Dry Lab: Making Ionic Compounds Puzzle Activity
Introduction
When metals and non-metals chemically react, the atoms will tend to form ions or charged
atoms. Ions form because electrons are either gained or lost. Metals will generally lose
electrons to form CAtIONS (positive ions). This is because metals tend to donate electrons in
order to achieve a stable octet. Non-metals will gain electrons to form ANIONS (negative ions),
since they tend to accept electrons in order to achieve a full valence shell (stable octet).
Activity
In this activity you will “build” models of binary ionic compounds (“binary” here means 2 types of
ions, a cation and an anion) and write their corresponding chemical formula. Some of the ions will
be polyatomic ions meaning molecules made up of 2 or more atoms that are considered an ionic
group, that is, a molecule with a charge e.g. sulfate (SO4)2-,___________________________.
Instructions:
1. You will each receive a baggie of individual “ion” puzzle pieces
2. Your job is to make the ionic compounds below by fitting
together as many pieces of each ion need until all the bonds for
each ion have been filled (the heights will be equal).
3. Record the formula by counting the number of each ion needed.
4. The first entry in the table is done as an example for you using
the puzzle pieces to the right 
Ionic Compound
Name
barium
chloride
aluminum
phosphide
Iron (II)
sulfate
Iron (II)
sulfide
Lithium
phosphate
Sodium
oxide
Calcium
nitride
Cation name (symbol)
barium (Ba2+)
Anion name (symbol)
chloride (Cl1-)
Ionic compound
Formula
BaCl2
Iron (III)
oxide
Ammonium
bromide
Ammonium
sulfide
Copper (II)
permanaganate
Copper (I)
nitrate
Make your own using
blank pieces
Make your own using
blank pieces
Follow up Questions (answer on a separate sheet):
1.
Is there any 2 ions you can’t combine to make a binary compound? Explain.
2. How is the # of ions in the compound’s formula related to the CHARGE of the ion?
3. What is the overall or “net” charge of EACH compound? (Hint: if you add up all the +’s and the –‘s)
4. How is lithium nitride different from lithium nitrate? How is it the same?
5. How does sodium sulfate compare to sodium sulfide?
6. What other ion on the periodic table is permanganate like? Explain.
7. What would be the formula for:
a. Potassium manganate ______________
d. zinc bromide
b. Potassium hydroxide _______________
e. lithium sulfate _______________
c. Calcium hydroxide _______________
f. calcium sulfide ________________
________________
Positive Ions
Sodium
iron (II)
Lithium
iron (III)
Calcium
copper (I)
Magnesium
copper (II)
Ammonium
Aluminum
Negative Ions
Fluoride
sulfide
nitride
nitrate
Chloride
oxide
phosphide
permanganate
Bromide
sulfate