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  • Created by: Lizzi
  • Created on: 19-05-13 15:54
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  • Electrolysis
    • Electrolysis
      • Splits up substances using electricity
      • Ionic compounds can only be electrolysed when molten/ in a solution (so ions are free to move around)
      • Positive ions move towards negative electrode (cathode)
      • Negative ions move to the positive electrode (anode)
    • Changes at Electrodes
      • Negative ions oxidise (lose electrons) at the anode
      • Positive ions reduce (gain electrons) at the cathode
      • Aqueous solutions (unless they contain a halide) produce oxygen at the anode
      • Aqueous solutions (unless the ions are of a metal less reactive than hydrogen) produce hydrogen at cathode
    • Aluminium Extraction
      • Aluminium Oxide is electrolysed to manufacture aluminium
      • Mixed with cryolite to lower melting point
      • Aluminium forms at anode, and oxygen and cathode
      • Positive carbon electrodes are replaced as they burn away
    • Brine Electrolysis
      • Produces three products: Chlorine(g), Hydrogen(g),and sodium hydroxide(l)
      • Sodium hydroxide uses: soap, paper, bleach, neutralisation, pH control
      • Chlorine uses: kills bacteria in water, bleach, disinfectant, plastics
      • Hydrogen uses: margarine, hydrochloric acid
      • Half equations: Positive= 2Cl- > Cl2+2e-    Negative= 2H+ + 2e- > H2
    • Electroplating
      • Electroplate objects to: improve appearance, protect, and to use smaller amounts of precious metals
      • Object because the negative electrode, plating metal is positive, electrolyte contain positive ions of the plating metal
    • Cathode: Negative electrode; Anode: Positive electrode


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