Ionic and
Covalent

Naming Ionic Compounds
 List the cation 1 st .
 The name of the cation is just the name of the element.
 If there is a number in parenthesis (ex.(II) ), that just represents the oxidation number for the cation.
 List the anion 2 nd .
 The name of the anion is the name of the element with the ending taken off and “-ide” added.
 Make sure that when writing name to formula, the oxidation numbers of the formula add up to
ZERO.

Ionic Compounds: You Try!
 K
2
O
 NaF
 sodium sulfide
 calcium bromide
 iron (II) oxide

Ionic Compounds: You Try!
 K
2
O
 NaF
Potassium Oxide
Sodium Flouride
 sodium sulfide
 iron (III) oxide
Na
2
S
 calcium bromide CaBr
2
Fe
2
O
3

Naming Covalent Compounds
 When naming Ionic compounds we simply changed the anions ending to – ide.
 With covalent compounds the naming is a little different…
 We know must consider the number of atoms that make up the compounds

Naming Covalent Rules
1.
2.
3.
The element with the lower group number is written first in the name.
If both elements are in the same group, the element with the higher period number is written first.
The second element in the name is given the suffix –ide

Naming Covalent Rules Continued…
4.
Greek prefixes are used to indicate the number of atoms of each atom in the
compound.
You don’t have to write mono in front of the first element if there is only one.
 Prefixes
3
4
1
2
5 monoditritetrapenta-
8
9
6
7
10 hexaheptaoctanonadeca-

Naming Covalent Rules Continued…
5. If there are only carbons and hydrogens, the carbons will be listed first.

Practice
 What is the name for HF
 Lowest group number?
 Suffix of second atom?
 Prefixes?
 Final answer: Hydrogen monoflouride!

More Practice
1.
N
2
H
6
2.
Disulfur tetrachloride

More Practice
1.
1.
N
2
H
6
Dinitrogen heptahydride
2.
1.
Disulfur tetrachloride
S
2
Cl
4