2. Ionic Nomenclature

3. Cation Defn: A positively charged particle. Name of metal+ the word “ion”. Ex. Potassium Potassium Ion

4. Anion Defn: a negatively charged particle. Name of non-metal w/ ending changed to “ide” Ex. Chlorine Chloride

5. Binary Ionic Compounds Contains only 2 different elements in the compound Naming the Compounds Name of metal + Name of non-metal with “ide” ending. Ex NaCl Sodium Chloride

6. More Examples MgO Magnesium Oxide MgCl 2 Magnesium Chloride LiBr Lithium Bromide Ca 3 P 2 Calcium Phosphide

7. Transition Metals Transition metals can give up different numbers of electrons Therefore they can have multiple charges (This applies to lead and tin, too.) Ex. If Titanium loses 3e- Ti 3+

8. Roman Numerals Tells the charge of the ion preceding it. When an ion can have more than one charge, you need to use a roman numeral to specify the charge. Ex Lead Pb 2+ Lead (II) ion Pb 4+ Lead (IV) ion

9. Exceptions If the transition metal only has one charge, then DO NOT use a roman numeral! Ex. Zinc Zn 2+  Zinc ion What are other examples of a transition metal with only one charge? Ag +, Cd 2+, Sc 3+

10. Reminder Roman numerals tell the charge of an ion, NOT HOW MANY! Ex. Gold (III) chloride What is the charge of the gold ion in gold (III) chloride? 3+

11. Example: Tin (II) bromide What is the charge of the tin ion in tin (II) bromide? 2+

12. Writing Formulas The positive and negative charges must equal ZERO in the compound. 1. Write the symbol and charge for each individual ion 2. Use the least common denominator (LCD) to determine how many of each ion is needed in order to make a zero net charge. 3. Write the formula, using a subscript(s) to indicate the number of each ion in the compound

13. Example Zinc sulfide ZZn 2+ S 2- ZZnS

14. Sodium Oxide Na + O 2- Na 2 O

15. Scandium bromide Sc 3+ Br – ScBr 3

16. Naming ionic compounds with polyatomic ions (tertiary ionic compounds): 1. Name of cation first 2. Name of anion second 3. Remember roman numerals, if necessary 4. Enclose polyatomic ions in parenthesis when it requires a subscript

17. Example Zn 2+ SO 4 2- Balanced Formula? ZnSO 4 Name? Zinc sulfate

18. Calcium Phosphate Ca 2+ PO 4 3- Balanced Formula? Ca 3 (PO 4 ) 2 Name? Calcium Phosphate

19. Manganese (IV) Nitrite Mn 4+ NO 2 - Balanced Formula? Mn(NO 2 ) 4 Name? Manganese(IV) Nitrite

20. MgCl 2

21. CuSO 4

22. Example: Copper (I) Chlorate Cu + ClO 3 - Balanced Formula? CuClO 3 Name? Copper (I) Chlorate

23. Chromium (III) Hydroxide Cr 3+ OH - Balanced Formula? Cr(OH) 3 Name? Chromium(III) hydroxide

24. NaNO 3

25. Al(OH) 3

26. Cu 3 PO 4

27. Covalent Nomenclature aka Molecular Compounds

28. To Name Covalent Compounds: 1. Translate the subscript of the first element into a prefix + the name of the element 2. Translate the subscript of the 2nd element into a prefix + root name of element with the “ide” ending 1 Mono4 Tetra7 Hepta 2 Di5 Penta8 Octa 3 Tri6 Hexa9 Nona 10 Deca

29. NOTE If there is only 1 of the 1st element, do not use a prefix Ex. CO carbon monoxide

30. Name the Following Compounds N 2 O Dinitrogen monoxide PCl 3 Phosphorus trichloride SF 6 Sulfur hexafluoride

31. CO 2 Carbon dioxide NO nitrogen monoxide CCl 4 carbon tetrachloride

32. To Write Formulas for Covalent Compounds: 1. Correlate the prefix of the 1st element to its numerical value…write it as the subscript 2. Correlate the prefix of the 2nd element to its numerical value…write it as the subscript 3. Prefix should match the subscript written for each element *Remember, if there is not a prefix, then it’s just 1.

33. Write the formula for each Tetraiodine nonoxide I 4 O 9 Sulfur trioxide Phosphorus pentafluoride

34. Nitrogen dioxide NO 2 Dichlorine heptoxide Cl 2 O 7 Carbon disulfide CS 2

35. Acid Nomenclature

36. Naming Acids Acids always have hydrogen. Binary Acids Hydrogen + 1 other element Oxy Acids Hydrogen + oxygen (from a polyatomic ion)

37. Binary Acids 1. Use “hydro” for hydrogen 2. Root of 2nd element + ic (take off the ending) 3. add “acid” to the end Ex : HCl Hydrochloric acid

38. Name the Binary Acids H 2 S Hydrosulfuric acid (notice here that it is sulfuric, not sulfic) HF Hydrofluoric acid HBr Hydrobromic acid

39. Oxy Acids “ite” The name of the acid comes from the name of the polyatomic ion. If the polyatomic ion ended in “–ite”, then the ending for the acid is “–ous” Take off the “ite” ending of the polyatomic ion and add –”ous” Add the word “acid” Ex. HNO 2 Nitrous Acid

40. Name the oxy acids H 2 SO 3 Sulfite Ion Sulfurous acid H 3 PO 3 Phosphite Ion Phosphorous acid

41. Oxy Acids “ate” If the polyatomic ion ended in “–ate”, then the ending for the acid is “–ic” Take off the “ate” ending of the polyatomic ion and add –”ic” Add acid Ex. HNO 3 nitrate ion Nitric acid

42. Name the oxy acids H 2 SO 4 Sulfate ion Sulfuric Acid H 3 PO 4 Phosphate ion Phosphoric Acid

43. Writing formulas for binary acids Determine what kind of acid it is; binary or oxy Does it have hydro at the front? If yes, then it is binary Determine the charges for the individual ions Write the formula so that the overall charge equals zero

44. Example Hydroiodic acid H + I - HI Hydroselenic acid H + Se 2- H 2 Se

45. Writing formulas for oxy acids Determine what kind of acid it is; binary or oxy Does it have -ous or –ic at the end? If yes, then it is an oxy acid Determine the charges for the individual ions Write the formula so that the overall charge equals zero

46. Example Chlorous acid from chlorite ion ClO 2 -  HClO 2 Boric acid From borate ion BO 3 3-  H 3 BO 3 Chloric acid from chlorate ion ClO 3 -  HClO 3

47. Examples Sulfurous acid from sulfite ion, SO 3 2-  H 2 SO 3 Carbonic acid from carbonate ion, CO 3 2-  H 2 CO 3