1. MULTIVALENT IONIC COMPOUNDS
Ions of some transition elements can have more than one possible charge.
WE use ROMAN NUMERALS to indicate the type of charge on these multivalent ions.
Such elements are called MULTIVALENT species.
1+  I
2+  II
3+  III
For example, what are the 2 possible charges for copper – Cu?
4+  IV
5+  V
6+  VI
_________________
ONLY USE WITH MULTIVALENT IONS!

2. GIVEN NAME, WRITE FORMULA
RULES
Use ROMAN NUMERALS to determine the ION CHARGE of the MULTIVALENT ION.
If ROMAN NUMERAL are NOT given, use the charge found on the top in each box on the table.
EXAMPLE:
copper (II) oxide _________________________

3. GIVEN NAME, WRITE FORMULA
lead (IV) sulfide _________________________
tin sulfide _________________________

4. GIVEN FORMULA, WRITE NAME
RULES
Write the names of the ions.
Write the ROMAN NUMERAL for the MULTIVALENT ION. There are 2 METHODS:
METHOD 1
Charges must add up to zero.
METHOD 2
Charge of Anion X Subscript of Anion
Subscript of Cation

5. GIVEN FORMULA, WRITE NAME
PbI2 _________________________
Fe2O3 _________________________

6. GIVEN FORMULA, WRITE NAME
CuCl _________________________
MnO2 _________________________

7. POLYATOMIC IONIC COMPOUNDS
DEFINITION:
EXAMPLES:
Polyatomic ions are GROUPS OF ATOMS acting as 1 ION, carrying an OVERALL CHARGE.
nitrate ________
nitrite ________
cyanide ________
hydroxide ________
bicarbonate ________
chlorate ________
On the back of your periodic table, there is a POLYATOMIC ION TABLE.
carbonate ________
sulfate ________
phosphate ________
Endings of polyatomic ions are easily recognizable as they are often –ATE or –ITE, providing a good clue.
ammonium ________
acetate ________

9. GIVEN NAME, WRITE FORMULA
lithium sulfate _____________________
ammonium carbonate _____________________

10. GIVEN NAME, WRITE FORMULA
hydrogen dichromate _____________________
sodium acetate _____________________

11. GIVEN FORMULA, WRITE NAME
HNO3 _____________________
NaOH _____________________

12. GIVEN FORMULA, WRITE NAME
KMnO4 _____________________
Cu2SO4 _____________________

13. SOME OTHER NAMES . . . hydrogen carbonate is AKA bicarbonate HCO3-
hydrogen sulfate is AKA bisulfate HSO4-
tetraborate B4O72-
silicate SiO32-
glutamate C5NH8O4-

14. HYDRATED IONIC COMPOUNDS
Hydrated ionic compounds have WATER attached to their crystal lattice structure.
Solutions become hydrated when they are crystallized from a water solution.
They are often recognizable by eye because they are often SHINY and TRANSLUCENT.
Examples:
Bluestone, Epsom salts, Rock salts
BLUESTONE  CuSO4 ∙5H2O
5 H2O molecules attached to each CuSO4 compound.
The “dot” represents a weak bond.

15. HYDRATED IONIC COMPOUNDS
We indicate the presence of water with the word HYDRATE and we indicate the number of water molecules with our GREEK PREFIXES:
MONO 1, DI 2, TRI 3, TETRA 4, PENTA 5, HEXA 6, HEPTA 7, OCTA 8, NONA 9, DECA 10
ANHYDROUS: NO water attached

16. GIVEN NAME, WRITE FORMULA
barium chloride dihydrate
_____________________
potassium hydroxide hexahydrate

17. GIVEN NAME, WRITE FORMULA
sodium carbonate octahydrate
_____________________
cobalt (II) chloride decahydrate

18. GIVEN FORMULA, WRITE NAME
CaSO4 ∙2H2O _____________________
Na3PO4 ∙4H2O ______________________

19. GIVEN FORMULA, WRITE NAME
HCN ∙ 3H2O _____________________
HOMEWORK:
DO THE SHEET ON HYDRATED IONIC COMPOUNDS ON THE NEXT PAGE OF YOUR HANDOUT.