Lithium metal carbon dioxide

Chemical Lithium metal Sulfur dioxide Acetonitrile Lithium bromide Carbon blaek... 

As with the hydroxides, we find that whilst the carbonates of most metals are insoluble, those of alkali metals are soluble, so that they provide a good source of the carbonate ion COf in solution the alkali metal carbonates, except that of lithium, are stable to heat. Group II carbonates are generally insoluble in water and less stable to heat, losing carbon dioxide reversibly at high temperatures. 

The in situ generation of the carbon dioxide adduct of an indole provides sufficient protection and activation of an indole for metalation at C-2 with r-butyl-lithium. The lithium reagent can be quenched with an electrophile, and quenching of the reaction with water releases the carbon dioxide. ... 

The stereochemistry of the carboxylation of 4-substituted ( + )-(/ S)-fra ,v-1-(4-mcthylphcnyl-sulfinylmethyl)cyclohexane after metalation with methyllithium and quenching with carbon dioxide was reported64. The results listed in Table 1 show that the d.r. of around 75 25 under kinetic control changes to 25 75 under thermodynamic control. This is the result of the equilibration of the two diastereomeric metalated species. As shown by the experiment in hexamethylphosphoric Iriamide (IIMI A) (d.r. = 57 43 under kinetic control) an electrophilic assistance of the lithium cation to the electrophilic approach is probably involved. 

Carbon dioxide reacts slowly with fragmented lithium at 20 C. With the powdered metal, its ignition is instantaneous. It also happens when it is hot. This is the reason why carbon dioxide extinguishers are forbidden for putting out lithium fires (and metals in general see later). 

Sodium is, like all other alkali metals, a very strong reducing agent (more reactive than lithium), which has extremely violent reactions with numerous compounds. It causes a large number of accidents. Sodium peroxide is a very reactive oxidant, which has violent interactions with reducing agents. Carbonates, and especially sodium hydroxide, are bases which react with acids (the reaction is aggravated by the formation of carbon dioxide). 

The aryl bromides undergo facile metalation with butyl lithium to produce aryllithium derivatives with the expected organometallic activity.9 For example, reaction of lithiated PPO with carbon dioxide produces a carboxylated PPO which exhibits unique blending characteristics18. 

Acetone Acetylene Alkali and alkaline earth metals, e.g. sodium, potassium, lithium, magnesium, calcium, powdered aluminium Anhydrous ammonia Concentrated nitric and sulphuric acid mixtures Chlorine, bromine, copper, silver, flourine or mercury Carbon dioxide, carbon tetrachloride, or other chlorinated hydrocarbons. (Also prohibit, water, foam and dry chemical on fires involving these metals - dry sand should be available.) Mercury, chlorine, calcium hypochlorite, iodine, bromine or hydrogen fluoride... 

Aluminium Aluminium halides, Carbon oxides Lithium Non-metal oxides Magnesium Carbon dioxide, etc. 

Although carbon dioxide reacts slowly with lithium at ambient temperature, the molten metal will bum vigorously in the gas, which cannot be used as an extinguisher on lithium fires. Carbon monoxide reacts in liquid ammonia to give the carbonyl which reacts explosively with water or air. Lithium rapidly attacks silica or glass at 250°C. 

A number of groups have been found to direct and stabilize o-metallation in aromatic systems since Meyers ( ) introduced the oxazolidine group for this purpose. It was reasoned that the imidazolinone group should also serve this purpose. It was gratifying to find that treatment of the pyridyl imidazolinone 22 th 2.2 equivalents of butyl lithium followed by carbon dioxide gave a good yield of the nicotinic acid 14 (R=H). 

The development of electrospray ionization (ESI) enabled multiply charged ions, solvated ions, and metal-coordinated species to be formed in the gas phase. Recently, Kass and coworkers showed that collision-induced dissociation (CID) of RC02Li containing ions (e.g. 1) leads to the loss of carbon dioxide and the attachment of Li to R (Scheme 1) . This is an exceptionally stable alkyl lithium compound that could be synthesized, in the gas phase, under relatively mild conditions. 

The most direct route towards functionalized aliphatic polyesters is based on the functionalization of polyester chains. This approach is a very appealing because a wide range of functionalized aliphatic polyesters could then be made available from a single precursor. This approach was implemented by Vert and coworkers using a two-step process. Eirst, PCL was metallated by lithium diisopropylamide with formation of a poly(enolate). Second, the poly(enolate) was reacted with an electrophile such as naphthoyl chloride [101], benzylchloroformate [101] acetophenone [101], benzaldehyde [101], carbon dioxide [102] tritiated water [103], ot-bromoacetoxy-co-methoxy-poly(ethylene oxide) [104], or iodine [105] (Fig. 26). The implementation of this strategy is, however, difficult because of a severe competition between chain metallation and chain degradation. Moreover, the content of functionalization is quite low (<30%), even under optimized conditions. 

Metallation of 3,4-dimethyl-l,2,5-thiadiazole (55) to the anion (56) was accomplished with the use of a nonnucleophilic base, lithium diisopropylamide <82JHC1247>. Nucleophilic attack at sulfur resulted in an alkyllithium reagent <70CJC2006>. The lithiomethyl derivative (56) was carboxylated to (57) with carbon dioxide and converted to the vinyl derivative (58) via an esterification, reduction, mesylation, and base elimination sequence (Scheme 12). 

Lithium hydride is a strong reducing agent and would, therefore, react with compounds that contain oxygen. Even many highly stable oxides of metals and nonmetals can be reduced. It reduces metal oxides to metals and carbon dioxide to carbon ... 

The hydroxy-alkoxides condense to form a polymeric gel with metal-oxygen-metal links. Lithium niobate is then formed when the gel is heated. Heating removes any remaining ethanol and any water formed during the condensation. The remaining ethyl groups are pyrolysed (i.e., oxidised to carbon dioxide and water) leaving the oxides. 

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