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IB Chemistry R3.2 Notes

This page contains our IB Chemistry notes for R3.2. By reading each one of these notes, you will fully cover the content for IB Chemistry 'Further electron transfer'.
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Electrochemical series

Whilst in the SL syllabus you learned about redox and electrochemical cells, you need to know more about electrolytic cells in the HL syllabus. This starts by learning more about the electrochemical series.

The activity series indicates which metals are more reactive reducing agents, allowing you to predict which reactions occur in a voltaic cell. However, it does not give any quantitative information about the voltage generation that occurs, which is given in the electrochemical series in the data booklet.

We can break down the electrochemical series:

Oxidised Species⇌Reduced SpeciesEø

Li+(aq) + e-

⇌Li(s)-3.04

K+(aq) + e-

⇌K(s)-2.93

Ca2+(aq) + 2e-

⇌Ca(s)-2.87

Na+(aq) + e-

⇌Na(s)-2.71

Mg2+(aq) + 2e-

⇌Mg(s)-2.37

Al3+(aq) + 3e-

⇌Al(s)-1.66

Mn2+(aq) + 2e-

⇌Mn(s)-1.18

H2O(l) + e-

⇌1/2 H2 (g) + OH-(aq)-0.83

Zn2+(aq) + 2e-

⇌Zn(s)-0.76

Fe2+(aq) + 2e-

⇌Fe(s)-0.45

Ni2+(aq) + 2e-

⇌Ni(s)-0.26

Sn2+(aq) + 2e-

⇌Sn(s)-0.14

Pb2+(aq) + 2e-

⇌Pb(s)-0.13
  1. The standard electrode potential (Eø) of a half-cell indicates a species's tendency for reduction.
  2. More negative values (top of table) indicate a weak tendency to reduce. This means they are more likely to undergo oxidation and act as a reducing agent.
  3. More positive values (bottom of table) indicate a strong tendency to reduce. Thus, they are more likely to undergo reduction and act as an oxidizing agent.
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