Reaction One
1) Set up and light a Bunsen burner
2) Obtain ~ 2 cm of magnesium ribbon (no longer)
3) Using test tube tongs, hold the magnesium ribbon in the flame – DON’T STARE DIRECTLY
AT THE FLAME
4) Dispose of the product in a damp paper towel
5) Record all observations (quantitative & qualitative)
Reaction Two
1) Set up and light a Bunsen burner
2) Place 0.10 grams of cupric carbonate in a small test tube
3) Hold the bottom of the test tube in the flame (with the mouth of the test tube pointed away from everyone)
4) After about 2 min, light the wooden splint and place it partially into the mouth of the test tube until it changes; quickly remove it.
5) Repeat if necessary
6) Record all observations (quantitative & qualitative)
Reaction Three
1) Measure ~ 50 mL of the 0.1 M Copper II Chloride into a beaker
2) Cut a piece of aluminum foil into 5 cm x 5 cm square
3) Loosely crumple the foil so that as much of it can be submerged into the beaker
4) Press all of the aluminum foil into the solution with a stirring rod
5) Observe any temperature change that occurs by feeling the outside of the beaker
6) Record all observations (every 5 minutes for 15 minutes) (quantitative & qualitative)
Reaction Four
1) Obtain 10 mL of 0.1 M sodium hydroxide
2) Obtain 10 ml of copper (II) sulfate
3) Pour the sodium hydroxide into the beaker containing the copper (II) sulfate
4) Record all observations (quantitative & qualitative

Data & Observations: Create data tables/charts to organize your quantitative measurements and qualitative observations for each reaction.
1
2
3 hydroxide and copper sulfate. with 2 cm of Mg strip.
Burned and got smaller, Started with .10 g of cupric carbonate.
Started with 50 mL copper II chloride and 5cm x 5cm square of aluminum foil. blue, Turned lighter blue and turned powdery and settled on to curved.
Turned from green to black, Put the flame out immediately.
5 min Beaker warmer,
Aluminum foil starting to disintegrate and turn brown/red color. Copper II chloride less blue.
10 min Same temperature,
Aluminum foil more brown and water less blue.
15 min Water gray, Beaker warmer, Foil in tiny red pieces.
Analysis Questions
Reaction One
1) What chemical in the air did the magnesium react with to produce the white powder? Oxygen
2) What is the balanced chemical equation for the reaction? 2Mg + O
2
 2MgO
3) What is the name of the final product in this reaction? Magnesium Oxide
4) Was this reaction endothermic or exothermic? Explain. Endothermic, because taking in heat for reaction to occur, and Exothermic, because energy needs to be released for reaction to take place.
5) Assuming calcium metal was combusted in the presence of the atmospheric gas that was reacted with magnesium metal, what would the name of the final product be? (Calcium was used instead of magnesium.) Calcium Oxide synthesis
Reaction Two
1) What happened to the wooden splint upon lowering it into the test tube? The lack of oxygen in the test tube caused the flame to go out.
2) What product must have been released into the air in order to do to the wooden splint what was done? Carbon Dioxide

3) When metal carbonates are heated, they decompose into the product listed in #2 and that metal’s oxide. What is the balanced chemical equation for the reaction? Cu(CO
3
)  CO
2
+
CuO
4) Was this reaction exothermic or endothermic? Explain. Endothermic because it had to bring in heat for the reaction.
5) Assuming sodium carbonate was heated in a similar fashion, what would the name of the oxide that would be produced? Sodium Oxide Carbon Dioxide
Reaction Three
1) What evidence is present that a chemical reaction is occurring? The heat from the beaker and the decomposition of the aluminum foil.
2) Given the dynamics of a single replacement reaction, what is forming on the outside of the aluminum foil? Write the balanced equation. 2 Al + 3 CuCl
2
 2 AlCl
3
+ 3 Cu… Copper is forming on the outside.
3) What can be said about the reactivity of aluminum compared to copper? Aluminum is more reactive and has a higher electronnegativity than Copper.
4) Assuming gold metal was placed in the beaker in lieu of aluminum foil, would a reaction be expected? Explain. Because gold has a lower electronnegativity value than Copper and the reaction would end in two (aq) products, which means it is unable to react.
Reaction Four
1) What is the balanced chemical reaction that occurred? SO
4
Cu
2) What evidence supports the fact that a chemical reaction occurred?
3) What product would remain if a boiling process was complete?
Discussion: Inductive Reasoning
Use the observations made in each reaction to describe the type of reaction that was observed. Each reaction type should be supported with details.