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III. Ionic Compounds (p. 210 – 224) Ch. 7 - Chemical Bonding.

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Presentation on theme: "III. Ionic Compounds (p. 210 – 224) Ch. 7 - Chemical Bonding."— Presentation transcript:

1 III. Ionic Compounds (p. 210 – 224) Ch. 7 - Chemical Bonding

2 Formula Unit

3 A. Energy of Bond Formation Lattice Energy –

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

5 C. Ionic Nomenclature Ionic Formulas Write each ion, _________ first. Dont show charges in the final formula. Overall charge must equal _________. –If charges cancel, just write symbols. –If not, use subscripts to balance charges. Use parentheses to show more than one _____________ _______. Stock System - ___________ __________ indicate the ions charge.

6 C. Ionic Nomenclature Ionic Names Write the names of both ions, ________ first. Change ending of monatomic ions to -_____. Polyatomic ions have special names. (listed on the chemical reference sheets!) Stock System - Use ________ __________ to show the ions charge if more than one is possible. Overall charge must equal zero.

7 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!

8 Common Ion Charges ±4± C. Ionic Nomenclature

9 potassium chloride magnesium nitrate copper(II) chloride C. Ionic Nomenclature

10 NaBr Na 2 CO 3 FeCl 3 C. Ionic Nomenclature

11 potassium chloride magnesium nitrate copper(II) chloride –K + Cl –Mg 2+ NO 3 –Cu 2+ Cl KCl Mg(NO 3 ) 2 CuCl 2 C. Ionic Nomenclature

12 NaBr Na 2 CO 3 FeCl 3 –sodium bromide –sodium carbonate –iron(III) chloride C. Ionic Nomenclature


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