Rules Sheet For Naming Binary Ionic Compounds
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1
2Rules for Naming Binary Ionic Compounds
Examples:
NaCl – sodium chloride BaF
– barium fluoride
2
CuO – copper (II) oxide
1. The full name of the cation is listed first. (A cation is a positive ion).
2. The root of the anion name is listed second and is followed by the suffix
“ide.”(An anion is a negative ion).
3. If the compound contains a transition metal, a Roman numeral is included after
the cation name to indicate the oxidation number of the metal.
4. Remember that the cation(s) and anion(s) combine in the simplest ratio that
balances the charge. That is, the sum of the charge must be equal to zero in the
compound formed.
Rules for Naming Ionic Compounds Containing
Polyatomic Ions
Examples:
CaCO
- calcium carbonate
Fe(OH)
-iron (III) hydroxide
3
3
(NH
)
SO
– ammonium sulfate
4
2
4
1. The full name of the cation is listed first.
2. The full name of the anion is listed second.
3. Use the table below for common polyatomic ions
4. Remember that the cation(s) and anion(s) combine in the simplest ratio that
balances the charge. That is, the sum of the charge must be equal to zero in the
compound formed.
5. Finally, use parentheses when the simplest ratio requires more than one
polyatomic ion in the compound formula.
Common Polyatomic Ions (these ions are also on pages 42 and 43 in the text).
+1
-1
-2
-3
-
CH
COO
(acetate)
+
3-
3
NH
PO
-
2-
4
4
CN
(cyanide)
CO
(carbonate)
3
(ammonium)
(phosphate)
-
OH
(hydroxide)
-
2-
NO
(nitrate)
SO
(sulfate)
3
4
-
2-
NO
(nitrite)
SO
(sulfite)
2
3
-
ClO
(hypochlorite)
-
2-
ClO
(chlorite)
CrO
(chromate)
2
4
-
ClO
(chlorate)
3
-
2-
ClO
(perchlorate)
Cr
O
(dichromate)
4
2
7
-
2-
MnO
(permanganate)
HPO
(hydrogen phosphate)
4
4
-
HCO
(hydrogen carbonate
3
or bicarbonate)
-
H
PO
(dihydrogen
2
4
phosphate)
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