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Nomenclature

Nomenclature. Unit 3- as can be found in Chapter 4 of your World of Chemistry textbook. Georgia Performance Standard. SC1d- Use IUPAC nomenclature for both chemical names and formulas: Ionic Compounds (Binary & Tertiary) Covalent Compounds (Binary & Tertiary)

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Nomenclature

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  1. Nomenclature Unit 3- as can be found in Chapter 4 of your World of Chemistry textbook

  2. Georgia Performance Standard • SC1d- Use IUPAC nomenclature for both chemical names and formulas: • Ionic Compounds (Binary & Tertiary) • Covalent Compounds (Binary & Tertiary) • Acidic Compounds (Binary & Tertiary)

  3. Types of Compounds • As identified by the International Union of Pure and Applied Chemistry (IUPAC) • Why do we do things the IUPAC way? • Having a standard way of naming and writing formulas for compounds eliminates error and misunderstandings.

  4. Type I Cation - is a metal from the representative element set! Anion - is a nonmetal Type II Cation - is a transition metal Transition metal elements can have more than one charge or oxidation number as we call it. Anion - is a nonmetal Binary Ionic Compounds

  5. Type I (Binary Ionic) Compounds • Naming • 1. The cation gets the element’s name. (Easy peasy!) • 2. The anion uses the element’s name but the ending changes to -ide. • Example - CaCl2 - calcium chloride Na3P - sodium phosphide

  6. Name these! • MgO • Magnesium oxide • AlF3 • Aluminum fluoride • Ca2N3 • Calcium nitride

  7. Type I (Binary Ionic) Compounds • Writing Formulas • Write the symbol for the cation • It’s element symbol and its charge • Write the symbol for the anion • It’s element symbol and its charge • Determine how many of each ion are necessary so that the total charge for the compound adds up to zero!

  8. Examples • Sodium sulfide • Na+ S2- • 2(Na+) + S2- = Na2S • Barium nitride • Ba2+ N3- • 3(Ba2+) + 2(N3-) = Ba3N2

  9. Write the formulas for these! • Potassium chloride • Gallium oxide • Beryllium iodide

  10. Writing Formulas- the easy way! • The criss- cross method • Write the symbols and charges for the cation and anion as before • The cross the charges over to the other element! (lose the +/- signs) • Example - strontium nitride • Sr2+ N3- Sr3N2 IT WORKS EVERY TIME!

  11. Type II (Binary Ionic) Compounds • Naming • The cation gets the element’s name. However, since it is a transition metal that can have more than 1 charge, you MUST write the original charge of the cation as Roman Numerals after the name of the cation. • The anion uses the element’s name, changing the ending to -ide.

  12. Examples • FeCl2 • Cation (Fe) - had an original charge of 2+ • Iron (II) chloride • FeCl3 • Cation (Fe) - had an original charge of 3+ • Iron (III) chloride

  13. Try These! • Cu2S • CuS • Au2S3 • V2O5

  14. Type II (Binary Ionic) Compounds • Writing Formulas - this is easy! • Cation- the name already gives you the charge of the element. • Anion is just like Type I, • Criss- cross the charges! • Examples • Cobalt (III) bromide  Tin (IV) sulfide • Co3+ Br-  Sn4+ S2- • CoBr3 Sn2S4 (can be reduced)  SnS2

  15. Try These! • Chromium (II) oxide • Lead (II) fluoride • Lead (IV) fluoride • Copper (II) carbide

  16. Polyatomic Ions • These are ions that have more than 1 atom in it BUT act as a single ion with a single charge!!!!!!! • See p. In your textbook • Yes, you need to know these!

  17. Type I (Tertiary Ionic) Compounds • Naming • Cation - Named the same way as Type I Binary is • Anion - Use the name of the polyatomic ion, don’t change the ending!

  18. Examples • NaNO3 • Sodium nitrate • Ca(OH)2 • Calcium hydroxide • Al(SO3)3 • Aluminum sulfite • (NH4)3PO4 • Ammonium phosphate

  19. Try These! • BaSO4 • Li2CO3 • Ga(NO2)3

  20. Type I (Tertiary Ionic) Compounds • Writing Formulas • Cation - Write the symbol and the charge • Anion - Write the polyatomic ion and charge • Criss- cross the charges! • IF you are going to cross a charge other than 1 over to the polyatomic ion… put the polyatomic ion in parentheses first!

  21. Examples • Magnesium cyanide Lithium phosphate • Mg2+ CN-Li+ PO43- • Mg(CN)2 Li3PO4

  22. Try These! • Strontium chlorate • Potassium sulfate • Ammonium oxide

  23. Type II (Tertiary Ionic) Compounds • Naming • Tie together using the Roman Numerals for the transition metals with the name of the polyatomic ion. • Example • Co(NO3)3 NiCO3 • Cobalt (III) nitrate  Nickel (II) carbonate

  24. Try These! • Ti(OH)2 • Zn(ClO)3 • Au(ClO3)3

  25. Type II (Tertiary Ionic) Compounds • Writing Formulas - this is easy too! • Cation - Write the symbol and charge for the transition metal • Anion - Write the symbol for the polyatomic ion and its charge • Criss - cross the charges. • Again, if you are crossing a number to the polyatomic ion that is larger than 1, then put the polyatomic ions in parentheses first!

  26. Lead (IV) sulfate Pb4+ SO42- Pb2(SO4)4 Pb(SO4)2 Copper (I) nitrite Cu+ NO3- CuNO3 Examples

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