1. Nomenclature Learn to name binary compounds of a metal and a nonmetal.
Learn how to name binary compounds containing only nonmetals.
Learn the names of common polyatomic ions and how to use them in naming compounds.
Learn names for common acids and how the anion composition determines the acids name.
Learn to write the formula of a compound, given its name.

2. Naming compounds
Common names are Epsom salts, milk of magnesia, laughing gas, and many more
There are over 4 million different compounds and more are discovered all the time
Memorizing the common names would be impossible so we have a system

3. Binary compounds Compounds composed of 2 elements Two types:
Compounds that contain a metal and nonmetal
Compounds that contain 2 nonmetals

4. Naming Compounds That Contain a Metal and a Nonmetal
To learn to name binary compounds of a metal and a nonmetal.

5. Binary Ionic Compound
Contain a positive ion (cation) and a negative ion (anion)
Two types of binary ionic compounds
Type I: contain elements with only one ion
Na+, Cs+, Ca+2, etc
Type II: contain elements with 2 or more ions
Cr+2 or Cr+3, Cu+ or Cu+2

6. Type I Binary Ionic Compounds
The cation is always named 1st
The cation is named as the element name
Na+ is sodium
The anion is named by taking the 1st part of the element name and adding –ide
Cl- is chloride

7. Type I Binary Ionic Compounds
NaI
sodium iodide
CaO
calcium oxide
NaCl
sodium chloride KI
potassium iodide
CaS
calcium sulfide
CsBr
cesium bromide
MgO
magnesium oxide
CsF
cesium fluoride
AlCl3
aluminum chloride
MgI2
magnesium iodide
Rb2O
rubidium oxide
SrI2
strontium iodide
K2S
potassium sulfide

8. Type II Binary Ionic Compounds
Some metals can produce 2+ ions
When this happens, we use Roman Numerals
The Roman numerals only tell us the charge, not how many of that ion there are in the compound
You do not need to use Roman numeral for metals that form only 1 cation

9. Type II Binary Ionic Compounds
What is FeCl2 made of?
Fe+2 and two Cl-
What would we name it?
Iron (II) chloride
What is PbO2 made of and what is its name?
Pb+4 and 2 O-2 called lead (IV) oxide

10. Type II Binary Ionic Compounds
Write out the following and give their name
CuCl
copper (I) chloride
HgO
mercury (II) oxide
Fe2O3
iron (III) oxide
MnO2
manganese (IV) oxide
PbCl4
lead (IV) chloride

11. Review Type I and II CoBr2 CaCl2 Al2O3 CrCl3
Co+2 + Br- cobalt (II) bromide
CaCl2
Ca+2 + Cl- calcium chloride
Al2O3
Al+3 + O-2 aluminum oxide
CrCl3
Cr+3 + Cl- chromium (III) chloride

12. Naming Binary Compounds That Contain Only Nonmetals (Type III)
To learn how to name binary compounds containing only nonmetals.

13. Rules for naming Type III
The 1st element in the formula is named 1st and the full element name is used.
The 2nd element is named as though it were an anion.
Prefixes are used to indicate the # of atoms present
The prefix mono- is never used for the 1st element
Prefixes for Type III
mono- 1
di- 2
tri- 3
tetra- 4
penta- 5
hexa- 6
hepta- 7
octa- 8

14. Type III BF3 notice they are both nonmetals
Name the 1st element – boron
Name the 2nd as an anion – fluoride
Add prefixes
boron trifluoride

15. Practice Problems NO N2O3 CCl4 NO2 IF3 I2O7 CO2 CF4 NH3 PCl3
nitrogen monoxide
N2O3
dinitrogen trioxide
CCl4
carbon tetrachloride
NO2
nitrogen dioxide
IF3
iodine trifluoride
I2O7
diiodine heptoxide
CO2
carbon dioxide
CF4
carbon tetrafluoride
NH3
nitrogen trihydride
PCl3
phosphorous trichloride

16. Naming Binary Compounds: A Review
To review the naming of Type I, II, and III binary compounds.

17. Naming binary compounds
Yes
Metal Present? No
Yes
Type III: Use prefixes
Does the metal form more than one cation?
Yes No
Type II: Determine the charge of the cation; use a Roman numeral after the cation
Type I: Use the element name for the cation

18. Type I, II, III AsF3 Al2S3 SnBr4 CS2 CdS AgCl KI NO P2O5 FeCl3
arsenic trifluoride
Al2S3
aluminum sulfide
SnBr4
tin (IV) bromide
CS2
carbon disulfide
CdS
cadmium sulfide
AgCl
silver chloride KI
potassium iodide NO
nitrogen monoxide
P2O5
diphosphorous pentoxide
FeCl3
iron (III) chloride

19. Naming compounds with polyatomic ions
Simply write the name of the polyatomic ion
No change is needed
What would NH4C2H3O2 be called?
Look at the table
NH4 – ammonium
C2H3O2 – acetate
Put the them together in the same order as the formula
Ammonium acetate

20. Naming compounds with polyatomic ions
If using a cation with more than one charge, use Roman numerals
Fe(NO3)3
The 2nd 3 tells us that there are 3 NO3 in the formula
Looking on our chart we see NO3 has a charge -1
If they’re totaled, that makes our total charge -3
Fe must be +3 to cancel it out
Iron (III) nitrate

21. Polyatomic Practice Na2SO4 KH2PO4 Mn(OH)2 Na2SO3 Cu(NO3)2 PbCO3 KHSO4
sodium sulfate
KH2PO4
potassium dihydrogen phosphate
Mn(OH)2
Manganese (II) hydroxide
Na2SO3
sodium sulfite
Cu(NO3)2
Copper (II) nitrate
PbCO3
Lead (II) carbonate
KHSO4
potassium hydrogen sulfate
NH4I
ammonium iodide
NaCN
sodium cyanide

22. Naming Chemical Compounds
Binary Compound?
Yes No
Metal Present?
Polyatomic Ion or Ions Present?
Yes No No
Yes
Type III: Use prefixes
Does the metal form more than one cation?
We will learn this procedure later.
Name the compound similar to naming binary compounds but use the polyatomic chart for their names No
Yes
Type I: Use the element name for the cation
Type II: Determine the charge of the cation; use a Roman numeral after the cation

23. Name the following chemical compounds to be turned in for a grade
Na2CO3
FeBr3
PCl3
CsClO4
CuSO4
NaHCO3
BaSO4
BrF5
NaBr
KOCl
Zn3(PO4)2
Ca(HCO3)2
MgI2
KMnO4
Sb2O3
Fe(OH)2

24. Na2CO3 sodium carbonate
FeBr3 iron (III) bromide
PCl3 phosphorous trichloride
CsClO4 cesium perchlorate
CuSO4 copper (II) sulfate
NaHCO3 sodium hydrogen carbonate
BaSO4 barium sulfate
BrF5 bromine pentafluoride
NaBr sodium bromide
KOCl potassium hypochlorite
Zn3(PO4)2 zinc (II) phosphate
Ca(HCO3)2 calcium hydrogen carbonate
MgI2 magnesium iodide
KMnO4 potassium permanganate
Sb2O3 antimony (III) oxide
Fe(OH)2 iron (II) hydroxide

25. Naming Acids
To learn how the anion composition determines the acid’s name
To learn names for common

26. Acids A molecule w/ one or more H+ ions attached to an anion
The rules for naming acids depend on whether it has oxygen

27. Rules for naming acids If no oxygen is present
Add prefix hydro- and suffix –ic to the root word and the word acid to the end
HCl
hydro + chlorine + ic + acid
hydrochloric acid

28. Rules for naming acids If oxygen is present
Named after the anion present
When anion ends in –ate
Add suffix –ic and the word acid
H2SO4
sulfate becomes sulfuric acid
When anion ends in –ite
Add suffix –ous and the word acid
HNO2
nitrite becomes nitrous acid

29. Naming Acids Does the anion contain oxygen? No Yes hydro- +anion root
+ -ic
hydro(anion root)ic acid
Check the ending of the anion name
-ite
-ate
anion or element root
+ -ous
(root)ous acid
anion or element root
+ -ic
(root)ic acid

30. Acid Practice HF H3PO3 HNO3 HBrO3 H2S Hydrofluoric acid
Phosphorous acid
HNO3
Nitric acid
HBrO3
Bromic acid
H2S
Hydrosulfuric acid

31. Writing Formulas from Names
To learn to write the formula of a compound, given its name

32. Formulas from names
So far you were given a name and you gave the formula
A lot of times the reverse is also necessary
calcium hydroxide
Ca+2 OH-
You will need 2 hydroxide ions to cancel out the +2 charge of Ca
Ca(OH)2
iron (II) oxide
Fe+2 O-2
The +2 and -2 cancel each other out
FeO