Lithium metal water

Lithium Iodide. Lithium iodide [10377-51 -2/, Lil, is the most difficult lithium halide to prepare and has few appHcations. Aqueous solutions of the salt can be prepared by carehil neutralization of hydroiodic acid with lithium carbonate or lithium hydroxide. Concentration of the aqueous solution leads successively to the trihydrate [7790-22-9] dihydrate [17023-25-5] and monohydrate [17023-24 ] which melt congmendy at 75, 79, and 130°C, respectively. The anhydrous salt can be obtained by carehil removal of water under vacuum, but because of the strong tendency to oxidize and eliminate iodine which occurs on heating the salt ia air, it is often prepared from reactions of lithium metal or lithium hydride with iodine ia organic solvents. The salt is extremely soluble ia water (62.6 wt % at 25°C) (59) and the solutions have extremely low vapor pressures (60). Lithium iodide is used as an electrolyte ia selected lithium battery appHcations, where it is formed in situ from reaction of lithium metal with iodine. It can also be a component of low melting molten salts and as a catalyst ia aldol condensations. 

An ethereal solution approximately 2.5 molar in methyllithium is prepared from 17 ml of methyl iodide and 4 g of lithium metal in 200 ml of anhydrous ether. A mixture consisting of 150 ml anhydrous ether, 3 g (10 mmoles) of 3jS-hydroxy-5a-androstane-ll,17-dione and 60 ml (0.15 moles) of the above methyllithium solution are stirred at room temperature for 40 hr. The reaction mixture is diluted with 100 ml of water and the ether is removed by distillation. Filtration of the chilled aqueous phase yields 2.6 g (77%) of 1 la,17a-dimethyl-5a-androstane-3a,l l/ ,17j5-triol mp 149-154°. Recrystallization from acetone-hexane yields pure material mp 164-166° [a] —5° (CHCI3). 

Dilithium phthctlocyanine (PcLi2) can be prepared by the method of Linstead.59 Lithium metal is added to pentan-l-ol and heated to dissolve the metal. Then, the phthalonitrile is added and the mixture is refluxed for some hours. Due to its lability toward water and acid, both have to be excluded during the reaction and purification.79131132... 

A piece of lithium metal was added to a flask of water on a day when the atmospheric pressure was 757.5 Torr. The lithium reacted completely with the water to produce 250,0 ml. of hydrogen gas, collected over the water at 23°C, at which temperature the vapor pressure of water is 21.07 Torr. (a) What is the partial pressure of hydrogen in the collection flask ... 

Lithium compounds, not lithium metal, are used in the treatment of some types of mental disorders. The chemical properties of lithium metal are very different from lithium compounds containing the ion, Li+. Li metal is very reactive with water, forming the strong base, LiOH, and hydrogen gas and releasing much heat, none of which are good for the human body. 

A 3-1. three-necked flask, equipped with a Dry Ice condenser (Note 1), a sealed Hershberg-type stirrer, and an inlet tube, is set up in a hood and charged with 108 g. (0.75 mole) of a-naphthol (Note 2). The stirrer is started, and to the rapidly stirred flask contents (Note 3) is added 11. of liquid ammonia as rapidly as possible (about 5 minutes). When the naphthol has gone into solution (about 10 minutes), 20.8 g. (3.0 g. atoms) of lithium metal (Note 4) is added in small pieces and at such a rate as to prevent the ammonia from refluxing too violently (Note 5). After the addition of the lithium has been completed (about 45 minutes), the solution is stirred for an additional 20 minutes and is then treated with 170 ml. (3.0 moles) of absolute ethanol which is added dropwise over a period of 30-45 minutes (Note 6). The condenser is removed, stirring is continued, and the ammonia is evaporated in a stream of air introduced through the inlet tube. The residue is dissolved in 1 1. of water, and, after the solution has been extracted with two 100-ml. portions of ether, it is carefully acidified with concentrated hydrochloric acid. The product formed is taken into ether with three 250-ml. extractions, and then the ether extract is washed with water and dried over anhydrous sodium sulfate. The ether is removed... 

Another synthetic route which gives a good yield of the labelled tin hydride involves the hydrolysis of an organometallic intermediate such as a trialkylstannyllithium46 with deuterated or tritiated water. The trialkylstannyllithium can be prepared by treating the trialkyltin chloride with lithium metal in THF46. This process is shown in equation 42. 

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,... 

Any reaction in solution may be considered to result from both EPD-EPA and ED-EA interactions. The sequence of functions follows the functional principle a chemical interaction is initiated when the reacting entity exhibits one of the four functions, while the other reactant exhibits the reverse correlated function. The reaction is completed when the resulting electronic changes are compensated for by the reverse non-correlated functions. This may be illustrated by the reaction of lithium metal with water 3, 5). 

Lithium metal functions in water as ED, therefore the lithium ion produced will compensate for the loss of the electron by functioning as EPA towards water molecules which in turn function as EPD towards the metal ion ... 

Lithium chloride is used in the production of lithium metal by electrolysis. It also is used in metallurgy as a eutectic melting composition with potassium chloride (LiCl 41 mol% KCl 59 mol%). Other applications are in low temperature dry-cell batteries as a dehumidifier in air conditioning in welding and soldering flux as a desiccant in fireworks and in mineral waters and soft drinks. 

Propylene Carbonate (PC) and Water. Data from both spectroscopic and thermodynamic studies for other solvent systems are sparse and some of it is of doubtful quality. For propylene carbonate, Salomon (40) has obtained emf data using lithium metal and thallium amalgam-thallous chloride or bromide electrodes. 

The emf values for Li+, Na+. Rh+, and Cs1- are -3.04, -2.71, -2.94, and -3.03 V, respectively. Although lithium metal is the most easily oxidized in the thermodynamic sense, it is less reactive in water than the other alkali metals because of its relatively high melting point (180 °C). The others become molten from the beat of reaction, melting at less than 100 °C, and as a result expose a much greater surface area. 

The entry of lithium batteries into the consumer market is still quite recent and not much attention has so far been paid to disposal and the possibility of recycling procedures. Lithium metal, although not toxic, is a safety hazard since it is very reactive, especially in contact with water or in high humidity. This makes lithium batteries which have not been fully... 

Because of the reactivity of lithium with water lo lomi its hydroxide. LiOH. and hydrogen, its properties when dissolved in other solvents have been studied extensively. It dries not decompose liquid H<. hut does form a blue solution, which decomposes to yield its amide, LIN IT. and hydrogen, when catalyzed by metallic salts. With the elements of main groups 2 to 7. lithium in liquid NIL, reacts lo form binaty compounds, which may vary from simple halides, as with the halogens, to inlermetallic phases, as with cadmium and mercury. Lithium amide in liquid NIL is regarded in the same class as a hydroxide ill aqueous solution. 

H.3 Write balanced chemical equations for the following reactions (a) Sodium metal reacts with water to produce hydrogen gas and sodium hydroxide, (b) The reaction of sodium oxide, Na20, and water produces sodium hydroxide, (c) Hot lithium metal reacts in a nitrogen atmosphere to produce lithium nitride, Li3N. (d) The reaction of calcium metal with water leads to the evolution of hydrogen gas and the formation of calcium hydroxide, Ca(OH)2. 

Assume that you wanted to prepare a small volume of pure hydrogen by reaction of lithium metal with water. How many grams of lithium would you need to prepare 455 mL of H2 if the density of hydrogen is 0.0893 g/L ... 

Lithium is the most difficult of the alkali metals with which to obtain stable solutions since it cannot be distilled in glass. Three runs were carried out with lithium and water, but the results are inconclusive. In the first run, lithium prepared by evaporating a lithium-ammonia solution was used, and in the other runs the lithium was cut in a dry box and introduced into the ethylenediamine just prior to the run by means of a break-seal sidearm. The first two runs appeared to yield three rate constants, with values around 100, 20, and 7 Af-1 sec.-1, respectively and involved both infrared and visible absorptions. In the third run, a very dilute solution showing no infrared absorbance was used and resulted in a single rate constant of about 30 Af-1 sec.-1, obtained by following the decay of the 660 m/z absorbance. 

Lithium shot or dispersion in liquid paraffin can be exposed to air during handling without deterioration. It may be transferred by pouring through a wide-necked funnel. Small quantities of the dispersion may be destroyed by washing with water to allow the lithium metal to react with water. Larger quantities should be suspended in ether and treated in a fume cupboard with dry t-butyl alcohol. Hydrogen is liberated in this reaction. 

There is no standard, universal, procedure for the Birch reduction. Experiment 7.19 illustrates some of the variants which have been reported in the literature. The original Birch procedure is to add small pieces of sodium metal to a solution of the aromatic compound in a mixture of liquid ammonia and the proton source (ethanol).18 After completion of the reaction, which is usually indicated by the disappearance of the blue colour, it is quenched by the addition of ammonium chloride and the ammonia allowed to evaporate before the cautious addition of water, and isolation of the product by ether extraction. In a modified procedure a co-solvent (ether, tetrahydrofuran, etc.) is initially added to the solution of aromatic compound/liquid ammonia prior to the addition of metal lithium metal is often used in place of sodium.19a,b In general these latter procedures are used for substrates which are more difficult to reduce. Redistilled liquid ammonia is found to be beneficial since the common contaminant iron, in collodial form or in the form of its salts, has a deleterious effect on the reaction.20 A representative selection of procedures is given in Expt 7.19 for the reduction of o-xylene, anisole, benzoic acid, and 3,4,5-trimethoxybenzoic acid. 

Lithium reacts with hydrogen to produce the hydride, LiH. Sometimes the product is contaminated with unreacted lithium metal. The extent of the contamination can be measured by measuring the amount of hydrogen gas generated by reacting a sample with water. 

A 0.205-g sample of contaminated LiH yielded 561 mL of gas measured over water at 22°C and a total pressure of 731 torr. Calculate the percent by weight of lithium metal in the sample. The vapor pressure of water at 22°C is 20 torr. 

The current primary method for production of lithium is by electrolysis. Spodumene, the most plentiful lithium bearing ore, is beneficiated to 3 to 5% Li20 and heated to 1000°C to convert it from its alpha form to its beta form. The beta form is treated with sulfuric acid to form Li2S04. The Li2S04 is water-soluble and is leached and reacted with sodium carbonate to form lithium carbonate. The lithium carbonate is then reacted with hydrochloric acid to form lithium chloride. Anhydrous lithium chloride is used to produce lithium metal by electrolysis (Austin 1984). 

Lithium metal precipitates at the cathode and causes a lag in base production due to slow reactivity towards water in the electrolyte. 

---