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The compound consists of separate [[tetrahedral molecular geometry|tetrahedral]] [[ammonium]] [[cation]]s and [[octahedral molecular geometry|octahedral]] [PtCl<sub>6</sub>]<sup>2−</sup> [[anion]]s. It is usually generated as a fine yellow precipitate by treating a solution of [[chloroplatinic acid|hexachloroplatinic acid]] with a solution of an ammonium salt.<ref name=Kauuf>{{cite journal | title = Ammonium Hexachloroplatinate(IV) | author = [[George B. Kauffman]] | year = 1967 | journal = [[Inorganic Syntheses]] | volume = 9 | pages = 182–185 | doi = 10.1002/9780470132401.ch51 | series = Inorganic Syntheses | isbn = 978-0-470-13240-1}}</ref> The complex is so poorly soluble that this step is employed in the isolation of platinum from ores and recycled residues.<ref>Cotton, S. A. ''Chemistry of Precious Metals'', Chapman and Hall (London): 1997. ISBN 0-7514-0413-6.</ref> |
The compound consists of separate [[tetrahedral molecular geometry|tetrahedral]] [[ammonium]] [[cation]]s and [[octahedral molecular geometry|octahedral]] [PtCl<sub>6</sub>]<sup>2−</sup> [[anion]]s. It is usually generated as a fine yellow precipitate by treating a solution of [[chloroplatinic acid|hexachloroplatinic acid]] with a solution of an ammonium salt.<ref name=Kauuf>{{cite journal | title = Ammonium Hexachloroplatinate(IV) | author = [[George B. Kauffman]] | year = 1967 | journal = [[Inorganic Syntheses]] | volume = 9 | pages = 182–185 | doi = 10.1002/9780470132401.ch51 | series = Inorganic Syntheses | isbn = 978-0-470-13240-1}}</ref> The complex is so poorly soluble that this step is employed in the isolation of platinum from ores and recycled residues.<ref>Cotton, S. A. ''Chemistry of Precious Metals'', Chapman and Hall (London): 1997. ISBN 0-7514-0413-6.</ref> |
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As analyzed by [[X-ray crystallography]], the salt crystallizes in a cubic motif reminiscent of the [[calcium fluoride|fluorite]] structure. The [PtCl<sub>6</sub>]<sup> |
As analyzed by [[X-ray crystallography]], the salt crystallizes in a cubic motif reminiscent of the [[calcium fluoride|fluorite]] structure. The [PtCl<sub>6</sub>]<sup>2−</sup> centers are octahedral. The NH<sub>4</sub><sup>+</sup> centers are [[hydrogen bond]]ed to the [[chloride]] [[ligands]].<ref>Verde-Gómez, Y.; Alonso-Nuñez, G.; Cervantes, F.; Keer, A. "Aqueous solution reaction to synthesize ammonium hexachloroplatinate and its crystallogrpahic and thermogravimetric characterization" Materials Letters, 2003, volume 57, p 4667-4672. {{doi|10.1016/S0167-577X(03)00381-1}}</ref> |
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==Uses and reactions== |
==Uses and reactions== |
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Revision as of 21:41, 20 February 2017
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| Names | |
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| IUPAC name
Ammonium hexachloroplatinate(IV)
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| Other names
ammonium chloroplatinate
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| Identifiers | |
3D model (JSmol)
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| ChEBI | |
| ChemSpider | |
| ECHA InfoCard | 100.037.233 |
CompTox Dashboard (EPA)
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| Properties | |
| (NH4)2PtCl6 | |
| Molar mass | 443.87 g/mol |
| Appearance | yellow crystals |
| Odor | odorless |
| Density | 3.065 g/cm3 |
| Melting point | 380 °C (716 °F; 653 K) decomposes |
| 0.289 g/100ml (0 °C) 0.7 g/100ml (15 °C)[1] 0.499 g/100ml (20 °C) 3.36 g/100ml (100 °C) | |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Ammonium hexachloroplatinate, also known as ammonium chloroplatinate, is the inorganic compound with the formula (NH4)2[PtCl6]. It is a rare example of a soluble platinum(IV) salt that is not hygroscopic. It forms intensely yellow solutions in water. In the presence of 1M NH4Cl, its solubility is only 0.0028 g/100 mL.
Preparation and structure
The compound consists of separate tetrahedral ammonium cations and octahedral [PtCl6]2− anions. It is usually generated as a fine yellow precipitate by treating a solution of hexachloroplatinic acid with a solution of an ammonium salt.[2] The complex is so poorly soluble that this step is employed in the isolation of platinum from ores and recycled residues.[3]
As analyzed by X-ray crystallography, the salt crystallizes in a cubic motif reminiscent of the fluorite structure. The [PtCl6]2− centers are octahedral. The NH4+ centers are hydrogen bonded to the chloride ligands.[4]
Uses and reactions
Ammonium hexachloroplatinate is used in platinum plating. Heating (NH4)2[PtCl6] under a stream of hydrogen at 200 °C produces platinum sponge. Treating this with chlorine gives H2PtCl6.[2]
References
- ^ "ammonium hexachloroplatinate(IV)". Chemister.ru. 2007-03-19. Retrieved 2014-06-03.
- ^ a b George B. Kauffman (1967). "Ammonium Hexachloroplatinate(IV)". Inorganic Syntheses. Inorganic Syntheses. 9: 182–185. doi:10.1002/9780470132401.ch51. ISBN 978-0-470-13240-1.
- ^ Cotton, S. A. Chemistry of Precious Metals, Chapman and Hall (London): 1997. ISBN 0-7514-0413-6.
- ^ Verde-Gómez, Y.; Alonso-Nuñez, G.; Cervantes, F.; Keer, A. "Aqueous solution reaction to synthesize ammonium hexachloroplatinate and its crystallogrpahic and thermogravimetric characterization" Materials Letters, 2003, volume 57, p 4667-4672. doi:10.1016/S0167-577X(03)00381-1