Name:_________________________________
Date:_______________________________
Types of Chemical Reactions
Station A
Part 1
Place a small crystal of copper (II) sulphate pentahydrate in a Pyrex test tube. Heat the tube gently at a 45° angle using a
Bunsen burner and a test tube holder. Make at least three distinctive qualitative observations during the heating process.
SAFETY: when heating, point the mouth of the test tube away from classmates. Do not touch the test tube
with your hands!
Part 2
Place the test tube in a test tube rack and let sit until cool to the touch. Using the water bottle provided add a few drops of
water to the test tube
SAFETY: do not add cold water to a hot test tube as you run the risk of shattering the glassware.
Observations
Appearance of compound(s) (including state) before the
experiment
Observations during/after the experiment
Part 1
1)
2)
3)
Part 2
Type of chemical reaction (be as specific as possible):
Part 1:
Part 2:
Balanced chemical equation:
Part 1:
Part 2:
Station B
1.
2.
3.
4.
Remove a small piece of steel wool from the wool pad on the lab bench.
Pull it apart so that the wool strands are loosely separated.
Use crucible tongs to hold the steel wool in the Bunsen burner flame.
Record any changes observed. Be specific in your descriptions. Fe will form a +3 charge product.
Appearance of compound(s) (including state) before the
.
experiment
Observations during/after the experiment
Observations
Type of chemical reaction (be as specific as possible):
Balanced chemical equation:
Station C
A strip of iron has been placed into a solution of copper (II) sulphate. Observe the change(s) in the submerged portion of the
iron strip as well as the solution.
Observations
Appearance of compound(s) (including state) before the
experiment
Type of chemical reaction (be as specific as possible):
Balanced chemical equation:
Observations during/after the experiment
Station D
Part 1
Add 1.0 M hydrochloric acid (until ¾ full) to a test tube. Place two pieces of mossy zinc into the test tube.
Part 2
Cover the mouth of the test tube with your thumb. When enough pressure has built up perform a “pop test” by having your
partner light a wooden splint and placing it at the mouth of the test tube.
Part 3
Carefully drain the HCl into a waste beaker and remove the mossy zinc. Rub the zinc against a piece of white paper.
Observations
Appearance of compound(s) (including state) before the
experiment
Part 1
Part 2
Part 3
Type of chemical reaction (be as specific as possible):
Part 1:
Part 2:
Part 3: ​
N/A
Balanced chemical equation:
Part 1:
Part 2:
Part 3: ​
N/A
Observations during/after the experiment
Station E
Part 1
Using a pipette or eyedropper add approximately 1 mL each of sodium sulphate and barium chloride into a test tube.
Part 2
Using a pipette or eyedropper add approximately 1 mL each of iron(III)sulphate and sodium hydroxide into a test tube.
Part 3
Using a pipette or eyedropper add approximately 1 mL each of sodium carbonate and calcium chloride into a test tube.
Observations
Appearance of compound(s) (including state) before the
experiment
Part 1
Part 2
Part 3
Type of chemical reaction (be as specific as possible):
Part 1:
Part 2:
Part 3:
Balanced chemical equation:
Part 1:
Part 2:
Part 3:
Observations during/after the experiment
Station F (TEACHER
​
DEMO)
Fill a test tube halfway with water and then place in a test tube rack. Add 3­4 drops of phenolphtalein Using a scupula place 1
or 2 pieces of calcium and perform a pop test.
Observations
Appearance of compound(s) (including state) before the
experiment
Observations during/after the experiment
Type of chemical reaction (be as specific as possible):
Balanced chemical equation:
Station G (​
TEACHER DEMO)
1.
2.
3.
4.
Place 1-2 cm of hydrogen peroxide into a test tube. Use a test tube holder.
Using a scoopula, add a pinch of copper(II)oxide as a catalyst for the reaction. Remember, a catalyst is not used up in
the reaction and its formula is written above the arrow in the reaction. .
Place your thumb over the mouth of the test tube to trap the gas. Wait a few minutes.
Test the gas that is being given off by placing a glowing splint into the tube. (Light a wooden splint, blow the flame out. If
when you place the glowing splint into the tube the flame returns, the presence of oxygen is indicated.)
Appearance of compound(s) (including state) before the
experiment
Observations
Type of chemical reaction (be as specific as possible):
Balanced chemical equation:
Observations during/after the experiment