Honors Chemistry                                           Name_______________________

Nomenclature Packet—PMP 1

Mr. McAfoos                                                  Period______ Date____________

 

This packet contains everything you need to know about formula writing and nomenclature, the naming of compounds. It is organized into several worksheets, this first sheet on identifying types of compounds, and the rest on naming and writing formulas for specific types of compounds.

 

A definition:

Compound—A substance made of two or more elements bonded together. (At this point you don’t need to know how they’re bonded or even what bonded means. The real issue is that compounds are things that aren’t single elements and whose formula is written together. Two common examples: H2O and NaCl)

 

Some information that I hope you already know:

In a formula, subscripted numbers tell how many of the thing that precedes the number are in the formula. When no number is written, it is assumed to be 1.

Examples:

            H2O = 2 hydrogens and 1 oxygen

            Fe2O3 = 2 irons, 3 oxygens

Example with a polyatomic ion:

Ba3(PO4)2 = 3 bariums. 2 phosphates (each phosphate contains 1 phosphorus and 4 oxygens…so…there are 3 bariums, 2 phosphorus atoms and 8 oxygens.)

 

Types of compounds:

In this course we will be working with three different types of compounds, acids, ionic compounds and non-ionic compounds. The first step to naming compounds and writing formulas is to recognize these different types. When you are identifying these compound types you should ALWAYS look for acids first. Then, if you are looking at a formula, identify ionic compounds before non-ionics. If you are looking at a name, identify non-ionics first then ionics.

 

Three more thoughts:

1.      When you are identifying types of compounds, the subscripted numbers don’t matter! They come in when you name compounds and write formulas.

2.     Elements above and to the right of the stepped blue line on the chart are non-metals. All others are metals (except H—that’s a non-metal in the “wrong” place)

3.     When polyatomic ions are in formulas, the charges are “invisible.” You will need to recognize them by the element patterns. Ex: SO4 or Cr2O7

 

Recognizing Acids:

Acids are compounds that begin with H.

Examples:

HCl, HNO3, H2SO4, H3PO4 (Obviously, it doesn’t matter how many H’s)

Note: HCO3-1 starts with an H but it is an ion, NOT a compound. So…it has the properties of an acid (next to last unit of the year), but it is NOT named as an ion…you already know the name—bicarbonate.

 

When the name of an acid is written, it always ends with the word acid.

Examples: perbromic acid, nitrous acid, hydrocyanic acid.

 

Recognizing Ionic Compounds:

Ionic compounds always contain a metal and a non-metal OR a polyatomic ion.

Examples:

NaCl, BaS, Fe2O3, NH4Cl, Ca(OH)2, (NH4)2SO3

The names of ionic compounds are recognized because they contain the name of a polyatomic ion OR they end in ide. Ionic compound names NEVER contain number prefixes (mono, di, tri, etc.)

Examples:

lithium chloride, barium bichromate, ammonium acetate

 

Recognizing Non-Ionic Compounds:

Non-ionic compound formulas contain ONLY non-metals and do not contain a polyatomic ion.

Examples:

CO2, SF6, BrI3, NO2, P4O10

Names of Non-ionic compounds contain number prefixes (mono, di, tri, tetra, penta, hexa, hepta, octa, nona, deca)

Examples:

Sulfur dioxide, carbon tetrachloride, iodine trifluoride,

diphosphorus pentoxide

 

 

Some practice:

Put an A (for acid), I (for ionic) or N (for non-ionic) next to each of the names and formulas on the next page. (Ignore the problem numbers!)

1. ammonium sulfide             26. nickel(II) iodide

2. sodium nitrate               27. mercurous oxide

3. cupric bromide               28. lead(II) chlorite

4. aluminum sulfate             29. hydrogen iodide

5. potassium nitrate            30. iron(II) bisulfite

6. ferrous carbonate            31. magnesium nitrate

7. lead(II) phosphate           32. iron(III) chromate

8. diphosphorus pentoxide       33. iron(II) chromate

9. cupric hydroxide             34. copper(II) hydroxide

10. calcium fluoride            35. cuprous carbonate

11. nickel(II) nitrate          36. chromic acetate

12. silver cyanide              37. calcium chlorate

13. ammonium sulfite            38. ammonium oxide

14. zinc sulfate                39. aluminum perchlorate

15. tin(II) chloride            40. zinc bicarbonate

16. antimony(III) chloride      41. sodium phosphate

17. silver sulfide              42. silver hypochlorite

18. magnesium hydroxide         43. ammonium phosphate

19. ammonium carbonate          44. ferrous chlorite

20. nickel(II) acetate          45. potassium sulfide

21. sodium chromate             46. tin(IV) bromide

22. chromic bisulfate           47. lithium chromate

23. potassium permanganate      48. magnesium bisulfate

24. silver perchlorate          49. ferrous phosphate

25. potassium phosphate         50. calcium sulfate

 

151. HgF2               176. H3PO4

152. KCl                177. LiMnO4

153. KMnO4              178. Fe2(HPO4)3

154. KClO4              179. Na2CO3

155. ZnO                180. Mg(HCO3)2

156. Ba(OH)2            181. Sn3(PO4)4

157. NH4MnO4             182. HNO3

158. CaCO3              183. ZnCl2

159. Ba3(PO4)2           184. NaH2PO4

160. Fe2O3               185. Hg2Cl2

161. CoF3               186. Fe(NO2)2

162. H2CO3               187. CuNH4PO4

163. K2SO4               188. NaMgPO4

164. NaHSO4             189. Sn(HCO3)4

165. PF5                190. NaMnO4

166. Ag2O               191. KF

167. Pb(ClO2)2           192. CaSO4

168. Cu2CrO4             193. HCl

169. Ca(ClO4)2           194. SbCl3

170. HC2H3O2             195. As4O10

171. LiI                196. NH4Cl

172. Al2(SO4)3           197. NH4NO3

173. HBr                198. IF5

174. Hg2(ClO)2           199. NaHCO3

175. CrCl3              200. Ba(OH)2