Classifying Chemical Reactions
Name:_____________________________
Partner’s Name:____________________
Date:______________________________
Warm Up
1. Name the type of reaction (4 marks, K)
a) NaBr + Ca(OH)2  CaBr2 + NaOH
Type of reaction: _________________________________
b) NH3+ H2SO4 (NH4)2SO4
Type of reaction: _________________________________
c) Pb + H3PO4  H2 + Pb3(PO4)2
Type of reaction: _________________________________
d) HgO  Hg + O2
Type of reaction: _________________________________
2. Come up with a UNIQUE analogy for one of the types of reactions and DRAW a picture. (2 marks, K)
Classifying Chemical Reactions
Purpose:
The purpose of this lab is to perform and classify different chemical reactions, to identify the reactants and
products of each reaction, and to write and balance equations for each reaction.
Materials: Materials and instructions will be provided for you at each station. You MUST wear goggles at
all times. Safety first!
Procedure:
1. This lab is divided into stations. Follow the instructions at each station carefully.
2. The reactants are written on the station cards. Record the reactants for each reaction in Table 1.
3. Record all observations for each reaction in Table 1.
Include any physical observations (colour, clarity and state) and observatios that suggest a
chemical reaction has occurred (gas formation, temperature change, colour change).
Revised Oct 2013
SCH4C Lab 1.4
Table 1: Observing Various Chemical Reactions
Station
A
Reactants
Observations
B
C
D
E
F
G
H
/7 C reactant names
/7 C colour, clarity, state
/7C other observations
Revised Oct 2013
Discussion Questions
1. For each reaction, write the balanced chemical equation including the states, and name the type of reaction
that occurred.
Station
A
Balanced Chemical Equation
Type of Reaction
B
C
D
E
F
G
H
/7 I reactants
/7 I products
/7 K states
/7 K
Revised Oct 2013
2. How can you tell if a chemical reaction has occurred? What did you look for? (3 marks, I)
3. For reaction A and B:
a) What colour is the CuSO4 ∙5 H2O ? (1 mark, I)
b) What colour is the CuSO4 ? (1 mark, I)
c) How are these two reactions related? (1 mark, I)
4. For reaction C:
a) What gas was formed in this reaction? (1 mark, I)
b) What gas test would you use to confirm that this gas was formed? Explain. (2 marks, I)
5. For reaction D:
a) What gas was formed in this reaction? (1 mark, I)
b) Name two other metals you could add to HCl to produce the same type of gas? (2 marks, I)
Hint: Use your Metal Activity Series
6. For reaction E and G:
a) What did you see form when the reactants were combined? (1 mark, I)
b) Name a different compound you could add to copper(II)chloride to form a precipitate. (2 marks, I)
Hint: Use your Solubility Table
7. For reaction F:
a) What happened to the nail? Explain why this happened. (1 mark, I)
8. For reaction H:
a) There is more than one possible product for this reaction. Name 2 possible product. (1 mark, I)
b) Explain how you would know which one formed in the reaction. (1 mark,I)
Revised Oct 2013
STATION A
Reactant:
Copper(II)sulfate pentahydrate (CuSO4 5H2O)
Procedure:
1. Record the reactant in your table.
2. Place a piece of copper(II)sulfate pentahydrate in a dry test tube in a wooden test tube
rack. Do not use a plastic test tube rack because it might melt when the test tube gets
hot!!!
3. Have a test tube holder ready to use.
4. Follow the ‘How to Light a Bunsen Burner’ instructions carefully and adjust the Bunsen
burner until you have a blue flame.
5. Pointing the test tube away from others, heat the copper(II) sulfate in the test tube until
you see a change in its appearance. (1-2 minutes).
6. Let the hot test tube cool in the wooden test tube rack. You will need the product for
Station B.
7. Record your observations.
STATION B
Reactant:
Copper(II)sulfate (CuSO4)
Water
Procedure:
1. Record the reactants in your table.
2. Add a few drops of water the product from your reaction in 1A.
3. Record your observations.
4. Dump the products into the blue waste beaker.
Revised Oct 2013
STATION C
Reactants:
calcium metal * Be very careful !! This metal is REACTIVE!!!!!
water
Procedure:
1. Record the reactants in your table.
2. Fill a beaker half full with water.
3. Using the tweezers or a scoopula add a small piece of calcium metal to the water in the
beaker
4. Describe the reaction that is occurring in your table.
5. Dispose of the calcium and liquid in the waste beaker.
6. Wash the test tube.
STATION D
Reactants:
3 mol/L hydrochloric acid (HCl)  This acid will burn your skin. Wash your hands
immediately if you spill any.
Mossy zinc metal
Procedure:
1. Record the reactants in your table.
2. In the test tube place about 2 cm of hydrochloric acid.
3. Use a scoopula to add a small amount of zinc to the test tube.
4. Record your observations.
5. Pour the product into the waste beaker.
6. Wash the test tube.
Revised Oct 2013
STATION E
Reactants:
sodium hydroxide
copper(II)sulfate
Procedure:
1. Record the reactants in your table.
2. In the test tube place about 2 cm of sodium hydroxide.
3. Add a few drops of copper(II)sulfate to the test tube.
4. Record your observations (use the centrifuge if needed)
5. Pour the products in the waste beaker.
6. Wash the test tubes.
2
cm
STATION F
Reactants:
Iron nail
copper (II) sulfate
Procedure:
1. Record the reactants in your table.
2. Use sandpaper to clean the iron nail before you begin.
3. Place the clean nail in a test tube and cover it with copper(II)sulfate solution.
4. After several minutes, pour off the liquid into the waste beaker.
5. Dump the nail onto a paper towel and examine the nail.
6. Record your observations.
Revised Oct 2013
STATION G
Reactants:
?
?
Procedure:
1. Use your solubility table to figure out which of the two reactants provided will result in a
double displacement reaction with a precipitate.
2. Add a few drops of each reactant to the test tube.
3. Record your observations. (use the centrifuge if necessary)
4. Pour the products into the waste beaker.
5. Wash your test tubes.
STATION I
TEACHER DEMO
Reactant:
hydrogen peroxide ( H2O2 ) <- Be very careful when pouring!
Wash hands immediately if you spill any!
Catalyst:
Potassium Iodide
*The catalyst is a substance that does not get used up in the reaction. It is not one of the
reactants, it just helps make the reaction go faster.
When writing the chemical equation, write the catalyst above the arrow.*
Procedure:
1. Record the reactant in your table.
2. Fill a small graduated cylinder with 5 mL of hydrogen peroxide.
3. In a large graduated cylinder put 2 drops of dish soap and use a scoopula to add a few
crystals of potassium iodide.
4. Add the hydrogen peroxide to the large graduated cylinder and record your observations.
5. The products can be washed down the sink with lots of water.
8. Wash the graduated cylinders.
Revised Oct 2013
STATION H
Reactant:
Copper metal + oxygen 
Procedure:
6. Record the reactants in your table
7. Sand down the copper metal until it is shiny
8. Heat the copper in a Bunsen burner flame until you see a colour change
9. Record
Revised Oct 2013