1. Ionic Compound Nomenclature

2. Binary Ionic Compounds Nomenclature w/ oxidation numbers
The name of the cation (metal) is first. It will have its entire element name.
The anion (nonmetal) will have its element name with its –ide ending
For example
NaCl
Sodium chloride

3. Try these examples ZnS Zinc Sulfide KCl Potassium Chloride BaO
AlF3
CaO
Zinc Sulfide
Potassium Chloride
Barium Oxide
Aluminum Fluoride
Calcium Oxide

4. Oxidation Numbers Group 1 (IA) +1 Group 2 (IIA) +2 Group 13 (IIIA) +3
Group 14 (IVA) ±4
Group 15 (VA) -3
Group 16 (VIA) -2
Group 17 (VIIA) -1

5. Criss Cross/Swap & Drop Method
Write the symbol and charge for each element.
The anion’s charge becomes the # of cations
The cation’s charge becomes the # of anions
Reduce if necessary. (if there is a common factor)

6. For example
Calcium chloride
Ca Cl 1-
cation anion
CaCl2

7. For example
Barium sulfide
Ba S 2-
cation anion
Ba2S2
Reduce.
BaS

8. Example KCl potassium chloride K 1+ Cl 1- cation anion
The charge of your anion = the # of cations K1
The charge of your cation = the # of anions Cl1
Reduce if necessary
KCl

9. Try these examples Lithium oxide Potassium sulfide Sodium iodide
Magnesium Nitride
Rubidium Phosphide

10. Writing Formulas without Oxidation Numbers

11. Writing Formulas without Oxidation Numbers
The charge of transition metals will be given in parenthesis.
Iron (III) oxide
Fe3+ O2-
Use the criss cross method.
Fe2O3

12. Try these examples Copper (II) iodide Tin (II) chloride Tin (IV) oxide
Chromium (VI) sulfide

13. Naming Binary Ionic Compounds without oxidation numbers

14. Naming Binary Ionic Compounds without oxidation numbers
*Use your reference sheet to determine ions of different transition metals.
The cation (metal) will have its entire name with its charge in parentheses.
The anion will have its element name with its –ide ending.
You will need to reverse the criss cross method to find the cations charge.

15. Example CoI2 CoX1 I1-2 1(x) + (1-)(2) = 0 1x - 2=0 X= 2+
Cobalt (?) iodide
Use the criss cross method in reverse.
Write the element symbols with their subscripts and the charge of the anion.
CoX1 I1-2
Set up an equation equal to zero using the charges and number of each element. The charge of the cation is x (unknown). Then solve for x.
1(x) + (1-)(2) = 0
1x - 2=0
X= 2+

16. Try these examples Cu2Se FeS SnO2 Copper (I) selenide
Iron (II) sulfide
Tin (IV) oxide

17. Tertiary Ionic Compound Nomenclature

18. Tertiary Ionic Compounds
Composed of
positively charged Polyatomic ion + nonmetal (anion)
Metal (cation) + negatively charged polyatomic ion
Two polyatomic ions (one positive and one negative charge)

19. Writing Formulas with oxidation #s
Write symbol and charge for each element or polyatomic ion
Use the crisscross method.
Polyatomic ions must remain in parenthesis with the amount written outside as a subscript.
i.e. 2 nitrate ions (NO3)2

20. Try these examples
Magnesium hydroxide
Potassium sulfate

21. Naming Must be able to recognize polyatomic ions.
Name the cation and (-) charge poly ion
Name the (+)polyatomic ion and name the anion.
Name both polyatomic ion.

22. Example
CaCr2O4
KClO3
Calcium dichromate
Potassium chlorate

23. Naming Formulas without Oxidation Numbers
Must include charge of the cation (transition metal).
Will only include the tertiary ionic compounds with a cation (transition metal) and polyatomic ion.
Name the cation with its charge. May require using the criss cross method reversed.
Name the polyatomic ion.

24. The charge of your cation is the number of anions.
Example: Sn3(PO4)2
The charge of your cation is the number of anions. Or
SnX3 (PO4)3-2
3x + (3-)(2)=0
3x-6=0
3x=6
X=2+
Tin (II) phosphate

25. Try this One:
Pb(C2H3O2)2
Lead (II) acetate

26. Writing Formulas Without Oxidation Numbers
Write elements or polyatomic ions with charges
Use the criss cross method
Chromium (III) nitrate
Cr 3+ NO31-
Cr(NO3)3
(3+)(1) + (1-)(3)=0

27. Try these examples Mercury (II) hydroxide Iron (III) chlorate Hg(OH)2
Fe(ClO3)3