A little humor for you..........
Two atoms walk into a bar.
One atom stops and says to the other, "I think I just lost an electron."
The second atom asks "Are you sure?"
The first atom replies, "I'm positive!"
Unit 6 - Nomenclature

How to use different naming conventions
based upon the type of compound
 Standard system for main group ionic cmpds
 Stock system for transition metal ionic cmpds
 Prefix system for molecules (non-metal/non-metal)

How to write formulas from names

Representative
Ionic
Compounds
Na2O
sodium oxide
Na2SO4
sodium sulfate

Cation
 Metal stays the same
as it appears on
Periodic Table

Anion
 monatomic, change the
ending to -ide
 polyatomic, use the
name of the polyatomic
ion –table given to you–
DON’T CHANGE
ANYTHING!
1. MgO
2. SrCl2
3. Al2S3
4. FrF
5. Na3N
6. LiBr
7. Ca2C
8. KI
9. Cs3As
10.Ba3P2
RbClO2 Rubidium chlorite
Aluminum phosphate
2. AlPO4
Calcium sulfite
3. CaSO3
4. FrBrO4 Francium perbromate
5. NaNO3 Sodium nitrate
6. Sr(ClO3)2 Strontium chlorate
7. BaCr2O7 Barium dichromate
8. CsC2H3O2 Cesium acetate
Potassium carbonate
9. K2CO3
Magnesium cyanide
10. Mg(CN)2
Magnesium oxide 1.
Strontium
chloride
Aluminum sulfide
Francium fluoride
Sodium nitride
Lithium bromide
Calcium carbide
Potassium iodide
Cesium arsenide
Barium phosphide

Transition
Metal Ionic
Compounds
Cu2O

 Metal remains unchanged
 Followed by charge of metal
in roman numerals

Copper (II)
sulfate
Anion
 Same rules as before
Copper (I) oxide
CuSO4
Cation

EXCEPTIONS:
 Zn+2, Ag+, Cd+2
 Sn & Pb (+2 or +4)
1. Find the charge of the anion
 How
does one
determine the
charge of the
transition
metal?
2. Calculate total negative
charges
3. Divide by the number of
cations
4. Write the roman number
corresponding to the charge
on the transition metal

Examples:
+3 total -3 total
+3
-1
CoCl3
Cobalt (III) chloride
1. Charge on Chlorine is 1
2.There are 3 chloride
ions, so 3 x -1 = -3
3. 3 ÷ 1 (# of Cobalt
atoms) = 3
4. 3 = III

1. Charge on phosphate
is -3
Examples:
+6 total -6 total
+2
-3
Ni3(PO4)2
Nickel (II) phosphate
2.There are two
phosphates, so…………..
2 x -3 = -6
3. 6 ÷ 3 (atoms of Ni) =2
4. 2 = II

Write the chemical compound name for:
 Na3N
 CaO
 KI
 Write the formula for:
 Aluminum Sulfide
 Strontium Chlorate
SnO
ScCl2
Co2S3
CuF
Pd3N2
MnBr7
RuI3
WS2
Ni3As4
Pb3P2
Tin (II) oxide
Scandium (II) chloride
Cobalt (III) sulfide
Copper (I) fluoride
Palladium (II) nitride
Manganese (VII)
bromide
Ruthenium (III) iodide
Tungsten (IV) sulfide
Nickel (IV) arsenide
Lead (II) phosphide
Co(NO3)3
AlP
Mn(SO4)2
NaF
Pb(CO3)2
KClO4
Ag2S
Ni(OH)2
CaCl2
CrO3
Cobalt (III) nitrate
Aluminum phosphide
Manganese (IV) sulfate
Sodium flouride
Lead (IV) carbonate
Potassium perchlorate
Silver (I) sulfide
Nickel (II) hydroxide
Calcium chloride
Chromium (VI) oxide

Steps to writing a 1. From the name, write
correct formula
the symbols
for ionic
compounds
2. Write the charges of
3.
4.
the ions above the
symbols
Reduce the charges to
the lowest whole number
ratio
Criss-cross the charges

Scandium (III)
chloride
No Reduction Necessary
+3
2.
-1
Sc Cl3
No
Number
if 1
1.
3.
4.
From the name,
write the symbols
Write the charges
of the ions above the
symbols
Reduce the charges
to the lowest whole
number ratio
Criss-cross the
charges

Calcium Oxide
+1
+2
2.
-1
-2
Ca O
No Number
if 1
1.
3.
No Number
if 1
4.
From the name,
write the symbols
Write the charges
of the ions above the
symbols
Reduce the charges
to the lowest whole
number ratio
Criss-cross the
charges
Sodium hydroxide
NaOH
Iron (II) bromide
FeBr2
Cobalt (III) sulfide
Copper (I) sulfate
Barium acetate
Co2S3
Cu2SO4
Lithium chlorite
Aluminum nitrite
Nickel (II) nitrate
Mercury (I) fluoride
Calcium dichromate
Ba(C2H3O2)2 Tin (IV) iodate
Potassium phosphide K P
3
Rhodium (V) cyanide Rh(CN)5
Lead (IV) oxide
Silver chloride
Sodium perbromate
PbO2
AgCl
NaBrO4
LiClO2
Al(NO2)3
Ni(NO3)2
HgF
CaCr2O7
Sn(IO3)4
Chromium (VI) sulfide CrS
Chromium (III) oxide
Strontium selenide
3
Cr2O3
SrSe

Covalently Bonded
Molecules

CO2
Carbon dioxide
P4O10
Tetraphosphorus
decoxide


Compounds are
named by using
prefixes to denote
the number of each
element
First non-metal
stays the same
Second non-metal
ending is changed to
-ide
Mono
1
Hexa
6
Di
2
Hepta
7
Tri
3
Octa
8
Tetra
4
Nona
9
Penta
5
Deca
10
Phosphorus pentachloride
PCl5
Sulfur trioxide
SO3
Hydrogen Fluoride
HF
Boron trichloride
BCl3
Carbon tetrachloride
CCl4
ICl3
Iodine trichloride
OF2
Oxygen difluoride
CO
Carbon monoxide
N2O4
Dinitrogen tetroxide