Redox Reactions
Work through the online lab activity above, following the procedure outlined below. Record your work in your Google doc.
Activity 1
Observe the reactions between each metal and each solution. Observe the reactions in Activity 1 on a molecular level as well.
Create a data table to record your observations in an organized and structured manner.
Do your results support the predictions you made?
Organize the metals in Activity 1 from least reactive to most reactive.
Organize the metal ions in Activity 1 from most reactive to least reactive.
Activity 2
Prior to starting the activity, make predictions regarding the results of each reaction.
Once the predictions are made, conduct the activity. Record your results in a data table.
Do your results support the predictions you made?
Add the metals and metal ions to your reactivity series from activity 1.
Activity 3
Repeat the process for the new metals. Record your results in a data table.
Add the metals and metal ions to your reactivity series.
Activity 4
Based on your reactivity series from activities 1-3, predict which metals will react more strongly with the acid.
Observe the reactions between each metal and the acid. Observe the reactions on a molecular level. What is actually reacting from the acid?
Create a data table to record your results.
How do these results compare to your activity series above?
Continue working in your Google doc to answer the following questions. If members of your group have different answers, record them all.
What did you intially base your predictions on? Did your predictions hold up throughout the exercise?
Write a balanced reduction half reactions for each ion observed in the lab. Arrange these metal ions in order of greatest reactivity to least. Do your results agree with the other lab groups?
Which material has the greatest tendency to reduce? Which material has the greatest tendency to oxidize? Explain your answers based on your tables.
Did your predictions get better as the lab activity progressed? If so, why do you think this is? If not, why not?
Compare your table above to the table in your text book on page 487.
If you were to make predictions regarding single replacement reactions in the future, what would you base the predictions on?
Assuming that the farther apart on the table two metals are, the greater the voltage produced in the battery made from them, what two metals might make an efficient, and reasonably inexpensive battery. (you may need to look up the cost of metals). Justify your answer based on your results from the lab.
Post Lab Activity
Lab 1
You will explore the reactivity of several metals and solutions and determine which metals are the most reactive and which are the least reactive.
Activity Series
The animation to the left is taken from:
Greenbowe, T. (2005). Metals in aqueous solutions. Retrieved April 4, 2015, from http://group.chem.iastate.edu/Greenbowe/sections/projectfolder/flashfiles/redox/home.html