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Competition System Trophy Media. Negative ions are attracted to the positive anode, and are discharged by losing electrons. For example, in the two cases above, you would get chlorine or bromine formed. The loss of electrons means that oxidation is taking place at the anode.

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It is essential to realise that in the melt, ions are moving, whereas in the circuit electrons are moving. The simplest way of thinking of the power source is as an electron pump.

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For every two Br - ions discharged, two electrons are deposited on the anode. You can think of the power source as pumping the electrons along the wires to fill up the gaps appearing in the cathode, and at the same time pumping away the new electrons being released at the anode. If this is the first set of questions you have done, please read the introductory page before you start. Essential ideas Conduction of electricity through metals and carbon The flow of electricity through a metal or carbon is due to the movement of electrons.

Electrolysis Electrolysis is defined as a chemical change produced when electricity is passed through a substance which is either molten or in solution. Electrolytes An electrolyte is a compound which undergoes electrolysis.

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It also follows, of course, that an electrolyte must contain ions. Electrodes, cations and anions The electrodes are the pieces of carbon or metal which are placed in the electrolyte and connected to a dc power source. Discharge of ions at the electrodes What gets discharged at the electrodes during electrolysis depends on whether the electrolyte is molten or in solution. We are starting with the simpler case - where the electrolyte is molten. The electrolysis of molten electrolytes Experimental One of the common compounds to electrolyse molten is lead II bromide - partly because the products are easily visible, and partly because its melting point isn't too high.

An experimental set-up would look something like this: Nothing happens at all until the lead II bromide is molten.

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What is happening? Nothing happens until the compound is molten because the ions aren't free to move. At the cathode Positive ions move to the cathode the negative electrode. For example, electrolysing molten lead II bromide gives lead at the cathode: Or if you electrolysed molten sodium chloride: Notice that the gain of electrons at the cathode means that reduction is taking place here.

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At the anode Negative ions are attracted to the positive anode, and are discharged by losing electrons. You could also show these equations as: The loss of electrons means that oxidation is taking place at the anode.