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8-3 Names and Formulas for Ionic Compounds

8-3 Names and Formulas for Ionic Compounds. P.221-227. Objectives. Write formulas for ionic compounds and oxyanions Name ionic compounds and oxyanions. Formula unit Monoatomic ion Oxidation number. Polyatomic ion Oxyanion. Key Terms. Formulas for Ionic Compounds.

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8-3 Names and Formulas for Ionic Compounds

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  1. 8-3 Names and Formulas for Ionic Compounds P.221-227

  2. Objectives • Write formulas for ionic compounds and oxyanions • Name ionic compounds and oxyanions

  3. Formula unit Monoatomic ion Oxidation number Polyatomic ion Oxyanion Key Terms

  4. Formulas for Ionic Compounds • A formula unit= simplest ratio of ions representing a compound • ALL ionic compounds are written as formula units (not the case for covalent compounds)

  5. Monoatomic Ions • Monoatomic ions contain a single element • Be2+, Na+, Fe3+ • Notice the charge on the elements!

  6. Polyatomic Ions • Polyatomic ions have more than one element, with a net charge • SO42-, NH4+, NO2-, C2H3O2- • Treat like a single unit, not individual ions

  7. Naming Binary Ionic Compounds • Step 1: Name the cation first and the anion second. • Step 2: Monoatomic cations use the element name. • Step 3: Monoatomic anions use the ion name with the –ide ending. • Step 4: For d-block cations you must write the cation charge as a roman numeral in parentheses. • Step 5: If the compound contains a polyatomic ion, just use the name of the ion.

  8. Naming Binary Ionic Compounds • Example: • NaCl: Sodium Chloride • FeO: Iron (II) Oxide • NH4Cl: Ammonium Chloride

  9. Writing a Chemical Formula from the Name • Step 1: Write the element symbol for name of the ion • Step 2: Write the charge of the ion • Step 3: If the total charge equals zero, you are done. If the total charge does not equal zero, you must change the subscripts so that the total charge equals zero (‘drop-n-cross’).

  10. Writing a subscript for a polyatomic ion: put a parenthesis around it with the subscript on the outside of the parenthesis • Example: Cr(SO4)2

  11. Example: Barium Fluoride • Step 1: Ba F • Step 2: Ba2+F- • Step 3: Total charge = +1 • Step 4: BaF2

  12. Example: Iron (III) Sulfate • Step 1: Fe SO4 • Step 2: Fe3+SO42- • Step 3: Total charge = +1 • Step 4: Fe2(SO4)

  13. Example: Beryllium Oxide • Step 1: Be O • Step 2: Be2+O2- • Step 3: Total charge = 0  BeO

  14. Homework • P.227 #35-36,38-39 • P.237 #74-79

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