1. III. Ionic Compounds (p. 176 – 180, 203 – 211)
Ch. 6 & 7 - Chemical Bonding
III. Ionic Compounds (p. 176 – 180, 203 – 211)

2. Formula Unit

3. A. Energy of Bond Formation
Lattice Energy
Energy released when one mole of an ionic crystalline compound is formed from gaseous ions

4. B. Lewis Structures Covalent – show sharing of e-
Ionic – show transfer of e-

5. B. Lewis Structures Covalent – show sharing of e-
Ionic – show transfer of e-

6. C. Ionic Nomenclature Ionic Formulas
Write each ion, cation first. Don’t 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 ion’s charge.

7. 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 ion’s charge if more than one is possible. Overall charge must equal zero.

8. 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!

9. C. Ionic Nomenclature
Common Ion Charges 1+ 2+ 3+ NA 3- 2- 1-

10. C. Ionic Nomenclature Writing Ionic Formulas: Calcium chloride
Ca2+ Cl1-
charges do not cancel, must criss-cross charges
Rewrite as complete formula without oxidation numbers
CaCl2 1 2

11. C. Ionic Nomenclature potassium chloride magnesium nitrate
copper(II) chloride
K+ Cl-
 KCl
Mg2+ NO3-
 Mg(NO3)2
Cu2+ Cl-
 CuCl2

12. C. Ionic Formulas calcium oxide aluminum chlorate Ca2+ O2-  CaO
magnesium chloride
Ca2+ O2-  CaO
Al3+ ClO3-  Al(ClO3)3
Mg2+ Cl-  MgCl2

13. C. Ionic Nomenclature NaBr Na2CO3 sodium bromide FeCl3
sodium carbonate
iron(III) chloride

14. D. Ionic Compounds with Transition Metals
For transition metals, valence electrons and oxidation #’s are variable
Exceptions: Sn (tin), Pb (lead), and Ag1+, Zn2+, Cd2+
Roman numerals indicate the oxidation #
Chromium (III) = Cr3+
Iron (II) = Fe2+
Lead (IV) = Pb4+

15. E. Naming Ionic Compounds with Transition Metals
Write the ox. # in parentheses using Roman numerals. To determine oxidation #, know that overall charge of compound = 0
Cr2O3
CrO
Chromium (III) oxide
3 x -2 = -6
2 x ___ = +6 -3
Chromium (II) oxide
2 x -2 = -4
2 x ___ = +4 +2

16. E. Ionic Formulas with Transition Metals
Copper (II) bromide
Tin (IV) oxide
Manganese (II) chloride
Cu2+ + Br -  CuBr2
Sn4+ + O2-  Sn2O4  SnO2
Mn2+ + Cl -  MnCl2

17. E. Ionic Names with Transition Metals
Cr2(SO4)3
HgO
FeCl3
Chromium (III) sulfate
Mercury (II) oxide
iron(III) chloride