Videos for Electrochemical and Electrolytic Cells
Electrochemistry Extra Worksheets and Answer Keys
Review Book Homework 6/1/15. Pages 168-172 #37-40 and #24-30
21. 4. Each Bromine atom gained 1 electrons for a net gain of 2 electrons to produce 2 bromide ions.
22. 3. The magnesium atom loses 2 electrons and oxidizes into Mg+2 when in the compound MgCl2
23. 2. A chloride ion has a charge of -1 and which attract to a positive electrode.
24. 4. Zn is the anode and is oxidized, Cu is the cathode and is reduced. Electrons ALWAYS flow anode to cathode.
25. 4. The Ni(s) is the positive anode and the spoon is the negative cathode. The spoon gains mass as Ni+2 ions reduce and plate onto the spoon.
26. 1. The electrons will always flow from the Al(s) anode electrode to the Ni (s) cathode electrode. Use Table J to determine which is the anode and which is the cathode.
27. 1. The Mg(s) anode is oxidized into Mg+2 ions which dissolve into solution.
28. 3. The zinc is oxidized and more Zn+2 ions are produced as the reaction proceeds.
29. 1. Pb is the more reactive metal and will be the anode which oxidizes. Electrons always flow through the wire from anode (Pb) to cathode (Cu).
30. 1. Reduction always takes place at the cathode and the Cu+2 ions are reduced in charge to form Cu ions by gaining electrons.
41. The negative cathode will attract the positive sodium ion.
42. The purpose of the battery is to force the redox reaction to occur. Electrolytic cells are non-spontaneous and need a power source to run.
43. Na+ + 1e --> Na