Name ___________________________ The following simulation by Tom Greenbowe allows you to test several metals with different aqueous solutions with an optional molecular view. When you view the simulation, notice that the metal atoms are losing electrons and that the ions in solution are gaining electrons. When the metal atoms lose electrons the metal ions produced become electrically charged and are pulled into solution by the electrostatically charged water molecules. http://www.chem.iastate.edu/group/Greenbowe/sections/projectfolder/flashfiles/redox/home.html Simulation Activity Questions: 1) To start the animation click start. Choose Activity 1. You will see four ionic solutions. Pick one of the four metals and follow the instructions on the screen. Write down your observations (i.e. what reactions occurred). Repeat this procedure for the other three metals and make sure to write all your observations down. 2) Considering magnesium, zinc, copper, and silver: a) Which of the four metals you tested is the most reactive? Explain why. b) Which is the least reactive? Why? c) Arrange the metals in order of increasing reactivity (from least reactive to most reactive). d) Locate magnesium, zinc, copper, and silver in the “standard reduction potential table” (Google it). Is there a pattern between the reactivity of metals (answer 2c) and the table? Explain why or why not. 3) Try Activities 2 and 3 as well, answering 2) a), b) and c) (above) with the new sets of metals. 4) Describe why some metals react with HCl and some do not (Activity 4).