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Reactivity of metals in electrochemical cells

Energy changes • Chemical and fuel cells

Key concepts

What you'll likely be quizzed about

  • An electrochemical cell consists of two different metal electrodes in contact with electrolyte solutions that contain their ions.
  • Electrons move through the external circuit from the electrode undergoing oxidation to the electrode undergoing reduction.
  • The cell produces an electromotive force (EMF), measured as the cell voltage between the two electrodes.
  • Cell notation specifies the anode on the left and the cathode on the right.
  • Oxidation occurs at the anode and reduction at the cathode, with the voltage reflecting the difference in the electrodes' tendencies to gain or lose electrons.

Flashcards

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What experimental factors can change apparent metal reactivity?

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Ion concentration, temperature, electrode surface condition, and impurities can affect observed voltages and the apparent reactivity of metals.

Key notes

Important points to keep in mind

More reactive metals oxidise and act as anodes; they have more negative electrode potentials.

E°cell = E°(cathode) minus E°(anode); larger differences create larger EMFs.

Standard electrode potentials require standard conditions; apply the Nernst equation for other conditions.

Experimental factors such as concentration, temperature, surface condition, and impurities alter measured voltages.

Cell notation places the anode on the left and the cathode on the right; oxidation occurs at the left electrode.

Measured voltages enable relative ranking only if experimental conditions are consistent across comparisons.

A negative calculated cell EMF indicates a non-spontaneous assumed reaction direction.

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