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Galvanic (Voltaic) Electrochemical Cells

Key Concepts

Galvanic (Voltaic) Cell: a type of electrochemical cell^* that converts chemical energy of oxidants and reductants into electrical energy
The redox reaction must be spontaneous in order to produce electricity E⁰ for the galvanic cell is positive.
E^o_(cell) is the maximum voltage that can be produced by the cell and is also known as electromotive force (emf).
A typical galvanic (voltaic) cell consists of

Electrolytes: conducting substances containing the species that take part in the oxidation and reduction reactions.
2 Electrodes^#: conductors used to permit the flow of electrons in an electrochemical cell and provide surfaces at which the oxidation and reduction reactions occur.
Negative electrode is the anode. Oxidation occurs at the anode.
Positive electrode is the cathode. Reduction occurs at the cathode.
Electrons flow from anode to cathode.
Conducting wires, or leads, connect the two electrodes.
Salt bridge: allows for migration of ions to complete the electrical circuit

Examples of Galvanic (Voltaic) Cells

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^*There are 2 types of electrochemical cells, the galvanic (voltaic) cells discussed here which convert chemical energy into electrical energy, and, electrolytic cells which convert electrical energy into chemical energy.

^#The are many different types of electrodes that can be used in galvanic (voltaic) cells. These include:

metal-metal ion electrodes (metal is in contact with its ions in solution)
gas-ion electrodes (a gas in contact with its anion or cation in solution)
metal-insoluble salt-anion electrodes (a metal in contact with one of its insoluble salts and also with a solution containing the anion of the salt)
inert, "oxidation-reduction" electrodes (strip of inert conductor such as platinum in contact with a solution containing ions of a substance in two different oxidation states)
membrane electrodes (a thin membrane, such as glass, separates the two electrolyte solutions)