.  The compound is neutral.  The total charge for the compound is 0.  The charges of each ion cancel out.

9. Binary Ionic Compounds  The metal will transfer electrons to the non-metal.  Both will now have a full, stable valence shell.

10. Formula Writing  Tile Activity

11. Formula Writing 1. Determine the charge of each atom. 2. Draw circles to represent each element until their charges cancel out. 3. Write the symbol of each atom, starting with the metal. 4. Add subscripts to show the number of atoms present (the number of circles).

12. Formula Writing  Example:  Lithium Sulfide  Li  1+  S  2-  Li ₂ S 1+2- 1+ Total Charges: 2+ 2- Total Charge When Combined = 0 Total Lithium atoms = 2 Total Sulfur atoms = 1

13. Formula Writing  Example:  Aluminum Oxide  Al  3+  O  2-  Al ₂ O ₃ 3+2- 3+ Total Charges: 6+ 6- 2-

14. Nomenclature  Naming Compounds  IUPAC  International Union of Pure and Applied Chemistry.  Rules for naming chemical compounds.

15. Nomenclature 1. Name the cation (the metal) 2. Name the anion (the non-metal)  Use the “ide” ending.  Example:  KBr  Potassium Bromide

16. Nomenclature  Examples:  NaCl Sodium Chloride  MgBr 2 Magnesium Bromide K2OK2O Potassium Oxide

17. Nomenclature  Examples:  Hydrogen and Chlorine  H 1+ and Cl 1- Hydrogen Chloride HCl  Phosphorus and Magnesium  P 3- and Mg 2+ Magnesium Phosphide Mg 3 P 2

18. Nomenclature  Examples:  Calcium and Carbon  Ca 2+ and C 4- Calcium Carbide Ca 4 C 2 Ca 2 C

19. Practice  Worksheet  Page 109 # 8  Page 113 # 8 – 10