75941
Description
Mind Map by Safiya Caesar, updated more than 1 year ago
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Created by Safiya Caesar
over 11 years ago
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Electrolysis
- Molten Salts
- At the anode: metal
- At the cathode: Non-metal
- At the anode: metal
- Salt solution
- At the cathode: More reactive metals stay
as ions in solution. Instead, H+ ions accept
electrons forming Hydrogen molecules
- At the anode: Non-metal except
sulfates in which case
O2
- At the cathode: More reactive metals stay
as ions in solution. Instead, H+ ions accept
electrons forming Hydrogen molecules
- CATIONS(+) --> CATHODE(-)
- ANIONS(-) --> ANODE(+)
- The process in which electricity is used to break
compounds down into their elements
- Industrially important as it is the only extraction method available for the
most reactive metals
- Industrially important as it is the only extraction method available for the
most reactive metals
- Electrolytes - liquids which conduct electricity by
movement of ions. When they conduct the ionic
compound is split up
- E.g. Molten salts, solutions of salts in water, solutions of acids,
solutions of alkalis
- E.g. Molten salts, solutions of salts in water, solutions of acids,
solutions of alkalis
- Rules for electroplating an object
- The object must be made at the cathode
- the electrolyte must be a solution of a
salt of the required metal
- the anode must be made of
a strip of the metal
- The object must be made at the cathode
- During electrolysis
- the oxidation of non-metal ions always takes
place at the anode
- the reduction of a metal or
hydrogen ions always take place
at the cathode
- the oxidation of non-metal ions always takes
place at the anode
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