• 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

• Type I
– 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 using the charge on anion

• 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 #2 Ions & Symbols List)
• Nonmetal anion named by changing the ending on the nonmetal name to -ide

• Cu +1 and N -3 • Iron (III) phosphide
• Hg +2 and O -2
• Cr +3 and P -3
• Sn +4 and Cl -1
• Ni +4 and S -2
• Manganous fluoride
• Gold (I) telluride
• Plumbic bromide
• Cobalt (III) arsenide

• 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.

• Au
2
S • NiS
2
• MnO
• Fe
3
N
2
• CuCl
2
• Cr
3
P
2
• PbF
4
• HgI

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!!!

Type III Binary Molecular Compounds
• Use a prefix in front of each name to indicate the number of atoms
• Never use the prefix monoon the first element but always put a prefix on the second element.
• Prefixes: 1-mono, 2-di, 3-tri, 4-tetra,5-penta,
6-hexa, 7-hepta, 8-octa, 9-nona, 10-deca, 11undeca, 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.

Naming Compounds
• SiF
2
Writing Formulas
• Nitrogen trichloride
• C
3
Cl
9
• Triphosphorus pentoxide
• S
4
I
7
• Hexasulfur monofluoride
• P
5
O
10
• Diselenium pentabromide

• 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.

• 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!!!

• Calcium hydrogen sulfate • Tin (IV) chromate
• Sodium chlorate • Nickel (II) dihydrogen phosphate
• Magnesium hydroxide
• Chromium (III) sulfate
• Potassium phosphate
• Copper (II) acetate
• Aluminum acetate
• Iron (II) permanganate

• When naming ternary compounds, name the cation (first symbol in the formula unless it is ammonium, NH
4
+1 ) first, and then the rest of the formula, which will only have one name, unless it contains hydrogen.

• Ca(NO
3
)
2
• KClO
3
• BaSO
3
• AlPO
4
• (NH
4
)
3
BO
3
• Ni
3
(PO
3
)
4
• Fe(CN)
2
• Mn(HCO
3
)
3
• Au
2
CO
3
• Cr
2
HPO
4

Naming Compounds Containing a metal with more than one possible charge and a
Polyatomic ion
• Ni
3
(PO
3
)
4
• CuOH
• Fe(CN)
2
• Mn(HCO
3
)
3
• Au
2
CO
3
• Cr
2
HPO
4
• Sn(SO
3
)
2
• Co
3
(BO
3
)
2
• Hg(C
2
H
3
O
2
)
2

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.

• -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

Naming Acids
Writing Formulas for Acids
• H
3
PO
3
• Sulfuric acid
• HI • Hydroarsenic acid
• HCN • Perchloric acid
• H
2
C
4
H
4
O
6
• Hypochlorous acid