Amines Ammoniation

I lic alkyl amides or substituted ammoni.as, nith both acid. iiul. tikyl radicals, also c.xist, and aic formed by the first two of the above reac tions and by heating the salt of the amine (see Piep. 54, ]). 15 )-... 

The alkali metals are soluble in liquid ammonia, and certain amines, to give solutions which are blue when dilute. The solutions ate paramagnetic and conduct electricity, the carrier being the solvated electron. In dilute solutions the metal is dissociated into metal ions and ammoniated electrons. The metal ions are solvated in the same way that they would be in a solution of a metal salt in ammonia, and so comparison can be made with, for example, [Na(NH3)4]+I-, the IR and Raman spectra of which indicate a tetrahedral coodination sphere for the metal.39... 

The perturbation of the Si-H vibration of ammoniated trichlorosilylated silica (figures 12.14 and 12.16) consists at first sight of at least 3 distinct bands, indicating that at least 3 different species with an Si-H band exist on the surface. The strong electron donating effect of the amine functions will cause a low wavenumber shift of the Si-H band. 

Based on this model, cycle 2 can be summarized as follows 0.9 mmol trichlorosilane react with the ammoniated silica, producing 1.3 mmol surface Cl species, and converting 1.1 mmol amines towards silazanes. Upon ammoniation, the 1.3 mmol Cl mostly convert towards new amine species and NH4C1. 

To this group belong the numerous hydrates and ammoniates (ammines) as well as the ion compounds which contain alcohol or ether of crystallization, amines, etc. 

SYNS AMINOMERCURIC CHLORIDE AMMONI-ATED MERCURY MERCURIC AMMONIUM CHLORIDE, solid MERCURIC CHLORIDE, AMMONIATED MERCURY AMINE CHLORIDE MERCURY AMMONIATED D WHITE MERCURY PRECIPITATED WHITE PRECIPITATE... 

For example, the one-electron models incorrectly predict (even at a qualitative level) the Knight shifts in and NMR spectra of ammoniated electron, and solvated electrons in amines (Sec. 4.1). The same problem arises in the explanation of magnetic (hyperfine) parameters obtained from ESEEM spectra of trapped (hydrated) electrons in low-temperature alkaline ices. The recent resonance Raman spectra of also appear to be incompatible with the one-... 

The metal-NHs reductions of carbonyl groups are exceedingly fast reactions for the reaction of acetone with an ammoniated electron the rate is 9 x 10 M" s". Although many, particularly older, published experimental procedures for the metal-NHs reduction of ketones employ prolonged reaction times with excess metal, these conditions are unnecessarily harsh. The reactions of carbonyl compounds with metals in NH3 are effectively instantaneous and by using short reaction times it appears that reduction of terminal alkenes and disubstituted alkynes can be avoided.In addition to the functional groups mentioned above, alcohols, amines and ethers, other than epoxides, are usually stable to reductions of aldehydes and ketones by dissolving metals. " ... 

The approximately constant expansion of the graphite lattice, which is practically independent of the size of the intercalated metal atom, appears at first sight unusual for, in the ammonia-free compounds, the distance between the layer planes increases, as expected, with increasing size of the alkali metal atom from potassium to cesium. The constancy of the expansion for the ammoniates is perhaps attributable to the effect of the positions of the ammonia molecules in the lattice in determining the increase in the interplanar distance. If this were so, metal atoms or ions could perhaps find sufficient room in holes in the ammonia lattice. In support of this view it may be added that the expansion becomes greater if, in place of ammonia, a layer of amine such as methylamine or ethylamine is intercalated. 

Solutions of alkali metals in ammonia have been the best studied, but other metals and other solvents give similar results. The alkaline earth metals except- beryllium form similar solutions readily, but upon evaporation a solid ammoniate," MINI-lj),. is formed. Lanthanide elements with stable + 2 oxidation states (europium, ytterbium) also form solutions. Cathodic reduction of solutions of aluminum iodide, beryllium chloride, and tetraalkylammonium halides yields blue solutions, presumably containing Al, 3e Be", 2e and R4N, e respectively. Other solvents such as various amines, ethers, and hexamethylphosphoramide have been investigated and show some propensity to form this type of solution. Although none does so as readily as ammonia, stabilization of the cation by complexation results in typical blue solutions... 

Other extraction procedures have been developed. For example, a system for volatile compounds is noted in Section 2.2.7 and one for extraction of aromatic amines from rainwater used sorption to rayon bearing covalently bound trisulfo-copper phthalocyanine followed by elution with an ammoni-acal solution (Wu et al. 1995). 

AMMONIATED MERCURY (10124-48-8) Reacts violently with halogens barium, chlorine, fluorine, and metal salts of amines. Contact with acids or acid fumes causes decomposition, producing hydrogen chloride fumes. Incompatible with organic anhydrides, acrylates, alcohols, aldehydes, alkylene oxides, substituted allyls, cresols, caprolactam solution, epichlorohydrin, ethylene dichloride, glycols, isocyanates, ketones, maleic anhydride, nitrates, nitromethane, phenols, vinyl acetate. May corrode aluminum, copper, zinc, and some stainless steel in the presence of moisture. 

Aminomercuric chloride Aminomercury chloride Ammoniated mercuric chloride Ammoniated mercury EINECS 233-335-8 HSDB 1175 Hydrargyrum ammonialum Hydrargyrum praecipitatum album Hydrargyrum precipitatum album Lemer/s white precipitate Mercuric amidochloride Mercuric ammonium chloride Mercuric chloride, ammoniated Mercury amide chloride (Hg(NH2)CI) Mercury amide chloride Mercury amine chloride Mercury, ammoniated Mercury ammonium chloride Mercury, ammonobasic (HgNHjCI) Mercury(ll) chloride ammonobasic Quecksilber(ll)-amid-chlorid UN1630 White mercuric precipitate White mercury precipitated White precipitate. Mercury ammonium chloride, used for the preparation of cinnabar and in medicine as a topical anti-intective. Powder d = 5.38 insoluble in H2O, EtOH, soluble in mineral xids. 

The ferrous halides combine with gaseous ammonia, forming several ammoniates of which the highest are the hexammoniates that contain the ion, [Fe(NH3)6]2+. Other anhydrous ferrous compounds also absorb ammonia. The ammine complexes are not stable in water, however, except in saturated aqueous ammonia. With chelating amine ligands, many complexes stable in aqueous solution are known. For example, ethylenediamine forms the entire series ... 

Since ethers may be formed from two molecules of alcohol, and secondary and tertiary amines from two molecules of amines of lower order it should be possible to combine alcohols and amines. Such compounds have been formed by treating alcohols with ammoniated zinc chloride (V. Merz and K. Gasiorowski, Ber. 17, 623 (1884)). 

An alternative approach to surface imprinting of silica was recently introduced [36,37]. The process is based on a sol-gel reaction inside reverse micelles (Fig. 18a). The template molecule acts as the headgroup of a surfactant. After mixing with a nonionic surfactant, cyclohexane, water and ammoniated ethanol, a water-in-oil microemulsion is formed. The co-condensation is then started by addition of Si(OEt)4 and amine-, dihydroimidazole- and carboxylate-terminated trialkoxysi-lanes to give silica particles with a diameter between 400 and 600 nm. Since the stemplate molecule was located at the interface of the micelle during the condensation reaction, the resulting imprints are formed at the surface of the particle. 

Mercury, aceto(chloromethoxypropyl)- Mercury, acetoxy (chloromethoxypropyl)-. See Chloromethoxy propyl mercuric acetate Mercury, acetoxy (2-methoxyethyl)-. See Methoxyethylmercury acetate Mercury-amide-chloride Mercury (II) amidochloride Mercury amine chloride Mercury ammoniated. See Mercury ammonium chloride... 

The secondary amine liA-2 and ammoniated water (32 atom% NH], 68 atom% HjO) were investigated because they include nitrogen which has a moderate thermal-neutron absorption cross section. The nitrogen causes a small shift in the plutonium concentration at which the minimum critical mass occurs. Representative compositions that were assumed for these materials in the calculations are listed in Table 1. For the secondary amine LA-2, the critical mass curve crosses that for water. Systems containing LA-2 are therefore more reactive, than water-moderated systems at higher plutonium deri- slties. ... 

Sivaev, I. B., Bruskin, A. B., Nesterov, V. V. et al. 1999. Synthesis of schiff bases derived from the ammoni-aundecahydro-cZoio-dodecaborate(l-) anion, [B,2H,NH = CHR] , and their reduction into monosubsti-tuted amines [Bi2HnNH2CH2R] A new route to water soluble agents for BNCT. Inorg. Chem., 38, 5887-93. 

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