Of iridium compounds

Synthesis. The principal starting material for synthesis of iridium compounds is iridium trichloride hydrate [14996-61-3], IrCl3-a H2 0. Another useful material for laboratory-scale reactions is [Ir20l2(cod)2] [12112-67-3]. 

Na,IrCl6 is a convenient starting material in the synthesis of iridium compounds. 

Review article Excellent source of information about Mossbauer spectroscopy of iridium compounds and alloys... 

The most common use of iridium coordination compounds remains in the catalysis field, although interest is developing in the luminescent properties of iridium compounds. The wide range of accessible oxidation states available to iridium (—1) to (VI) is reflected in the diverse nature of its coordination compounds. 

Other silicon derivatives containing Si—X—C bonds (where X is O and/or N) can be successfully prepared by using iridium-catalyzed reachons such as the asymmetric hydrosilylation of ketones and amines, the silylcarbonylation of alkenes, and the alcoholysis of Si—H bonds. Indeed, oxygenation of the latter bond to silanol also proceeds smoothly in the presence of iridium compounds. 

The elemental metal form of iridium is almost completely inert and does not oxidize at room temperatures. But, as with several of the other metals in the platinum group, several of iridiums compounds are toxic. The dust and powder should not be inhaled or ingested. 

Moreover, the already known abihty of iridium compounds to catalyze hydrogen transfer reactions has been excellently applied in Oppenauer-type and domino-type reactions for valuable organic chemicals and further developments, including asymmetric variants to kinetic resolution of alcohols and fine chemicals, can be expected. 

Ammonia forms complex derivatives with all three classes of iridium compounds. When added to iridious chloride, IrCl2, or to iridic chloride, IrCl4, the complex salts formed are analogous to the series of platinous and platinic ammine derivatives. When ammonia is added to the trichloride, many complex derivatives are formed which are similar to rhodic, cobaltic, and chromic compounds. For example, when ammonia acts upon ammonium iridiochloride a compound is produced having the formula [Cl(NHj)5lr]Cl2, and called chloro-pentammine-iridium dichloride. 

The majority of catalysts mentioned so far have been complexes of rhodium or of iridium. Compounds of the other member of this triad, cobalt, may also catalyse alkene isomerisation. A recent example is provided by the cluster compound [Co(CO)2(PRs)] the catalytically... 

As mentioned earlier, a number of iridium compounds have been shown to be effeetive catafysts for the methanol earbonylation reaction [11,13]. Nickel catalysts have also been found to be effective, partieularfy when used with compounds of Sn, Cr, Mo, or W [10c,15]. Heterogenized rhodium catalysts, prepared by supporting rhodium eompounds on a solid or by anehoring a rhodium eomplex to a polymer matrix, are also catalysts. However, none of these have been commercialized. In the latter case, the slow dissolution of rhodium is a major problem. 

The conditions employed for iridium-catalyzed carbonylation (ca. 180-190 °C, 20-40 bar) are comparable to those of the rhodium-based process. A variety of iridium compounds (e.g., I1CI3, IrU, H2I1CI6, Ir4(CO)i2) can be used as catalyst precursors, as conversion into the active iodocarbonyl species occurs rapidly under process conditions. In a working catalytic system, the principal solvent component is acetic acid, so the methanol feedstock is substantially converted into its acetate ester (Equation (2)). Methyl acetate is then activated by reaction with the iodide co-catalyst (Equation (3)). Catalytic carbonylation of methyl iodide formally gives acetyl iodide (Equation (4)) prior to rapid hydrolysis to the product acetic acid (Equation (5)). However, it is difficult to establish the true intermediacy of acetyl... 

The most common oxidation states, corresponding electronic configurations, and coordination geometries of iridium are +1 (t5 ) usually square plane although some five-coordinate complexes are known, and +3 (t7 ) and +4 (t5 ), both octahedral. Compounds ia every oxidation state between —1 and +6 (<5 ) are known. Iridium compounds are used primarily to model more active rhodium catalysts. 

Binary Compounds. The fluorides of indium are IrF [23370-59-4] IrF [37501-24-9] the tetrameric pentafluoride (IiF ) [14568-19-5], and JIrFg [7789-75-7]. Chlorides of indium include IrCl, which exists in anhydrous [10025-83-9] a- and p-forms, and as a soluble hydrate [14996-61-3], and IrCl [10025-97-5], Other haUdes include IrBr [10049-24-8], which is insoluble, and the soluble tetrahydrate IrBr -4H20 IrBr [7789-64-2]-, and Irl [7790-41-2], Iridium forms indium dioxide [12030-49-8], a poorly characteri2ed sesquioxide, 11203 [1312-46-5]-, and the hydroxides, Ir(OH)3 [54968-01-3] and Ir(OH) [25141-14-4], Other binary iridium compounds include the sulfides, IrS [12136-40-2], F2S3 [12136-42-4], IrS2 [12030-51 -2], and IrS3 [12030-52-3], as well as various selenides and teUurides. 

Ca.ta.lysis, Iridium compounds do not have industrial appHcations as catalysts. However, these compounds have been studied to model fundamental catalytic steps (174), such as substrate binding of unsaturated molecules and dioxygen oxidative addition of hydrogen, alkyl haHdes, and the carbon—hydrogen bond reductive elimination and important metal-centered transformations such as carbonylation, -elimination, CO reduction, and... 

L = P(CH3)3 or CO, oxidatively add arene and alkane carbon—hydrogen bonds (181,182). Catalytic dehydrogenation of alkanes (183) and carbonylation of bensene (184) has also been observed. Iridium compounds have also been shown to catalyse hydrogenation (185) and isomerisation of unsaturated alkanes (186), hydrogen-transfer reactions, and enantioselective hydrogenation of ketones (187) and imines (188). 

The voltammograms of complex compounds of iridium with azodye appears considerably more clear separate than in the case of tritane dyes, but a sensitivity and selectivity of this method is considerably less. 

Table 26.2 Oxidation states and stereochemistries of some compounds of cobalt, rhodium and iridium...

Reaction of the cyclopentadienyl rhodium and iridium tris(acetone) complexes with indole leads to the species 118 (M = Rh, Ir) [77JCS(D)1654 79JCS(D)1531]. None of these compounds deprotonates easily in acetone, but the iridium complex loses a proton in reaction with bases (Na2C03 in water, r-BuOK in acetone) to form the ri -indolyl complex 119. This reaction is easily reversed in the presence of small amounts of trifluoroacetic acid. 

In synthesis (b), the initial product is a 5-coordinate (sp) iridium(III) hydride complex, which is rapidly oxidized in solution to the planar iridium(II) complex. Both of the compounds are paramagnetic with one unpaired electron, as expected for square planar d7 complexes. 

M(NO)2(PPh3)2]+. The coordination number of the metal in both is four, in a distorted tetrahedral geometry. The position of i/(N—O) in the IR spectrum is essentially the same, and the rhodium and iridium compounds have similar slight bending of the M—N—O linkage. 

M(NO)(OCOCF3)2(PPh3)2. Both these complexes have 5-coordinate geometries with monodentate carboxylates. The rhodium compound has a square pyramidal structure with bent Rh-N-O (122°) but the iridium compound has a tbp structure with straight equatorial Ir-N—O (178°). The position of i/(N—O) reflects this difference (1800 cm-1 (Ir) and 1665 cm-1 (Rh)). 

The trimesityl of iridium can be made by reaction of IrCl3(tht)3 with MesMgBr, while IrMes4 can be oxidized to the cationic iridium(V) species [IrMes4]+, also tetrahedral (with concomitant slight Ir-C bond changes from 1.99-2.04 A in the neutral compound to 2.004-2.037 A in the cation). Another iridium(V) species, IrO(Mes)3 has been made [190], it has a tetrahedral structure (lr=0 1.725 A). 

An unusual variation in kinetics and mechanisms of decomposition with temperature of the compound dioxygencarbonyl chloro-bis(triphenyl-phosphine) iridium(I) has been reported by Ball [1287]. In the lowest temperature range, 379—397 K, a nucleation and growth process was described by the Avrami—Erofe ev equation [eqn. (6), n = 2]. Between 405 and 425 K, data fitted the contracting area expression [eqn. (7), n = 2], indicative of phase boundary control. At higher temperatures, 426— 443 K, diffusion control was indicated by obedience to eqn. (13). The... 

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