| |
| Names | |
|---|---|
| IUPAC name
(dioxo-λ5-stibanyl)oxy-dioxo-λ5-stibane
| |
| Other names
antimony(V) oxide
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| Identifiers | |
3D model (JSmol)
|
|
| ChemSpider | |
| ECHA InfoCard | 100.013.853 |
| EC Number |
|
PubChem CID
|
|
| UNII | |
CompTox Dashboard (EPA)
|
|
| |
| |
| Properties | |
| Sb2O5 | |
| Molar mass | 323.517 g/mol |
| Appearance | yellow, powdery solid |
| Density | 3.78 g/cm3, solid |
| Melting point | 380 °C (716 °F; 653 K) (decomposes) |
| 0.3 g/100 mL | |
| Solubility | insoluble in nitric acid |
| Structure | |
| cubic | |
| Thermochemistry | |
Heat capacity (C)
|
117.69 J/mol K |
Std enthalpy of
formation (ΔfH⦵298) |
–1008.18 kJ/mol |
| Hazards | |
| GHS labelling: | |
   
| |
| Danger | |
| H302, H315, H319, H335, H411 | |
| P261, P264, P270, P271, P273, P280, P301+P312, P302+P352, P304+P340, P305+P351+P338, P312, P321, P330, P332+P313, P337+P313, P362, P391, P403+P233, P405, P501 | |
| NFPA 704 (fire diamond) | |
| NIOSH (US health exposure limits): | |
PEL (Permissible)
|
TWA 0.5 mg/m3 (as Sb)[1] |
REL (Recommended)
|
TWA 0.5 mg/m3 (as Sb)[1] |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
| |
Antimony pentoxide (molecular formula: Sb2O5) is a chemical compound of antimony and oxygen. It contains antimony in the +5 oxidation state.
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Transcription
Structure
Antimony pentoxide has the same structure as the B form of niobium pentoxide and can be derived from the rutile structure, with antimony coordinated by six oxygen atoms in a distorted octahedral arrangement. The SbO6 octahedra are corner- and edge-sharing.[2]
 |
 |
|
| Sb coordination | edge sharing | corner sharing |
Preparation
The hydrated oxide is prepared by hydrolysis of antimony pentachloride; or by acidification of potassium hexahydroxoantimonate(V). It may also be prepared by oxidation of antimony trioxide with nitric acid.[3]
Uses
Antimony pentoxide finds use as a flame retardant in ABS and other plastics and as a flocculant in the production of titanium dioxide, and is sometimes used in the production of glass, paint and adhesives.[4][5]
It is also used as an ion exchange resin for a number of cations in acidic solution including Na+ (especially for their selective retentions), and as a polymerization and oxidation catalyst.
Properties and reactions
The hydrated oxide is insoluble in nitric acid, but dissolves in a concentrated potassium hydroxide solution to give potassium hexahydroxoantimonate(V), or KSb(OH)6.[6]
When heated to 700 °C (1,290 °F), the yellow hydrated pentoxide converts to an anhydrous white solid with the formula Sb6O13, containing both antimony(III) and antimony(V). Heating to 900 °C (1,650 °F) produces a white, insoluble powder of Sb2O4 in both α and β forms. The β form consists of antimony(V) in octahedral interstices and pyramidal SbIIIO4 units. In these compounds, the antimony(V) atom is octahedrally coordinated to six hydroxy groups.
The pentoxide can be reduced to antimony metal by heating with hydrogen or potassium cyanide.[7]
References
- ^ a b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
- ^ M. Jansen (March 1979). "Die Kristallstruktur von Antimon(V)-oxid". Acta Crystallogr. B. 35 (3): 539–542. Bibcode:1979AcCrB..35..539J. doi:10.1107/S056774087900409X.
- ^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
- ^ Bartlett, Jeffrey (1997-03-19). "Colloidal Antimony Pentoxide in Flame Retarded ABS". Nyacol Products, Inc. Archived from the original on 3 August 2006. Retrieved 2006-07-28.
- ^ "ANTIMONY PENTOXIDE". chemicalLAND21.com. Archived from the original on 27 August 2006. Retrieved 2006-07-28.
- ^ Pradyot Patnaik (2002). Handbook of Inorganic Chemicals. McGraw-Hill. p. 54. ISBN 0-07-049439-8.
- ^ "Antimony" in Handbook of Preparative Inorganic Chemistry, 2nd Ed. Edited by G. Brauer, Academic Press, 1963, NY. Vol. 1. p. 606.
This page was last edited on 21 January 2024, at 14:07