Electrolysis

Electrolysis is the process of splitting up a liquid with electricity into its components. This process needs a liquid that conducts electricity - an electrolyte. Electrolytes have free ions that move around in them at random. Salts like NaCl, when dissolved in water forms an effective electrolyte, that can easily been used to perform electrolysis with ease.


In short, any substance that has free ions is an electrolyte. Molten ionic substances have free ions and therefore form electrolysis. However, the high temperature involved in the process has to be taken into account, when using them.
In electrolysis, a battery is connected to two 'rods' that goes into the electrolyte.

They are called electrodes - electrode connected to the negative terminal is called cathode and the one that is connected to the positive terminal is called anode.


electrolysis

A cathode is a source of electrons; it has a collection of them. The positive ions which are hungry for electrons, naturally, approach the cathode to get them. However, if there are different types of positive ions, then a competition breaks out in reaching the cathode - the kind of things that happen at sales, when announced suddenly. It is now a matter of survival of the most active. The most active positive ions get electrons and become their respective atoms: if it is a metal, it deposit itself on the cathode; if it is a gas, they just bubble out from the cathode.


At anode, the negative ions undergo similar scenario. In the end, most active negative ions abandon their excess electrons and become their respective atoms. If it is a gas, it bubbles out from the anode and if it is a metal, it gets deposited on the anode.


The animation is using NaCl as the electrolyte. The ions in it are H+ , Na+ , Cl- and OH- . However, the main players are H+ and Cl- , as they are the stronger ions that dominate the electrolysis process.


As you can see, the hydrogen ions approach the cathode and obtain electrons and become hydrogen gas. At the anode, on the other hand, chloride ions give up their electrons and become chlorine gas. Both sodium ions and hydroxyl ions have been prevented from active participation by the dominance of hydrogen and chloride ions.


In the end, the NaCl solution breaks up into hydrogen and chlorine. This is electrolysis.



 

 

 

 

Resources at Fingertips

This is a vast collection of tutorials, covering the syllabuses of GCSE, iGCSE, A-level and even at undergraduate level. They are organized according to these specific levels.
The most popular tutorial is the Book of Electricity, which comes at the top of Google search for electricity tutorials for GCSE / AS/ A-Level at present.
In addition, there are a few more which come at the top of Google search.They are all supported by an extensive collection of animations and interactive labs.

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