ࡱ> \^[@ `jbjbqq .l Wljjjj8$j########,$ &##****#*,>,#** |w$'Mjj{w##'*'w*Ionic compounds are generally composed of a metal and a nonmetal. Formulas for ionic compounds are always written using the lowest whole number ratios of the cation (positive ion) and anion (negative ion). Ionic compounds are named by first naming the cation and then the anion. For monatomic cations with only one possible positive charge (elements in group 1, 2, 3 and Al3+, see oxidation numbers on the Periodic Table), simply name the element of the cation, i.e. Na+ is the sodium ion. For monoatomic anions (nonmetals), the negative charges typically are the same as the number of electrons required to obtain a Noble Gas electronic configuration. To name a monoatomic anion, take the root of the elements name and add the suffix ide, i.e. Cl- is the chloride ion. Therefore, to name a simple binary ionic compound such as NaCl, name the cation and then the anion ending in ide, i.e. sodium chloride. In some cases the cation can have more than one possible charge (usually a d-block metal). It is therefore necessary to use the so-called stock naming system by indicating the charge of the cation using a Roman numeral after the cations name. For example, Fe2O3 is named iron (III) oxide, whereas FeO is iron (II) oxide. In some cases, the ionic compound will contain polyatomic ions. To name these compounds, again simply name the cation and then the anion. Table 1 contains a list of cations and anions, along with their names. These ions can be used to complete the following. Table 1. Formulas and Names of various selected cations and anions. FormulaNameFormula NameNH4+Ammonium ionF-Fluoride ionLi+Lithium ionCl-Chloride ionNa+Sodium ionBr-Bromide ionK+Potassium ionI-Iodide ionMg2+Magnesium ionO2-Oxide ionCa2+Calcium ionS2-Sulfide ionSr2+Strontium ionN3-Nitride ionSc3+Scandium ionC4-Carbide ionCr2+Chromium (II) ionNO3-Nitrate ionCr3+Chromium (III) ionNO2-Nitrite ionCr6+Chromium (VI) ionCO32-Carbonate ionFe2+Iron (II) ionSO42-Sulfate ionFe3+Iron (III) ionSO32-Sulfite ionMn2+Manganese (II) ionPO43-Phosphate ionMn3+Manganese (III) ionPO33-Phosphite ionCu+Copper (I) ionClO-Hypochlorite ionCu2+Copper (II) ionClO2-Chlorite ionPb2+Lead (II) ionClO3-Chlorate ionZn2+Zinc ionClO4-Perchlorate ionAl3+Aluminium ionOH-Hydroxide ion Fill in the blank spaces of the following table. FormulaCationAnionName of ionic compound KCl  Ca2+  CO32- Iron (II) sulfate  Fe2(SO4)3  Mg2+  Cl- Chromium (III) Chloride Zn3(PO4)2  Al3+  OH- ammonium nitrate  (NH4)2SO4  Na+  F- Copper (II) sulfate  Ca(NO3)2  Zn2+  N3-Answers FormulaCationAnionName of ionic compound KCl  K+ Cl- Potassium chloride CaCO3 Ca2+  CO32- Calcium carbonate FeSO4 Fe2+ SO42- Iron (II) sulfate  Fe2(SO4)3  Fe3+ SO42- Iron (III) sulfate MgCl2 Mg2+  Cl- Magnesium chloride CrCl3 Cr3+ Cl- Chromium (III) Chloride Zn3(PO4)2  Zn2+ PO43- Zinc phosphate Al(OH)3 Al3+  OH- Aluminum hydroxide NH4NO3 NH4+ NO3- ammonium nitrate  (NH4)2SO4  NH4+ SO42- Ammonium sulfate NaF Na+  F- Sodium fluoride CuSO4 Cu2+ SO42- Copper (II) sulfate  Ca(NO3)2  Ca2+ NO3- Calcium nitrate Zn3N2 Zn2+  N3- Zinc nitride Name _________________________ Naming Ionic Compounds Van Der Sluys, 2004 xz 2 ' B E F H V X h j x z   # 2 5 C F U X l m o ~ !$9:=NQghk|~H*H*5b & ' / 4 = B $$Ifa$ ! !  & ' / 4 = B C H U X e f j v z   # / 0 5 B F R S X j o { | $7=KLQekyz~ bB C H U X e f j v z n````n````n $$Ifa$ !$$Ifl\:,"064 la ``$$Ifl\:,"064 la $$Ifa$ !   ``$$Ifl\:,"064 la $$Ifa$ !  # / 0 5 B F R S X j o ``$$Ifl\:,"064 la $$Ifa$ ! o { | ``$$Ifl\:,"064 la $$Ifa$ ! n````n````n $$Ifa$ !$$Ifl\:,"064 la $7=KLQekyz~``$$Ifl\:,"064 la $$Ifa$ ! ~``$$Ifl\:,"064 la $$Ifa$ ! .0s#%*,IJKLNOYZ^`  "#$%'*+-.1IJMN5H*5H*5H*H*_,0>?@rs{ !&'(,-./012CDEFPQRSTUVW[\] b,0``$$Ifl\:,"064 la $$Ifa$ ! 0>?@rs{`ZZZ`( !$$Ifl\:,"064 la $$Ifa$ ! `D$$Ifl\:,"064 la $$Ifa$ ! ```@$$Ifl\:,"064 la $$Ifa$ ! `<$$Ifl\:,"064 la $$Ifa$ ! `t`@$$Ifl\:,"064 la $$Ifa$ !  !&'(`<$$Ifl\:,"064 la $$Ifa$ ! 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