1. Naming Review

2. Step 1 What type of compound is it? Covalent? Ionic? (aka salt) Acid?
Two non-metals
Ionic? (aka salt)
Two ions
Binary ionic includes 2 elements, one metal and one non-metal
Ionic compounds with more than 2 elements contain polyatomic ions
Acid?
Binary acid – starts with hydrogen, ends in non-metal
Oxyacid- starts with hydrogen, ends in polyatomic ion
Base?
Starts with metal, end with hydroxide group (OH)

3. If Covalent…..
The prefix tells you the number of each element you have
Example: sulfur trioxide
One sulfur (because no prefix) and three oxygen's
SO3

4. If Ionic Step 1: Figure out two ions that make up compound
First ion is always positive (either a metal or ammonium)
Second ion is always negative (either a non-metal or a polyatomic ion)
If a non-metal the ending will be –ide
If polyatomic the ending will be –ate or –ite
Except hydroxide and cyanide

5. If Ionic Step 2 Determine the charges on both ions
If cation is group 1, 2, 3, Zn, or Ag we know the charge by looking at the periodic table
If cation is ammonium we look at list of polyatomics
If cation is not in group 1, 2, 3, Zn or Ag, we need at the roman numeral in the middle of the compounds name
If anion is a non-metal we know the charge by looking at periodic table
If anion is a polyatomic ion we look at the list of polyatomics

6. If Ionic Step 3 Make a neutral compound
Crisscross charges (charges are the superscripts that we just determined) to become opposite ions subscript
Put polyatomic ions in parenthesis

7. If Ionic
Step 4
Reduce newly made subscripts if they are divisible by the same number

8. Ionic Example Calcium Sulfide Iron (III) Carbonate Step 1: Ca S
Step 4: both are divisible by 2 so CaS
Iron (III) Carbonate
Step 1: Fe CO3
Step 2: Fe+3 CO3-2
Step 3: Fe2(CO3)3
Step 4: already reduced as far as possible

9. If Acid Step 1 Determine the type of acid it is
If starts with hydro it is a binary acid
If starts with per-, hypo-, or no prefix, it is an oxyacid

10. If Acid Step 2: Write the cation and anion Cation ALWAYS H+ Anion:
if binary acid, the anion is a metal from the periodic table
If oxyacid, the anion is from the list of polyatomic ions
If acid name ends in –ic than the polyatomic ended in –ate
If the acid name ends in –ous than the polyatomic ended in –ite
If there is a prefix on the acid (per or –hypo) then that is part of the polyatomic ion

11. If Acid Step 3: Write charges of ions
Cation, which is hydrogen, always has a +1 charge
Anion, if non-metal, look at periodic table for charge, if polaytomic ion, look at polyatomic list

12. If Acid Step 4: Make a neutral compound
Crisscross charges (charges are the superscripts that we just determined) to become opposite ions subscript

13. Examples of Acids Hydrophosphoric Acid Sulfuric Acid
Step1: binary because starts with hydro-
Step2: H P
Step3: H+1 P-3
Step4: H3P
Sulfuric Acid
Step1: oxyacid because no prefix
Step 2: H SO4 (because acid name ended in –ic, which comes from –ate ending, so sulfate ion)
Step3: H+1 SO4-2
Step 4: H2SO4

14. If Base
Step 1:
Figure out cation and anion (anion is always hydroxide group)

15. If Base Step 2: Determine charges for ions
Cation- look on periodic table for metals in group 1,2,3, Zn, Ag or look in middle of compound for roman numeral, if ammonium look on list of polyatomics
Anion always has a -1 charge

16. If Base Step 3: Make neutral compound
Crisscross charges (charges are the superscripts that we just determined) to become opposite ions subscript
Put polyatomic ion (hydroxide) into parenthesis

17. Base Examples Aluminum hydroxide Ammonium hydroxide Step1: Al OH
Step1: NH4 OH
Step 2: NH4+1 OH-1
Step 3: NH4OH