1. Ionic Compounds
Level 2

2. Metal Cations Type I * metals whose ions can only have one possible
charge
Groups IA & IIA
Al, Ga, In, Zn, Cd, & Ag
* determine charge by position on the Periodic Table
IA = 1+; IIA = 2+
Al, Ga, and In = 3+; Zn & Cd = 2+; Ag = 1+

3. Type II * metals whose ions can have more than one possible charge
* Mostly transition and
post transition metals

4. Polyatomic Ions * made of more than one atom.
* groups of atoms that travel
together—NEVER apart.
* The given charge is on the entire
polyatomic ion—not on
individual atoms within the
polyatomic ion.

5. Naming & Writing Formulas

6. Type I Metals
Naming
* ALWAYS name the cation first and the anion second
* Cation – metal name
* Anion – 1. if nonmetal change end of name to -ide
2. if polyatomic ion use the name

7. Name the following Potassium Chloride KCl NaCl MgO Sodium Chloride
Li3PO4
NH4Cl
Potassium Chloride
Sodium Chloride
Magnesium Oxide
Lithium Phosphate
Ammonium Chloride

8. MgF2 Writing the Formula Magnesium Fluoride Mg+2 F-1 F-1
1. Write the ions that make up the compound
Mg+2
F-1
2. Do the charges add to equal zero?
No – go to 3; Yes – go to 4.
F-1
3. Add ions as needed so the compound has a charge of zero
MgF2
4. Write the number of each ion as a subscript and you have the formula
(DO NOT include charges & DO NOT write 1s)

9. Zn(NO3)2 Zinc Nitrate Zn+2 NO3-1 NO3-1
1. Write the ions that make up the compound
Zinc Nitrate
2. Do the charges add to equal zero?
No – go to 3; Yes – go to 4.
Zn+2
NO3-1
3. Add ions as needed so the compound has a
charge of zero
NO3-1
4. Write the number of each ion as a subscript
and you have the formula
(DO NOT include charges & DO NOT write 1s)
*If you have more than 1 of a polyatomic ion,
you must put the ion in parenthesis*
Zn(NO3)2

10. Write the formula for the following
Calcium Oxide
Aluminum Chloride
Ammonium Nitrate
Ca O2-
CaO
Al Cl-
AlCl3
NH NO3-
NH4NO3

11. Type II Metals PbI4 Lead (IV) Iodide Writing the Formula Pb+4 I-1 I-1
1. Write the ions that make up the compound
I-1
I-1
2. Do the charges add to equal zero?
No – go to 3; Yes – go to 4.
I-1
3. Add ions as needed so the compound has a charge of zero
PbI4
4. Write the number of each ion as a subscript and you have the formula
(DO NOT include charges & DO NOT write 1s)

12. CuCO3 Copper (II) Carbonate Cu+2 CO3-2
1. Write the ions that make up the compound
Copper (II) Carbonate
2. Do the charges add to equal zero?
No – go to 3; Yes – go to 4.
Cu+2
CO3-2
3. Add ions as needed so the compound has a
charge of zero
CuCO3
4. Write the number of each ion as a subscript
and you have the formula
(DO NOT include charges & DO NOT write 1s)
*If you have more than 1 of a polyatomic ion,
you must put the ion in parenthesis*

13. Co2O3 Cobalt (III) oxide Co+3 O-2 Co+3 O-2 O-2
1. Write the ions that make up the compound
2. Do the charges add to equal zero?
No – go to 3; Yes – go to 4.
Co+3
O-2
Co+3
O-2
3. Add ions as needed so the compound has a
charge of zero
O-2
4. Write the number of each ion as a subscript
and you have the formula
(DO NOT include charges & DO NOT write 1s)
Co2O3

14. Write the formula for the following:
Tin (II) Nitrate
Iron (III) Phosphate
Copper (I) Oxide
Sn NO3-
Sn(NO3)2
Fe PO4-3
FePO4
Cu+ O-2
Cu2O

15. Naming * ALWAYS name the cation first and the anion second
* Cation – metal name (charge of metal)
*** you must determine the charge of the metal
and use that after the name***
* Anion – 1. if nonmetal change end of name to -ide
2. if polyatomic ion use the name

16. FeCl3 Iron (III) chloride Cl- Fe+? Cl- Cl- Name the following:
1. Name the metal
2. Use a Roman Numeral to show the charge of the metal (because Type II)
Use the anion and the number of atoms in the formula to determine the charge
Cl-
Fe+?
Cl-
The anion side has a total charge of -3
Cl-
There is only one cation so it must have a charge of +3 to cancel the charge of the anion side -3
3. Name the anion

17. Fe3P2 Iron (II) phosphide Fe+? P-3 Name the following:
1. Name the metal
2. Use a Roman Numeral to show the charge of the metal (because Type II)
USE the anion and the number of atoms in the formula to determine the charge
Fe+?
P-3
The anion side has a total charge of -6 -6
There are three cations so each must have a charge of +2 to cancel the charge of the anion side
3. Name the anion

18. Name the following CuSO4 VCl5 Fe2O3 Cu?+ SO42- Copper (II) Sulfate
If there is one SO4 with a (-2) charge, the one Cu must have a (+2) to balance it
CuSO4
VCl5
Fe2O3
Cu?+ SO42-
Copper (II) Sulfate
If there are five Cl’s with a (-1) charge each, the one V must have a (+5) to balance the (-5) from Chlorine
V? Cl-
Vanadium (V) Chloride
Three O’s with a (-2) charge add up to -6. There are two Fe’s to cancel it out. Each Fe must have a (+3) to balance it.
Fe?+ O2-
Iron (III) Oxide