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Lab WorkWe got our original insight about trends that can be related to position on the periodic table by doing some experiments with the elements and seeing how their reactivity compared with one another (in CH 104). Let's do the same for oxidation-reduction reactions by having you do the experiment for this lesson. The instructions are in your workbook. When you are doing this experiment, be sure to use fresh cuts; if the material you are working with has already been cut, scrape the oxide film off of the metals so that the metal itself is exposed. Then look for changes occurring at that shiny surface. If you are in the lab now, I suggest that you do the lab work now. After you have done that and answered the questions included there, then continue with the comments below. If you will be in the lab at a later time, you can come back to these comments after you have done the lab work or, if you prefer, look at the comments now as something to keep in mind when you do the lab work. CommentsThese comments won't follow directly along the line of the questions asked in the workbook, but they will touch upon some of the same things. Which of these metals was most reactive, or most easily oxidized? Start from the top of your table of observations. You should have noted that zinc metal reacted with two of these solutions. Magnesium metal reacted with all of them. Copper metal reacted with none of the solutions. Lead metal reacted with just one of the solutions. Since all of these reactions involve the loss of electrons by the metal, we can say that magnesium metal is the most easily oxidized. Zinc is the next most easily oxidized. Lead is third. Copper is the least easily oxidized of these particular metals. Expand List
E-mail instructor: Eden Francis
Clackamas Community College |
