Difference between revisions 6001799 and 6001800 on simplewiki

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===Redox chemistry – the ferrocenium ion===
{{main article|Ferrocenium}}
Unlike the majority of organic compounds, ferrocene undergoes a one-electron oxidation at a low potential, around 0.5&nbsp;V versus a [[saturated calomel electrode]] (SCE). This reversible oxidation has itself been used as standard in electrochemistry as Fc<sup>+</sup>/Fc&nbsp;= 0.
640&nbsp;V versus the [[standard hydrogen electrode]]<ref>C. E. Housecroft &
 A. G. Sharpe, <i>Inorganic Chemistry 4th editiom</i>, 2012, p. 925.</ref>. Some [[electron]]-rich organic compounds (e.g., [[aniline]]) also are oxidized at low potentials, but only irreversibly. Oxidation of ferrocene gives the stable blue-colored iron(III) cation {{chem|Fe(C|5|H|5|)|2|+}} originally called ferricinium, but now more commonly ferrocenium (these terms denote the ''same'' ion, contrary to what one would expect from the fact that [[ferric]] and [[ferrous]] denote different ions of a single iron atom).  On a preparative scale, the oxidation is co(contracted; show full)
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[[Category:Organoiron compounds]]
[[Category:Metallocenes]]
[[Category:Antiknock agents]]
[[Category:Sandwich compounds]]
[[Category:Cyclopentadienyl complexes]]