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Naming and Writing Ionic Compound Formulas Easily

Learn to write formulas and name ionic compounds and oxyanions effectively. Understand monoatomic and polyatomic ions, oxidation numbers, and key terms. Practice naming binary ionic compounds with step-by-step examples. Master the skill of writing chemical formulas from names with clear guidelines. Complete the homework exercises for further practice.

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Naming and Writing Ionic Compound Formulas Easily

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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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