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(pg 49) Common Ion Charges

(pg 49) Common Ion Charges. Loses e -. Gains e -. 1+. 1. 18. 0. Ion charge (oxidation #). NA. 14. 2+. 2. 3+. 13. 15. 3-. 16. 2-. 17. 1-. Group #. Ionic Bonding. Writing Ionic Formulas Write the symbols for each ion, cation first.

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(pg 49) Common Ion Charges

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  1. (pg 49) Common Ion Charges Loses e- Gains e- 1+ 1 18 0 Ion charge (oxidation #) NA 14 2+ 2 3+ 13 15 3- 16 2- 17 1- Group #

  2. Ionic Bonding

  3. Writing Ionic Formulas • Write the symbols for each ion, cation first. • Place the charge (oxidation #) of each element above the symbol • If there areRoman numerals, they indicate the cation’s charge. • Criss-Cross the charges and use them as subscripts. • Use parentheses to show more than one polyatomic ion. • Reduce if Possible

  4. Mg Cl Mg2+ Cl1- • Magnesium Chloride • Aluminum Oxide • Calcium Sulfide Mg1 Cl2 MgCl2 Al3+ O2- Al2 O3 Al2O3

  5. Sodium Nitrate • Magnesium Hydroxide • Ammonium Sulfate

  6. Iron (III) Oxide • Iron (II) Sulfate • Zinc Nitride

  7. Naming Ionic Compounds • Write the names of both ions, cation first! • If your anion is one element, change the ending to -ide. • If it is a polyatomic, no change.

  8. Naming Practice • NaBr • K2CO3 • NH4Cl • Fe(SO4) sodium bromide potassium carbonate ammonium chloride iron sulfate

  9. Naming Practice • AgNO3 • CuCO3 • LiC2H3O2 silver nitrate copper carbonate lithium acetate

  10. Ionic Bonding: Naming Compounds Get your homework when you finish!

  11. Ionic Bonding: Naming Compounds

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