1. IIIIIIIV III. Ionic Compounds Chemical Bonding

2. A. Energy of Bond Formation zLattice Energy yEnergy released when one mole of an ionic crystalline compound is formed from gaseous ions

3. B. Lewis Structures zCovalent – show sharing of e - zIonic – show transfer of e -

4. B. Lewis Structures zCovalent – show sharing of e - zIonic – show transfer of e -

5. C. Ionic Nomenclature Ionic Formulas zWrite each ion, cation first. Don’t show charges in the final formula. zOverall charge must equal zero. yIf charges cancel, just write symbols. yIf not, use subscripts to balance charges. zUse parentheses to show more than one polyatomic ion. zStock System - Roman numerals indicate the ion’s charge.

6. C. Ionic Nomenclature Ionic Names zWrite the names of both ions, cation first. zChange ending of monatomic ions to -ide. zPolyatomic ions have special names. zStock System - Use Roman numerals to show the ion’s charge if more than one is possible. Overall charge must equal zero.

7. C. Ionic Nomenclature zConsider the following: yDoes it contain a polyatomic ion? x-ide, 2 elements  no x-ate, -ite, 3+ elements  yes yDoes it contain a Roman numeral? xCheck the table for metals not in Groups 1 or 2. yNo prefixes!

8. Common Ion Charges 1+ 2+3+NA3-2-1- 0 C. Ionic Nomenclature

9. zpotassium chloride zmagnesium nitrate zcopper(II) chloride  K + Cl   Mg 2+ NO 3   Cu 2+ Cl   KCl  Mg(NO 3 ) 2  CuCl 2 C. Ionic Nomenclature

10. zNaBr zNa 2 CO 3 zFeCl 3 ysodium bromide ysodium carbonate yiron(III) chloride C. Ionic Nomenclature