Tetraethyl ammonium ion

A good phase-transfer catalyst must be soluble in both aqueous and nonpolar organic solvents. Use SpartanView to compare electrostatic potential maps of benzyltrimethyl-ammnnium inn, tetraethyl ammonium ion, and tetrabenzylammonium ion. Which ion is likely to be the most water-soluble, and which the least water-soluble ... 

Fukano, M., T. Fujimori, J. Segalini et al. 2013. Vertically oriented propylene carbonate molecules and tetraethyl ammonium ions in carbon slit pores. Journal of Physical... 

There are many adsorbents available in the market. Rohm Haas, to name one vendor, supplies the Amberlite class of adsorbents, which includes Amberlite XAD-4, ZAD-7, XAD-7HP, ZAD-16, and XAD-1180 [169]. These nonfimctionalized materials are reported to adsorb chlorinated solvents, herbicides, nonaromatic compounds, and aromatic species, among many others. A typical example is the use of XAD-7 to remove phenolics from brine. Another class of adsorbents is the Ambersorb series. Ambersorb 572 is claimed to remove quaternary ammonium salts such as chloromethyl tetraethyl ammonium ions from brine [171],... 

Iron hahdes react with haHde salts to afford anionic haHde complexes. Because kon(III) is a hard acid, the complexes that it forms are most stable with F and decrease ki both coordination number and stabiHty with heavier haHdes. No stable F complexes are known. [FeF (H20)] is the predominant kon fluoride species ki aqueous solution. The [FeF ] ion can be prepared ki fused salts. Whereas six-coordinate [FeCy is known, four-coordinate complexes are favored for chloride. Salts of tetrahedral [FeCfy] can be isolated if large cations such as tetraphenfyarsonium or tetra alkylammonium are used. [FeBrJ is known but is thermally unstable and disproportionates to kon(II) and bromine. Complex anions of kon(II) hahdes are less common. [FeCfy] has been obtained from FeCfy by reaction with alkaH metal chlorides ki the melt or with tetraethyl ammonium chloride ki deoxygenated ethanol. 

The reaction of toluene-3,4-dithiol(3,4-dimercaptotoluene) and antimony trichloride ia acetone yields a yeUow soHd Sb2(tdt)2, where tdt is the toluene-3,4-dithiolate anionic ligand (51). With the disodium salt of maleonitnledithiol ((Z)-dimercapto-2-butenedinitrile), antimony trichloride gives the complex ion [Sb(mnt)2] , where mat is the maleonitnledithiolate anionic ligand. This complex has been isolated as a yeUow, crystalline, tetraethyl ammonium salt. The stmctures of these antimony dithiolate complexes have apparendy not been unambiguously determiaed. 

Dehalogenation of monochlorotoluenes can be readily effected with hydrogen and noble metal catalysts (34). Conversion of -chlorotoluene to Ncyanotoluene is accompHshed by reaction with tetraethyl ammonium cyanide and zero-valent Group (VIII) metal complexes, such as those of nickel or palladium (35). The reaction proceeds by initial oxidative addition of the aryl haHde to the zerovalent metal complex, followed by attack of cyanide ion on the metal and reductive elimination of the aryl cyanide. Methylstyrene is prepared from -chlorotoluene by a vinylation reaction using ethylene as the reagent and a catalyst derived from zinc, a triarylphosphine, and a nickel salt (36). 

The polarographic determination of metal ions such as Al3 + which are readily hydrolysed can present problems in aqueous solution, but these can often be overcome by the use of non-aqueous solvents. Typical non-aqueous solvents, with appropriate supporting electrolytes shown in parentheses, include acetic acid (CH3C02Na), acetonitrile (LiC104), dimethylformamide (tetrabutyl-ammonium perchlorate), methanol (KCN or KOH), and pyridine (tetraethyl-ammonium perchlorate), In these media a platinum micro-electrode is employed in place of the dropping mercury electrode. 

Diagram (6) shows similar, but opposite, phenomena with the capillary active cations, tetramethyl and tetraethyl ammonium. The phenomena are reversed the rising part of the curve is not affected the falling part, and the maximum, are depressed and the maximum is shifted to more positive potentials. This is because the adsorption tends to form a double layer in the water, with the positive ions nearer the surface than the negative, and this positive adsorption potential aids in attracting electrons to the mercury surface and neutralizing it, so that the maximum is reached with the application of smaller negative potentials E. 

Under proper conditions, aromatic radical ions may show unexpectedly long lifetimes. This is the case for the radical anions of 9,10-dicyanoanthracene and of 2,6,9,10-tetracyanoanthracene, which, when generated by irradiation of the arenes in the presence of triethylamine in acetonitrile containing tetraethyl-ammonium phosphate have been reported to persist for days (Scheme 1) [6], However, aromatic radical ions have a chemistry of their own, and in many cases react efficiently, offering access to novel and useful synthetic processes. They show, in fact, a double reactivity, behaving both as radicals and as ions. 

TrANSPORT number t OF THE PICRATE ION IN A SOLUTION OF TETRAETHYL-AMMONIUM PICRATE IN MOIST DI-IJ OPROPYL KETONE... 

Su2Se5] ion, which has a chair configuration. Chains of [803807] using tetraethyl ammonium in place of an alkali metal ion. ... 

Figure 15. Ion difiusion coefficients in macroporous sulfonated cation exchange resins (1) Tetramethyl (2) tetraethyl (3) tetrabutyl ammonium ions.

Table 1.1 shows a list of dopant ions and their source electrolytes which are currently being used in the electrochemical synthesis of conducting polymers. All of these dopant ions with the exception of the last two (marked by ) are anions and are associated with electrochemical oxidation of the polymers at the anode. Aizawa et al. [104] reported the first example of the reductive doping of an electrochemically synthesized polythioenylene film with cations like tetraethyl ammonium (Et4N" )... 

Hexachloro- and tetrachlorometallate ions are unsolvated and not associated in solutions. The reluctance of di- and tetrachlorides to accept a second chloride ion from triphenylchloromethane is remarkable, showing that the chloride ion-donor properties of triphenylchloromethane are weak. In solvents of lower donor number such as benzoyl chloride two chloride ions can be accepted from triphenylchloromethane. In the stronger donor solvents, phosphorus oxychloride and phenylphosphonic dichloride, stronger chloride ion donors, such as tetraethyl-ammonium chloride, are neccessary to obtain the fully chloride-coordinated anionic species. 

Figure 5.3 Water content of (a) Nafion 117, (b) Flemion F-1.44 and (c) Flemion F-1.8 membranes of various ionic forms. Abbreviations used for alkyl ammonium ions are TMA, TEA, TPrA, TBA for tetramethyl, tetraethyl, tetrapropyl and tetrabutyl ammonium ions, respectively (Reprinted with permission from Asaka, K., Fujiwara, N., Oguro, K. et al. State of water and ionic conductivity of solid polymer electrolyte membranes in relation to polymer actuators, J. Electroanalytical Chem., 505 (1 2), 24-32. Copyright (2001) Elsevier).

Fluoride ion from tetraethyl ammonium fluoride acts as a strong base in aprotic solvents it mediates a-elimination of HX from CX3H to generate a carbene, ond it catalyzes p-elimination of HBr from p-phenethyl bromide to afford styrene in almost quantitative yield S. 

To study FT responses of Fc Au MFCs on more explicitly controlled electrode surfaces, Murray et al. performed voltammetry on Au225(SCgFc)43 adsorbed onto anionic SAMs (Figure 3.27). From this study, it was concluded that there are three different interactions that can contribute to MFC adsorption (1) interaction between MFCs and SAM surface (if present), (2) lateral interactions between MFCs due to bridging electrolyte ions, and (3) specific adsorption between electrolyte ions and the bare electrode surface. The use of SAMs for Fc MFC attachment yields the strongest absorption, which is important for stable Fc voltammetry. In another study, some positively charged tetraethyl ammonium-thiolate ligands were incorporated into the shell of the Fc MFC to yield a similarly robust adsorption onto the electrode surface, without the use of SAMs. This supports the hypothesis that multiple ion-pair interactions are central in the irreversibility of adsorption. 

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