Английская Википедия:Iridium compounds
| Oxidation statesШаблон:Efn | |
|---|---|
| −3 | Шаблон:Chem |
| −1 | Шаблон:Chem2 |
| 0 | Шаблон:Chem2 |
| +1 | Шаблон:Chem2 |
| +2 | Шаблон:Chem2 |
| +3 | Шаблон:Chem2 |
| +4 | Шаблон:Chem2 |
| +5 | Шаблон:Chem2 |
| +6 | Шаблон:Chem |
| +7 | Шаблон:Chem2 |
| +8 | Шаблон:Chem2 |
| +9 | Шаблон:Chem2[1] |
Iridium compounds are compounds containing the element iridium (Ir). Iridium forms compounds in oxidation states between −3 and +9, but the most common oxidation states are +1, +2, +3, and +4.[2] Well-characterized compounds containing iridium in the +6 oxidation state include [[iridium(VI) fluoride|Шаблон:Chem2]] and the oxides Шаблон:Chem2 and Шаблон:Chem2.[2][3] iridium(VIII) oxide (Шаблон:Chem2) was generated under matrix isolation conditions at 6 K in argon.[4] The highest oxidation state (+9), which is also the highest recorded for any element, is found in gaseous Шаблон:Chem2.[1]
Oxides
Only one binary oxide is well-characterized: Iridium dioxide, Шаблон:Chem. It is a blue-black solid. The compound adopts the TiO2 rutile structure, featuring six coordinate iridium and three coordinate oxygen.[5] It adopts the fluorite structure.[2] A sesquioxide, Шаблон:Chem, has been described as a blue-black powder, which is oxidized to Шаблон:Chem by Шаблон:Chem.[6] The corresponding disulfides, diselenides, sesquisulfides, and sesquiselenides are known, as well as Шаблон:Chem.[2]
Another oxide, iridium tetroxide, is also known, with iridium in the +8 oxiation state.[7] This compound was formed by photochemical rearrangement of Шаблон:!((η1-O2)IrO2Шаблон:)! in solid argon at a temperature of Шаблон:Convert. At higher temperatures, the oxide is unstable.[8] The detection of the iridium tetroxide cation Шаблон:Chem by infrared photodissociation spectroscopy with formal oxidation state +9 has been reported, the highest currently known of any element, though the +10 oxidation state has been theorized for platinum, but not confirmed.[9][10]
Halides
Binary trihalides, Шаблон:Chem are known for all of the halogens.[2] For oxidation states +4 and above, only the tetrafluoride, pentafluoride and hexafluoride are known.[2] Iridium hexafluoride, Шаблон:Chem, is a volatile yellow solid, composed of octahedral molecules. It decomposes in water and is reduced to Шаблон:Chem,.[2] Iridium pentafluoride is also a strong oxidant, but it is a tetramer, Шаблон:Chem, formed by four corner-sharing octahedra.[2]
Complexes
The coordination complexes of iridium are extensive.
Iridium in its complexes is always low-spin. Ir(III) and Ir(IV) generally form octahedral complexes.[2] Polyhydride complexes are known for the +5 and +3 oxidation states.[11] One example is Шаблон:Chem2.[12] The ternary hydride Шаблон:Chem is believed to contain both the Шаблон:Chem and the 18-electron Шаблон:Chem anion.[13]
Iridium also oxyanions with oxidation states +4 and +5. Шаблон:Chem and Шаблон:Chem can be prepared from the reaction of potassium oxide or potassium superoxide with iridium at high temperatures. Such solids are not soluble in conventional solvents.[14]
As for many elements, the chlorides are key complexes. Hexachloroiridic(IV) acid, Шаблон:Chem, and its ammonium salt are the most common iridium compounds from an industrial and preparative perspectives.[15] They are intermediates in the purification of iridium and used as precursors for most other iridium compounds, as well as in the preparation of anode coatings. The Шаблон:Chem ion has an intense dark brown color, and can be readily reduced to the lighter-colored Шаблон:Chem and vice versa.[15] Iridium trichloride, Шаблон:Chem, which can be obtained in anhydrous form from direct oxidation of iridium powder by chlorine at 650 °C,[15] or in hydrated form by dissolving Шаблон:Chem in hydrochloric acid, is often used as a starting material for the synthesis of other Ir(III) compounds.[2] Another compound used as a starting material is ammonium hexachloroiridate(III), Шаблон:Chem.
In the presence of air, iridium metal dissolves in molten alkali-metal cyanides to produce the Шаблон:Chem (hexacyanoiridate) ion.
Oxyanions
Iridium forms oxyanions in the +4 oxidation state. It forms compounds such as lithium iridate (Li2IrO3), which forms black crystals with three slightly different layered atomic structures, α, β, and sometimes γ. Lithium iridate exhibits metal-like, temperature-independent electrical conductivity,[16] and changes its magnetic ordering from paramagnetic to antiferromagnetic upon cooling to 15 K.[17] Lithium iridate is a potential electrode material for the lithium-ion battery.[16] This application is hindered by the high costs of Ir, as compared to the cheaper Li2MnO3 alternative.[18]
Organoiridium chemistry
Organoiridium compounds contain iridium–carbon bonds. Early studies identified the very stable tetrairidium dodecacarbonyl, Шаблон:Chem.[2] In this compound, each of the iridium atoms is bonded to the other three, forming a tetrahedral cluster. The discovery of Vaska's complex (Шаблон:Chem) opened the door for oxidative addition reactions, a process fundamental to useful reactions. For example, Crabtree's catalyst, a homogeneous catalyst for hydrogenation reactions.[19][20] Iridium is usually supplied commercially in the Ir(III) and Ir(IV) oxidation states. Important starting reagents being hydrated iridium trichloride and ammonium hexachloroiridate. These salts are reduced upon treatment with CO, hydrogen, and alkenes. Illustrative is the carbonylation of the trichloride:
- IrCl3(H2O)x + 3 CO → [Ir(CO)2Cl2]− + CO2 + 2 H+ + Cl− + (x-1) H2O
Many organoiridium(III) compounds are generated from pentamethylcyclopentadienyl iridium dichloride dimer. Many of derivatives feature kinetically inert cyclometalated ligands.[23] Related half-sandwich complexes were central in the development of C-H activation.[24][25]
Iridium complexes played a pivotal role in the development of carbon–hydrogen bond activation (C–H activation), which promises to allow functionalization of hydrocarbons, which are traditionally regarded as unreactive.[26]
See also
Notes
References
- ↑ 1,0 1,1 Шаблон:Cite journal
- ↑ 2,00 2,01 2,02 2,03 2,04 2,05 2,06 2,07 2,08 2,09 2,10 Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Greenwood&Earnshaw
- ↑ Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ 15,0 15,1 15,2 Шаблон:Cite book
- ↑ 16,0 16,1 Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite book
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
- ↑ Шаблон:Cite journal
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