Aluminums alkali metals

Phenylhydrazine Phosgene Phosphine Lead dioxide, oxidizers Aluminum, alkali metals, 2-propanol Air, boron trichloride, bromine, chlorine, nitric acid, nitrogen oxides, nitrous acid, oxygen, silver nitrate... 

Incompatibilities and Reactivities Anhydrous chlorides of iron, tin, and aluminum peroxides of iron and aluminum alkali metal hydroxides iron strong acids, caustics peroxides [Note Polymerization may occur due to high temperatures or contamination with alkalis, aqueous acids, amines acidic alcohols ] ... 

There is some uncertainty as to whether zinc embrittles aluminum. However, indium severely embrittles aluminum. Alkali metals, sodium, and lidiium also are known to embrittle aluminum. Aluminum alloys containing either lead, cadmium, or bismuth inclusions embrittle when impact-tested near the melting point of these inclusions the sevoity of embrittlement increases from lead to cadmium to bismuth. 

Cesium, an alkali metal, occurs in lepidolite, pollucte (a hydrated silicate of aluminum and cesium), and in other sources. One of the world s richest sources of cesium is located at Bernic Lake, Manitoba. The deposits are estimated to contain 300,000 tons of pollucite, averaging 20% cesium. 

From Metals and Alcohol. Alkali metals, alkaline earth metals, and aluminum react with alcohols to give metal alkoxides (2,3,65) ... 

Metals do not generally react with vitreous siUca below 1000°C or their melting point, whichever is lower. Exceptions are alurninum, magnesium, and alkah metals. Aluminum readily reduces siUca at 700—800°C. Alkali metal vapors attack at temperatures as low as 200°C. Sodium vapor attack involves a diffusion of sodium into the glass, followed by a reduction of the siUca. 

The most common catalysts in order of decreasing reactivity are haUdes of aluminum, boron, zinc, and kon (76). Alkali metals and thek alcoholates, amines, nitriles, and tetraalkylureas have been used (77—80). The largest commercial processes use a resin—catalyst system (81). Trichlorosilane refluxes in a bed of anion-exchange resin containing tertiary amino or quaternary ammonium groups. Contact time can be used to control disproportionation to dichlorosilane, monochlorosilane, or silane. 

Metallic Antimonides. Numerous binary compounds of antimony with metallic elements are known. The most important of these are indium antimonide [1312-41 -0] InSb, gallium antimonide [12064-03-8] GaSb, and aluminum antimonide [25152-52-7] AlSb, which find extensive use as semiconductors. The alkali metal antimonides, such as lithium antimonide [12057-30-6] and sodium antimonide [12058-86-5] do not consist of simple ions. Rather, there is appreciable covalent bonding between the alkali metal and the Sb as well as between pairs of Na atoms. These compounds are useful for the preparation of organoantimony compounds, such as trimethylstibine [594-10-5] (CH2)2Sb, by reaction with an organohalogen compound. 

Lewis acids are defined as molecules that act as electron-pair acceptors. The proton is an important special case, but many other species can play an important role in the catalysis of organic reactions. The most important in organic reactions are metal cations and covalent compounds of metals. Metal cations that play prominent roles as catalysts include the alkali-metal monocations Li+, Na+, K+, Cs+, and Rb+, divalent ions such as Mg +, Ca +, and Zn, marry of the transition-metal cations, and certain lanthanides. The most commonly employed of the covalent compounds include boron trifluoride, aluminum chloride, titanium tetrachloride, and tin tetrachloride. Various other derivatives of boron, aluminum, and titanium also are employed as Lewis acid catalysts. 

The combination of alkali metal acid fluorides and porous aluminum fluoride IS a stable, solid, and efficient substitute for anhydrous hydrogen fluoride for promoting the ring-opening reactions of simple aliphatic oxiranes to give the fluorohydrins under sonication [/5] (equations 14 and 15)... 

Chlor-. of or combined with chlorine, chloro (as Chlorbenzoeadure, chlorobenzoic acid), chloride of (as Chlorzink, zinc chloride), chlorahnlich, a. like chlorine, chlorinous. Chlor-alaun, m. chloralum, -alkalien, n.pl. alkali-metal chlorides, -allyl, n, allyl chloride, -aluminium, n. aluminum chloride, -ammon, m., -ammonium, n. ammonium chloride, -amyl, n, amyl chloride, -antimon, n, antimony chloride, -arsenlk, n. chloride of arsenic, -arsenikldsung, /, (Pkarm.) solution of arsenious add, hydrochloric solution of arsenic, -arsinkampfstoff, m. chlorodi-phenylarsine, adamsite, chlorartig, a. like chlorine, chlorinous,... 

No aluminum silicates of alkali metals are known in which the A1+3 R+1 ratio is less than 1 1. 

It is further shown that the theory requires that no stable basic silicates of divalent metals exist, and that in aluminum silicates of alkali metals there should be at least one aluminum ion for every alkali ion. 

Alkali metal derivatives of 2-(trimethylsilyl)aminopyridines can be further derivatized by insertion of 1,3-dicyclohexylcarbodiimide. Functionalized guani-dinates are formed in this reaction via a 1,3-silyl shift. Scheme 170 illustrates the reaction sequence as well as the preparation of an aluminum complex of the modified ligand, which exhibits pseudo jS-diketiminate binding of the metal center, thus exemplifying the coordinative versatility of this new multi-N-donor system. ... 

Brown, H. C., The Reactions of Alkali Metal Hydrides and Boro-hydrides with Lewis Acids of Boron and Aluminum, Congr. Lect., 17th Int. Congr. Pure Appl. Chem. p. 167. Butterworths, London, 1960. 

B. Bogdanovic, M. Felderhoff, S. Kaskel, A. Pommerin, K. Schlichte, F. Schiith, Reversible Storage of Hydrogen using Doped Alkali Metal Aluminum Hydrides, 2001, WO 03/053848 Al. 

Cases exist, however, where for fundamental reasons aqueous solutions cannot be used. One such case is that of devices in which electrochemical processes take place at elevated temperatures (above 180 to 200°C) for example, the electrowinning of aluminum performed at temperatures close to 1000°C. Another case is that of devices in which electrodes consisting of alkali metals are used, which are unstable in aqueous solutions, such as batteries with a lithium negative electrode. 

Since these early reports, several groups have continued to improve these catalytic reactions. The most successful catalysts to date are rare earth/alkali metal/BINOL complexes like LLB, while htanium, aluminum, and zinc catalysts have also been described. 

The elements that form only one cation are the alkali metals (group IA), the alkaline earth metals (group IIA), zinc, cadmium, aluminum, and most often silver. The charge on the ions that these elements form in their compounds is always equal to their periodic table group number (or group number minus 10 in the newest labeling system in the periodic table). 

Bogdanovic, B. and M. Schwickardi, Ti-doped alkali metal aluminum hydrides as potential novel reversible hydrogen storage materials, /. Alloys Compd., 1-9, 253-254, 1997. 

Some of the investigations carried out in the first half of the twentieth century were related to CL associated with thermal decomposition of aromatic cyclic peroxides [75, 76] and the extremely low-level ultraviolet emission produced in different reaction systems such as neutralization and redox reactions involving oxidants (permanganate, halogens, and chromic acid in combination with oxalates, glucose, or bisulfite) [77], In this period some papers appeared in which the bright luminescence emitted when alkali metals were exposed to oxygen was reported. The phenomenon was described for derivatives of zinc [78], boron [79], and sodium, potassium, and aluminum [80]. 

Even the Cannizzaro reaction might have a similar transition state. Although the coordinating tendency of alkali metals is less than that of aluminum or magnesium, it is not negligible. An alternative structure is possible in this case in which a proton occupies the bridging position. 

All sulfides (except alkali metals, ammonium, magnesium, calcium, and barium) are insoluble. Aluminum and chromium sulfides are hydrolyzed and precipitate as hydroxides. 

Copper(II) sulfate Cumene hydroperoxide Cyanides Cyclohexanol Cyclohexanone Decaborane-14 Diazomethane 1,1-Dichloroethylene Dimethylformamide Hydroxylamine, magnesium Acids (inorganic or organic) Acids, water or steam, fluorine, magnesium, nitric acid and nitrates, nitrites Oxidants Hydrogen peroxide, nitric acid Dimethyl sulfoxide, ethers, halocarbons Alkali metals, calcium sulfate Air, chlorotrifluoroethylene, ozone, perchloryl fluoride Halocarbons, inorganic and organic nitrates, bromine, chromium(VI) oxide, aluminum trimethyl, phosphorus trioxide... 

Maleic anhydride Manganese dioxide Alkali metals, amines, KOH, NaOH, pyridine Aluminum, hydrogen sulfide, oxidants, potassium azide, hydrogen peroxide, peroxosulfuric acid, sodium peroxide... 

Alkali metals, finely divided aluminum and magnesium particles, hydrazine, diborane, metal hydrides, and hydrogen are strong reducing agents [35]. An example of a significant problem is the possible explosive reaction between light metals and carbon tetrachloride which is itself a stable compound [57]. 

A similar type of catalyst including a supported noble metal for regeneration was described extensively in a series of patents assigned to UOP (209-214). The catalysts were prepared by the sublimation of metal halides, especially aluminum chloride and boron trifluoride, onto an alumina carrier modified with alkali or rare earth-alkali metal ions. The noble metal was preferably deposited in an eggshell concentration profile. An earlier patent assigned to Texaco (215) describes the use of chlorinated alumina in the isobutane alkylation with higher alkenes, especially hexenes. TMPs were supposed to form via self-alkylation. Fluorinated alumina and silica samples were also tested in isobutane alkylation,... 

Chemical Incompatibility Hazards While N2 and C02 may act as inerts with respect to many combustion reactions, they are far from being chemically inert. Only the noble gases (eg., Ar and He) can, for practical purposes, be regarded as true inerts. Frank (Frank, Inerting for Explosion Prevention, Proceedings of the 38th Annual Loss Prevention Symposium, AIChE, 2004) lists a number of incompatibilities for N2, C02, and CO (which can be present in gas streams from combustion-based inert gas generators). Notable incompatibilities for N2 are lithium metal and titanium metal (which is reported to burn in N2). C02 is incompatible with many metals (eg., aluminum and the alkali metals), bases, and amines, and it forms carbonic acid in water,... 

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