WRITING IONIC FORMULAS. Write the symbol for the cation, then the symbol for the anion. Balance the charges - use the crisscross method - by placing subscripts and “( )” for polyatomic ions if needed. Monatomic ions don’t need “( )”.
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Al3+ Cl1- Al3 Cl1 Don’t need to record “1”s
+3 -1 -1 -1 = 0
Cations can have more than one oxidation number.
Example: Cu+1 and Cu+2.
It is important to distinguish which ion is in the compound.
There are two ways used in chemistry.
Stock SystemClassical (Latin)
Cu+1 copper (I) cuprous
Cu+2 copper (II) cupric
Sn+2 tin(II) stannous
Sn+4 tin (IV) stannic
Hg2+2 mercury (I) mercurous
Hg+2 mercury (II) mercuric
The lower charge ends in –ous and the higher charge ends in –ic.
You are only responsible for only the Stock system but I just wanted you to see the other.
You are only responsible in class for the Stock system but I wanted to make you familiar with the classic.
cupric sulfate/copper (II) sulfate CuSO4
ferrous oxide/iron (II) oxide
cobaltic chloride/cobalt (III) chloride
mercurous nitrate/mercury (I) nitrate
You need to make sure that you can distinguish between ionic, covalent, and acid compounds.