9.4
Types of Reversible Electrodes
For electrode reversibility to be maintained, all the reactants and products involved in the half-reaction must be present at the electrode. There are…
A reversible electrode is one in which the electrode reaction can proceed in both forward and reverse directions with a small change in potential.
Based on the species present at the electrode surface, reversible electrodes are classified into different types.
The metal–metal ion electrode forms when a metal, like copper, is placed in a solution of its ions. The metal can dissolve as ions. Simultaneously, metal ions in solution can gain electrons and deposit back onto the metal surface.
In an amalgam electrode, a reactive metal like sodium is dissolved in mercury. The resulting amalgam remains in equilibrium with its ions in solution.
A redox electrode involves a solution containing two oxidation states of the same species, such as Fe²⁺ and Fe³+. An inert electrode, often platinum, enables electron transfer between them.
In a metal–insoluble salt electrode, a metal is coated with a sparingly soluble salt and placed in a solution containing the same anion. A common example is the silver–silver chloride electrode immersed in potassium chloride solution.
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Q1: What makes an electrode reversible in electrochemistry?
A reversible electrode is one where the electrode reaction proceeds in both forward and reverse directions with only a small change in potential. For reversibility to be maintained, all reactants and products involved in the half-reaction must be present at the electrode surface. This allows the system to respond predictably to potential changes and maintain equilibrium conditions.
Q2: How does a metal-metal ion electrode function?
A metal-metal ion electrode forms when a metal like copper is placed in a solution of its ions. The metal can dissolve as ions while simultaneously metal ions in solution gain electrons and deposit back onto the metal surface, establishing equilibrium. Examples include Cu²⁺|Cu and Zn²⁺|Zn electrodes, though reactive metals like sodium cannot be used due to solvent reactions.
Q3: What is the purpose of mercury in an amalgam electrode?
In an amalgam electrode, a reactive metal like sodium or calcium is dissolved in liquid mercury. The mercury remains inert in the electrode reaction, serving only as a solvent medium. This design allows chemists to use active metals that would otherwise react with aqueous solutions, expanding the range of available reversible electrodes.
Q4: How do redox electrodes differ from metal-metal ion electrodes?
Redox electrodes involve a solution containing two oxidation states of the same species, such as Fe²⁺ and Fe³⁺, with an inert metal like platinum enabling electron transfer between them. Unlike metal-metal ion electrodes where the metal itself participates, the metal in redox electrodes serves solely to supply or accept electrons without reacting.
Q5: What is the silver-silver chloride electrode and how is it prepared?
The silver-silver chloride electrode, symbolized as Ag|AgCl(s)|Cl⁻(aq), consists of a metal coated with a sparingly soluble salt immersed in a solution containing the same anion. It is prepared by electrodepositing a layer of silver on platinum and then electrolytically converting some silver to silver chloride, creating a stable reversible electrode.
Q6: Why can't all metals be used in metal-metal ion electrodes?
Metals that react with the solvent, such as group 1 metals and most group 2 metals that react with water, cannot be used in metal-metal ion electrodes. Additionally, zinc reacts with aqueous acidic solutions. To prevent metal oxidation by dissolved oxygen, nitrogen gas may be needed to expel air from the cell.
Q7: What challenges arise when creating a reversible oxygen electrode?
Creating a reversible oxygen electrode is challenging due to metal oxide layer formation and other complications at the electrode surface. These issues prevent oxygen electrodes from maintaining the stable equilibrium conditions required for true reversibility, making them difficult to implement in practical electrochemical systems.