Classifying Chemical Reactions

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  • 10 minutes
    Prep Time
  • 30 minutes
    Class Time

Materials

  • Nail (3″ or longer)
  • ½ tsp Yeast (in a labeled test tube)
  • 20 mL Hydrogen Peroxide, 3% (in a labeled 250-mL Erlenmeyer flask)
  • ½ Steel Wool Pad
  • 3 Wooden Splints
  • Evaporating Dish
  • 1 tsp Baking Soda
  • Test Tube Rack
  • 15 mL CuSO4 Solution, 0.5 M (in a labeled test tube)
  • Bunsen Burner
  • 30 mL Vinegar (in a labeled 250-mL beaker)
  • 1 mL (20 drops) Ethanol (in a labeled, stoppered test tube)
  • Laboratory Thermometer
  • Rubber Band
  • Paper Towels
  • 2 Test Tubes

Introduction

Writing and balancing chemical equations is an essential skill for chemistry students, who must learn to predict the products of a reaction when given only the reactants. This becomes much easier for students to do when they learn the pattern of 5 basic categories of chemical reactions: synthesis, decomposition, single replacement, double replacement, and combustion.

This activity is based on Carolina Chemonstrations®: Reaction Types Kit. This kit comes with the materials to perform the reactions described below and more.

Each lab group requires the following items to perform all the activities. You may want to set up the activities at stations and have student teams rotate through them. If so, print the instructions onto a card for each station.

Types of Chemical Reactions

Synthesis reactions

Two or more reactants combine to make 1 new product.
Examples:
C(s) + O2(g) + CO2(g)
H2O(l) + SO3(g) + H2SO4(aq)

Decomposition reactions​

A single reactant breaks down to form 2 or more products.
Examples:
H2CO3(aq) + H2O(l) + CO2(g)
CaCO3(s) + CaO(s) + CO2(g)

Single-replacement reactions​

A single element replaces a similar element of an adjacent reactant compound.
Example:
Zn(s) + CuSO4(aq) + ZnSO4(aq) + Cu(s)

Double -replacement reactions​

Two ionic compounds exchange ions, producing 2 new ionic compounds.
Examples:
NaCl(aq) AgNO3(aq) + NaNO3(aq) + AgCl(s)
HCl(aq) + NaOH(aq) + NaCl(aq) + H2O(l)

Combustion reactions​

A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning.
Examples:
C(s) + O2(g) + CO2(g) + energy
2Mg(s) + O2(g) + 2MgO(s) + energy

Next Generation Science Standards*

The activities described in this article address the following dimensions of the Next Generation Science Standards: HS-PS1-2. Construct and revise an explanation for the outcome of a simple chemical reaction based on the outermost electron states of atoms, trends in the periodic table, and knowledge of the patterns of chemical properties.

Developing and Using Models

  • Use a model to predict the relationships between systems or between components of a system.

Constructing Explanations and Designing Solutions

  • Construct and revise an explanation based on valid and reliable evidence obtained from a variety of sources (including students’ own investigations, models, theories, simulations, peer review) and the assumption that theories and laws that describe the natural world operate today as they did in the past and will continue to do so in the future.

PS1. B: Chemical Reactions

  • The fact that atoms are conserved, together with knowledge of the chemical properties of the elements involved, can be used to describe and predict chemical reactions.

Patterns

  • Different patterns may be observed at each of the scales at which a system is studied and can provide evidence for causality in explanations of phenomena.

Safety

Note: Use safety glasses or goggles and be cautious with the burning splints and Bunsen burner. Follow all local and state recommendations for chemical disposal.

Procedure

Synthesis Activity

  1. Measure room temperature and record: ____°C.
  2. Soak a steel wool pad in 30 mL of vinegar in a 250-mL beaker.
  3. Remove pad and squeeze the excess vinegar back into the beaker.The vinegar strips away the coating on the steel filaments, which are 96 to 98% iron.
  4. Wrap the pad around the thermometer bulb, secure it with a rubber band, and observe the temperature over 5 min.
  5. Record the final temperature of the steel wool: _____°C. Was there a temperature change?
  6. Describe any changes to the steel wool. ________________________________.
  7. Write a balanced equation for this reaction. Include heat as a reactant or product.

Decomposition Activity

  1. Pour the yeast from the test tube into the flask containing the 20 mL of hydrogen peroxide (H2O2). The yeast contains the enzyme catalase that decomposes hydrogen peroxide. What gas or gases could be produced?
  2. Review the table below for confirming 3 common gases.
  3. Insert a flaming splint into the flask held at a 45° angle. Is the test positive for hydrogen (see Fig. 1)?
  4. Insert a glowing splint into the flask. Is the test positive for oxygen (see Fig. 1)?
  5. Write a balanced equation for this decomposition reaction.
Figure 1 Standard test for 3 common gases.

Single-replacement activity

  1. Hold the test tube containing 0.5 M CuSO4 solution at a 45° angle and insert the nail.
  2. Place the test tube in the test tube rack. What happens?
  3. If you use a plain iron nail, here is the reaction:
    Fe(s) + CuSO4(aq) + ______(aq) + ______(s)
    A galvanized nail (coated with Zn), undergoes a different reaction:
    Zn(s) + CuSO4(aq) +______(aq) + ______(s)
  4. Complete and balance both equations.

Double-replacement activity

  1. Pour the baking soda (sodium hydrogen carbonate, NaHCO3) from the spoon into the 250-mL beaker containing the vinegar (acetic acid, HC2H3O2).
  2. Describe what happens.
  3. Complete and balance the equation below for this reaction:
    NaHCO3 + HC2H3O2 + ______(aq) + ______(aq)
  4. One of the products, carbonic acid (H2CO3), immediately decomposes into water and a gas. Complete and balance this equation, and identify the gas with a flaming or glowing splint:
    H2CO3+ H2O + ______(g)

Combustion activity

  1. Pour the 1 mL of ethanol from the stoppered test tube into the evaporating dish.
  2. With a flaming splint, carefully ignite the ethanol in the dish. (This reaction occurs in your car’s engine if you use gasoline that contains ethanol.) Do not touch the dish until 5 min after the flame extinguishes.
  3. Complete and balance the equation for this reaction:
    C2H5OH(l) + O2(g) + ______(g) + ______(g) + energy
  4. The combustion reaction for a Bunsen burner uses methane (CH4) or propane (C3H8). Complete and balance these 2 reactions:
    CH4(g) + O2(g) +______(g) + ______(g) + energy
    C3H8(g) + O2(g) + ______(g) + ______(g) + energy

Extension activities

  1. Have students use the metal activity series to predict whether a free metal will replace another metal ion in an ionic compound for single-replacement reactions.
  2. Have students use a digital camera to document examples of the 5 types of chemical reactions in their local communities. Then, they can share these examples with the class in a PowerPoint® presentation.
  3. As a way to illustrate the relevance of synthesis and single-replacement reactions, have students research corrosion reactions (e.g., the verdigris on the Statue of Liberty) and some of the ways of preventing corrosion on ships and pipelines.
Carolina Chemonstrations®: Reaction Types Kit

Buy the Reaction Types Kit

Carolina Chemonstrations®: Reaction Types Kit

Buy the Kit

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