Conventional Cell Representation (Edexcel International A Level Chemistry): Revision Note

Conventional Cell Representation

Conventional Representation of Cells

• As it is cumbersome and time-consuming to draw out every electrochemical cell in full, a system of notation is used which describes the cell in full, but does not require it to be drawn.

• An electrochemical cell can be represented in a shorthand way by a cell diagram (sometimes called cell representations or cell notations)

The conventional representation of voltaic cells

• By convention, the half cell with the greatest negative potential is written on the left of the salt bridge, so E^ꝋ_cell = E^ꝋ_right – E^ꝋ_left

  • In this case, E^ꝋ_cell = +0.34 – -0.76 = +1.10 V.

• The left cell is being oxidized while the right is being reduced

• If there is more than one species in solution, and the species are on different sides of the half-equation, the different species are separated by a comma

• This method of representing electrochemical cells is known as the conventional representation of a cell, and it is widely used

• If both species in a half reaction are aqueous then an inert platinum electrode is needed which is recorded on the outside of the half cell diagram

Some Examples

• For the iron(II) and iron(III) half cell reaction a platinum electrode is needed as an electron carrier

• The half equation is

Fe³⁺(aq) + e^- ⇌ Fe²⁺(aq)

• So the cell convention as a left hand electrode would be

Pt 丨Fe²⁺(aq), Fe³⁺(aq)

• Notice the order must be Fe(II) then Fe(III) as the left side is an oxidation reaction, so Fe(II) is oxidised to Fe(III) by the loss of an electron

• The platinum electrode is separated by the phase boundary (vertical solid line), but the iron(II) and iron(III) are separated by a comma since they are in the same phase

• Non-metals will also require a platinum electrode

• If chlorine is used as an electrode the reduction reaction is

Cl₂(g) + 2e^- ⇌ 2Cl^-(aq)

• The conventional representation of the half reaction would be

Cl₂ (g), 2Cl^- (aq) | Pt 

• Notice that the half cell reaction is balanced; however, it would be also correct to write it as

Cl₂ (g), Cl^- (aq) | Pt 

• This is because conventional cell diagrams are not quantitative- they are just representations of the materials and redox processes going on

  • Most chemists tend to show them balanced anyway

• Combining these two half cells together gives

Pt  | Fe²⁺(aq), Fe³⁺(aq)  ∥  Cl₂ (g) | 2Cl^- (aq) | Pt

• As you can see the overall cell diagram is not quantitative as the left side is a one electron transfer and the right side is a two electron transfer