Antimony pentoxide
Names | |
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IUPAC name
(dioxo-
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Other names
antimony(V) oxide
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Identifiers | |
3D model (JSmol)
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ChemSpider | |
ECHA InfoCard | 100.013.853 |
EC Number |
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PubChem CID
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UNII | |
CompTox Dashboard (EPA)
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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)
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117.69 J/mol K |
Std enthalpy of
formation ( |
–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)
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TWA 0.5 mg/m3 (as Sb)[1] |
REL (Recommended)
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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).
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Antimony pentoxide (molecular formula: Sb2O5) is a chemical compound of antimony and oxygen. It contains antimony in the +5 oxidation state.
Structure[edit]
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[edit]
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[edit]
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[edit]
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
The pentoxide can be reduced to antimony metal by heating with hydrogen or potassium cyanide.[7]
References[edit]
- ^ 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.