6'3 Ionic Compounds p' 190194, 219226

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6.3 Ionic Compounds(p. 190-194, 219-226)

• Ch. 6 7 - Chemical Bonding

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A. Energy of Bond Formation

• Lattice Energy
• Energy released when one mole of an ionic
  crystalline compound is formed from gaseous ions

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B. Lewis Structures

• Covalent show sharing of e-
• Ionic show transfer of e-

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B. Lewis Structures

• Covalent show sharing of e-
• Ionic show transfer of e-

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C. Ionic Nomenclature

• Ionic Formulas
• Write each ion, cation first. Dont show charges
  in the final formula.
• Overall charge must equal zero.
• If charges cancel, just write symbols.
• If not, use subscripts to balance charges.
• Use parentheses to show more than one polyatomic
  ion.
• Stock System - Roman numerals indicate the ions
  charge.

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C. Ionic Nomenclature

• Ionic Names
• Write the names of both ions, cation first.
• Change ending of monatomic ions to -ide.
• Polyatomic ions have special names.
• Stock System - Use Roman numerals to show the
  ions charge if more than one is possible.
  Overall charge must equal zero.

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C. Ionic Nomenclature

• Consider the following
• Does it contain a polyatomic ion?
• -ide, 2 elements ? no
• -ate, -ite, 3 elements ? yes
• Does it contain a Roman numeral?
• Check the table for metals not in Groups 1 or 2.
• No prefixes!

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C. Ionic Nomenclature

• Common Ion Charges

1
0
2
3
NA
3-
2-
1-
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C. Ionic Nomenclature

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

? KCl

• K Cl-

• Mg2 NO3-

? Mg(NO3)2
? CuCl2

• Cu2 Cl-

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C. Ionic Nomenclature

• NaBr
• Na2CO3
• FeCl3

• sodium bromide

• sodium carbonate

• iron(III) chloride

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D. Polyatomic Ions

• To find total of valence e-
• Add 1e- for each negative charge.
• Subtract 1e- for each positive charge.
• Place brackets around the ion and label the
  charge.

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D. Polyatomic Ions

• ClO4-

1 Cl 7e- 7e- 4 O 6e- 24e- 31e-
O O Cl O O
1e- 32e-
- 8e- 24e-
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D. Polyatomic Ions

• NH4

1 N 5e- 5e- 4 H 1e- 4e- 9e-
H H N H H
- 1e- 8e-
- 8e- 0e-