ELECTROLYSIS

ELECTROLYSIS

WHAT IS ELECTROLYSIS?
1. The decomposition of a compound using electricity.
  1. Negative electrode-cathode
  2. Positive electrode-anode
  3. Compound must be molten not solid!
HOW DOES LEAD BROMIDE DECOMPOSE?
1. Lead Bromide - Lead + Bromine Gas
2. oppositely charged ions are attracted to oppisetly charged electrodes;
3. CATIONS ARE POSITIVE IONS (metal ions and hydrogen).
4. ANIONS ARE NEGATIVE IONS (non-metal ions).
SUMMARY
1. All ionic compounds when molten can be decomposed using electrolysis.
2. Cations travel to the cathode.
3. Anions travel to the anode
4. Non-metal always forms at the anode.
5. The metal and hydrogen always forms at the cathode.
6. The molten substance been electrolysed is called the electrolyte.
7. The electrodes do not involve themselves with the reaction because of the material.
THE ELECTROLYSIS OF SOLUTIONS
1. products from the salt solution will be different to the molten solution because there is water, which produces ions.
2. During electrolysis, these ions compete with the metal and non-metal ions
3. The more reactive a metal is the more it prefers being ions.
4. If a less reactive metal, such as copper or silver is present it would rather accept the electrons than H+.
  1. Hence, the metal forms at the cathode
THE ELECTROLYSIS OF SALTY WATER
1. This industry has been based around the electrolysis of brine, salty water
2. Brine - Sodium Hydroxide + Chlorine + Hydrogen
  1. At the Cathode-Hydrogen bubbles off
  2. At the Anode- Chlorine bubbles off
  3. Na+ and OH- ions are left behind, which means a solution of sodium hydroxide forms.
3. products from the electrolysis of brine
  1. sodium hydroxide
    1. soaps, detergents and paper
  2. Chlorire
    1. solvents, bleach, drugs, hydrochloric acid , paints and dyes
  3. Hydrogen
    1. fuel for rockets and nylon.
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	Created by Connie Blackburn over 8 years ago