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Cation reactivity series1/1/2024 ![]() ![]() The activity of the metal depends on its tendency to lose electron or electrons, i.e., tendency to form cation (M" +). ![]() The activity of non-metals increases from top to bottom.Īpplications of Electrochemical Series Reactivity of Metals Have the tendency to accept electrons readily. The non-metals on the bottom (having high positive values of standard reduction potentials) The activity of metals decreases from top to bottom. The metals on the top (having high negative values of standard reduction potentials) have the tendency to lose electrons readily. The substances which are stronger oxidising agents than H +ion are placed below hydrogen in the series. The substances which are stronger reducing agents than hydrogen are placed above hydrogen in the series and have negative values of standard reduction potentials.Īll those substances which have positive values of reduction potentials and placed below hydrogen in the series are weaker reducing agents than hydrogen. Similarly, the +ve sign of standard reduction potential indicates that the electrode when joined with SHE acts as cathode and reduction occurs on this electrode. ![]() When zinc electrode is joined with SHE, it acts as anode (-ve electrode) i.e., oxidation occurs on this electrode. The negative sign of standard reduction potential indicates that an electrode when joined with SHE acts as anode and oxidation occurs on this electrode.įor example, standard reduction potential of zinc is -0.76 volt. Standard Electrode Reduction potential E o, volt Standard Aqueous Electrode Potentials at 25☌ 'The Electrochemical Series' The electrochemical series is shown in the following table. When the electrodes (metals and non-metals) in contact with their ions are arranged on the basis of the values of their standard reduction potentials or standard oxidation potentials, the resulting series is called the electrochemical or electromotive or activity series of the elements.īy international convention, the standard potentials of electrodes are tabulated for reduction half reactions, indicating the tendencies of the electrodes to behave as cathodes towards SHE.Įlectrodes with positive E° values for reduction half reactions do in fact act as cathodes versus SHE, while those with negative E° values of reduction half reactions behave instead as anodes versus SHE.
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