Naming Ionic Compounds
Learning the Language of
Chemistry
Naming Ionic Compounds

Ionic Compounds are composed of two parts.


Metal (Positive, Cation)
Non-Metal (Negative, Anion)
Naming Ionic Compounds

There are two types of Ionic compounds:

Binary Ionic Compounds


Ternary Ionic Compounds


Two ions present (one metal and one non-metal)
Three or more elements (one metal and one
polyatomic ion)
When combining ions to form an ionic
compound it must have a net charge of
ZERO!
Naming Ionic Compounds

Calcium and Oxygen



Calcium has what
charge when it
becomes an ion?
Oxygen has what
charge when it
becomes an ion?
What ratio will these
two ions combine to
form a compound?
(Remember the
charges must add up to
equal zero!)
Ca2+
O2-
CaO
The charges
cancel each other
out!
+2 + (-2) = 0
Naming Ionic Compounds

Barium and Nitrogen



Barium has what
charge when it
becomes an ion?
Nitrogen has what
charge when it
becomes an ion?
What ratio will these
two ions combine to
form a compound?
(Remember the
charges must add up to
equal zero!)
Ba2+
N3-
Ba3N2
The charges
cancel each other
out!
3(+2) + (2(-3)) = 0
Naming Ionic Compounds

When naming binary ionic
compounds:
1.
2.
You first name the cation (metal, positive),
which is the same name as the element
Second you name the anion (non-metal,
negative) with the ending –ide
Naming Ionic Compounds
NaCl
Sodium Chloride
CaCl2
Calcium Chloride
Sr3N2
Strontium Nitride
Naming Ionic Compounds
Acetate- C2H3O2Nitrite- NO2 Nitrate- NO3 Silicate- SiO32 Cyanide- CN Phosphate- PO43 Phosphite- PO33 Ammonium- NH4+
 Hydrogen carbonate or
bicarbonate- HCO3 Dichromate- Cr2O72 Chromate- CrO42

Carbonate- CO32Oxalate- C2O42 Permanganate- MnO4 Sulfate- SO42 Sulfite- SO32 Hydroxide- OH Hypochlorite- ClO Chlorite- ClO2 Chlorate- ClO3 Perchlorate- ClO4

Naming Ionic Compounds

Barium and Nitrate



Barium has what
charge when it
becomes an ion?
Nitrate has what charge
when it becomes an
ion?
What ratio will these
two ions combine to
form a compound?
(Remember the
charges must add up to
equal zero!)
Ba2+
NO3-
Ba(NO3)2
The charges
cancel each other
out!
+2 + (2(-1)) = 0
We use () to
keep the
polyatomic
together and
show the
number of
nitrates
present
Naming Ionic Compounds

When naming Ternary ionic compounds
1.
2.
You first name the cation (metal, positive),
which is the same name as the element
Second you name the polyatomic anion
(non-metal, negative) with the ending of
either –ite or –ate (some polyatomics do
end in –ide)
Naming Ionic Compounds
NaNO3
Sodium nitrate
CaCO3
Calcium carbonate
Ba(OH)2
Barium hydroxide
Naming Ionic Compounds

But what about those pesky transition
metals?


Those ions that have more than one
possible charge?
We use Roman numerals to describe the
charge!

Example: Iron (III) ion
Naming Ionic Compounds
Iron (III) oxide
Fe2O3
Iron (II) oxide
FeO
Copper (II) nitrate
Cu(NO3)2