Ionic Compound Worksheet Packet

Name ______Period ____

Ionic compounds are when one or more electrons are transferred from one atom to another, creating a neutralcompound. It consists of a cation and an anion. Usually it is a metal and a nonmetal, but it can contain polyatomic ions. The goal of making the compound is to get the positive charge to equal the negative charge.

Na+ + Cl- = NaCl

The sodium chloride ion is neutral because the positive charge of sodium is cancelled out by the negative charge of the chlorine.

Ca2+ + Cl- = CaCl2

In order for the calcium chloride ion to be neutral, there has to be two chloride ions for every one calcium ion. This is because the calcium ion has a positive two charge and the chloride ion is negative one. You can use the criss-cross method to figure out how many of each atom you need. To figure out the correct formula, you can criss-cross the number of the charge of the ion to become the subscript of the opposite ion. You do not write a positive or negative symbol for the subscript. See examples below. If one of the ions is a polyatomic ion, you must use parenthesis if there is more than one ion. You always want the lowest whole numbers as subscripts.

Combine the following ions to make compounds

  1. Na+ and F-______
  2. NH4+ and O2-______
  3. LI+ and P3-______
  4. Na+ and ClO3-______
  5. Al3+ and Se2-______
  6. Ca2+ and OH-______

To write the formula from the name of a compound is done by following these steps.

  1. Write the ionic symbol for the cation.
  2. Write the ionic symbol for the anion.
  3. Combine the two ions in the correct amount to get a neutral compound.

Remember: certain metals can make more than one ion. These ions must use roman numerals to tell you the charge of the ion. Below you will find a chart of the common metals with more than one ion.

Element / Ion / Name of Ion
Chromium / Cr2+ / Chromium (II) ion
Cr3+ / Chromium (III) ion
Cobalt / Co2+ / Cobalt (II) ion
Co3+ / Cobalt (III) ion
Copper / Cu+ / Copper (I) ion
Cu2+ / Copper (II) ion
Iron / Fe2+ / Iron (II) ion
Fe3+ / Iron (III) ion
Lead / Pb2+ / Lead (II) ion
Pb4+ / Lead (IV) ion
Manganese / Mn2+ / Manganese (II) ion
Mn3+ / Manganese (III) ion
Mn4+ / Manganese (IV) ion
Mercury / Hg22+ / Mercury (I) ion
Hg2+ / Mercury (II) ion
Tin / Sn2+ / Tin II) ion
Sn4+ / Tin (IV) ion
  1. Complete the following chart.

Name of Compound / Cation / Anion / Compound Formula
Lithium Chloride / Li+ / Cl- / LiCl
Potassium Phosphate
Sodium Sulfide
Lead (II) Oxide
Ammonium Oxide
Lithium Carbonate
Copper (I) Sulfate
Calcium Chloride
Potassium Iodide
Ammonium Nitrate
Manganese (IV) Nitride
Calcium Bromide
Aluminum Oxide

To name an ionic compound, you take the name of the cation and the name of the anion drop the ion ending and combine the names.

KNO3 the potassium ion and the nitrate ion = potassium nitrate

Cu3N the copper (I) ion and the nitride ion = copper (I) nitride

  1. Write the name of the following compounds.

Compound Formula / Compound Name
BaCO3
Sr(C2H3O2)2
NaOH
NH4Cl
Ca3(PO4)2
Fe(NO3)3
Ag2CO3
KC2H3O2
Fe(OH)2
Name of Compound / Positive ion / Negative ion / Formula
  1. Sodium Iodide
/ Na+ / I- / NaI
  1. Silver sulfide
/ Ag+ / S2- / Ag2S
  1. Barium sulfate

  1. Lithium sulfide

  1. Sodium hydroxide

  1. Ammonium chlorate
/ ClO3-
  1. Zinc sulfate
/ Zn2+
  1. Iron(III) phosphate
/ Fe3+
  1. Nickel (II) hydroxide
/ Ni2+
  1. Chromium (III) oxide
/ Cr3+
  1. Iron (III) sulfate

  1. Copper (II) nitrate

  1. copper (II) carbonate

  1. magnesium phosphide

  1. aluminum nitrate

  1. sodium phosphate

  1. aluminum sulfate

  1. aluminum sufide

  1. iron (III) sulfite

  1. ammonium carbonate

Complete the chart. Remember these rules:

  1. The number of atoms of each element (or polyatomic ions) is written in the space below the line and to the right of the symbol as a subscript.
  2. When the number of atoms (or polyatomic ions) is one, the one is “understood” and you do not write anything.
  3. The cation is written first in the formula.
  4. Use (parentheses) only when necessary.

Compound made of / Cation / Anion /

Formula

/

Compound Name

/

Number of atoms in compound

  1. calcium and
nitrate
  1. tin (IV) and
chloride
  1. copper (II) and
carbonate
4. barium and
bromide
  1. tin (II) and
sulfite
  1. Ammonium and
Nitrate
  1. Lithium and
phosphorus
  1. Sodium and
Bicarbonate
  1. Lead (II) and
Phosphate
  1. magnesium and
hydroxide
  1. silver and
sulfide
  1. barium and
acetate
  1. fluorine and
manganese (II)