The cathode receives those electrons and uses them for reduction. Oxidation (at the anode) produces electrons (and cations), and shoots out the electrons toward the cathode.Or, think about AC power - the A comes first and stands for anode) Electrons always flow from the Anode to the Cathode.The cell potential for all electrolytic cells is negative, because the electrolytic cell requires potential input.Oxidation half reaction: 2Ag → 2Ag + + 2e.Reduction half reaction: Cu 2+ + 2e - → Cu.Another example, the cell potential for the electrolytic cell shown in the diagram is:.The cell potential for all galvanic/voltaic cells is positive, because the voltaic cell generates potential.Oxidation half reaction: Cu → Cu 2+ + 2e.Reduction half reaction: 2Ag + + 2e - → 2Ag.For example, the cell potential for the galvanic cell shown in the diagram is:.Cell potential = Reduction potential + Oxidation potential.Oxidation potential = potential of the oxidation half reaction = reverse the sign of the reduction potential.Reduction potential = potential of the reduction half reaction.Similarly, species like potassium and other reactive metals have negative reduction potentials. Thus, it has a very negative reduction potential. It is very hard to force electrons onto the stable cation to reduce it. Sodium hates its electron, it gets rid of it to obtain a full outer shell and be stable as a cation. Hydrogen is set to have a standard reduction potential of zero Similarly, species like oxygen, halogens, and nonreactive metals have positive reduction potentials.
0 Comments
Leave a Reply. |
AuthorWrite something about yourself. No need to be fancy, just an overview. ArchivesCategories |