why are carbon electrodes commonly used in electrolytic cells
- egative electrode (cations attracted to cathode), e.g. in the diagram, sodium ions Na+ , move to the negative electrode (-ve),
- and negatively charged ions move to the positive electrode (anions attracted to anode), e.g. in the diagram, chloride ions Cl-, move to the positive electrode (+ve).
- The diagram shows the industrial electrolysis process (in a Down's Process Cell) to extract sodium metal from sodium chloride (common salt).
- During electrolysis, gases may be given off, or metals dissolve or are deposited at the electrodes.
- Metals and hydrogen are formed at the negative electrode from positive ions by electron gain (reduction), e.g. in molten sodium chloride
- sodium ions change to silvery grey liquid sodium
- Na+ + e- == Na (a reduction electrode reaction)
- sodium ions change to silvery grey liquid sodium
- and non-metals e.g. oxygen, chlorine, bromine etc. are formed from negative ions changing on the positive electrode by electron loss (oxidation), e.g. in molten sodium chloride
- chloride ions change to green chlorine gas
- 2Cl- - 2e-== Cl2 or 2Cl-== Cl2 + 2e-(an oxidation electrode reaction)
- chloride ions change to green chlorine gas
- The electrons released by the oxidation at the positive anode, flow round through the anode and wire to the positive cathode and so bring about the reduction i.e. of the sodium ion.
- Metals and hydrogen are formed at the negative electrode from positive ions by electron gain (reduction), e.g. in molten sodium chloride
- In a chemical reaction, if an oxidation occurs, a reduction must also occur too (and vice versa) so these reactions 'overall' are called redox changes.
- You need to be able to complete and balance electrode equations or recognise them and derive an overall equation for the electrolysis.