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==Preparation and structure== |
==Preparation and structure== |
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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 |
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 book | chapter = Ammonium Hexachloroplatinate(IV) | author = George B. Kauffman | title = Inorganic Syntheses | author-link = George B. Kauffman | year = 1967 | 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>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 crystallographic and thermogravimetric characterization" Materials Letters, 2003, volume 57, p 4667-4672. {{doi|10.1016/S0167-577X(03)00381-1}}</ref> |
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 crystallographic and thermogravimetric characterization" Materials Letters, 2003, volume 57, p 4667-4672. {{doi|10.1016/S0167-577X(03)00381-1}}</ref> |
Revision as of 13:52, 19 December 2021
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 |
EC Number |
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PubChem CID
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UNII | |
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) | |
Hazards | |
GHS labelling: | |
Danger | |
H290, H301, H317, H318, H334 | |
P234, P261, P264, P270, P272, P280, P285, P301+P310, P302+P352, P304+P341, P305+P351+P338, P310, P321, P330, P333+P313, P342+P311, P363, P390, P404, P405, P501 | |
Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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195 mg/kg rat |
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 H2[PtCl6].[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. Vol. 9. pp. 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 crystallographic and thermogravimetric characterization" Materials Letters, 2003, volume 57, p 4667-4672. doi:10.1016/S0167-577X(03)00381-1