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Galvanization

Galvanization, named after the Italian scientist Luigi Galvani, was originally the administration of electric shocks (in the 19th century also termed Faradism, after Michael Faraday). It stemmed from Galvani's induction of twitches in severed frog's legs, by his accidental generation of electricity (see galvanism). This archaic sense is the origin of the meaning of galvanized when meaning 'stirred to sudden action'.

Later the word was used for processes of electrodeposition. Nowadays it typically means hot-dip galvanizing, a chemical process that is used to coat steel or iron with zinc. This is done to reduce corrosion (specifically rusting) of the steel or iron item. The zinc coating prevents oxidation of the protected metal by forming a barrier. Zinc oxide[?] in contrast to iron oxide is a fine white dust which does not cause a breakdown of the zinc's surface integrity as it is formed. Indeed the zinc oxide, if undisturbed, can act as a barrier to further oxidation in a similar way to the protection afforded to aluminium and stainless steels[?] by their oxide layers.

Galvanic[?] or sacrificial anode protection uses ingots of zinc electrically bonded to the metal it is to protect where the metals will be subject to an electrolytic solution. In such a solution the zinc is absorbed into the electrolyte in preference to the metal that it protects.

Obviously in some environments both mechanisms can be at work. For example, the traditional measure of a coating's effectiveness is resistance to a salt spray[?]. Galvanisation can however only be used in a low-friction environment.



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