1. Warm -Up
When Sodium and Sulfur react, what compound is produced?
When Calcium and Bromine react, what compound is produced?

2. Write the Name or formula for the following
calcium phosphide
Na2O
Titanium(III) bromide
Copper(I) phosphide
SnS2

3. Name or write the following compounds
Chromium (VI) Oxide
Ca3P2
Strontium Sulfide
Cu2O

4. Name or write the correct formula for the following compounds
1. Zinc Chloride
2. Fe3P2
3. Sodium Selenide
4. CrN2
5. Gold (II) Iodide

5. Name the following compounds
1. CuO
2. Co3N2
3. Fe2O3
4. CrI6 5

6. Write the formula for the following names
Write formulas for:
1. barium oxide
2. cobalt (II) fluoride
3. silver phosphide
4. zinc chloride
5. Titanium (IV) oxide

7. Naming Ternary Compounds
Ternary compounds are named similar to binary ionic compounds:
Still going to be using the cation’s name but this time you are going to be using the polyatomic name as the anion’s name

8. Ternary Compounds contain at least 3 different elements
A ternary compound contains a polyatomic ion
Always write the polyatomic ion in parenthesis before crossing the charges 8

9. Examples of Polyatomic Ions
(CN)- Cyanide Ion
(OH)- Hydroxide Ion
(CO3)2- Carbonate Ion
(NH4)+ Ammonium Ion
(SO4) -2 Sulfate Ion
(NO3)-1 Nitrate Ion 9

10. Example: Write the formula for:
Magnesium and Nitrate -1
(NO3) Mg 2+
Mg(NO3)2

11. Examples of Naming Polyatomic Ion Compounds
1. Li(NO3)
2. Ca(OH)2
3. Sn(CO3)

12. Write the compound formula or name the following formula for the following:
1) Sodium Acetate
2) Calcium Nitride
3) Ca3(PO4)2
4) Rb3P

13. Practice Naming the following:
4. MgSO3
5. Na2CO3
6. Ba(OH)2
7. Fe(CN)3
8. Mn2(Cr2O7)3
9. (NH4)2SO4

14. Practice
1. Magnesium Sulfate
2. Ammonium Chloride
3. Iron (III) Carbonate
4. Ammonium Phosphate
5. Aluminum Cyanide

15. Practice
Name or write the following compounds
Ca(MnO4)2
Cobalt (III) Nitrate
CsC2H3O2
Calcium Sulfate

16. Practice Name the following: 6. Ba3(PO4)2 7. ZnCO3 8. (NH4)Cl 9. KMnO4
Write formulas for:
1. Sodium Dichromate
2. Iron (II) sulfate
3. Silver hydroxide
4. Ammonium Phosphate
5. Copper (II) Sulfite
Name the following:
6. Ba3(PO4)2
7. ZnCO3
8. (NH4)Cl
9. KMnO4
10. Cu(NO3)2

17. Practice Naming or writing Compounds
Mn(ClO2)7
PbS
NH4HSO3
KCN
Cd(NO3)2
Lead (IV) perchlorate
Beryllium Acetate
Copper (II) Bisulfate

18. Practice
Name the following:
1. (NH4)3P
2. Na2CO3
3. Fe(OH)3
4. CuSO4
5. AlCl3

19. Naming/Writing Hydrates
Hydrates are substances that include water in their formula. The water is not actually part of the chemical substance and this is reflected in the way the formula is written.
Example: CuSO4 ⋅ 5H2O

20. Rules
1) The ionic compound (WITHOUT the waters of hydration) is named first by using the rules for naming ionic compounds (e.x., Ba(OH)2•8H2O = "barium hydroxide”
2) Greek Prefixes are attached to the word "hydrate" to indicate the number of water molecules per formula unit for the compound (e.g., Ba(OH)2•8H2O; 8 water molecules = "octahydrate")
3) When the chemical formula for a hydrated ionic compound is written, the formula for the ionic compound is separated from the waters of hydration by a centered "dot".

21. Practice 2) MgSO4 • 7 H2O 3) CrBr3• 6H2O 4) Pb(ClO3)2 • 3H2O
1) MnBr2• 4 H2O
2) MgSO4 • 7 H2O
3) CrBr3• 6H2O
4) Pb(ClO3)2 • 3H2O

22. 2) Cobalt(II) chloride hexahydrate 3) Mercury(II) nitrate monohydrate
Practice
1) Beryllium hydroxide octahydrate
2) Cobalt(II) chloride hexahydrate
3) Mercury(II) nitrate monohydrate
4) Tin(IV) chloride pentahydrate