1. Unit 6 - Nomenclature A little humor for you.......... Two atoms walk into a bar. One atom stops and says to the other, "I think I just lost an electron." The second atom asks "Are you sure?" The first atom replies, "I'm positive!"

2.  How to use different naming conventions based upon the type of compound  Standard system for main group ionic cmpds  Stock system for transition metal ionic cmpds  Prefix system for molecules (non-metal/non-metal)  How to write formulas from names

3.  Representative Ionic Compounds  Cation  Metal stays the same as it appears on Periodic Table  Anion  monatomic, change the ending to -ide  polyatomic, use the name of the polyatomic ion –table given to you– DON’T CHANGE ANYTHING! Na 2 O sodium oxide Na 2 SO 4 sodium sulfate

4. 1. MgO 2. SrCl 2 3. Al 2 S 3 4. FrF 5. Na 3 N 6. LiBr 7. Ca 2 C 8. KI 9. Cs 3 As 10. Ba 3 P 2 Magnesium oxide Strontium chloride Aluminum sulfide Francium fluoride Sodium nitride Lithium bromide Calcium carbide Potassium iodide Cesium arsenide Barium phosphide 1. RbClO 2 2. AlPO 4 3. CaSO 3 4. FrBrO 4 5. NaNO 3 6. Sr(ClO 3 ) 2 7. BaCr 2 O 7 8. CsC 2 H 3 O 2 9. K 2 CO 3 10. Mg(CN) 2 Rubidium chlorite Aluminum phosphate Calcium sulfite Francium perbromate Sodium nitrate Strontium chlorate Barium dichromate Cesium acetate Potassium carbonate Magnesium cyanide

5.  Transition Metal Ionic Compounds  Cation  Metal remains unchanged  Followed by charge of metal in roman numerals  Anion  Same rules as before  EXCEPTIONS:  Zn +2, Ag +, Cd +2  Sn & Pb (+2 or +4) Cu 2 O Copper (I) oxide CuSO 4 Copper (II) sulfate

6.  How does one determine the charge of the transition metal? 1.Find the charge of the anion 2.Calculate total negative charges 3.Divide by the number of cations 4.Write the roman number corresponding to the charge on the transition metal

7.  Examples: 1.Charge on Chlorine is - 1 2.There are 3 chloride ions, so 3 x -1 = -3 3. 3 ÷ 1 (# of Cobalt atoms) = 3 4. 3 = III CoCl 3 -3 total+3 total +3 Cobalt (III) chloride

8.  Examples: 1.Charge on phosphate is -3 2.There are two phosphates, so………….. 2 x -3 = -6 3. 6 ÷ 3 (atoms of Ni) =2 4. 2 = II Ni 3 (PO 4 ) 2 -3 -6 total+6 total +2 Nickel (II) phosphate

9.  Write the chemical compound name for:  Na 3 N  CaO  KI  Write the formula for:  Aluminum Sulfide  Strontium Chlorate

10. SnO ScCl 2 Co 2 S 3 CuF Pd 3 N 2 MnBr 7 RuI 3 WS 2 Ni 3 As 4 Pb 3 P 2 Tin (II) oxide Scandium (II) chloride Cobalt (III) sulfide Copper (I) fluoride Palladium (II) nitride Manganese (VII) bromide Ruthenium (III) iodide Tungsten (IV) sulfide Nickel (IV) arsenide Lead (II) phosphide Co(NO 3 ) 3 AlP Mn(SO 4 ) 2 NaF Pb(CO 3 ) 2 KClO 4 Ag 2 S Ni(OH) 2 CaCl 2 CrO 3 Cobalt (III) nitrate Aluminum phosphide Manganese (IV) sulfate Sodium flouride Lead (IV) carbonate Potassium perchlorate Silver (I) sulfide Nickel (II) hydroxide Calcium chloride Chromium (VI) oxide

11.  Steps to writing a correct formula for ionic compounds 1. From the name, write the symbols 2. Write the charges of the ions above the symbols 3. Reduce the charges to the lowest whole number ratio 4. Criss-cross the charges

12.  Scandium (III) chloride 1. From the name, write the symbols 2. Write the charges of the ions above the symbols 3. Reduce the charges to the lowest whole number ratio 4. Criss-cross the charges Sc Cl +3 No Reduction Necessary 3 No Number if 1

13.  Calcium Oxide 1. From the name, write the symbols 2. Write the charges of the ions above the symbols 3. Reduce the charges to the lowest whole number ratio 4. Criss-cross the charges Ca O +2 -2 +1 -1 No Number if 1

14. NaOH FeBr 2 Co 2 S 3 Cu 2 SO 4 Ba(C 2 H 3 O 2 ) 2 K3PK3P Rh(CN) 5 PbO 2 AgCl NaBrO 4 Sodium hydroxide Iron (II) bromide Cobalt (III) sulfide Copper (I) sulfate Barium acetate Potassium phosphide Rhodium (V) cyanide Lead (IV) oxide Silver chloride Sodium perbromate LiClO 2 Al(NO 2 ) 3 Ni(NO 3 ) 2 HgF CaCr 2 O 7 Sn(IO 3 ) 4 CrS 3 Cr 2 O 3 SrSe Lithium chlorite Aluminum nitrite Nickel (II) nitrate Mercury (I) fluoride Calcium dichromate Tin (IV) iodate Chromium (VI) sulfide Chromium (III) oxide Strontium selenide

15.  Covalently Bonded Molecules  Compounds are named by using prefixes to denote the number of each element  First non-metal stays the same  Second non-metal ending is changed to -ide CO 2 Carbon dioxide P 4 O 10 Tetraphosphorus decoxide

16. Mono1Hexa6Di2Hepta7 Tri3Octa8 Tetra4Nona9 Penta5Deca10

17. Phosphorus pentachloride PCl 5 Sulfur trioxide SO 3 Hydrogen Fluoride HF Boron trichloride BCl 3 Carbon tetrachloride CCl 4 ICl 3 Iodine trichloride OF 2 Oxygen difluoride CO Carbon monoxide N2O4N2O4N2O4N2O4 Dinitrogen tetroxide