1. Writing Formulas and Naming Compounds Binary Ionic Compounds

2. Oxidation Number Tells how many electrons an atom has gained, lost, or shared to become stable Oxidation Number = Charge of the Ion Examples: Sodium Ion  charge (1+)  oxidation # (1+) Chloride Ion  charge (1-)  oxidation # (1-)

3. Compounds are Neutral Calcium charge  2+ Fluoride charge  1- You need 2 Fluorides for every 1 Calcium  CaF 2

4. Compounds are Neutral Aluminum charge  3+ Oxygen charge  2+ Must find the least common multiple  Al ? O ?  Al 2 O 3

5. Binary Ionic Compound Compound composed of a Metal and a Nonmetal Binary means Two Each Compound will have a First Name and a Last Name

6. Rules for the First Name 1.Name the first metal cation as it appears on your Periodic Table, if you only have one cation. 2.If the metal has two or more cations (as transition metals do), the first name will be followed be Roman Numerals that match the charge of the given cation.

7. Rules for the Second Name 1.IF YOU HAVE A SINGLE NONMETAL: Change the ending of the Nonmetal Anion Name to an –ide ending. 2.IF YOU HAVE A NONMETAL GROUP (POLYATOMIC ANION): Use the name of the Anion group. Do not add an –ide ending.

8. Examples Type I Al +3 and F -1  AlF 3  Aluminum Fluoride

9. Examples Type II Cu +1 and O -2  Cu 2 O  Copper (I) Oxide Cu +3 and O -2  Cu 2 O 3  Copper (III) Oxide

10. Examples Polyatomic Ions K +1 and C 2 H 3 O 2 -1  KC 2 H 3 O 2  Potassium Acetate