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Chemical Nomenclature Naming compounds and writing chemical formulas.

Canton South Chemistry!. Chemical Nomenclature Naming compounds and writing chemical formulas. Predicting Charges on Monatomic Ions. +1 +2 +3 +4 +5 +2 +3

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Chemical Nomenclature Naming compounds and writing chemical formulas.

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  1. Canton South Chemistry! Chemical NomenclatureNaming compounds and writing chemical formulas.

  2. Predicting Charges on Monatomic Ions +1 +2 +3 +4 +5 +2 +3 -4 -3 -2 -1 0

  3. Understanding Nomenclature Nomenclature refers to the process of naming chemicals. Initially the focus is on the most basic rules and ideas involved in the naming of compounds.

  4. I. Binary Compounds A binary compound contains just two element 1. The element with the positive charge ( more metallic ), is written first. 2. The element with the negative charge( more non-metallic) is written second

  5. Understanding Nomenclature The first word (metal or positive ion) remains the same word • The second word(negative ion) is formed by changing the ending of the element name to “ide”. • For example: fluorine changes to fluoride, and oxygen to oxide sodium chloride ex: NaCl potassium bromide KBr

  6. 1. Using the rules given , name the compounds listed below. 1. MgO ____________________ 2. CaI2__________________ 3. BaS ____________________ 4. ZnI2 ______________________ 5. CaO ____________________ 6. Ag2O_____________________ 7. K3P ____________________ 8. AlBr3_____________________ 9. Na3N ____________________ 10. MgS_____________________

  7. Writing proper Chemical formulas. The net charge of the formula must be zero potassium and chlorine = potassium chloride 1+ 1- = 0 KCl = KCl

  8. Crisscross Method simplified method for writing these formulas Calcium and bromide = calcium bromide Ca2+Br1-=0 Ca2+Br1- 2 1 Subscripts Ca2+Br1- 1 2 2+ 2- = 0 Ca1Br2 **But we don’t write ones!!! CaBr2

  9. Crisscross Method simplified method for writing these formulas aluminum and sulfide = aluminum sulfide Al3+S2-=0 Al3+S2- 3 2 Subscripts Al3+S2- 2 3 6+ 6- = 0 Al2S3 Al2S3

  10. Using the rule given , give the formula for these compounds 12. sodium chloride ____________13. potassium iodide __________ 14. magnesium sulfide __________15. aluminum bromide __________ 16. strontium oxide ____________ 17. sodium sulfide __________ 18. rubidium phosphide _________19. barium nitride __________

  11. Groups/Families VIIIA IA • 23, 24, 23, 23, 23, 12, 2 • 1, 2 • 24, 13, 12 IIA VIIA VA VIA Cr Mn Fe Co Ni Cu Zn Zn Zn +1 +2 -4 -3 -2 -1 0 +2 +3 +2 +4 +2 +3 +2 +3 +2 +3 +1 +2 +2 +2 +4 +3 +5 +3 Ag Cd I-VIIIB +1 +2 multiple charges Au Pt Hg Hg +2 +4 +1 +3 +1 +2

  12. Type II Binary Compounds (Stock System) Some metallic element are capable of more than one positivecharge. We will indicated these with a roman numeral in parenthesis following the name of the positive element. Roman numeral = the + charge iron (II) = 2+ and iron (III) = 3+ ***Used only when:*** MORE THAN 1 POSITIVE CHARGE

  13. Type II Binary Compounds (Stock System) Compare FeCl2 & FeCl3 iron and chloride = iron chloride (II) 2+ 2- = 0 FeCl 1- 2 1 iron chloride (III) iron chloride FeCl1- 3 3+ 3- = 0 1 ***Used only when:*** MORE THAN 1 POSITIVE CHARGE

  14. Type II Binary Compounds 4. Name the following compounds. 21. CuO ______________________ 22. PbS ________________________ 23. HgCl ______________________ 24. MnO2 _________________________ 25. Fe2S3 ______________________ 26. SnBr2 ________________________ 27. BiCl3 ______________________ 28. PbCl4 ________________________ lead (II) sulfide

  15. Classical or “Old School” The "ous"-"ic" System Another method of indicating metallic ions with more than one charge is: a suffix The suffix -ous is used for the lower charge. while the suffix -icis used for thehigher ionic charge

  16. *  Chemistry trivia time: In the James Bond movie Goldfinger who was the villian? Auric Goldfinger What was the license plate number on Goldfinger's Rolls Royce?    AU3 What was the name of Goldfinger's business establishment?  Auric Enterprises ** Mercury's name was changed because hydroargentous and hydroargentic would be just to much to handle

  17. “Old School” The "ous"-"ic" System (“old school”)(Stock)formula 29. ferric chloride ________________________ _____________ 30. stannic oxide ________________________ _____________ 31. mercuric iodide ________________________ _____________ 32. cuprous oxide ________________________ _____________ 33. plumbous sulfide ________________________ _____________ 34. antimonic bromide _______________________ ____________ 35. aurous phosphide ________________________ _____________ SnO2 tin (IV) oxide

  18. Ternary Compounds It takes “3” or more A ternary compound contains three or more different elements. Ternary compounds usually contain one or morepolyatomic ions( radicals ). Examples: Fe(ClO4)2 ; NaOH : NH4MnO4 When writing the formula – the basic rules apply. Polyatomic ions ( radicals )are treated just like an ion.

  19. Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions Ex: Calcium hydroxide Calcium and hydroxide = calcium hydroxide Ca2+OH1-=0 Ca2+OH1- CaOH2 2 1 Subscripts But OH2 = H2O = water !!! ***Parentheses : need to be used whenever more than a single polyatomic ion is needed to balance the charges - in other words if you add a subscript put the polyatomic radical in parentheses. ( ) Ca OH 2

  20. Practice with Polyatomic Ions

  21. ... the `ate chart Polyatomic Ions – they all contain oxygen -3 -2 -1 PO43- SO42- NO3- CrO42- ClO3- CO32- MnO3-

  22. ... the `ate chart -3 -2 -1 Please Study Nomenclature Crazy Class Manana ? Chemistry

  23. ... the `ate become… `ites – they all lose an oxygen.. -3 -2 -1 PO33- SO32- NO2- CrO32- ClO2- CO22- MnO2- but the charge remains the same

  24. ... the `ate; the `ite; now the hypo- – subtract another oxygen !! -3 -2 -1 PO23- SO22- NO- CrO22- ClO - CO 2- MnO - and the charge remains the same

  25. ... the `ate; the `ite; the hypo.. – lets add an oxygen … the Per- -3 -2 -1 PO53- SO52- NO4- CrO52- ClO4- CO42- MnO4- and the charge remains the same

  26. `ate `ite hypo- per- ClO4-1 perchlorate ClO3-1 chlorate ClO2-1 chlorite hypochlorite ClO-1

  27. carbonate versus bicarbonate Na2CO3 CO3-2 carbonate sodium carbonate HCO3-1 bicarbonate NaHCO3 sodium bicarbonate add H+ and drop a negative charge

  28. Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions 36. AlPO4 ______________________ 37. (NH4)2CO3 _______________________ 38. __________ lithium cyanide 39. ___________ copper(II) nitrate 40. KClO ______________________ 41. Zn(C2H3O2)2 ______________________ 42. __________ calcium phosphate 43. ___________ ammonium sulfite 44. __________ ammonium acetate 45. NaMnO4 _______________________

  29. Naming Covalent Molecular Compounds Nonmetal to Nonmetal( or to the right of the zigzag red line) • Use these Prefixes: Greek prefixes to indicate number • (never use mono on first) • mono - 1 di - 2 tri - 3 tetra - 4 • penta - 5 hexa - 6 hepta - 7 octa - 8 • nona - 9 deca – 10 boron trifluoride nitrogen monoxide Ex: BF3NO N2O5 dinitrogen pentoxide

  30. Naming Covalent Molecular Compounds 1. CO __________________________ 8. diphosphorus pentoxide _________________ 2. PBr3 ______________________________ 9. carbon dioxide _________________ 3. CCl4 ______________________________ 10. selenium trioxide _________________ 4. NCl3 ______________________________ 11. sulfur hexafluoride _________________ 5. SeO2 ______________________________ 12. phosphorus pentiodide ________________ 6. P2O3 _____________________________ 13. sulfur tribromide ________________ 7. NH3 ______________________________ 14. phosphorus hexachloride______________

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