Transcript Chapter 6 Notes Part II Naming Ionic Compounds Naming Ionic Compounds For naming an ionic compound, 1) Name the metal. 2) Write the name of.

Chapter 6 Notes
Part II
Naming Ionic Compounds
Naming Ionic Compounds
For naming an ionic compound,
1) Name the metal.
2) Write the name of the nonmetal, and change the end to
–ide.
Naming Ionic Compounds
 Example:
NaBr
 Sodium bromide
 Example: CaF2
 Calcium fluoride
Polyatomic Ions
 Polyatomic
ion – a charged
covalently bonded group of
atoms
-2
 Example: Sulfate SO4
Naming Ionic Compounds
If there is a polyatomic anion,
then you do not change the
ending:
Ex) Na2SO4 – Sodium sulfate
Name these:
Na2O
MgCl2
Na2CO3
Name these:
Na2O – sodium oxide
MgCl2 – magnesium chloride
Na2CO3 – sodium carbonate
Naming Ionic Compounds
3) If a positive ion (a metal) can
have more than one oxidation
number, you have to designate
its charge in the name!
Naming Ionic Compounds
We do this by putting the
charge as a roman numeral in
parenthesis between the
positive and negative ion.
Naming Ionic Compounds
Why do we need to do that?
Name: Fe2O3 and FeO
These both exist in nature, so
we have to show which one
we mean.
Naming Ionic Compounds
Use the reverse of the criss
cross to figure out the charge
of the positive ion.
 Fe2O3 is Iron III Oxide
 FeO is Iron II Oxide
Naming Ionic Compounds
Metals that don’t need
parentheses:
Group I, II and IIIA
Zn, Cd (always +2)
Ag (always +1)
Naming Ionic Compounds
Which means transition, inner
transition and other metals
do need parentheses!
Naming Ionic Compounds
1. Name the positive ion.
2. Does it need a roman
numeral?
If so, reverse criss cross, if not,
ignore.
Naming Ionic Compounds
 Name
 If
the negative ion and:
a nonmetal end in -ide; if a
polyatomic ion, end normally.
Name these:
Na2S
CuCl2
K2SO4
Pb(NO3)3
Name these:
Na2S – sodium sulfide
CuCl2 – copper chloride
K2SO4 – potassium sulfate
Pb(NO3)3 – lead nitrate