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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!". Unit 6 - Nomenclature. What will we learn?.

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Unit 6 - Nomenclature

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  1. 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!" Unit 6 - Nomenclature

  2. What will we learn? • 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. Standard Naming Convention • 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! Na2O sodium oxide Na2SO4 sodium sulfate

  4. Standard Naming Practice RbClO2 AlPO4 CaSO3 FrBrO4 NaNO3 Sr(ClO3)2 BaCr2O7 CsC2H3O2 K2CO3 Mg(CN)2 Rubidium chlorite Aluminum phosphate Calcium sulfite Francium perbromate Sodium nitrate Strontium chlorate Barium dichromate Cesium acetate Potassium carbonate Magnesium cyanide • MgO • SrCl2 • Al2S3 • FrF • Na3N • LiBr • Ca2C • KI • Cs3As • Ba3P2 Magnesium oxide Strontium chloride Aluminum sulfide Francium fluoride Sodium nitride Lithium bromide Calcium carbide Potassium iodide Cesium arsenide Barium phosphide

  5. Stock System • 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) Cu2O Copper (I) oxide CuSO4 Copper (II) sulfate

  6. Stock System Nomenclature • Find the charge of the anion • Calculate total negative charges • Divide by the number of cations • Write the roman number corresponding to the charge on the transition metal • How does one determine the charge of the transition metal?

  7. +3 -1 Stock System Nomenclature • Charge on Chlorine is -1 • There are 3 chloride ions, so 3 x -1 = -3 • 3 ÷ 1 (# of Cobalt atoms) = 3 • 3 = III • Examples: +3 total -3 total • CoCl3 Cobalt (III) chloride

  8. +2 -3 Stock System Nomenclature • Charge on phosphate is -3 • There are two phosphates, so………….. 2 x -3 = -6 • 6 ÷ 3 (atoms of Ni) =2 • 2 = II • Examples: +6 total -6 total • Ni3(PO4)2 Nickel (II) phosphate

  9. Bellringer (12/2) Tuesday • Write the chemical compound name for: • Na3N • CaO • KI • Write the formula for: • Aluminum Sulfide • Strontium Chlorate

  10. Combined Naming Practice SnO ScCl2 Co2S3 CuF Pd3N2 MnBr7 RuI3 WS2 Ni3As4 Pb3P2 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 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 Co(NO3)3 AlP Mn(SO4)2 NaF Pb(CO3)2 KClO4 Ag2S Ni(OH)2 CaCl2 CrO3

  11. Writing Formulas • Steps to writing a correct formula for ionic compounds • From the name, write the symbols • Write the charges of the ions above the symbols • Reduce the charges to the lowest whole number ratio • Criss-cross the charges

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

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

  14. Formula Writing Practice Lithium chlorite Aluminum nitrite Nickel (II) nitrate Mercury (I) fluoride Calcium dichromate Tin (IV) iodate Chromium (VI) sulfide Chromium (III) oxide Strontium selenide LiClO2 Al(NO2)3 Ni(NO3)2 HgF CaCr2O7 Sn(IO3)4 CrS3 Cr2O3 SrSe NaOH FeBr2 Co2S3 Cu2SO4 Ba(C2H3O2)2 K3P Rh(CN)5 PbO2 AgCl NaBrO4 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

  15. Prefix System • 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 CO2 Carbon dioxide P4O10 Tetraphosphorusdecoxide

  16. Prefixes

  17. Formula Writing Practice ICl3 Iodine trichloride OF2 Oxygen difluoride CO Carbon monoxide N2O4 Dinitrogen tetroxide Phosphorus pentachloride PCl5 Sulfur trioxide SO3 Hydrogen Fluoride HF Boron trichloride BCl3 Carbon tetrachloride CCl4

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