Ch. 11 - Chemical Bonds

1
Ch. 11 - Chemical Bonds

• IV. Naming Ionic Compounds
• (p. 314-320)
• Oxidation Number
• Ionic Names
• Ionic Formulas

2
A. Oxidation Number

• The charge on an ion.
• Indicates the of e- gained/lost to become
  stable.

1
0
2
3
4
3-
2-
1-
3
B. Ionic Names

• Write the names of both elements, cation first.
• Change the anions ending to -ide.
• Write the names of polyatomic ions.
• For ions with variable oxidation s, write the
  ox. in parentheses using Roman numerals.
  Overall charge 0.

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B. Ionic Names

• NaBr
• Na2CO3
• FeCl3

• sodium bromide

• sodium carbonate

• iron(III) chloride

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C. Ionic Formulas

• Write each ion. Put the cation first.
• Overall charge must equal zero.
• If charges cancel, just write the symbols.
• If not, crisscross the charges to find
  subscripts.
• Use parentheses when more than one polyatomic ion
  is needed.
• Roman numerals indicate the oxidation .

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C. Ionic Formulas

• potassium chloride
• magnesium nitrate
• copper(II) chloride

• K Cl- ? KCl

• Mg2 NO3- ? Mg(NO3)2

• Cu2 Cl- ? CuCl2

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C. Ionic Formulas

• calcium oxide
• aluminum chlorate
• iron(III) oxide

• Ca2 O2- ? CaO

• Al3 ClO3- ? Al(ClO3)3

• Fe3 O2- ? Fe2O3