1. Nomenclature Chapter 5 1

2. Classifying Binary Compounds
Compounds containing a metal and a nonmetal are binary ionic
Type I and II
Compounds containing two nonmetals
Type III
Compounds containing H and a nonmetal = Acids 4

3. Type III - Binary Compounds of 2 Nonmetals
These binary compounds always start with a nonmetal or a metalloid. That’s the easiest way to identify them. They will contain no metals!
Name first element in formula first, use the full name of the element
Name the second element in the formula as if it were an anion
However, remember these compounds do not contain ions, so DO NOT USE THE CRISS-CROSS METHOD!!! 10

4. Type III Binary Molecular Compounds
Use a prefix in front of each name to indicate the number of atoms
Never use the prefix mono- on the first element
Prefixes: 1-mono, 2-di, 3-tri, 4-tetra,5-penta, 6-hexa, 7-hepta, 8-octa, 9-nona, 10-deca, 11-undeca, 12-dodeca.
To write the formula for binary molecular compounds, write the number next to the compound if there is a prefix, if not just write the symbol itself.

5. Binary Molecular Compounds Examples
Naming Compounds
SiF2 - silicon difluoride
C3Cl9 - tricarbon nonachloride
S4I7 – tetrasilicon heptaiodide
P5O10 – pentaphosphorus octoxide
Writing Formulas
Nitrogen trichloride – NCl3
Triphosphorus pentoxide - P3O5
Hexasulfur monofluoride - S6F
Diselenium pentabromide – Se2Br5

6. Metal Cations Type I Type II
Metals that can only have one possible charge
Determine charge by position on the Periodic Table
Type II
Metals that can have more than one possible charge
Determine metal cation’s charge from the charge on anion 6

7. Type II Binary Ionic Compounds
Contain Metal Cation + Nonmetal Anion
Metal listed first in formula & name
Name metal cation first, name nonmetal anion second
Metal cation name is the metal name followed by a Roman Numeral in parentheses to indicate its charge
Determine charge from anion charge
Common Type II cations in Table 5.2 (page 128 or on Week #3 Ions & Symbols List)
Nonmetal anion named by changing the ending on the nonmetal name to -ide 8

9. Naming Binary Type II Compounds
Cu+1 and N-3
Hg+2 and O-2
Cr+3 and P-3
Sn+4 and Cl-1
Ni+4 and S-2
Iron (III) phosphide
Manganese (II) fluoride
Gold (I) telluride
Lead (IV) bromide
Cobalt (III) arsenide

10. Ionic Compounds
Sometimes you can use the reverse of the criss-cross method to determine the charges for the transition metals.
When naming compounds, you do not need to tell how many atoms of each ion are present.

11. Naming Ionic Compounds Examples
Au2S
MnO
Fe3N2
CuCl2
NiS2
Cr3P2
PbF4
HgI

12. Figure 5.1: A flow chart for naming binary compounds.

13. Ionic Compounds
Ternary ionic compounds – contain atoms of three or more different elements, usually a polyatomic ion.
Writing the formulas for ternary compounds is done in the same way as binary compounds. The polyatomic ions stays together though.

14. Ionic Compounds
When you need more than one polyatomic ion in your formula, put parentheses around the ion, and how many of them you need outside the parentheses as a subscript.
NEVER MOVE SUBSCRIPTS OF THE IONS, ONLY THE CHARGES!!!

15. Writing Formulas for Ternary Ionic Compound Examples
Calcium sulfate
Ca+2 and SO4-2
Sodium chlorate
Na+1 and ClO3-1
Magnesium hydroxide
Mg+2 and OH-1
Potassium phosphate
K+1 and PO4-3
Iron (III) carbonate
Fe+3 and CO3-2
Tin (IV) chromate
Sn+4 and CrO4-2
Nickel (II) dihydrogen phosphate
Ni+2 and H2PO4-1
Chromium (III) sulfate
Cr+3 and SO4-2
Copper (II) acetate
Cu+2 and C2H3O2-1
Iron (II) permanganate
Fe+2 and MnO4-1

16. Ionic Compounds
When naming ternary compounds, name the cation (first symbol in the formula unless it is ammonium, NH4+1) first, and then the rest of the formula, which will only have one name, unless it contains hydrogen.

17. Naming Ternary Ionic Compounds
Ca(NO3)2
KClO3
BaSO3
AlPO4
CuOH
Ni3(PO3)4
Fe(CN)2
Mn(HCO3)3
Au2CO3
Cr2HPO4

18. Acids Naming & Writing Formulas for Acids
All acids begin with a hydrogen, and are neutral compounds.
In all acids, the cation is the hydrogen ion, H+1.
Anions change their endings when they become acids.

19. Acids -ide ions become hydro root ic acid
Ex: chloride becomes hydrochloric acid
-ate ions become root ic acid
Ex: nitrate becomes nitric acid
-ite ions become root ous acid
Ex: chlorite becomes chlorous acid

20. Acids Naming & Formula Writing Examples
Writing Formulas for Acids
Sulfuric acid
Hydroarsenic acid
Perchloric acid
Hypoiodous acid
Naming Acids
H3PO3 HI
HCN
H2C4H4O6

21. Hydrates
Hydrates are when you have a certain number of water molecules attached to a compound (usually an ionic compound)
The number of water molecules is shown after the formula for a compound and separated from the remainder of the compound by a dot.

22. Hydrates
Use the same prefixes as you did when naming binary molecular compounds to tell how many water molecules are present in a hydrate (1 = mono, 2 = di, …)
An anhydrous compound is one that contains no water molecules.

23. Hydrate Examples CuSO4 . 5H2O Mg(NO3)2 . 3 H2O
Barium chloride dihydrate
Ammonium acetate octahydrate

24. Basic Organic Compounds
You will need to know the names of the first 10 alkanes (hydrocarbons containing only single bonds).
The generic formula of these alkanes is:
CnH2n+2

25. Basic Organic Compounds
Methane – CH4
Ethane – C2H6
Propane – C3H8
Butane – C4H10
Pentane – C5H12
Hexane - C6H14
Heptane - C7H16
Octane - C8H18
Nonane - C9H20
Decane - C10H22