Classifying Chemical Reactions Stufy Guide
Writing and 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 article outlines some simple protocols your class can follow so that student pairs can produce each of Types of Chemical Reactions. Synthesis reactions Two or more reactants combine to make 1 new product. Examples: C(s) + O 2(g) → CO 2(g) H 2O(l) + SO 3(g) → H 2SO 4(aq). Decomposition reactions A single reactant breaks down to form 2 or more products. Examples: H 2CO 3(aq) → H 2O(l) + CO 2(g) CaCO 3(s) → CaO(s) + CO 2(g).
Single-replacement reactions A single element replaces a similar element of an adjacent reactant compound. Examples: Zn(s) + CuSO 4(aq) → ZnSO 4(aq) + Cu(s). Double-replacement reactions Two ionic compounds exchange ions, producing 2 new ionic compounds. Examples: NaCl(aq) AgNO 3(aq) → NaNO 3(aq) + AgCl(s) HCl(aq) + NaOH(aq) → NaCl(aq) + H 2O(l).
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Combustion reactions A single element or compound combines with oxygen gas releasing energy. This rapid oxidation is called burning. Examples: C(s) + O 2(g) → CO 2(g) + energy 2Mg(s) + O 2(g) → 2MgO(s) + energy.
Science and Engineering Practices 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. Crosscutting Concepts 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 and be cautious with the burning splints and Bunsen burner.
Classifying Types Of Chemical Reactions
Follow all local and state recommendations for chemical disposal. Materials This activity is based on 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. 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 CuSO 4 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 Procedure Synthesis activity. Measure room temperature and record: °C.
Soak a steel wool pad in 30 mL of vinegar in a 250-mL beaker. 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. Wrap the pad around the thermometer bulb, secure it with a rubber band, and observe the temperature over 5 min.
Record the final temperature of the steel wool: °C. Was there a temperature change?. Describe any changes to the steel wool. Write a balanced equation for this reaction. Include heat as a reactant or product.
Decomposition activity. Pour the yeast from the test tube into the flask containing the 20 mL of hydrogen peroxide (H 2O 2). The yeast contains the enzyme catalase that decomposes hydrogen peroxide.
What gas or gases could be produced?. Review the table below for confirming 3 common gases.
Insert a flaming splint into the flask held at a 45° angle. Is the test positive for hydrogen (see Fig. Insert a glowing splint into the flask. Is the test positive for oxygen (see Fig. Oxygen Gas Insert a glowing splint into the container. If it bursts back into flame, the test is positive. Hydrogen Gas Insert a flaming splint into the container held at a 45° angle.
If there is a small explosion or barking sound, the test is positive. Carbon Dioxide Gas Insert a flaming splint into the container.
If the flame is extinguished, the test is positive. Figure 1 Standard tests for 3 common gases. Write a balanced equation for this decomposition reaction. Single-replacement activity. Hold the test tube containing 0.5 M CuSO 4 solution at a 45° angle and insert the nail.
Place the test tube in the test tube rack. What happens?. If you use a plain iron nail, here is the reaction: Fe(s) + CuSO 4(aq) → (aq) + (s) A galvanized nail (coated with Zn), undergoes a different reaction: Zn(s) + CuSO 4(aq) → (aq) + (s). Complete and balance both equations. Double-replacement activity. Pour the baking soda (sodium hydrogen carbonate, NaHCO 3) from the spoon into the 250-mL beaker containing the vinegar (acetic acid, HC 2H 3O 2). Describe what happens.
Classifying Chemical Reactions Study Guide
Complete and balance the equation below for this reaction: NaHCO 3 + HC 2H 3O 2 → (aq) + (aq). One of the products, carbonic acid (H 2CO 3), immediately decomposes into water and a gas. Complete and balance this equation, and identify the gas with a flaming or glowing splint: H 2CO 3 → H 2O + (g) Combustion activity. Pour the 1 mL of ethanol from the stoppered test tube into the evaporating dish. 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.
Complete and balance the equation for this reaction: C 2H 5OH(l) + O 2(g) → (g) + (g) + energy. The combustion reaction for a Bunsen burner uses methane (CH 4) or propane (C 3H 8). Complete and balance these 2 reactions: CH 4(g) + O 2(g) → (g) + (g) + energy C 3H 8(g) + O 2(g) → (g) + (g) + energy Extension activities. Have students use the to predict whether a free metal will replace another metal ion in an ionic compound for single-replacement reactions. 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. 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.Next Generation Science Standards® is a registered trademark of Achieve.
Neither Achieve nor the lead states and partners that developed the Next Generation Science Standards were involved in the production of, and do not endorse, these products.
This two-page test on chemical reactions could be assigned as a study guide with the adjustment or omission of point values for each section. I proctored this test to my eighth physical science students, but it could be utilized in a high school physical science class or in an introductory unit in chemistry. In Part I, students balance eleven chemical reactions with coefficients. They also classify each reaction as a synthesis, decomposition, combustion, or replacement reaction. In Part II, students answer five quantitative questions from the reactions in Part I relating to coefficients, subscripts, and atoms involved. In Part III, students identify whether the twelve stated changes are physical or chemical.
Part IV features a crossword puzzle that covers the key terminology relating to reaction types and rate of reaction - concentration, exothermic, inhibitor, temperature, surface area, catalyst, endothermic, and activation energy. A word bank is provided with a surplus of terms. The test also includes two additional accommodations for struggling students in the form of legends - one that outlines the blueprint for each classification of reaction and the other the four-step rule for balancing reactions. A two-page colored answer key is included.