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)  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.  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. Binary Ionic Compounds  Type I  Cation - is a metal from the representative element set!  Anion - is a nonmetal  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

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 - CaCl 2 - calcium chloride Na 3 P - sodium phosphide  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 - CaCl 2 - calcium chloride Na 3 P - sodium phosphide

6. Name these!  MgO  Magnesium oxide  AlF 3  Aluminum fluoride  Ca 2 N 3  Calcium nitride  MgO  Magnesium oxide  AlF 3  Aluminum fluoride  Ca 2 N 3  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!  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 + S 2-  2(Na + ) + S 2- = Na 2 S  Barium nitride  Ba 2+ N 3-  3(Ba 2+ ) + 2(N 3- ) = Ba 3 N 2  Sodium sulfide  Na + S 2-  2(Na + ) + S 2- = Na 2 S  Barium nitride  Ba 2+ N 3-  3(Ba 2+ ) + 2(N 3- ) = Ba 3 N 2

9. Write the formulas for these!  Potassium chloride  Gallium oxide  Beryllium iodide  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  Sr 2+ N 3- Sr 3 N 2 IT WORKS EVERY TIME!  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  Sr 2+ N 3- Sr 3 N 2 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.  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  FeCl 2  Cation (Fe) - had an original charge of 2+  Iron (II) chloride  FeCl 3  Cation (Fe) - had an original charge of 3+  Iron (III) chloride  FeCl 2  Cation (Fe) - had an original charge of 2+  Iron (II) chloride  FeCl 3  Cation (Fe) - had an original charge of 3+  Iron (III) chloride

13. Try These!  Cu 2 S  CuS  Au 2 S 3  V 2 O 5  Cu 2 S  CuS  Au 2 S 3  V 2 O 5

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  Co 3+ Br -  Sn 4+ S 2-  CoBr 3  Sn 2 S 4 (can be reduced)  SnS 2  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  Co 3+ Br -  Sn 4+ S 2-  CoBr 3  Sn 2 S 4 (can be reduced)  SnS 2

15. Try These!  Chromium (II) oxide  Lead (II) fluoride  Lead (IV) fluoride  Copper (II) carbide  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!  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!  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  NaNO 3  Sodium nitrate  Ca(OH) 2  Calcium hydroxide  Al(SO 3 ) 3  Aluminum sulfite  (NH 4 ) 3 PO 4  Ammonium phosphate  NaNO 3  Sodium nitrate  Ca(OH) 2  Calcium hydroxide  Al(SO 3 ) 3  Aluminum sulfite  (NH 4 ) 3 PO 4  Ammonium phosphate

19. Try These!  BaSO 4  Li 2 CO 3  Ga(NO 2 ) 3  BaSO 4  Li 2 CO 3  Ga(NO 2 ) 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!  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  Mg 2+ CN -  Li + PO 4 3-  Mg(CN) 2  Li 3 PO 4  Magnesium cyanide  Lithium phosphate  Mg 2+ CN -  Li + PO 4 3-  Mg(CN) 2  Li 3 PO 4

22. Try These!  Strontium chlorate  Potassium sulfate  Ammonium oxide  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(NO 3 ) 3  NiCO 3  Cobalt (III) nitrate  Nickel (II) carbonate  Naming  Tie together using the Roman Numerals for the transition metals with the name of the polyatomic ion.  Example  Co(NO 3 ) 3  NiCO 3  Cobalt (III) nitrate  Nickel (II) carbonate

24. Try These!  Ti(OH) 2  Zn(ClO) 3  Au(ClO 3 ) 3  Ti(OH) 2  Zn(ClO) 3  Au(ClO 3 ) 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!  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. Examples  Lead (IV) sulfate  Pb 4+ SO 4 2-  Pb 2 (SO 4 ) 4  Pb(SO 4 ) 2  Lead (IV) sulfate  Pb 4+ SO 4 2-  Pb 2 (SO 4 ) 4  Pb(SO 4 ) 2  Copper (I) nitrite  Cu + NO 3 -  CuNO 3