1. Classify each of the substance as an atomic element, molecular element, molecular compound or ionic compound
N2O
Fluorine
K2O
Silver
Fe2O3

2. Naming of Ionic Compounds
Common names
Systematic names – can be determined from its chemical formula
Ionic compounds
Metals form only one type of Ion
Metals form more than one type of Ion

3. Metals form only one type of cation

4. Metals that form more than one cation
Metals of this type are mainly the transition elements
Example : Iron forms +2 cation in some compounds and +3 in others
Exception : Zn and Ag forms ions that cannot be inferred from their group number
Some main group elements form more than one cation
Example: Pb and Sn

5. Naming Binary Ionic Compound
Binary compound contains two different elements
KCl , CaO
Base name of Anion(non-metal)
+ - ide
Name of Cation

6. Some common monoatomic anions

7. Practice Name the compound CaBr2 Name the Compound Ag3N
Write the formula for Rubidium Sulfide

8. Naming Binary Ionic Compounds Containing a Metal That Forms more than one type of Cations
For these type of Metals, the name of the cation followed by a roman numeral (in parenthesis) that indicates the charge of the metal in that particular compound.

9. Some Metals That Forms Cations With Different Charges

10. Their names have the form
Name of Cation(metal)
Charge of cation in Roman numerals in paranthesis
Base name of anion(non metal)
+ -ide

11. Practice
CrBr3
CuO
PbCl4
FeS
Write the formula for Ruthenium (IV)Oxide

12. Naming Ionic Compounds Containing Polyatomic ions
Follow the same way as other ionic compounds
We us the name of the polyatomic ion whenever it occurs
Most of the polyatomic ions are oxyanions, anions containing oxygen and other element
NaNo2
FeSO4
NH4NO3

13. Naming Ionic Compounds Containing Polyatomic ions
If there are two ions in the series one with more oxygen atom has an ending -ate and the one with fewer has an ending -ite
Example : No Nitrite
NO Nitrate

14. Naming Ionic Compounds Containing Polyatomic ions
If there are more than two ions in the series then the prefixes
Hypo – less than
Per – more than
Example : ClO- - Hypochlorite
ClO Chlorite
ClO Chlorate
ClO Perchlorate

16. Practice Name the compound Li2Cr2O7 Name the compound Sn(ClO3)2
Write the formula for Cobalt(II) phosphate
Cobalt (II) means an ion Co 2+
Phosphate means an ion PO4 3-
As the compound needs to be electrically neutral, there must be 3 Cobalt (II) ions, and 2 phosphate ions. So the formula is Co3(PO4)2

17. Hydrated Ionic Compounds
Hydrates – Contain specific number of water molecules associated with each formula unit
Example : Epsom salt
The formula for Epsom salt is MgSO4·7H2O
Systematic name is magnesium sulfate heptahydrate . The seven water molecule associated with the formula unit is called waters of hydration
Waters of hydration can be easily removed by heating the substance

19. Examples
Cobalt(II) chloride hexahydrate is pink and when its heated it forms anhydrous cobalt chloride which is blue in color
Common hydrated ionic compounds and their names
CaSO4·1/2H2O – Calcium sulfate hemihydrate
BaCl2·6H2O Barium Chloride hexahydrate
CuSO4·5H2O Copper(II) sulfate pentahydrate

20. Name these Hydrates A) MgCO3  5 H2O B) CuI2  2 H2O
C) Cr(NO3)3• 7 H2O
D) BaCl2• 2 H2O

21. Write the formula for the following
Magnesium Sulfate hexahydrate
Sodium Carbonate decahydrate
Lithium Nitrate trihydrate
Calcium Sulfate hexahydrate
Cesium Carbonate dihydrate