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Ionic Formulas and Nomenclature

Ionic Formulas and Nomenclature. Formulas. What types of elements are found in ionic compounds? What holds the elements together? Even though there are ions in ionic compounds, the overall compound must be neutral. Electrolytes. What type of compounds are electrolytes?

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Ionic Formulas and Nomenclature

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  1. Ionic Formulas and Nomenclature

  2. Formulas • What types of elements are found in ionic compounds? • What holds the elements together? • Even though there are ions in ionic compounds, the overall compound must be neutral.

  3. Electrolytes • What type of compounds are electrolytes? • Why are ionic compounds electrolytes? • Consider sodium chloride: • Is this an electrolyte? • Why? • Consider sucrose (sugar, C12H22O11): • Is this an electrolyte? • Why? • Consider ammonium chloride (NH4Cl): • Is this an electrolyte? • Why?

  4. Conductivity of Ammonium Chloride • Why does it light up? • What type of bonding actually occurs in ammonium chloride? • Where are the ions in NH4Cl?

  5. Two Types of Ions • Monatomic ions – ions made of a single atom. • Polyatomic ions – ions made of many atoms • Polyatomic ions can be found on your reference table.

  6. Ionic Formulas Activity

  7. Writing Ionic Formulas • A compound made from barium and phosphate ions. • Figure out the charges on the ions involved. • Ba2+ • PO43- • Find the lowest common multiple of the charges: • LCM of 2 and 3 is 6 • When you have 6 total positive charges and 6 total negative charges the compound will be neutral. • Determine the individual number of ions • To get 6 total positives you need 3 barium ions • To get 6 total negatives you need 2 phosphate ions • Write the formula with those numbers • Ba3(PO4)2

  8. Writing Ionic Formulas • Write the formula of the following • A compound made from aluminum and hydroxide ions. • A compound made from magnesium and sulfur. • A compound made from strontium and nitrite ions.

  9. Naming Ionic Compounds • Based on you already knowing the charges of the ions involved. • Does not tell you how many of each ion there are.

  10. The Rules • Name the positive ion first • Na+ = sodium ion • (Leave a couple lines of blank space here) • Name the negative ion last • Change the name of a monatomic anion to have an –ide ending. • Polyatomic ions names are not changed

  11. Practice Problems • Name the following: • BaCl2 • MgO • Na3P • Al2(SO4)3

  12. Those Stupid d-Orbitals • Consider the following copper oxides: Cu2O CuO Determine the charge on the copper ions in both compounds.

  13. Multi-valent metals • Most metal ions can have multiple stable charges because of the d-orbitals. • The ones that can’t are: • Group 1 • Group 2 • Silver (+1) • Zinc (+2) • Aluminum(+3) • For everything that can have a multiple charge you must specify the charge in the name. • Use Roman numerals to tell the charge.

  14. The Rules • Name the positive ion first • Na+ = sodium ion • Specify the charge of all metal ions with a Roman numeral • Except Group 1, Group 2, Ag, Zn, Al • Name the negative ion last • Change the name of a monatomic anion to have an –ide ending. • Polyatomic ions names are not changed

  15. Those Stupid d-Orbitals CuO Cu2O • Name the compounds above: • Black = copper(II) oxide • Red = copper(I) oxide • Remember the Roman numeral is the charge not the number of atoms.

  16. Practice Problems • Name the following compounds • Fe2O3 • Co(NO3)2 • CaCO3 • NH4C2H3O2

  17. Practice Problems • Name the following compounds • MnO2 • AgCl • CrN2 • W2O5

  18. Practice Problems • Write the formulas for the following compounds: • Tin(IV) oxide • Aluminum chloride • Ammonium sulfide

  19. Practice Problems • Write the formulas for the following compounds: • Potassium dichromate • Chromium(II) nitrate • Technetium(VII) oxide

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