1. Chapter 5: Molecules and Compounds

2.  Distinguish between common and systematic names for compounds.  Name binary ionic compounds containing a metal that forms only one type of ion.  Name binary ionic compounds containing a metal that forms more than one type of ion.  Name ionic compounds containing a polyatomic ion.

3.  Chemists have developed systematic ways to name compounds.  If you learn the naming rules, you can examine a compound’s formula and determine its name, and vice versa.  Many compounds also have a common name.  NaCl has the common name salt and the systematic name sodium chloride.

4.  Identify if the metal cation has more than one potential charge.  Such metals are usually (but not always) found in the transition metals section of the periodic table.  Notable Exceptions: ▪ Always Zn 2+ and Ag + ▪ Sn and Pb can have multiple charges

7.  Binary compounds are those that contain only two different elements. The names for binary ionic compounds containing a metal that forms only one type of ion have the following form: Name of Cation + Base Name of Anion + ide

8.  Since the charge of the metal is always the same for these types of compounds, it need not be specified in the compound’s name.  Example: MgF 2

10.  Name these compounds:  CaO  Al 2 O 3  KF  MgCl 2  Li 3 N

11.  Write the formula for these ionic compounds:  Potassium bromide  Sodium oxide  Zinc nitride

12.  If the cation could have more than one charge, then the charge must be specified in the metal’s name.  We specify the charge with a Roman numeral (in parentheses) following the name of the metal.

13.  For example, we distinguish between Cu + and Cu 2+ by writing a (I) to indicate the 1+ ion or a (II) to indicate the 2+ ion:  Cu + Copper(I)  Cu 2+ Copper(II)

14.  These compounds are named using the following form: Name of Cation Base Name of Anion + ide (charge of metal in roman numerals) ++

15.  We can determine the charge of the metal from the chemical formula of the compound.  The sum of all the charges must be zero.

16.  What is the charge of iron in FeCl 3 ?  +3  What is the name for FeCl 3 ?  Iron (III) Chloride

17.  Name the following compounds:  PbCl 4  PbO  Explain why CaO is not named calcium (II) oxide.

18.  Write the formula for the following compounds:  Chromium (II) chloride  Tin (IV) oxide  Iron (III) oxide

19.  Ionic compounds containing polyatomic ions are named using the same procedure we apply to other ionic compounds, except that we use the name of the polyatomic ion whenever it occurs.

20.  For example, we name KNO 3 using its cation, K +, potassium, and its polyatomic anion, NO 3 -, nitrate.  KNO 3 potassium nitrate

21.  Fe(OH) 2  NH 4 NO 3

22.  Write the formula for the following compounds:  barium nitrate  ammonium iodide  iron (III) hydroxide

23.  Many polyatomic ions are oxyanions, anions containing oxygen.  When a series of oxyanions contain different numbers of oxygen atoms, they are named systematically according to the number of oxygen atoms in the ion.

24.  If there are two ions in the series, the one with more oxygen atoms is given the ending -ate and the one with fewer is given the ending -ite.  NO 3 − nitrate SO 4 2− sulfate NO 2 − nitriteSO 3 2− sulfite

25.  If there are more than two ions in the series, then the prefixes hypo-, meaning “less than,” and per-, meaning “more than,” are used.  ClO − hypochloriteBrO − hypobromite ClO 2 − chloriteBrO 2 − bromite ClO 3 − chlorateBrO 3 − bromate ClO 4 − perchlorateBrO 4 −perbromate

26.  K 2 CrO 4  Mn(NO 3 ) 2

27.  Write the formula for the following compounds:  sodium perchlorate  sodium chlorite  sodium nitrate  sodium nitrite