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Ch. 11 - Chemical Bonds

Ch. 11 - Chemical Bonds. IV. Naming Ionic Compounds Oxidation Number Ionic Names Ionic Formulas. A. Oxidation Number. The charge on an ion. Indicates the # of e - gained/lost to become stable. 1+. 0. 2+. 3+. 4+. 3-. 2-. 1-. B. Ionic Names.

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Ch. 11 - Chemical Bonds

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  1. Ch. 11 - Chemical Bonds IV. Naming Ionic Compounds Oxidation Number Ionic Names Ionic Formulas

  2. A. Oxidation Number • The charge on an ion. • Indicates the # of e- gained/lost to become stable. 1+ 0 2+ 3+ 4+ 3- 2- 1-

  3. B. Ionic Names • Write the names of both elements, cation first. • Change the anion’s ending to -ide. • Write the names of polyatomic ions. • For ions with variable oxidation #’s, write the ox. # in parentheses using Roman numerals. Overall charge = 0.

  4. B. Ionic Names • NaBr • Na2CO3 • FeCl3 • sodium bromide • sodium carbonate • iron(III) chloride

  5. C. Ionic Formulas • Write each ion. Put the cation first. • Overall charge must equal zero. • If charges cancel, just write the symbols. • If not, crisscross the charges to find subscripts. • Use parentheses when more than one polyatomic ion is needed. • Roman numerals indicate the oxidation #.

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

  7. C. Ionic Formulas • calcium oxide • aluminum chlorate • iron(III) oxide • Ca2+ O2- CaO • Al3+ ClO3-  Al(ClO3)3 • Fe3+ O2- Fe2O3

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