Cobalt(III) hexammine chloride
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| Cobalt(III) hexammine chloride | |
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| General | |
| Systematic name | Hexammine cobalt(III) chloride |
| Other names | Cobalt hexammine chloride |
| Molecular formula | H18N6Cl3Co |
| SMILES | ? |
| Molar mass | 267.48 g/mol |
| Appearance | yellow crystals |
| CAS number | [10534-89-1] |
| Properties | |
| Density and phase | ? g/cm3, ? |
| Solubility in water | 0.26M (20 °C) tribromide: 0.04M (18 °C) |
| Other solvents | soluble in NH3 |
| Melting point | ? °C (? K) |
| Acidity (pKa) | ? |
| Structure | |
| Coordination geometry |
octahedral |
| Crystal structure | ? |
| Dipole moment | 0 D |
| Hazards | |
| MSDS | External MSDS |
| Main hazards | poison |
| NFPA 704 | |
| R/S statement | R: 36/37/38 S: none |
| RTECS number | ? |
| Supplementary data page | |
| Structure and properties |
n, εr, etc. |
| Thermodynamic data |
Phase behaviour Solid, liquid, gas |
| Spectral data | UV:475 (ε=58), 340 (ε=49) |
| Related compounds | |
| Other anions | [Co(NH3)6]Br3 [Co(NH3)6](OAc)3 |
| Other cations | [Cr(NH3)6]Cl3 [Ni(NH3)6]Cl2 |
| Related compounds | [Co(H2NCH2CH2NH2)3]Cl3 |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
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Cobalt(III) hexammine chloride is the chemical compound with the formula [Co(NH3)6]Cl3. This coordination compound is considered an archetypal "Werner complex", named after the pioneer of coordination chemistry, Alfred Werner. This salt consists of [Co(NH3)6]3+ tri[cation]]s with three Cl- anions. The term "ammine" is used for ammonia complexes of metal ions.
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[edit] Properties and structure
[Co(NH3)6]3+ is diamagnetic, with a low-spin octahedral Co(III) center. The cation obeys the 18-electron rule and is considered to be a classic example of an exchange inert metal complex. As a manifestation of its inertness, [Co(NH3)6]Cl3 can be recrystallized unchanged from concentrated hydrochloric acid: the NH3 is so tightly bound to the Co(III) centers that it does not dissociate to allow its protonation. In contrast, labile metal ammine complexes, such as [Ni(NH3)6]Cl2, react rapidly with acids due to the lability of the Ni(II)-NH3 bonds.
Upon heating, hexamminecobalt(III) begins to lose some of its ligands, and suddenly becomes a strong oxidant.
[Co(NH3)6]3+ is a moderately strong Bronsted acid.
The chlorides in [Co(NH3)6]Cl3 can be exchanged with a variety of other anions such as nitrate and bromide, and iodide to afford the corresponding [Co(NH3)6]X3 derivative. Such salts are bright yellow and display varying degrees of water solubility.
[edit] Preparation
Since CoCl3 is not available, [Co(NH3)6]Cl3 is prepared from cobalt(II) chloride. The latter is treated with ammonia and ammonium chloride followed by oxidation. Oxidants include hydrogen peroxide or oxygen in the presence of charcoal catalyst.[1] This salt appears to have been first reported by Fremy.[2]
The acetate salt can be prepared by aerobic oxidation of cobalt(II) acetate, ammonium acetate, and ammonia in methanol.[3] The acetate salt is highly water-soluble to the level of 1.9M (20 °C), vs. 0.26M for the trichloride.
[Co(NH3)6]3+ is a component of some protein crystallization methods to help solve their structures by X-ray crystallography.
[edit] References
- ^ Bjerrum, J.; McReynolds, J. P. "Hexamminecobalt(III) Salts" Inorganic Syntheses, 1978, volume XVIII, pages 216-221.
- ^ Fremy Ann. chim. phys., 1852, volume 35, page 257ff.
- ^ Lindholm, R. D. "Hexamminecobalt(III) Salts" Inorganic Syntheses, 1978, volume XVIII, pages 67-69.
