Periodic Table Worksheet - SCASD



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 cation’s 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.

|Formula |Name |Formula |Name |

|NH4+ |Ammonium ion |F- |Fluoride ion |

|Li+ |Lithium ion |Cl- |Chloride ion |

|Na+ |Sodium ion |Br- |Bromide ion |

|K+ |Potassium ion |I- |Iodide ion |

|Mg2+ |Magnesium ion |O2- |Oxide ion |

|Ca2+ |Calcium ion |S2- |Sulfide ion |

|Sr2+ |Strontium ion |N3- |Nitride ion |

|Sc3+ |Scandium ion |C4- |Carbide ion |

|Cr2+ |Chromium (II) ion |NO3- |Nitrate ion |

|Cr3+ |Chromium (III) ion |NO2- |Nitrite ion |

|Cr6+ |Chromium (VI) ion |CO32- |Carbonate ion |

|Fe2+ |Iron (II) ion |SO42- |Sulfate ion |

|Fe3+ |Iron (III) ion |SO32- |Sulfite ion |

|Mn2+ |Manganese (II) ion |PO43- |Phosphate ion |

|Mn3+ |Manganese (III) ion |PO33- |Phosphite ion |

|Cu+ |Copper (I) ion |ClO- |Hypochlorite ion |

|Cu2+ |Copper (II) ion |ClO2- |Chlorite ion |

|Pb2+ |Lead (II) ion |ClO3- |Chlorate ion |

|Zn2+ |Zinc ion |ClO4- |Perchlorate ion |

|Al3+ |Aluminium ion |OH- |Hydroxide ion |

Fill in the blank spaces of the following table.

|Formula |Cation |Anion |Name 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

|Formula |Cation |Anion |Name 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 |

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