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

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

3. 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. Understanding Nomenclature

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 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 ex:NaCl sodium chloride KBr potassium bromide The first word (metal or positive ion) remains the same word

7. 1. Using the rules given, name the compounds listed below. 1. MgO ____________________2. CaI 2 __________________ 3. BaS ____________________4. ZnI 2 ______________________ 5. CaO ____________________6. Ag 2 O_____________________ 7. K 3 P ____________________8. AlBr 3 _____________________ 9. Na 3 N ____________________10. MgS_____________________

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

9. Crisscross Method simplified method for writing these formulas Calcium and bromide = calcium bromide Ca 2+ Br 1- = 0 Ca 2+ Br 1- Ca 2+ Br 1- 1 2 2+ 2- = 0 1 2 **But we don’t write ones!!!CaBr 2 Subscripts Ca 1 Br 2

10. Crisscross Method simplified method for writing these formulas aluminum and sulfide = aluminum sulfide Al 3+ S 2- = 0 Al 3+ S 2- Al 3+ S 2- 2 3 6+ 6- = 0 2 3 Al 2 S 3 Subscripts Al 2 S 3

11. 12. sodium chloride ____________13. potassium iodide __________ 14. magnesium sulfide __________15. aluminum bromide__________ 16. strontium oxide ____________17. sodium sulfide__________ 18. rubidium phosphide _________19. barium nitride__________ Using the rule given, give the formula for these compounds

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

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

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

16. 4. Name the following compounds. 21. CuO ______________________ 22. PbS ________________________ 23. HgCl ______________________ 24. MnO 2 _________________________ 25. Fe 2 S 3 ______________________ 26. SnBr 2 ________________________ 27. BiCl 3 ______________________ 28. PbCl 4 ________________________ Type II Binary Compounds lead (II) sulfide

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

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. 29. ferric chloride_____________________________________ 30. stannic oxide_____________________________________ 31. mercuric iodide_____________________________________ 32. cuprous oxide_____________________________________ 33. plumbous sulfide_____________________________________ 34. antimonic bromide ___________________________________ 35. aurous phosphide_____________________________________ “Old School” The "ous"-"ic" System (“old school”) (Stock) formula tin (IV) oxide SnO 2

21. A ternary compound contains three or more different elements. Ternary compounds usually contain one or more polyatomic ions ( radicals ). Polyatomic ions ( radicals )are treated just like an ion. When writing the formula – the basic rules apply. Ternary Compounds It takes “3” or more Examples: Fe(ClO 4 ) 2 ; NaOH : NH 4 MnO 4

23. Ex: Calcium hydroxide Calcium and hydroxide = calcium hydroxide Ca 2+ OH 1- = 0 Ca 2+ OH 1- 1 2 Ca OH 2 Subscripts CaOH 2 But OH 2 = H 2 O = 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. ( ) Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions

24. Practice with Polyatomic Ions NH 4 OH Ba(OH) 2 Fe(CN) 3 Zn(C 2 H 3 O 2 ) 2 ammonium sulfide plumbous hydroxide ammonium hydroxide barium hydroxide iron (III) cyanide zinc acetate (NH 4 ) 2 S Pb(OH) 2

25. ... the `ate chart CO 3 2- NO 3 - ClO 3 - CrO 4 2- PO 4 3- MnO 3 - SO 4 2- -3-2 Polyatomic Ions – they all contain oxygen

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

27. ... the `ate become… `ites – they all lose an oxygen.. but the charge remains the same CO 2 2- NO 2 - ClO 2 - CrO 3 2- PO 3 3- MnO 2 - SO 3 2- -3-2

28. ... the `ate; the `ite; now the hypo- – subtract another oxygen !! and the charge remains the same CO 2- NO - ClO - CrO 2 2- PO 2 3- MnO - SO 2 2- -3-2

29. – lets add an oxygen … the Per-... the `ate; the `ite; the hypo.. and the charge remains the same CO 4 2- NO 4 - ClO 4 - CrO 5 2- PO 5 3- MnO 4 - SO 5 2- -3-2

30. ClO 2 -1 ClO 4 -1 ClO 3 -1 ClO -1 perchlorate chlorate chlorite hypochlorite `ate `ite hypo- per-

31. Na 2 CO 3 CO 3 -2 HCO 3 -1 carbonate bicarbonate carbonate versus bicarbonate NaHCO 3 sodium carbonate sodium bicarbonate add H + and drop a negative charge

32. 36. AlPO 4 ______________________37. (NH 4 ) 2 CO 3 _______________________ 38. __________ lithium cyanide39. ___________ copper(II) nitrate 40. KClO ______________________41. Zn(C 2 H 3 O 2 ) 2 ______________________ 42. __________ calcium phosphate43. ___________ ammonium sulfite 44. __________ ammonium acetate45. NaMnO 4 _______________________ Determining Names and Formulas of Ionic Compounds Containing Polyatomic Ions

33. Naming Covalent Molecular Compounds Use these Prefixes: Greek prefixes to indicate number (never use mono on first) mono - 1 di - 2 tri - 3 tetra - 4 penta - 5hexa - 6 hepta - 7 octa - 8 nona - 9 deca – 10 Nonmetal to Nonmetal ( or to the right of the zigzag red line) Ex: BF 3 NO N 2 O 5 boron trifluoride dinitrogen pentoxide nitrogen monoxide

35. 1. CO __________________________ 8. diphosphorus pentoxide _________________ 2. PBr 3 ______________________________ 9. carbon dioxide _________________ 3. CCl 4 ______________________________ 10. selenium trioxide _________________ 4. NCl 3 ______________________________ 11. sulfur hexafluoride _________________ 5. SeO 2 ______________________________ 12. phosphorus pentiodide ________________ 6. P 2 O 3 _____________________________ 13. sulfur tribromide ________________ 7. NH 3 ______________________________ 14. phosphorus hexachloride______________ Naming Covalent Molecular Compounds