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

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Presentation on theme: "IIIIIIIV III. Ionic Compounds (p. 176 – 180, 203 – 211) Ch. 6 & 7 - Chemical Bonding."— Presentation transcript:

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

2 Formula Unit

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

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

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

6 C. Ionic Nomenclature Ionic Formulas zWrite each ion, cation first. Dont 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 ions charge.

7 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 ions charge if more than one is possible. Overall charge must equal zero.

8 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!

9 Common Ion Charges NA C. Ionic Nomenclature

10 zWriting Ionic Formulas: zCalcium chloride zCa 2+ Cl 1- zcharges do not cancel, must criss-cross charges zRewrite as complete formula without oxidation numbers zCaCl 2 2 1

11 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

12 zcalcium oxide zaluminum chlorate zmagnesium chloride Ca 2+ O 2 CaO Al 3+ ClO 3 Al(ClO 3 ) 3 Mg 2+ Cl MgCl 2 C. Ionic Formulas

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

14 D. Ionic Compounds with Transition Metals zFor transition metals, valence electrons and oxidation #s are variable Sn (tin), Pb (lead), and Ag 1+, Zn 2+, Cd 2+ yExceptions: Sn (tin), Pb (lead), and Ag 1+, Zn 2+, Cd 2+ zRoman numerals indicate the oxidation # yChromium (III) = Cr 3+ yIron (II) = Fe 2+ yLead (IV) = Pb 4+

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

16 zCopper (II) bromide zTin (IV) oxide zManganese (II) chloride yCu 2+ + Br - CuBr 2 ySn 4+ + O 2- Sn 2 O 4 SnO 2 yMn 2+ + Cl - MnCl 2 E. Ionic Formulas with Transition Metals

17 zCr 2 (SO 4 ) 3 zHgO zFeCl 3 yChromium (III) sulfate yMercury (II) oxide yiron(III) chloride E. Ionic Names with Transition Metals


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