1. Nomenclature
Chapter 9

2. Chemical Formula Chemical Formulas tell two things: Letters = elements
Subscripts = # of atoms of each element
Ex. Fe2O3 2 iron atoms & 3 oxygen atoms
CaCO3  # elements?
# atoms?
Al2(SO4)3  # elements? 3 5 3 17

3. Compounds Binary compound  has 2 elements
Ex. NaCl
Ternary compound  has 3 elements
NaNO3

4. Review of Ionic Compounds
Attraction of (+) and (-) ions. (transfer e-)
Metal loses e-  (+)
Nonmetal gains e-  (-)
Cation (metal) is written FIRST!!
The OVERALL charge of the compound is ZERO.

5. Binary Ionic Names How do you know it’s binary ionic? metal + nonmetal
Rules:
1) Name the first element as it is on
the periodic table.
2) Change the ending of the second
element to “ide”.
3) Check if the metal is a transition
metal. If so, figure out the charge on
it and use Roman numerals to show the
CHARGE.

6. Binary Ionic Naming Examples
sodium bromide
NaBr 
CaCl2 
Cu2O 
Fe2O3 
K2S 
Sr3P2 
CoBr 
Mn3N 
calcium chloride
copper (I) oxide
iron (III) oxide
potassium sulfide
strontium phosphide
cobalt (I) bromide
manganese (I) nitride

7. Binary Ionic Naming Exceptions
Lead (Pb) and Tin (Sn) are not transition metals, but THEY DO NEED ROMAN NUMERALS!!
Silver (Ag) and Zinc (Zn) are transition metals, but DO NOT NEED ROMAN NUMERALS!
Sliver is ALWAYS +1
Zinc is ALWAYS +2

8. Binary Ionic Formulas Rules: 1) Write the element symbols.
2) Write the oxidation #s (charges).
* If it’s a transition metal, you won’t know
the charge – so look at the Roman
numeral!
3) Criss-cross the charges down.
4) Simplify the ratio if needed.

9. Binary Ionic Formula Examples
Write the formula for each name:
copper (II) oxide
zinc bromide
copper (I) oxide
barium chloride
lead (IV) sulfide
calcium nitride
iron (III) sulfide
aluminum fluoride
silver oxide
CuO
ZnBr2
Cu2O
BaCl2
PbS2
Ca3N2
Fe2S3
AlF3
Ag2O

10. Ternary Ionic Compounds
Involve polyatomic ions (group of atoms with an overall charge)
Most polyatomic ions have “ite” or “ate”, meaning oxygen is in it.
Treat the polyatomic ion as a unit and never change its name!! (Don’t use “ide” for it.)
Put polyatomic ions in parentheses unless the subscript is 1.
NEVER change the subscripts within the polyatomic ion!!

11. Naming Ternary Ionic Compounds
1) Name the (+) ion.
2) Name the (-) ion (no “ide” if it’s a polyatomic ion!).
3) Use Roman numerals if the metal is a transition metal, lead or tin.

12. Name Ternary Ionic Examples
BaSO4
NH4OH
Cu(NO3)2
Fe2(CO3)3
KNO3
Co(OH)2
barium sulfate
ammonium hydroxide
copper (II) nitrate
iron (III) carbonate
potassium nitrate
cobalt (II) hydroxide

13. Writing Formulas for Ternary Ionic Compounds
Use the same criss-cross method as with binary compounds.
Remember to use ( ) if the subscript of a polyatomic ion is more than 1! (Watch out for hydroxide!)

14. Ternary Ionic Formula Examples
Write the formula for each:
aluminum sulfate
ammonium carbonate
tin (IV) phosphate
sodium nitrite
zinc hydroxide
potassium sulfite
Al2(SO4)3
(NH4)2CO3
Sn3(PO4)4
NaNO2
Zn(OH)2
K2SO3

15. Molecular Compounds Review of Molecular Compounds:
Involves a sharing of e-
Molecules can exist independently
Covalently bonded
How do you know it’s molecular?
All nonmetals!

16. Naming Molecular Compounds
Use prefixes to indicate the number of atoms.
1 Exception: Do NOT begin a name with “mono”.
Change the ending of the second element to “ide”.
mono 1
hexa 6 di 2
hepta 7
tri 3
octa 8
tetra 4
nona 9
penta 5
deca 10

17. Naming Molecular Compounds - Examples
N2O
carbon monoxide
carbon dioxide
diphosphorous pentoxide
tetraphosphorous decoxide
dinitrogen monoxide

18. Molecular Formulas The prefix tells you what subscript to write.
Remember if there is no prefix for the first element, it is “mono”.

19. Molecular Formula Examples
dinitrogen monoxide
sulfur trioxide
dinitrogen pentoxide
nitrogen trihydride
pentaphosphorous decoxide
N2O
SO3
N2O5
NH3
P5O10

20. When you look at a compound:
First – Decided if it’s ionic or molecular!! * Ionic m – nm polyatomic ions * Molecular nm - nm

22. Acids What is an acid? How do you know something is an acid?
An aqueous solution (in water) of hydrogen compounds
How do you know something is an acid?
It starts with H

23. Binary Acids Binary acid  Includes H + one other element. (Ex. HBr)
To name: “hydro ic acid”

24. Naming Binary Acid Examples
HCl
HBr
H2S
hydrochloric acid
hydrobromic acid
hydrosulfuric acid

25. Binary Acid Formulas Don’t forget to use the criss-cross method!
Examples:
hydroiodic acid
hydrofluoric acid
hydrophosphoric acid HI HF
H3P

26. Ternary Acids Ternary acid  H + polyatomic ion. (Ex. HNO3)
If the polyatomic ion’s name ends in “ate”, the acid’s name ends in “ic”.
(I “ate” it and it made me s”ic”k.)
If the polyatomic ion’s name ends in “ite”, the acid’s name ends in “ous”.

27. Naming Ternary Acids phosphoric acid sulfurous acid sulfuric acid
H2CO3
HNO2
HNO3
H3PO4
H2SO3
H2SO4
carbonic acid
nitrous acid
nitric acid

28. MEMORIZE THESE!! Hydrochloric acid – HCl Nitric acid – HNO3
Sulfuric acid – H2SO4
Acetic acid – HC2H3O2 or CH3COOH