Electrolytic+cells

//Electrolysis// is where electrical energy is used to bring about a non-spontaneous redox reaction. Electricity is passed through a liquid called an electrolyte. The electrolyte contains ions which can move and carry the current. These ions move towards the electrodes and are therefore decomposed in the process. 


 * The electrodes are the solid conductors which are dipped into the electrolyte. **

* The //anions// are attracted to the __//positive//__ electrode, where they are //oxidised// (this is called the //anode//)

* The //cations// are attracted to the //__negative__// electrode, where they are //reduced// (this is called the //cathode//)

Eg. Electrolysis of molten sodium chloride (NaCl)

// At the anode: //

Chloride ions release electrons and are thus oxidised

2Cl -  (l) ---> Cl 2  (g) + 2e -

// At the cathode: //

Sodium ions gain electrons and are thus reduced

Na + <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> (l) + e - <span style="font-family: Tahoma,sans-serif; font-size: 14pt;"> ---> Na (l)

<span style="font-family: Tahoma,sans-serif; font-size: 14pt;">Electrolysis of a molten electrolyte is usually the method used in obtaining a reactive metal from its ore.

By the end of this lesson you should be able to: media type="googleplusone" key="" width="360" height="18" media type="facebooklike" key="http%3A%2F%2Fibchem4u.wikispaces.com%2FElectrolytic%20cells" width="360" height="74" __**<span style="color: #0000ff; font-family: 'Palatino Linotype','Book Antiqua',Palatino,serif;">Next up- Organic Chemistry **__
 * Know the essential components of an electrolytic cell
 * State that oxidation occurs at the positive electrode (anode) and reduction occurs at the negative electrode (cathode)
 * Describe how current is conducted in an electrolytic cell
 * Deduce the products of electrolysis of a molten salt