Activity Description: Students will be able to create balanced equations and understand the conservation of mass.
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1 Activity Description: Students will be able to create balanced equations and understand the conservation of mass. Materials: 1 Attachment: Student Lab Sheet (1 per student) 1 Set of colored paperclips* in a resealable baggie (1 per group of four students) 1 Pencil or pen (1 per student) *Set of paperclips include: 15 red, 15 yellow, 15 blue, 15 green, 15 black, and 15 silver paperclips. If paperclips are not available, interlocking blocks can be used, such as Legos. Procedure: Prepare materials for the students in advance. Print Student Lab Sheets for each student and place paperclips in a resealable baggies. Each group of students should have a resealable baggie containing the paperclips. Each student should be given a Student Lab Sheet. 1. Give each group of students a resealable baggie with paperclips. 2. Give each student a Student Lab Sheet. Explain to the students that each paperclip represents an element. Different elements are represents by different colors. For example, H 2 O will be created using by clipping together two red paperclips for hydrogen and one yellow paperclip for oxygen. 3. Students will use the paperclips to assemble compounds, molecules, or elements. Each paperclip represents an atom. Explain to students that they should create several of each compound, molecule, or element. Explain that when balancing equations, the entire compound must be added, not just the needed element of that compound or molecule. 4. Students balance the equations using the paperclips and place their answers on the Student Lab Sheet. 5. Once the students complete their Student Lab Sheet, students should place the paperclips back into the resealable baggie and return them.
2 Teacher Attachment: Student Lab Sheet (Key) Directions: Balance the equations by placing the correct coefficient in front of each element, molecule, or compound. Key to paperclip colors: Hydrogen = Red Oxygen = Yellow Chlorine = Green Iron = Blue Sodium = Black Aluminum = Silver 1. 1 FeCl NaOH 1 Fe(OH) NaCl 2. 1 Na 2 O + 1 H 2 O 2 NaOH 3. 4 Al + 3 O 2 2 Al 2 O Al + 6 HCl 3 H AlCl H O 2 2 H 2 O 6. 4 Fe + 3 O 2 2 Fe 2 O 3
3 Teacher Attachment: Student Lab Sheet (Key) Directions: Complete the questions. 1. Which number can be added within a chemical equation coefficient or subscript? Coefficient 2. Which number cannot be added or subtracted within an equation coefficient or subscript? Subscript 3. Which side of the equation is the location of the reactants? Left 4. What does the mean? Yields or makes Conclusion 1. How does a balanced equation show the conservation of mass? A balanced equation show how mass is conserved because the amount of each element on the reactant side is the same amount of each element that is on the product side. 2. Explain what the parentheses mean in a chemical reaction, and how they are used (see the first equation that needed balancing.) The parentheses are placed around polyatomic ions to keep them grouped together. The subscript after the parentheses tells how many of those polyatomic ions there are in the formula. This is necessary to know when balancing the equation to guarantee that mass is conserved. 2
4 Student Lab Sheet Directions: Balance the equations by placing the correct coefficient in front of each element, molecule, or compound. Key to paperclip colors: Hydrogen = Red Oxygen = Yellow Chlorine = Green Iron = Blue Sodium = Black Aluminum = Silver 1. FeCl 3 + NaOH Fe(OH) 3 + NaCl 2. Na 2 O + H 2 O NaOH 3. Al + O 2 Al 2 O 3 4. Al + HCl H 2 + AlCl 3 5. H 2 + O 2 H 2 O 6. Fe + O 2 Fe 2 O 3
5 Student Lab Sheet Directions: Complete the questions. 1. Which number can be added within a chemical equation coefficient or subscript? 2. Which number cannot be added or subtracted within an equation coefficient or subscript? 3. Which side of the equation is the location of the reactants? 4. What does the mean? Conclusion 1. How does a balanced equation show the conservation of mass? 2. Explain what the parentheses mean in a chemical reaction, and how they are used (see the first equation that needed balancing.) 2
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