1. Unit 5 Nomenclature

2. ChemNotes 5.1: Naming of Ionic Compounds How do we communicate with other scientists? Obj: In this lesson you should learn: How to identify an ionic compound How to correctly name an ionic compound

3. Compound : Pure Substance composed of 2 or more different elements chemically combined; have a net charge of zero 4- 3

4.  Contain a cation (+) and an anion (-) Transfer electrons from the metal to the non-metal (definition of ionic bond) Usually solids at room temperature When dissolved, break apart into ions and conduct an electrical current. These are called electrolytes. Copyright © Houghton Mifflin Company 4- 4

5.  Group 1 +1 (loss of one electron)  Group 2 +2  Group 3 +3  Group 5/15 -3 (gain of 3 electrons)  Group 6/16 -2  Group 7/17 -1  Group 8/18 0

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9. 1) Write the symbol for the cation 2) Write the symbol for the anion  3) Balance the charges of the anion and cation  Count towards the noble gas – this will give you the charge If you go forward the charge is negative If you go back the charge is positive  Multiple as necessary so the charges cancel out! -

10. Magnesium chloride Potassium oxide Aluminum iodide Copyright © Houghton Mifflin Company 4-10

11.  Sodium bromide Calcium nitride  Lithium oxide Radium oxide  Barium chloride Aluminum phosphide  Strontium iodide Potassium fluoride  Aluminum sulfide Beryllium phosphide Copyright © Houghton Mifflin Company 4-11

12.  1) Ignore subscripts  2) Name the cation  3) Name the anion – remember the ending changes to -ide Copyright © Houghton Mifflin Company 4- 12

13.  KBr  Na 3 P  Al 2 O 3 Copyright © Houghton Mifflin Company 4- 13 Potassium Bromide Sodium Phosphide Aluminum Oxide

14.  CaS MgO  Li 2 O RaI 2  AlP Al 2 O 3  BaCl 2 K 2 S  Na 3 N BeCl 2 Copyright © Houghton Mifflin Company 4- 14

15. ChemNotes 5.2: Naming of Ionic Compounds cont…. How do we communicate with other scientists?   Obj: In this lesson you should learn:  How to correctly name an ionic compound that contains a transition metal Copyright © Houghton Mifflin Company 4- 15

16. Type II – Ionic Salts (Transition Metal, Tin, or Lead & Nonmetal) Copyright © Houghton Mifflin Company 4- 16

17. Table 4.2 Copyright © Houghton Mifflin Company 4- 17

18. Writing Formulas  Transition Metals have more than one oxidation number  Roman numerals are used to show oxidation state Copyright © Houghton Mifflin Company 4- 18

19.  1) Write down the symbols of the cation and anion  2) Balance the charges of the anion and cation  Count towards the noble gas – this will give you the charge of the ANION ONLY!  Multiple by the subscript as necessary.  3) Determine the charge of the cation – remember the whole compound must equal zero!!  Use Roman numerals to show charge of the cation Copyright © Houghton Mifflin Company 4- 19

20. Examples  Chromium (III) sulfide  Iron (III) bromide  Manganese (II) phosphide Copyright © Houghton Mifflin Company 4- 20

21. Practice  Chromium (III) bromide  Iron (III) sulfide  Lead (IV) chloride  Cobalt (II) oxide  Silver (I) nitride Copyright © Houghton Mifflin Company 4- 21

22. Practice cont.  Copper (II) fluoride  Scandium (III) phosphide  Iron (II) chloride  Zinc oxide  Tin (IV) oxide Copyright © Houghton Mifflin Company 4- 22

23. Naming Compounds  Write the name of the transition metal  Leave a space  Write the name of the anion  Determine the charge of the metal  Find the charge of the anion from the periodic table  Use the charge to determine the charge of the transition metal (remember the compound must equal ZERO!)  Write the number of the transition metal in roman numerals – place in parenthesis Copyright © Houghton Mifflin Company 4- 23

24. Examples  CuCl 2  Fe 2 O 3  PbS  FeP Copyright © Houghton Mifflin Company 4- 24

25. Practice  MnCl 3 Fe 2 O 3  PbCl 2 SnBr 4  AgCl AgS  ScP CdF 2  CrN Ti 2 O 3 Copyright © Houghton Mifflin Company 4- 25

26. Obj: In this lesson you should learn: How to identify a polyatomic ion How to correctly name an ionic compound that contains a polyatomic ion Copyright © Houghton Mifflin Company 4-26

27. 3 or more elements – contain at least one polyatomic ion Polyatomic ion – a group of atoms that work together as a single. This group of atoms has it’s own name and oxidation number 4-27 Copyright © Houghton Mifflin Company

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29. 1) Name the metal or positive polyatomic ion (Remember: transition metals, tin, & lead need a Roman numeral) 2) Name the nonmetal (use – ide) or negative poly atomic ion (don’t change name) Copyright © Houghton Mifflin Company 4-29

30. Al 2 (SO 4 ) 3 NH 4 Br Mg(OH) 2 NH 4 BrO 2 Sn 3 (PO 4 ) 2 ZnCrO 4 Copyright © Houghton Mifflin Company 4-30

31. Li 2 SO 4 Be 2 NO 3 Na 2 CO 3 KOH Al 2 SO 3 NH 4 Cl Al 2 (SO 4 ) 3 Copyright © Houghton Mifflin Company 4-31

32. NH 4 NO 3 Ba(C 2 H 3 O 2 ) 2 Mg(OH) 2 Cs 2 CrO 4 CaC 2 O 4 Co(ClO 3 ) 3 AgNO 3 Copyright © Houghton Mifflin Company 4-32

33. 1) Write the symbol for the cation (either metal or ammonium) 2) Write the symbol for the anion (either nonmetal or neg. poly) 3) Crisscross – if more than one poly is needed, put poly in parenthesis Copyright © Houghton Mifflin Company 4-33

34. Sodium carbonate Ammonium chloride Ammonium phosphate Iron (II) nitrate Barium hydroxide Copyright © Houghton Mifflin Company 4-34

35. Sodium sulfate Rubidium nitrate Cesium phosphate Francium oxalate Magnesium hydroxide Calcium carbonate Ammonium phosphate Copyright © Houghton Mifflin Company 4-35

36. Ammonium carbonate Calcium hydroxide Iron (III) chlorate Zinc (II) nitrate Strontium phosphate Aluminum hydroxide Radium cyanide Copyright © Houghton Mifflin Company 4-36

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38. Type III – Molecular Compounds ChemNotes 5.4: Naming of Molecular Compounds Obj: In this lesson you should learn: How to identify a molecular compound How to correctly name a molecular compound Copyright © Houghton Mifflin Company 4- 38

39. Molecular Compounds (Covalent Compounds) Contain only nonmetals Share electrons (covalent bond) Usually liquids or gases at room temperature Copyright © Houghton Mifflin Company 4- 39

40. Writing formulas Prefixes tell how many atoms (subscripts) of each element are present: 1mono 6hexa 2di 7hepta 3tri 8octa 4tetra 9nona 5penta 10deca 4- 40

41. Examples Carbon tetrachloride Sulfur dioxide Dinitrogen pentoxide Copyright © Houghton Mifflin Company 4- 41

42. Practice Nitrogen monoxide Sulfur trioxide Dinitrogen tetraoxide Oxygen dibromide Diphosphorus pentoxide Copyright © Houghton Mifflin Company 4- 42

43. Practice cont. Phosphorus trioxide Nitrogen trichloride Carbon monoxide Carbon dioxide Silicon dioxide Copyright © Houghton Mifflin Company 4- 43

44. Naming Molecular Compounds 1) Write the complete name of the first element - use a prefix only if there is more than one atom present 2) Write the second name as an anion (-ide) – always use a prefix Copyright © Houghton Mifflin Company 4- 44

45. Examples I 2 S 5 SeB 3 N 2 O Copyright © Houghton Mifflin Company 4- 45

46. Practice SO 3 NO 2 N 2 O 4 PCl 3 CO 2 SiO 2 NF 3 CBr 4 I 2 F 6 CO Copyright © Houghton Mifflin Company 4- 46