At which electrodes do oxidation of cations & reduction of anions occurs in elctrolytic cells?
607202
Oxidation always occurs at the anode and reduction at the cathode.
98966
I think you can find everythin u are lookin for and more on this site.. good luck!!!http://www.tannerm.com/electrochem.htm
468302
they oxidize. they are positive (+2, +3....), so have empty spots in their electron shell.  they want to stabilize, so absorb some electrons.  oxygen has -2, they go together and stabilize.\nmetals are reactive in pure metal form, like pure sodium metal. so they are usually submerged in a liquid, or kept in with another gas. like pure sodium metal is submerged in kerosene (i think, kerosene)
902000
They usually are not defined that way, but you can have:\n\n1. Redox in base solutions\n2. Redox in acid solutions\n3. Single species where the same species (such as I2) is bothe the oxidizing and reducing agent.\n4. Non water based\n5. Molten (no solvent at all) other than the components\n6.spontaneous/non-spontaneous
483935
I'm not sure what you mean by reaction to take place *of* copper sulphate...  There is a reaction that takes place *at* the electrodes.  If you use a set of graphite electrodes, the anode is unaffected by the electrolysis.  The cathode will slowly develop a film of copper, first on the bottom of the electrode and then moving upward.  \n\nThere is no actual reaction between the electrodes and copper sulphate, because graphite (and platinum) electrodes are inert.
562057
pumping ions across the cell membrane requires energy which is produced by glycosis, the Krebs cycle, and Phosphorilic oxidization.  This electron transfer process yeilds a lot of ATP which is used as energy.
136930
Try the Journal of Electrochemical Society. You may have to go to a local university library to get access to it. Or, try a Google search.
199855
Electrolysis. Running a current through water will separate it into hydrogen and oxygen.
513117
use a potato and two different metals as electrodes. The link will help you, do your own homework, or web searching atleast! it was the second link in google for g** sake!
788768
Just the usual stuff.  Use an electrolyte (H2SO4/HNO3), a couple of electrodes, a reduction table of half cell potentials, and some electricity.
964894
IF U ARRANGE THE IONS IN ORDER OF increasing oxidation potentials then it's first Mg+2 , Zn+2, Cu+2\nso in a soln of these 3 ions Cu ions have highest reduction potential i.e.\nhigh tendency to accept e~ (to get reduced)\nso Cu will get first discharged & not Mg\nif Cu ions get exhausted then Zn will get deposited then Mg
359323
The dry cell (Leclanché cell):\n\nThe dry cell dry cell, invented in 1867 by the French engineer Georges Leclanché (1839 - 1889), is widely used as a source of electric energy in electric torches and small appliances such as transistor radios. It makes use of the two reactions, which (in a simplified form) may be described as\n\nDry cell reactions 1\n\nThe manganese is supplied as manganese dioxide, and the actual cathode reaction taking place is\n\nDry cell reactions 2\n\nThe H+ ions are in turn provided by ammonium ions NH4+, through the reaction\n\nDry cell reactions 3\n\nThe dry cell is an example of a primary cell, as once it is discharged it cannot be recharged, and must be discarded.\n\nA typical dry cell is shown below, with a section cut away in order to expose the interior parts.\n\nDiagram of dry cellThe top of the battery is closed with a non-conducting sealing material (A).\n\nThe cathode consists of a graphite (carbon) rod (B)(tipped with a metal contact), which serves as the positive pole of the battery.\n\nThe anode is a cylindrical zinc casing (C) (the bottom of the battery is normally exposed and serves as the negative pole).\n\nThe battery is filled with a mixture of manganese dioxide (MnO2) as oxidant, ammonium chloride (NH4Cl) as a source of H+ ions, and zinc chloride (ZnCl2) (D). These two salts serve as electrolytes.\n\nThe above mixture is separated from the zinc walls of the battery by a porous material soaked in a solution of the two salts. The e.m.f. of the battery is about 1.5 V.\n\nIn 1859, the French physicist Gaston Planté (1834 - 1889) invented a device called the lead-acid accumulator, which, with minor design changes, is still used today as the motor car battery. It is an example of a secondary electrochemical cell, since it can be recharged.\nLead-acid 1 The battery consists of 6 cells connected in series, each cell having an emf of about 2 V, giving 12 V as the overall emf of the battery,\nThe general appearance of the battery is shown on the right, with part of its casing removed to show the individual cells. Lead-acid 2\n\nWhen the battery is discharging, i.e., when it is supplying a current, the reactions are\n\nAt the anode:\n\nLead-acid reaction 1\n\nAt the cathode:\n\nLead-acid reaction 2\n\nThe overall reaction (during discharge) is therefore\n\nLead-acid reaction 3\n\nNote that the electrolyte is sulphuric acid (H2SO4), which is gradually used up. Both electrodes become coated with an insoluble layer of lead sulphate, which, being an insulator, would eventually ruin the battery.\n\nDuring the manufacturing process, the electrodes are filled with litharge (PbO), and immersed in the electrolyte (H2SO4, 6 mol.dm-3). When an electric current is passed through the battery, the negative electrode is converted to lead, while the positive electrode is converted to PbO2. There is no net change in the concentration of acid. This process is called forming the battery.\n\nLead-acid charging\n\nWhen the battery is fully charged, the anode consists of metallic lead in a spongy form (with a high area per unit mass), while the cathode consists of lead dioxide:\n\nCharging reactions\n\nThe electrolyte is an aqueous solution of sulphuric acid, at a concentration of approximately 6 mol.dm-3. This is the battery acid that one can buy at service stations.\n\nAs the battery provides energy, it is discharged and this lead to the gradual formation of lead sulphate at the electrodes, and a steady decrease in the concentration of the sulphuric acid:\n\nLead-acid discharging\n\nAt the anode:\n\nDischarging reaction at anode\n\nAt the cathode:\n\nDischarging reaction at cathode\n\nIf the battery is totally discharged, both electrodes will have been converted to lead sulphate. It will no longer be able to provide a current, and cannot be recharged. It is only good for scrap!\n\nWhen the battery is being charged, (using a battery charger or the motor car's alternator), electrons are supplied to the anode o
1084692
ionic: electrons are transfered.... i.e. NaCl, MgO\ncovalent: electrons are shared.... i.e. water, sulfur dioxide
706257
Diode (Cathode > Plate or Anode), \nTriode (Cathode > Grid > Anode). Also:\nIgnitron (high voltages rectifiers, smelting aluminum).
174141
"Redox" metals have more than one oxidation state.  e.g. Fe2+/Fe3+ or Cu1+/Cu2+.  Zn and Ca only occur in biological systems in the 2+ state (therefore they cannot redox cycle).
925200
The scientific supply companies like VWR probably have them.\n\nI searched for "oxygen reduction potential electrode" and got a bunch of hits.  Try that.\n\nYou'll also need a meter to attach it to.  Many better pH meters can handle this kind of probe as well.
728017
This is essentially correct as far as you have gotten.  The answer to the second part of the question is no.  Reduction of a water solution of CaCl2 will result in H2 being produced at the cathode because the reduction potential is much lower than that of the Ca+2 ion.