1. Naming and determining the formula of ionic compounds

2. Naming ionic compounds For monoatomic anions only drop the ending and add “-ide” so F - fluoride Cl -, O 2-, C 4- chloride, oxide and carbide

3. Continuing… cations keep the name of the element. When naming compounds always name the positive (cation) first and the negative (anion) last. so mixing ions of chlorine and sodium give you sodium chloride (positive) (negative)

4. Determining the formula of ions Ionic compounds are neutral You need to find the lowest number of each ion to make it neutral for example: Na + and O 2- 2 sodium for every one oxygen Na 2 O

5. More examples Al 3+ and O 2- Al 2 O 3 K + and Cl - KCl the subscripts don’t effect the name if there is only one possibility still (cation)(anion) Aluminum oxide Potassium chloride

6. Several atoms can form a couple of different ions. These are all metals that aren’t in group 1, 2 or aluminum. for example iron can form Fe 2+ or Fe 3+ These are said as iron (II) and iron (III) Cu + and Cu 2+ is Copper (I) and Copper (II)

7. Figuring out charge on these elements If the ion is named, the charge is in the name. If you have the formula, use the charges of the other ions present to determine the charge. Remember Alkali will always be +1 Alkaline Earth +2, Halogens -1, oxygen group -2 Aluminum will always be +3

8. Examples Copper (II) chloride CuCl 2 Cobalt (III) sulfide Co 2 S 3 NiF 2 Nickel (II) fluoride Ag 2 S Silver (I) sulfide

9. Polyatomic ions Polyatomic Ions- many atoms in one ion You can NOT break these apart in this section. the “ide” suffix only applies to monoatomic anions

10. Common polyatomic ions Ammonium NH 4 + PerchlorateClO 4 - SulfateSO 4 2- Acetate CH 3 COO - ChlorateClO 3 - SulfiteSO 3 2- Nitrate NO 3 - ChloriteClO 2 - CarbonateCO 3 2- Nitrite NO 2 - HypochloriteClO - DichromateCr 2 O 7 2- Cyanide CN - IodateIO 3 - ChromateCrO 4 2- Thiocyante SCN - BromateBrO 3 - OxalateC 2 O 4 2- Hydrogen Carbonate HCO 3 - HydroxideOH - SilicateSiO 3 2- Hydrogen Sulfate HSO 4 - PermanganateMnO 4 - PhosphatePO 4 3- Hydrogen Sulfite HSO 4 - ManganateMnO 4 2- ArsenateAsO 4 3-

11. Don’t worry you don’t have to memorize them!! They are given to you for tests. You will however have to be able to recognize them with the list. You have to look at polyatomic ions like they are one thing. Don’t alter their formula in anyway

12. Determining the formula of ions Ionic compounds are neutral Remember-- you cannot break a polyatomic ion apart for example: Ammonium carbonate NH 4 + and CO 3 2- (NH 4 ) 2 CO 3