Alkali metals compound solubility

Nitrates, acetates, and alkali metal compounds are water-soluble. Zn(N03)2, Pb(C2H302)2, and Nal are soluble. Most halides are soluble in water CuCl2 is soluble in water. Although most sulfates are soluble in water, BaSO s) is not soluble in water. Only a few hydroxides are soluble in water Al(OH)3(s) is not soluble in water. 

Alkali metal compounds Li, Na, K, Rb, Cs All soluble Some complex (ternary) alkali metal salts... 

The extensive use of alkyllithium initiators is due to their solubility in hydrocarbon solvents. Alkyls or aryls of the heavier alkali metals are poorly soluble in hydrocarbons, a consequence of their more ionic nature. The heavier alkali metal compounds, as well as alkyllithiums, are soluble in more polar solvents such as ethers. The use of most of the alkali metal compounds, especially, the more ionic ones, in ether solvents is somewhat limited by their reactivity toward ethers. The problem is overcome by working below ambient temperatures and/or using less reactive (i.e., resonance-stabilized) anions as in benzylpotassium, cumylcesium and diphenylmethyllithium. 

The ordinary tellurates of colourless metallic radicals are colourless substances. The salts of the alkali metals are soluble in water but have no definite solubility. In many respects these salts resemble colloids, many of the basic and so-called acid salts which have been described having been shown to be adsorption compounds.7 When the alkali tellurates are heated, they decompose with the formation of tellurites, and they are generally more easily reducible than the latter salts. 

Scrubbing solutions containing sodium (or other alkali metals) compounds have been extensively studied for removal of S02. Justification for the use of sodium compounds includes (a) complete solubility in water with no formation of scale and (b) simple reactions with S02 Na2C03 +... 

The synthesis of the first cyclopentadienylberyllium compound was reported by Fischer and Hofmann in 1959 (49). Reaction of cyclopentadienyl alkali-metal compounds with BeCl2 in diethyl ether or benzene leads to dicyclopentadienylberyllium (beryllocene), a rather volatile, colorless, diamagnetic complex, easily soluble in benzene, diethyl ether, and hydrocarbons, and very sensitive to air and moisture. 

Nearly all alkali metal compounds are soluble in water. Sulfide and phosphate compounds are usually insoluble. How, then, do you account for the fact that sodium sulfide and potassium phosphate are soluble, while iron sulfide and calcium phosphate are insoluble Why do some ions form soluble compounds, while other ions form insoluble compounds ... 

We can often apply a generality to answer a specific question. For example, you can tell that Na2Mo04 is soluble in water even if we have never seen this formula before. According to Table 8.3, all alkali metal compounds are soluble, and this compound is an alkali metal salt. 

The carbazole compounds, (77 -Af-carbazolyl)2Ca(pyridine)4, (Tj -N-car-bazolyl)2Sr(NH3)(DME)2, and (i7 -Af-carbazolyl)2Ba(DME)3 (Fig. 9), are colorless or yellow solids that have good solubility in donor solvents such as pyridine. They are monomeric in the solid state with the carbazolyl ligands bonded only through the nitrogen atom (tj ) to the metals. The metal coordination spheres are completed by incorporation of the Lewis bases pyridine, DME, and ammonia. A smooth increase in coordination number with metal size, from 6 (Ca) to 7 (Sr) to 8 (Ba), is observed in these compounds. The reason for the Tj -Af-bondingof the carbazolyl ligand instead of multihapto bonding as occurs in the alkali metal compounds of carbazole and the fluorenyl compounds of the alkaline-earth metals (see Section III,G,2) is presently unclear. ... 

It was shown that the alkali metal compounds increase steadily in solubility along the series given above, and that they are dissociated to an extent sufiicient to enable precipitation reactions involving the CsH.- " ion to be possible. On adding anhydrous metal salts which are soluble in liquid ammonia, such as nitrates and thiocyanates, the following type of reaction takes place ... 

The polymerization of the higher aliphatic aldehydes has many similarities with formaldehyde polymerization. Notable differences are a lower ceilii temperature and the possibility of different steric configurations due to the substituted carbon atom. Especially anionic catalysts such as alkali metal alkoxides, soluble hydrides, and organo metal compounds lead to polymerizations during which crystalline isotactic polymer is produced 96). Little is known about the morphology and the detailed crystallization mechanism of the polyaldehydes. 

Organolithium compounds are among the very few alkali-metal compounds that have properties—solubility in hydrocarbons or other non-polar liquids and high volatility—typical of covalent substances. They are generally liquids or low-melting solids, and molecular association is an important structural feature,26... 

Carbon dispersed in liquid alkali metals is hydrided by the reaction with dissolved hydrogen or hydrides to evolve methane. Some reactions of non-metals dissolved in the molten metals are important for the compatibility of materials with the alkali metals. Transition metals are almost insoluble in molten alkali metals. Their solubilities can be considerably raised by dissolved non-metals. Several metals of the fourth and fifth group form one or more intermetallic compounds with alkali metals. 

On the other hand 1 2 electrolytes and polyelectrolytes are frequently less soluble. Examples are numerous carbonates, sulphates, phosphates and oxides. Halides and pseudohalides of the alkaline earth metals, which belong also to this group, show considerably smaller solubilities than the corresponding alkali metal compounds. 

Because of their chemical reactivity, the Group lA elements never occur as free metals in nature. They do occur extensively in silicate minerals, which weather to form soluble compounds of the elements (particularly of sodium and potassium). These soluble compounds eventually find their way to landlocked lakes and oceans, where they concentrate. Enormons nnderground beds of sodium and potassium compounds formed when lakes and seas became isolated by geologic events the wate eventually evaporated, leaving solid deposits of alkali metal compounds. Commercially, sodium and potassium compounds are conunon, and both sodium and lithium metals arc available in quantity. 

There are fewer reports of linear, acyclic, ion-binding polymers. It has been reported that poly(oxyethylene) improves the solubility of alkali metals in ethers such as tetrahydrofuran, dime thoxy ethane, and diglyme, stabilizes fluorenyl alkali metal compounds, accelerates Williamson reactions and accelerates several other nucleophilic reactions.All of these effects were attributed to the ability of poly(oxyethylene) to complex with cations in solution. Yanagida and coworkers studied the alkali metal cation complexation of poly(oxyethylene), using a picrate salt extraction technique similar to the one used by Pedersen and Frensdorff. Polymers with more than 23 oxyethylene units were effective iono-phores for potassium, with degrees of extraction (percent extracted) comparable to crown ethers. The extractability per oxyethylene unit was nearly constant, and the complex stability increased linearly with increasing numbers of repeating oxyethylene units. Seven oxyethylenes were the minimum number of repeat units necessary to bind potassium ion effectively in the aqueous phase. The less efficient extraction of short-chain poly(oxyethylene) is apparently caused by its hydrophilic character. 

Because most alkali metal compounds are water soluble, a number of Li, Na, and K compounds, including chlorides, carbonates, and sulfates, can be obtained from natural brines. A few alkali metal compoimds, such as NaCl, KCl, and Na2C03, can be mined as solid deposits. Sodium chloride is also obtained from seawater. An important source of lithium is the mineral spodumene, LiAl(Si03)2, shown in the margin. Rubidium and cesium are obtained as by-products in the processing of lithium ores. 

Lithium-ammonia reduction of l7a-ethyl-19-nortestosterone (68) using Procedure 8a (section V) affords the 4,5a-dihydro compound (69) in 85% yield after a reaction time of 12 minutes after a reaction time of 80 minutes, the yield of (69) is 76%. Lfsing sodium in the same reduction, the yields of compound (69) are 79 and 77 % after reaction times of 8 and 80 minutes respectively. Both the lithium and sodium enolates appear to be reasonably stable in liquid ammonia in the presence of alkali metal. Since the enolate salts are poorly soluble in ammonia, their resistance to protonation by it may be due in part to this factor. 

Lithium was recognized as a new alkali metal by J. A. Arfved.son in 1817 whilst he was working as a young assistant in J. J. Berzelius s laboratory. He noted that Li compounds were similar to those of Na and K but that the carbonate and hydroxide were much less soluble... 

The small size of lithium frequently confers special properties on its compounds and for this reason the element is sometimes termed anomalous . For example, it is miscible with Na only above 380° and is immiscible with molten K, Rb and Cs, whereas all other pairs of alkali metals are miscible with each other in all proportions. (The ternary alloy containing 12% Na, 47% K and 41% Cs has the lowest known mp, —78°C, of any metallic system.) Li shows many similarities to Mg. This so-called diagonal relationship stems from the similarity in ionic size of the two elements / (Li ) 76pm, / (Mg ) 72pm, compared with / (Na ) 102pm. Thus, as first noted by Arfvedson in establishing lithium as a new element, LiOH and LiiCOs are much less soluble than the corresponding... 

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