Tetraalkylammonium amalgam

At very negative potentials, using a mercury cathode, tetraalkylammonium ions are deposited as a crystalline tetraalkylammonium amalgam. Tetramethylammo-nium amalgam slowly decomposes at 0 C to give trimethylamine and a methyl radical [30, 31]. The amalgam fomred by reduction of dimetfaylpyrrolidinium cation 7 is more stable and characterisation of this class of materials has centred on... 

Later, Kariv-Miller et al. have studied the properties of tetraalkylammonium amalgams both in situ, applying electrochemical techniques [218], and ex situ, applying solid-state techniques [219, 220]. It has been concluded that the solid products, which belong to R4N metals, are formed in chemically and electrochemi-cally reversible process ... 

Reduction in aprotic media of ammonium compounds having four aliphatic substituents at mercury or some other metals yields tetraalkylammonium amalgam or tetraalkylammonium metals. This phenomenon is discussed in Chapter 28. 

In both polarographic and preparative electrochemistry in aptotic solvents the custom is to use tetraalkylammonium salts as supporting electrolytes. In such solvent-supporting electrolyte systems electrochemical reductions at a mercury cathode can be performed at —2.5 to —2.9 V versus SCE. The reduction potential ultimately is limited by the reduction of the quaternary ammonium cation to form an amalgam, (/ 4N )Hg , n = 12-13. The tetra-n-butyl salts are more difficult to reduce than are the tetraethylammonium salts and are preferred when the maximum cathodic range is needed. On the anodic side the oxidation of mercury occurs at about +0.4 V versus SCE in a supporting electrolyte that does not complex or form a precipitate with the Hg(I) or Hg(II) ions that are formed. 

Tetraalkylammonium ions, RtN+, especially those with bulky R groups, are selective and robust phase transfer catalysts and also of use where large cations are required to allow precipitation of crystalline solids. Radicals R,N in the form of amalgams (—12Hg/NR,) can be obtained electrolytically or by reduction of R X with Na/Hg in media where the resulting NaX is insoluble. 

Amalgrams are alloys between mercury and a metal however, compounds that are not proper amalgams but function in a way similar to amalgams are also treated in this chapter. Thus, alloys between tetraalkylammonium and mercury or some other metals and also some interstitial compounds, for example, with graphite, are included in this review, even if these compounds have only a limited lifetime and are formed only as intermediates during direct electrolysis. 

If a mercury cathode is expected to be necessary, the aprotic solvent-alkali-metal salt system appears to be inconvenient since many compounds are cathodically cleaved, reduced, or/and deprotected at potentials beyond that of alkali-metal amalgam formation. nevertheless, in certain cases the use of lithium salts as an electrolyte possessing strong electrophilic properties appears necessary in order to avoid the possibility of a Hofmann degradation of the tetraalkylammonium ion by electrogenerated bases. Under such experimental conditions, the cathodic synthesis of some aza and aza-oxa ligands [31] has been successfully achieved from the corresponding and readily obtained poly-... 

It is the preconcentration period that enhances the sensitivity of this technique. In the preconcentration phase precise potential control permits the selection of species whose decomposition potentials are exceeded. The products should form an insoluble solid deposit or an alloy with the substrate. At Hg electrodes the electroreduced metal ions form an amalgam. Usually the potential is set 100-200 mV in excess of the decomposition potential of the analyte of interest. Moreover, electrolysis may be carried out at a sufficiently negative potential to reduce aU of the metal ions possible below hydrogen ion reduction at Hg, for example. Concurrent H" " ion reduction is not a problem, because the objective is to separate the reactants from the bulk electrolyte. In fact, methods have been devised to determine the group I metals and NEC " ion at Hg in neutral or alkaline solutions of the tetraalkylammonium salts. Exhaustive electrolysis is not mandatory and 2-3% removal suffices. Additionally, the processes of interest need not be 100% faradaically efficient, provided that the preconcentration stage is reproducible for calibration purposes, which is usually ensured by standard addition. 

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