Chapter 5: Molecules and Compounds
Date:____________
Section 3: Naming Ionic Compounds - Notes
Objectives:
 Distinguish between common and systematic names for compounds.
 Name binary ionic compounds containing a metal that forms only one type of ion.
 Name binary ionic compounds containing a metal that forms more than one type of ion.
 Name ionic compounds containing a polyatomic ion.
Naming Ionic Compounds:
 Identify if the metal cation has ____________________________________ potential charge.
o
Such metals are usually (but not always) found in the ____________________________
________________ section of the periodic table.
o
Notable Exceptions:

Always __________ and ____________

________ and _________ can have multiple charges
Binary Ionic Compounds:

Binary compounds are those that contain only ________________________________________
elements. The names for binary ionic compounds containing a metal that forms only one type of
ion have the following form
+

Since the charge of the metal is always the same for these types of compounds, it need not be
specified in the compound’s name.
o


Example: MgF2
Practice: Name these compounds:
o
CaO
o
MgCl2
o
Al2O3
o
Li3N
o
KF
Write the formula for these ionic compounds:
o
Potassium bromide
o
Sodium oxide
o
Zinc nitride

If the cation could have ___________________________________ charge, then the charge
must be specified in the metal’s name.
o

We specify the charge with a __________________________________ (in parentheses)
following the name of the metal.
For example, we distinguish between Cu+ and Cu2+ by writing a _______ to indicate the 1+ ion or
a _______to indicate the 2+ ion:
o
o

These compounds are named using the following form:
+


+
We can determine the charge of the metal from the chemical formula of the compound.
o
The sum of all the charges must be ________________.
o
What is the charge of iron in FeCl3?
o
What is the name for FeCl3?
Practice:
o
Name the following compounds:

PbCl4
o
Explain why CaO is not named calcium (II) oxide.
o
Write the formula for the following compounds:

Chromium (II) chloride

Tin (IV) oxide

Iron (III) oxide

PbO
Polyatomic Ionic Compounds:

Ionic compounds containing polyatomic ions are named using the same procedure we apply to
other ionic compounds, except that we use the name of the _____________________________
whenever it occurs.

For example, we name KNO3 using its cation, K+, ______________________, and its polyatomic
anion, NO3-, _________________.
o

KNO3
Practice:
o
Name the following compounds:

o

Fe(OH)2
NH4NO3
Write the formula for the following compounds:

barium nitrate

ammonium iodide

iron (III) hydroxide

Many polyatomic ions are ______________________, anions containing _________________.

When a series of oxyanions contain different numbers of oxygen atoms, they are named
systematically according to the ______________________________________ atoms in the ion.

If there are two ions in the series, the one with more oxygen atoms is given the ending _______
and the one with fewer is given the ending __________.
o

NO3−
SO42−
NO2−
SO32−
If there are more than two ions in the series, then the prefixes _______________, meaning “less
than,” and _____________, meaning “more than,” are used.
o
ClO −
BrO −
ClO2−
BrO2−
ClO3−
BrO3−
ClO4−
BrO4−

Practice:
o
Name the following compounds:

o
K2CrO4
Write the formula for the following compounds:

sodium perchlorate

sodium chlorite

sodium nitrate

sodium nitrite

Mn(NO3)2