1. Naming Ionic Compounds

2. Charges
Elements will gain or lose electrons to have 8 valence electrons. (This is the octet rule)
Group 1A  +1
Group 2A  +2
Group 3A  +3
Group 4A  N/A
Group 5A  -3
Group 6A  -2
Group 7A  -1
Group 8A  STABLE
The charges of monatomic ions, or ions containing only one atom, can be determined by referring to the periodic table

3. Ionic Compounds ion : atom or group of atoms that has a charge
A monatomic ion is one element with a charge
A polyatomic ion is more than one element with a charge
Example: SO42-
ionic compound: compound formed between a cation ( +) and an anion (-).
usually between a metal and a nonmetal.
also form between a polyatomic ion (like ammonium) and either a metal or nonmetal.
TRANSFER valence electrons

4. Ions A cation An anion A monatomic ion is one element with a charge
positive ion
formed when an atom loses electrons.
Example: Na+
An anion
negative ion
is formed when an atom gains electrons
Example: Cl-
A monatomic ion is one element with a charge
A polyatomic ion is a group of covalently bonded atoms with a charge
Example: SO42-

5. Formation of Ionic Compounds
objects with opposite charges attract each other.
ionic bond = the strong attractive force between ions of opposite charge
Strongest type of bond!!
the overall charge of the compound will be …
ZERO!

6. Examples of Formula Writing
Write the formula for the compound formed between calcium and nitrogen
Step One: Write the symbols and charges of the ions formed
Ca2+ N3-
Step Two: Balance the charges so the total is ZERO
You will need 3 Calcium’s and 2 Nitride’s
Step Three: Write the Formula
Use subscripts to show the number of each ion needed
Ca3N2

7. More examples
Write the formula between Mg and Br
Mg+2 Br -1
MgBr2

8. More examples
Write the formula for the compound formed between Ca and S
Ca S-2
CaS

9. Polyatomic Ions Polyatomic ions are groups of atoms that have a charge
For example:
SO4 -2
NO3 –1
ClO3 –1
NH4 +1

10. Polyatomic Ions
You must use parentheses when using subscripts with a polyatomic ion
Ex: Calcium nitrate
Ca +2 NO3 -1
Ca(NO3)2

11. Formula writing with polyatomic Ions
Write the formula between ammonium and sulfate
NH SO4 -2
(NH4)2 SO4

12. More examples Copper (II) and chlorine Silver and Nitrate
Magnesium and sulfite
Calcium and sulfur
Potassium and oxygen
Ammonium and phosphate
Ammonium and chlorine
CuCl2
AgNO3
MgSO3
CaS
K2O
(NH4)3PO4
NH4Cl

13. Multiple Charges!
There are some elements that form multiple charges That roman numeral will tell you the charge!
For example: Copper (II)  Cu +2

14. Multiple Charges to Remember
Copper
Iron
Lead
Tin
Manganese
Gold
Cobalt
+1 and +2
+2 and +3
+2 and +4
+2, +4, and +7
+1 and +3

15. Naming ionic compounds
In naming ionic compounds, name the cation first, then the anion.
Cation name does not change.
If the cation can have more than one charge (mostly transition metals), use a Roman Numeral after the element name to indicate the charge
Ex. Iron (II) for Fe2+ or Iron (III) for Fe3+
Monatomic anions: change the ending to -ide. (ex. Br -, Cl-, O2-)
Polyatomic Ions: do not change the name (ex. SO42-, CO32-, PO43-

16. Examples NaCl MgSO4 CuSO3 K3PO4 Fe(NO3)2 Ca(ClO3)2 NH4NO2 Al(ClO)3
Sodium chloride
Magnesium sulfate
Copper (II) sulfite
Potassium phosphate
Iron (II) nitrate
Calcium chlorate
Ammonium nitrite
Aluminum hypochlorite

17. More examples Lead (IV) Oxide Ammonium Permanganate
Cobalt (II) chloride
Calcium sulfide
Lithium nitrate
Sodium acetate
Tin (II) chloride
PbO2
NH4MnO4
CoCl2
CaS
LiNO3
NaCH3COO
SnCl2