1. Warm UP - 10/24/2016
Write the compound formula or name the following formula for the following:
1) Sodium Acetate
2) Calcium Nitride
3) Ca3(PO4)2
4) Rb3P

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

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

4. 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

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

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

7. 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

8. 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".

9. 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

10. 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

11. Naming & Identifying Acids
All acids contain hydrogen
When acids are dissolved in water, H+ ions are generated
Acids that generate a lot of H+ are strong acids
Acids that generate only a small amount of H+ are weak acids

12. Strong Acids
HCl is a strong acid because no HCl molecules are in a water solution of HCl.
Because of the strong attraction between the water molecules and HCl molecules, every HCl molecule ionizes.

13. Naming & Identifying Acids Cont.
The formula for an acid is: HX
Where X = an anion

14. Naming Binary Acids
Naming Acids:
1. Begin with the regular name
Example HCl is Hydrogen Chloride
2. If the anion ends is “-ide,” add “hydro” as a prefix
3. Replace “-ide” with “-ic”and add acid
Example: HCl
Hydrogen chloride becomes hydrochloric acid
NOTE: It is only an acid with the ending ends in aqueous. If the compound is either gas, liquid, or solid it is not an acid, it is the normal compound.

15. Name the following binary acids
Answers:
1. Hydrofluoric Acid
2. Hydrobromic Acid
3. Hydroiodic Acid
1. HF
2. HBr
3. HI

16. Naming Ternary Acids Ternary acids contain polyatomic ions
To name acids (with 3 or more different elements):
1. Determine regular name of the compound
2. If the anion end in “-ite,” add “-ous” in place of “-ite” and add acid to the end
3. If the anion ends in “-ate,” add “-ic” in place of “-ate” and add acid to the end

17. Examples of Naming Ternary Acids
1. H2SO3
Name: Hydrogen Sulfite
Name of Acid: Sulfurous Acid
2. HNO3
Name: Hydrogen Nitrate
Name of Acid: Nitric Acid
Begin 3rd 4-28

18. Name the following ternary acids
1. H3PO4
2. H2CO3
3. H3PO3

19. Write formulas for the following acids:
1. Chlorous Acid
2. Acetic Acid