Electricity and Chemical Change

State that electrolysis
1. The chemical effect of electricity on ionic compounds, causing them to break up into simpler substances, usually elements
Use the terms electrode, electrolyte, anode and cathode
1. Electrode
  1. Anode and Cathode
2. Anode
  1. It is positive
3. Cathode
  1. It is negative
Describe electrolysis in terms of the ions present and the reactions at the electrodes
1. Electrolysis breaks down molten ionic compound down to ist elements, giving the metal at the cathode and non-metal at the anode.
Describe the electrode products, using inert electrodes, in the electrolysis
1. Molten lead bromide
  1. Lead ions attach to the cathode each receives 2 electrons and become lead atoms.
2. Aqueous copper chloride
  1. At the cathode H, positive ions accept electrons much faster than copper as hydrogen is less reactive than copper. At the anode, chlorine gives up electrons more readily than the hydroxide.
3. Dilute sulfuric acid
  1. At the cathode, hydrogen wins and at the anode, hydroxide wins.
State and use the general principle
1. Metals or hydrogen are formed at the negative electrode (cathode), and that non-metals (other than hydrogen) are formed at the positive electrode (anode)
Relate the products of electrolysis to the electrolyte and electrodes used,
1. The ions in the electrolyte attracted to the electrode, and the molecule leftover is the product.
Describe the electroplating of metals,
1. Electroplating means using electricity to coat one metal with another, to make it look better or to prevent corrosion.
Predict the products of the electrolysis of a specified binary compound in the molten state, or in aqueous solution
Describe, in outline, the manufacture of
1. Aluminium from pure aluminium oxide in molten cryolite
2. chlorine, hydrogen and sodium hydroxide from concentrated aqueous sodium chloride.

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Electricity and Chemical Change

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