1 / 35

Chemical Nomenclature Naming compounds and writing chemical formulas.

Chemical Nomenclature Naming compounds and writing chemical formulas. Predicting Charges on Monatomic Ions. +1 +2 +3 +4 +5 +2 +3 -4 -3 -2 -1 0.

sandro
Télécharger la présentation

Chemical Nomenclature Naming compounds and writing chemical formulas.

An Image/Link below is provided (as is) to download presentation Download Policy: Content on the Website is provided to you AS IS for your information and personal use and may not be sold / licensed / shared on other websites without getting consent from its author. Content is provided to you AS IS for your information and personal use only. Download presentation by click this link. While downloading, if for some reason you are not able to download a presentation, the publisher may have deleted the file from their server. During download, if you can't get a presentation, the file might be deleted by the publisher.

E N D

Presentation Transcript

  1. 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. Cations Anions Formula Name Formula Name Charge Charge H+ hydrogen H- hydride Li+ lithium F- fluoride Na+ sodium Cl- chloride K+ potassium Br- bromide Cs+ cesium I- iodide Ag+ silver Mg2+ magnesium O2- oxide Ca2+ calcium S2- sulfide Sr2+ strontium Ba2+ barium Zn2+ zinc Cd2+ cadmium Al3+ aluminum N3- nitride Common Monoatomic Ions +1 -1 Common + ions are in blue. +2 -2 Common - ions are in red. +3 -3

  7. 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_____________________

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

  9. 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

  10. 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

  11. 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 __________

  12. 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

  13. 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

  14. Copper Cu+1 copper(I) Cu+2 copper(II) Co+2 cobalt(II) Cobalt Co+3 Fe+2 cobalt (III) iron(II) Iron Fe+3 iron(III) Pb+2 lead(II) Lead Pb+4 lead(IV) Sn+2 tin(II) Tin Sn+4 tin(IV) Metals With Several Oxidation States Table 2.4 (partial) Classical Old School Element Ion Formula Stock Name

  15. 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

  16. 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

  17. 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

  18. Copper Cu+1 copper(I) cuprous Cu+2 copper(II) cupric Co+2 cobalt(II) Cobalt Co+3 Fe+2 cobalt (III) iron(II) ferrous Iron Fe+3 iron(III) ferric Pb+2 lead(II) Lead Pb+4 lead(IV) Sn+2 tin(II) stannous cobaltous plumbous Tin Sn+4 tin(IV) plumbic stannic cobaltic Metals With Several Oxidation States Table (partial) Element Ion Formula Stock Name Old School

  19. *  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

  20. “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

  21. 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.

  22. CO3-2 carbonate CrO4-2 chromate OH- hydroxide Cr2O7-2 dichromate chlorate ClO3- O2-2 peroxide NO2- nitrite SO4-2 sulfate PO4-3 NO3- nitrate phosphate MnO4- permanganate Some Common Polyatomic Ions ( Radicals) Formula Formula Name Name Cations ammonium NH4+ Common Anions acetate C2H3O2- CN- cyanide

  23. 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

  24. Practice with Polyatomic Ions

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

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

  27. ... 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

  28. ... 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

  29. ... 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

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

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

  32. 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 _______________________

  33. 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

  34. PROBLEM: SOLUTION: Determining Names and Formulas of Covalent Compounds (a) What is the formula of carbon disulfide? (b) What is the name ofPCl5? (c) Give the name and formula of the compound whose molecules each consist of two N atoms and four O atoms. CS2 (a) Carbon is C, sulfide is sulfur S and di-means 2 • P is phosphorous, Cl is chloride, the prefix for 5 is penta-. Phosphorous pentachloride. • N is nitrogen and is in a lower group number than O (oxygen). • Therefore the formula is: • and the name is: N2O4 dinitrogen tetraoxide.

  35. 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______________

More Related