1. Write balanced net ionic equations for all reactions that occurred during Activity I.
2. Identify the color of the mineral oil layer in the test tube when each of the following species is present: I2, Br2, Cl2, I–, Br–, and Cl–.
3. Identify the color that should have been present in the mineral oil layer in test tubes 1–6 if no reaction had occurred in any of the test tubes. Explain your answer.
4. Use the answers to the first three questions to create an activity series of metals by listing the metals in order of decreasing activity.
5. Write reduction half-reactions for each metal ion. Check a table of standard reduction potentials (E°). Arrange the list in order of increasing reduction potential (decreasing oxidation potential). How does the activity series of metals from Question 4 compare to the list based on increasing reduction potential?
6. Explain why it was necessary to test the halide ions for their color in mineral oil.
7. In which test tubes did a reaction occur when halogen water was mixed with halide solutions? Explain how to reach this conclusion.
8. Write balanced net ionic equations for each of the halogen reactions that occurred during this experiment.
9. Use the answers to Question 8 to create an activity series of halogens by listing the halogens in order of decreasing activity.
10. Write reduction half-reactions for each halogen ion. Check a table of standard reduction potentials. Rearrange the list in order of decreasing reduction potential. How does the activity series of halogens from Question 9 compare to the list based on reduction potential?
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