1. Names and Formulas of Ionic Compounds
5.3

2. Naming Binary Ionic Compounds
Binary Ionic Compound (BIC) -ionic compound made up of two ions
To name cation – use name of atom
Na+ = sodium K+ = potassium
Ca2+ = calcium Ba2+ = barium

3. Naming Anions
To name anions, use the atom’s base name and –ide at the end
Cl- = Chloride S2- = Sulfide
P3- = Phosphide O2- = Oxide
KBr = Potassium bromide
Mg3N2 = Magnesium nitride

4. Writing Ionic Formulas
Write the symbol and charge of each ion side by side (cation first)
If total = 0, just write symbols & you are done!
If total does not = 0, criss cross charges to have overall 0 charge

5. Examples
CaS
CsF
K3P
Rubidium Chloride
Barium Sulfide
Beryllium Iodide

6. Multiple Charge Cations/Transition Metals
If cation has multiple charges, use a roman numeral to indicate charge
Cu+ =Copper (I) Cu+2 =Copper (II)
I = 1 II = 2 III = 3 IV = 4
V = 5 VI= 6 VII = 7 VIII = 8
IX = 9 X = 10

7. Determining Charge on Transition Metals
The charge on ionic compounds has to be electrically neutral
Figure out overall charge on anion and then determine what charge cation has to be
CuCl2 ~Each Cl has a charge of -1 (needs 1 e-) and since there are 2 of them, the overall charge of Cl is -2. Cu must be +2 = Copper (II) chloride

8. Determining Charge on Transition Metals
PbO2 Charge on O is -2 and there are 2 of them so overall on O is -4.
Pb has to be +4
Lead (IV) oxide

9. Examples Magnesium sulfide Rubidium Oxide Strontium Bromide
Aluminum Oxide
Vanadium (III) Iodide
Platinum (IV) oxide

10. Naming
FrF
SrBr2
CuO
Hg2O
Cu2O
Li2Se

11. Polyatomic Ions
Polyatomic Ion – an ion made of 2 or more atoms that behave like a single ion
Bonded covalently
Bond ionically with other simple ions as salts

12. Name changes as number of O changes
Oxyanions
Name changes as number of O changes
Gain 1 O = perchlorate ClO4-
Base Name = chlorate ClO3-
Lose 1 O = chlorite ClO2-
Lose 2 O = hypochlorite ClO-

13. Hydrogen and Sulfur
The name usually starts with the word hydrogen, but use mono- and di-
HPO4 –monohydrogen phosphate
H2PO4 – dihydrogen phosphate
Thio – replace O with S
K2S2O3 – Potassium thiosulfate

14. Naming Compounds w/polyatomics
Name the ion that is not a polyatomic like simple cations or anions and then name the polyatomic as the chart says
NaOH = Sodium hydroxide
CaCO3 = Calcium carbonate

15. Polyatomic Ions
AlPO3
LiSCN
FeSO4
Mn(Cr2O7)2

16. Formula Writing w/polyatomics
Determine charge of overall polyatomic and then the other ion.
Follow same rules as before.
Beryllium cyanide
Copper (II) nitrate

17. Polyatomic Ions Barium sulfide Potassium oxalate
Chromium (III) cyanide
Vanadium (V)silicate