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.


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


Compounds composed of 2 elements

Two types:

Compounds that contain a metal and nonmetal

Compounds that contain 2 nonmetals

To learn to name binary compounds of a metal and a nonmetal.


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


The cation is always named 1 st


The cation is named as the element name

Na + is sodium
The anion is named by taking the 1 st part of the element name and adding –ide

Cl is chloride








NaI
 sodium iodide
CaO
 calcium oxide
NaCl
 sodium chloride
KI
 potassium iodide
CaS
 calcium sulfide
CsBr
 cesium bromide
MgO
 magnesium oxide






CsF
 cesium fluoride
AlCl

3 aluminum chloride
MgI

2 magnesium iodide
Rb
2
O
 rubidium oxide
SrI
2
 strontium iodide
K
2
S
 potassium sulfide


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


What is FeCl
2
 made of?
Fe +2 and two Cl -

What would we name it?

Iron (II) chloride

What is PbO
2
 made of and what is its name?
Pb +4 and 2 O -2 called lead (IV) oxide


Write out the following and give their name





CuCl
 copper (I) chloride
HgO
 mercury (II) oxide
Fe
2

O
3 iron (III) oxide
MnO

2 manganese (IV) oxide
PbCl

4 lead (IV) chloride


CoBr
2

Co +2 + Br cobalt (II) bromide

CaCl
2

Ca +2 + Cl calcium chloride

Al
2
O
3

Al +3 + O -2 aluminum oxide

CrCl
3

Cr +3 + Cl chromium (III) chloride

To learn how to name binary compounds containing only nonmetals.





The 1 st element in the formula is named 1 st and the full element name is used.
The 2 nd 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 1 st element

Prefixes for Type III







 monoditritetrapentahexaheptaocta-
6
7
8
3
4
1
2
5


BF
3
 notice they are both nonmetals

Name the 1 st element – boron

Name the 2 nd as an anion – fluoride

Add prefixes
 boron trifluoride






NO
 nitrogen monoxide
N

2
O
3 dinitrogen trioxide
CCl

4 carbon tetrachloride
NO
2
 nitrogen dioxide
IF

3 iodine trifluoride





I
2

O
7 diiodine heptoxide
CO

2 carbon dioxide
CF

4 carbon tetrafluoride
NH

3 nitrogen trihydride
PCl

3 phosphorous trichloride

To review the naming of Type I, II, and III binary compounds.

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






AsF

3 arsenic trifluoride
Al

2
S
3 aluminum sulfide
SnBr

4 tin (IV) bromide
CS
2
 carbon disulfide
CdS
 cadmium sulfide





AgCl
 silver chloride
KI
 potassium iodide
NO
 nitrogen monoxide
P
2
O
5
 diphosphorous pentoxide
FeCl

3 iron (III) chloride

Naming compounds with polyatomic ions

Simply write the name of the polyatomic ion

No change is needed

What would NH
4
C
2
H
3
O
2

Look at the table be called?



NH
4
– ammonium
C
2
H
3
O
2
– acetate
Put the them together in the same order as the formula

Ammonium acetate

Naming compounds with polyatomic ions

If using a cation with more than one charge, use
Roman numerals


Fe(NO
3
)
3

The 2 nd 3 tells us that there are 3 NO
3 in the formula
Looking on our chart we see NO
3
 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






Na
2
SO
4
 sodium sulfate
KH
2
PO
4
 potassium dihydrogen phosphate
Mn(OH)
2

Manganese (II) hydroxide
Na
2
SO
3
 sodium sulfite
Cu(NO
3
)
2

Copper (II) nitrate




PbCO
3

Lead (II) carbonate
KHSO
4
 potassium hydrogen sulfate
NH
4
I
 ammonium iodide
NaCN
 sodium cyanide

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

1.
2.
3.
4.
5.
6.
7.
8.
9.
Name the following chemical compounds to be turned in for a grade
Na
2
CO
3
FeBr
3
PCl
3
CsClO
4
CuSO
4
NaHCO
3
BaSO
4
CsClO
4
BrF
5
13.
14.
15.
16.
17.
10.
11.
12.
NaBr
KOCl
Zn
3
(PO
4
)
2
Ca(HCO
3
)
MgI
2
2
KMnO
4
Sb
2
O
3
Fe(OH)
2

13.
14.
15.
16.
17.
9.
10.
11.
12.
7.
8.
5.
6.
3.
4.
1.
2.
Na
2
CO
3
FeBr
3
PCl
3
CsClO
4
CuSO
4
NaHCO
3
BaSO
4
CsClO
4
BrF
5
NaBr
KOCl
Zn
3
(PO
4
)
2
Ca(HCO
3
)
2
MgI
2
KMnO
4
Sb
2
O
3
Fe(OH)
2 sodium carbonate iron (III) bromide phosphorous trichloride cesium perchlorate copper (II) sulfate sodium hydrogen carbonate barium sulfate cesium perchlorate bromine pentafluoride sodium bromide potassium hypochlorite zinc (II) phosphate calcium hydrogen carbonate magnesium iodide potassium permanganate antimony (III) oxide iron (II) hydroxide

To learn how the anion composition determines the acid’s name
To learn names for common

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


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


If oxygen is present

Named after the anion present

When anion ends in –ate



Add suffix –ic and the word acid
H
2
SO
4 sulfate becomes sulfuric acid

When anion ends in –ite



Add suffix –ous and the word acid
HNO
2 nitrite becomes nitrous acid

hydro-
+anion root
+ -ic hydro(anion root)ic acid
Does the anion contain oxygen?
No Yes
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






HF

Hydrofluoric acid
H
3

PO
3
Phosphorous acid
HNO

3
Nitric acid
HBrO

3
Bromic acid
H
2
S

Hydrosulfuric acid

To learn to write the formula of a compound, given its name





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