1. Naming Ionic Compounds

2. Remember… Metals form positive ions or cation.
The charges on ions formed from groups 1A, 2A and the upper part of 3A is the same as the group number.
Hydrogen can have a +1 or a -1 charge.

3. Remember… Transition metals have a variable charge.
Example: Iron can have a +2 or a +3 charge depending on the compound.
EXCEPTION: Zn, Cd, Ag are not transition metals; ALWAYS Zn2+, Cd2+, and Ag+1

4. Remember… Non-metals form negative ions or anions
The charge on ions formed from group 7A is -1, 6A is -2 and 5A is -3.

5. Ionic Compounds (metal and a non metal) If given the Formula, to write the name you must…
The full name of the cation is listed first.
If the compound is a transition metal, you must determine its’ charge. Include a roman numeral after the name to indicate the charge of the metal.
Then list root of the anion name with the suffix “ide.”

6. Naming Binary Ionic Compounds
Examples: NaCl BaF2 CuO
Na2O
CaBr2
CuCl2
sodium chloride
sodium oxide
barium fluoride
calcium bromide
copper (II) oxide
copper (II) chloride

7. Ionic Compounds (metal and a non metal) If given the Name, to write the formula you must…
Write the symbol of the first ion in the compound’s name, then the symbol of the second ion in the compound ’s name.
Indicate the ratio of each ion in the compound using subscripts after each ion.
Note: The ratio of the ions are determined by balancing the charges of the ions.

8. Naming Binary Ionic Compounds
Examples: Lithium Iodide Gallium Chloride Lead (II) Nitride
Sodium hydride
Magnesium Oxide
Tin (IV) sulfide
LiI
NaH
GaCl3
MgO
Pb3N2
SnS2

9. Polyatomic Ion
A charged particle with two or more atoms held together.
Example: SO42-

10. Rules for Polyatomic Ions Naming/Writing Formulas
Same rules EXCEPT:
Naming - You will NOT change the suffix to “ide”; write the name of the polyatomic ion as is.
Formulas - Use parentheses when the simplest ratio requires more than one polyatomic ion in the compound formula.

11. Naming Binary Ionic Compounds with Polyatomic Ions
ammonium phosphate
iron (II) phosphate
ammonium carbonate
CaCO3 K2CrO4 Fe(OH)3
calcium carbonate
(NH4)3PO4
potassium chromate
Fe3(PO4)2
iron (III) hydroxide
(NH4)2CO3