Antimony trioxide: Difference between revisions

Antimony(III) oxide
Names
	IUPAC name Antimony(III) oxide
	Other names Antimony sesquioxide; Antimonous oxide; Flowers of Antimony
Identifiers
CAS Number	1309-64-4 ;
3D model (JSmol)	Interactive image;
ChemSpider	25727 ;
ECHA InfoCard	100.013.796
EC Number	215-474-6;
KEGG	C19192 ;
PubChem CID	14794;
RTECS number	CC5650000;
UNII	P217481X5E ;
CompTox Dashboard (EPA)	DTXSID4023880 ;
	InChI InChI=1S/3O.2Sb Key: ADCOVFLJGNWWNZ-UHFFFAOYSA-N ; InChI=1/3O.2Sb/rO3Sb2/c1-4-3-5-2 Key: ADCOVFLJGNWWNZ-VTKDZCJOAA;
	SMILES O=[Sb]O[Sb]=O;
Properties
Chemical formula	Sb2O3
Molar mass	291.518 g/mol
Appearance	white solid
Odor	odorless
Density	5.2 g/cm3, α-form ; 5.67 g/cm3 β-form
Melting point	656 °C (1,213 °F; 929 K)
Boiling point	1,425 °C (2,597 °F; 1,698 K) (sublimes)
Solubility in water	370±37 μg/L between 20.8 °C and 22.9 °C
Solubility	soluble in acid
Magnetic susceptibility (χ)	−69.4×10−6 cm3/mol
Refractive index (nD)	2.087, α-form ; 2.35, β-form
Structure
Crystal structure	cubic (α) < 570 °C; orthorhombic (β) > 570 °C
Coordination geometry	pyramidal
Dipole moment	zero
Hazards
	GHS labelling:
Pictograms
Signal word	Warning
Hazard statements	H351
Precautionary statements	P281
NFPA 704 (fire diamond)	2 0 0
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	7000 mg/kg, oral (rat)
	NIOSH (US health exposure limits):
PEL (Permissible)	TWA 0.5 mg/m3 (as Sb)
REL (Recommended)	TWA 0.5 mg/m3 (as Sb)
Related compounds
Other anions	Antimony trisulfide; Antimony triselenide; Antimony telluride
Other cations	Dinitrogen trioxide; Phosphorus trioxide; Arsenic trioxide; Bismuth trioxide
Related compounds	Diantimony tetraoxide; Antimony pentoxide
Supplementary data page
	Antimony trioxide (data page)
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). verify (what is ?) Infobox references

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Antimony(III) oxide is the inorganic compound with the formula Sb₂O₃. It is the most important commercial compound of antimony. It is found in nature as the minerals valentinite and senarmontite.^[3] Like most polymeric oxides, Sb₂O₃ dissolves in aqueous solutions with hydrolysis. A mixed arsenic-antimony oxide occurs in nature as the very rare mineral stibioclaudetite.^[4]^[5]

Production and properties

Global production of antimony(III) oxide in 2012 was 130,000 tonnes, an increase from 112,600 tonnes in 2002. China produces the largest share followed by US/Mexico, Europe, Japan and South Africa and other countries (2%).^[6]

As of 2010, antimony(III) oxide was produced at four sites in the EU. It is produced via two routes, re-volatilizing of crude antimony(III) oxide and by oxidation of antimony metal. Oxidation of antimony metal dominates in Europe. Several processes for the production of crude antimony(III) oxide or metallic antimony from virgin material. The choice of process depends on the composition of the ore and other factors. Typical steps include mining, crushing and grinding of ore, sometimes followed by froth flotation and separation of the metal using pyrometallurgical processes (smelting or roasting) or in a few cases (e.g. when the ore is rich in precious metals) by hydrometallurgical processes. These steps do not take place in the EU but closer to the mining location.

Re-volatilizing of crude antimony(III) oxide

Step 1) Crude stibnite is oxidized to crude antimony(III) oxide using furnaces operating at approximately 500 to 1,000 °C. The reaction is the following:

2 Sb₂S₃ + 9 O₂ → 2 Sb₂O₃ + 6 SO₂

Step 2) The crude antimony(III) oxide is purified by sublimation.

Oxidation of antimony metal

Antimony metal is oxidized to antimony(III) oxide in furnaces. The reaction is exothermic. Antimony(III) oxide is formed through sublimation and recovered in bag filters. The size of the formed particles is controlled by process conditions in furnace and gas flow. The reaction can be schematically described by:

4 Sb + 3 O₂ → 2 Sb₂O₃

Properties

Antimony(III) oxide is an amphoteric oxide. It dissolves in aqueous sodium hydroxide solution to give the meta-antimonite NaSbO₂, which can be isolated as the trihydrate. Antimony(III) oxide also dissolves in concentrated mineral acids to give the corresponding salts, which hydrolyzes upon dilution with water.^[7] With nitric acid, the trioxide is oxidized to antimony(V) oxide.^[8]

When heated with carbon, the oxide is reduced to antimony metal. With other reducing agents such as sodium borohydride or lithium aluminium hydride, the unstable and very toxic gas stibine is produced.^[9] When heated with potassium bitartrate, a complex salt potassium antimony tartrate, KSb(OH)₂·C₄H₂O₆, is formed.^[8]

Structure

The structure of Sb₂O₃ depends on the temperature of the sample. Dimeric Sb₄O₆ is the high temperature (1560 °C) gas.^[10] Sb₄O₆ molecules are bicyclic cages, similar to the related oxide of phosphorus(III), phosphorus trioxide.^[11] The cage structure is retained in a solid that crystallizes in a cubic habit. The Sb–O distance is 197.7 pm and the O–Sb–O angle of 95.6°.^[12] This form exists in nature as the mineral senarmontite.^[11] Above 606 °C, the more stable form is orthorhombic, consisting of pairs of -Sb-O-Sb-O- chains that are linked by oxide bridges between the Sb centers. This form exists in nature as the mineral valentinite.^[11]


Sb₄O₆	senarmontite	valentinite

Uses

The annual consumption of antimony(III) oxide in the United States and Europe is approximately 10,000 and 25,000 tonnes, respectively. The main application is as flame retardant synergist in combination with halogenated materials. The combination of the halides and the antimony is key to the flame-retardant action for polymers, helping to form less flammable chars. Such flame retardants are found in electrical apparatuses, textiles, leather, and coatings.^[13]

Other applications:

Antimony(III) oxide is an opacifying agent for glasses, ceramics and enamels.
Some specialty pigments contain antimony.
Antimony(III) oxide is a useful catalyst in the production of polyethylene terephthalate (PET plastic) and the vulcanization of rubber.

Safety

Antimony(III) oxide has suspected carcinogenic potential for humans.^[13] Its TLV is 0.5 mg/m³, as for most antimony compounds.^[14] Before 2021, no other human health hazards were identified for antimony(III) oxide, and no risks to human health and the environment were identified from the production and use of antimony trioxide in daily life. However, the 15th Report on Carcinogens released on December 21, 2021, by the US Department of Health and Human Services categorised antimony(III) oxide as carcinogenic.^[15]

References

^ ^a ^b ^c ^d Record of Antimony trioxide in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 23 August 2017.
^ ^a ^b NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).
^ Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.
^ "Stibioclaudetite".
^ "List of Minerals". 21 March 2011.
^ European Union Risk Assessment Report: DIANTIMONY TRIOXIDE (draft) (PDF) (Report). Sweden. November 2008. CAS No: 1309-64-4; EINECS No: 215-175-0. Archived from the original (PDF) on 2014-01-06.
^ Housecroft, C. E.; Sharpe, A. G. (2008). "Chapter 15: The group 15 elements". Inorganic Chemistry (3rd ed.). Pearson. p. 481. ISBN 978-0-13-175553-6.
^ ^a ^b Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. p. 56. ISBN 0-07-049439-8.
^ Bellama, J. M.; MacDiarmid, A. G. (1968). "Synthesis of the Hydrides of Germanium, Phosphorus, Arsenic, and Antimony by the Solid-Phase Reaction of the Corresponding Oxide with Lithium Aluminum Hydride". Inorganic Chemistry. 7 (10): 2070–2072. doi:10.1021/ic50068a024.
^ Wiberg, E.; Holleman, A. F. (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5.
^ ^a ^b ^c Wells, A. F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 0-19-855370-6.
^ Svensson, C. (1975). "Refinement of the crystal structure of cubic antimony(III) oxide, Sb₂O₃". Acta Crystallographica B. 31 (8): 2016–2018. doi:10.1107/S0567740875006759.
^ ^a ^b Grund, S. C.; Hanusch, K.; Breunig, H. J.; Wolf, H. U. "Antimony and Antimony Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_055.pub2. ISBN 978-3527306732.
^ Newton, P. E.; Schroeder, R. E.; Zwick, L.; Serex, T. (2004). "Inhalation Developmental Toxicity Studies In Rats With Antimony(III) oxide (Sb₂O₃)". Toxicologist. 78 (1–S): 38.
^ "15th Report on Carcinogens". National Toxicology Program. Retrieved 2023-06-15.

External links

[GESTIS-1] Record of Antimony trioxide in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 23 August 2017.

[PGCH-2] NIOSH Pocket Guide to Chemical Hazards. "#0036". National Institute for Occupational Safety and Health (NIOSH).

[3] Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. ISBN 0-7506-3365-4.

[4] "Stibioclaudetite".

[5] "List of Minerals". 21 March 2011.

[6] European Union Risk Assessment Report: DIANTIMONY TRIOXIDE (draft) (PDF) (Report). Sweden. November 2008. CAS No: 1309-64-4; EINECS No: 215-175-0. Archived from the original (PDF) on 2014-01-06.

[InorgChem-7] Housecroft, C. E.; Sharpe, A. G. (2008). "Chapter 15: The group 15 elements". Inorganic Chemistry (3rd ed.). Pearson. p. 481. ISBN 978-0-13-175553-6.

[Handbook-8] Patnaik, P. (2002). Handbook of Inorganic Chemicals. McGraw-Hill. p. 56. ISBN 0-07-049439-8.

[9] Bellama, J. M.; MacDiarmid, A. G. (1968). "Synthesis of the Hydrides of Germanium, Phosphorus, Arsenic, and Antimony by the Solid-Phase Reaction of the Corresponding Oxide with Lithium Aluminum Hydride". Inorganic Chemistry. 7 (10): 2070–2072. doi:10.1021/ic50068a024.

[Wiberg&Holleman-10] Wiberg, E.; Holleman, A. F. (2001). Inorganic Chemistry. Elsevier. ISBN 0-12-352651-5.

[Wells-11] Wells, A. F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 0-19-855370-6.

[12] Svensson, C. (1975). "Refinement of the crystal structure of cubic antimony(III) oxide, Sb₂O₃". Acta Crystallographica B. 31 (8): 2016–2018. doi:10.1107/S0567740875006759.

[Ullmann-13] Grund, S. C.; Hanusch, K.; Breunig, H. J.; Wolf, H. U. "Antimony and Antimony Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. doi:10.1002/14356007.a03_055.pub2. ISBN 978-3527306732.

[14] Newton, P. E.; Schroeder, R. E.; Zwick, L.; Serex, T. (2004). "Inhalation Developmental Toxicity Studies In Rats With Antimony(III) oxide (Sb₂O₃)". Toxicologist. 78 (1–S): 38.

[15] "15th Report on Carcinogens". National Toxicology Program. Retrieved 2023-06-15.

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@@ Line 25: / Line 25: @@
 | KEGG_Ref = {{keggcite|correct|kegg}}
 | KEGG = C19192
+| PubChem = 14794
+| EC_number = 215-474-6
   }}
 |Section2={{Chembox Properties
@@ Line 32: / Line 34: @@
 | Odor = odorless
 | Density = 5.2 g/cm<sup>3</sup>, α-form <br> 5.67 g/cm<sup>3</sup> β-form
-| Solubility = Dissolved concentration of 370 ± 37 µg/L was obtained with a loading of 10 mg/L after 7 days of exposure. Temperature varied between 20.8°C (t=0; start of the test) and 22.9°C
+| Solubility = {{val|370|37}} μg/L between 20.8&nbsp;°C and 22.9&nbsp;°C
 | SolubleOther = soluble in acid
 | MeltingPtC = 656
@@ Line 39: / Line 41: @@
 | pKa =
 | RefractIndex = 2.087, α-form <br> 2.35, β-form
-| MagSus = -69.4·10<sup>−6</sup> cm<sup>3</sup>/mol
+| MagSus = {{val|-69.4e-6|u=cm<sup>3</sup>/mol}}
   }}
 |Section3={{Chembox Structure
 | Coordination = pyramidal
-| CrystalStruct = [[Cubic crystal system|cubic]] (α)<570 °C<br />[[orthorhombic]] (β) >570 °C
+| CrystalStruct = [[Cubic crystal system|cubic]] (α) <&nbsp;570&nbsp;°C<br />[[orthorhombic]] (β) >&nbsp;570&nbsp;°C
 | Dipole = zero
   }}
 |Section7={{Chembox Hazards
 | ExternalSDS =
-| EUClass = Harmful ('''Xn''')<br />Carc. Cat. 2 (H351)
 | NFPA-H = 2
 | NFPA-F = 0
 | NFPA-R = 0
+| GHSPictograms = {{GHS08}}<ref name="GESTIS">{{GESTIS|Name=Antimony trioxide|ZVG=3440|CAS=1309-64-4|Date=23 August 2017}}</ref>
-| RPhrases = {{R40}}
+| GHSSignalWord = Warning<ref name="GESTIS" />
-| SPhrases = {{S2}}, {{S22}}, {{S36/37}}
+| HPhrases = {{H-phrases|351}}<ref name="GESTIS" />
+| PPhrases = {{P-phrases|281}}<ref name="GESTIS" />
 | LD50 = 7000 mg/kg, oral (rat)
 | REL = TWA 0.5 mg/m<sup>3</sup> (as Sb)<ref name=PGCH>{{PGCH|0036}}</ref>
@@ Line 59: / Line 62: @@
   }}
 |Section8={{Chembox Related
-| OtherAnions = [[Antimony trisulfide]]
+| OtherAnions = [[Antimony trisulfide]]<br>[[Antimony triselenide]]<br>[[Antimony telluride]]
-| OtherCations = [[Bismuth trioxide]]
+| OtherCations = [[Dinitrogen trioxide]]<br>[[Phosphorus trioxide]]<br>[[Arsenic trioxide]]<br>[[Bismuth trioxide]]
 | OtherCompounds = [[Diantimony tetraoxide]]<br />[[Antimony pentoxide]]
   }}
 }}
-'''Antimony(III) oxide''' is the [[inorganic compound]] with the [[Chemical formula|formula]] Sb<sub>2</sub>O<sub>3</sub>.  It is the most important commercial compound of [[antimony]].  It is found in nature as the minerals [[valentinite]] and [[senarmontite]].<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref>  Like most polymeric [[oxide]]s, Sb<sub>2</sub>O<sub>3</sub> dissolves in aqueous solutions with [[hydrolysis]].
+'''Antimony(III) oxide''' is the [[inorganic compound]] with the [[Chemical formula|formula]] Sb<sub>2</sub>O<sub>3</sub>.  It is the most important commercial compound of [[antimony]].  It is found in nature as the minerals [[valentinite]] and senarmontite.<ref>Greenwood, N. N.; & Earnshaw, A. (1997). Chemistry of the Elements (2nd Edn.), Oxford:Butterworth-Heinemann. {{ISBN|0-7506-3365-4}}.</ref>  Like most polymeric [[oxide]]s, Sb<sub>2</sub>O<sub>3</sub> dissolves in aqueous solutions with [[hydrolysis]]. A mixed arsenic-antimony oxide occurs in nature as the very rare mineral stibioclaudetite.<ref>{{Cite web|url=https://www.mindat.org/min-32285.html|title = Stibioclaudetite}}</ref><ref>{{Cite web|url=https://www.ima-mineralogy.org/Minlist.htm|title=List of Minerals|date=21 March 2011}}</ref>
 ==Production and properties==
-Global production of antimony(III) oxide  in 2012 was 130,000 tonnes, an increase from 112,600 tonnes in 2002.  China produces the largest share followed by US/Mexico, Europe, Japan  and South Africa  and other countries (2%).<ref>{{cite web|url=http://esis.jrc.ec.europa.eu/doc/risk_assessment/REPORT/datreport415.pdf |title=Archived copy |accessdate=2014-01-06 |deadurl=yes |archiveurl=https://web.archive.org/web/20140106155610/http://esis.jrc.ec.europa.eu/doc/risk_assessment/REPORT/datreport415.pdf |archivedate=2014-01-06 |df= }}</ref>
+Global production of antimony(III) oxide  in 2012 was 130,000 tonnes, an increase from 112,600 tonnes in 2002. China produces the largest share followed by US/Mexico, Europe, Japan and South Africa and other countries (2%).<ref>{{cite report|url=http://esis.jrc.ec.europa.eu/doc/risk_assessment/REPORT/datreport415.pdf |title=European Union Risk Assessment Report: DIANTIMONY TRIOXIDE (draft)|date=November 2008|location=Sweden|id=CAS No: 1309-64-4; EINECS No: 215-175-0|url-status=dead |archive-url=https://web.archive.org/web/20140106155610/http://esis.jrc.ec.europa.eu/doc/risk_assessment/REPORT/datreport415.pdf |archive-date=2014-01-06 }}</ref>
-As of 2010, antimony(III) oxide was produced at four sites in EU27. It is produced via two routes, re-volatilizing of crude antimony(III) oxide and by oxidation of antimony metal.
+As of 2010, antimony(III) oxide was produced at four sites in the EU. It is produced via two routes, re-volatilizing of crude antimony(III) oxide and by oxidation of antimony metal.
 Oxidation of antimony metal dominates in Europe. Several processes for the production of crude antimony(III) oxide or metallic antimony from virgin material. The choice of process depends on the composition of the ore and other factors.  Typical steps include mining, crushing and grinding of ore, sometimes followed by [[froth flotation]] and separation of the metal using pyrometallurgical processes (smelting or roasting) or in a few cases (e.g. when the ore is rich in precious metals) by hydrometallurgical processes. These steps do not take place in the EU but closer to the mining location.
 ===Re-volatilizing of crude antimony(III) oxide===
 Step 1) Crude stibnite is oxidized to crude antimony(III) oxide using furnaces operating at approximately 500 to 1,000&nbsp;°C. The reaction is the following:
-:2 Sb<sub>2</sub>S<sub>3</sub>  +  9 O<sub>2</sub>  →   2 Sb<sub>2</sub>O<sub>3</sub>  +  6 SO<sub>2</sub>
+:2&nbsp;Sb<sub>2</sub>S<sub>3</sub>  +  9&nbsp;O<sub>2</sub>  →   2&nbsp;Sb<sub>2</sub>O<sub>3</sub>  +  6&nbsp;SO<sub>2</sub>
 Step 2) The crude antimony(III) oxide is purified by sublimation.
 ===Oxidation of antimony metal===
-Antimony metal is oxidized to antimony(III) oxide in furnaces. The reaction is exothermic. Antimony(III) oxide is formed through sublimation and recovered in bag filters (bag house). The size of the formed particles is controlled by process conditions in furnace and gas flow.  The reaction can be schematically described by:<br />
+Antimony metal is oxidized to antimony(III) oxide in furnaces. The reaction is exothermic. Antimony(III) oxide is formed through sublimation and recovered in bag filters. The size of the formed particles is controlled by process conditions in furnace and gas flow.  The reaction can be schematically described by:
-:4 Sb  +  3 O<sub>2</sub>   →   2 Sb<sub>2</sub>O<sub>3</sub>
+:4&nbsp;Sb  +  3&nbsp;O<sub>2</sub>   →   2&nbsp;Sb<sub>2</sub>O<sub>3</sub>
 ===Properties===
-Antimony(III) oxide is an [[amphoteric oxide]], it dissolves in aqueous [[sodium hydroxide]] solution to give the meta-antimonite NaSbO<sub>2</sub>, which can be isolated as the trihydrate. Antimony(III) oxide also dissolves in concentrated [[mineral acids]] to give the corresponding salts, which hydrolyzes upon dilution with water.<ref name="InorgChem">{{cite book | title = Inorganic Chemistry | edition = 3rd | chapter = Chapter 15: The group 15 elements | author1 = Housecroft, C. E. | author2 = Sharpe, A. G. | publisher = Pearson | year = 2008 | isbn = 978-0-13-175553-6 | page = 481 }}</ref> With [[nitric acid]], the trioxide is oxidized to [[antimony(V) oxide]].<ref name="Handbook">{{cite book | title = Handbook of Inorganic Chemicals | author = Patnaik, P. | publisher = McGraw-Hill | year = 2002 | isbn = 0-07-049439-8 | page = 56 }}</ref>
+Antimony(III) oxide is an [[amphoteric oxide]]. It dissolves in aqueous [[sodium hydroxide]] solution to give the meta-antimonite NaSbO<sub>2</sub>, which can be isolated as the trihydrate. Antimony(III) oxide also dissolves in concentrated [[mineral acids]] to give the corresponding salts, which hydrolyzes upon dilution with water.<ref name="InorgChem">{{cite book | title = Inorganic Chemistry | edition = 3rd | chapter = Chapter 15: The group 15 elements | author1 = Housecroft, C. E. | author2 = Sharpe, A. G. | publisher = Pearson | year = 2008 | isbn = 978-0-13-175553-6 | page = 481 }}</ref> With [[nitric acid]], the trioxide is oxidized to [[antimony(V) oxide]].<ref name="Handbook">{{cite book | title = Handbook of Inorganic Chemicals | author = Patnaik, P. | publisher = McGraw-Hill | year = 2002 | isbn = 0-07-049439-8 | page = 56 }}</ref>
-When heated with [[carbon]], the oxide is reduced to [[antimony]] metal. With other reducing agents such as [[sodium borohydride]] or [[lithium aluminium hydride]], the unstable and very toxic gas [[stibine]] is produced.<ref>{{ cite journal |author1=Bellama, J. M. |author2=MacDiarmid, A. G. | title = Synthesis of the Hydrides of Germanium, Phosphorus, Arsenic, and Antimony by the Solid-Phase Reaction of the Corresponding Oxide with Lithium Aluminum Hydride |journal = [[Inorganic Chemistry (journal)|Inorganic Chemistry]] | year = 1968 | volume = 7 | issue = 10 | pages = 2070–2072 | doi = 10.1021/ic50068a024 }}</ref> When heated with [[potassium bitartrate]], a complex salt potassium antimony tartrate, KSb(OH)<sub>2</sub>•C<sub>4</sub>H<sub>2</sub>O<sub>6</sub> is formed.<ref name="Handbook" />
+When heated with [[carbon]], the oxide is reduced to [[antimony]] metal. With other reducing agents such as [[sodium borohydride]] or [[lithium aluminium hydride]], the unstable and very toxic gas [[stibine]] is produced.<ref>{{ cite journal |author1=Bellama, J. M. |author2=MacDiarmid, A. G. | title = Synthesis of the Hydrides of Germanium, Phosphorus, Arsenic, and Antimony by the Solid-Phase Reaction of the Corresponding Oxide with Lithium Aluminum Hydride |journal = [[Inorganic Chemistry (journal)|Inorganic Chemistry]] | year = 1968 | volume = 7 | issue = 10 | pages = 2070–2072 | doi = 10.1021/ic50068a024 }}</ref> When heated with [[potassium bitartrate]], a complex salt [[potassium antimony tartrate]], KSb(OH)<sub>2</sub>·C<sub>4</sub>H<sub>2</sub>O<sub>6</sub>, is formed.<ref name="Handbook" />
 ==Structure==
-The structure of Sb<sub>2</sub>O<sub>3</sub> depends on the temperature of the sample.  Dimeric Sb<sub>4</sub>O<sub>6</sub> is the high temperature  (1560&nbsp;°C<!--seems high-->) gas.<ref name ="Wiberg&Holleman">{{ cite book |author1=Wiberg, E. |author2=Holleman, A. F. | year = 2001 | title = Inorganic Chemistry | publisher = Elsevier | isbn = 0-12-352651-5 }}</ref>  Sb<sub>4</sub>O<sub>6</sub> molecules are bicyclic cages, similar to the related oxide of phosphorus(III), [[phosphorus trioxide]].<ref name = "Wells">{{ cite book | author = Wells, A. F. | year = 1984 | title = Structural Inorganic Chemistry | location = Oxford | publisher = Clarendon Press | isbn = 0-19-855370-6 }}</ref>  The cage structure is retained in a solid that crystallizes in a cubic habit.  The Sb-O distance is 197.7 pm and the O-Sb-O angle of 95.6°.<ref>{{ cite journal | author = Svensson, C. | title = Refinement of the crystal structure of cubic antimony(III) oxide, Sb<sub>2</sub>O<sub>3</sub> | journal = Acta Crystallographica B | year = 1975 | volume = 31 | issue = 8 | pages = 2016–2018 | doi = 10.1107/S0567740875006759 }}</ref>  This form exists in nature as the [[mineral]] [[senarmontite]].<ref name = "Wells"/> Above 606&nbsp;°C, the more stable form is [[orthorhombic]], consisting of pairs -Sb-O-Sb-O- chains that are linked by oxide bridges between the Sb centers.  This form exists in nature as the mineral [[valentinite]].<ref name = "Wells"/>
+The structure of Sb<sub>2</sub>O<sub>3</sub> depends on the temperature of the sample.  Dimeric Sb<sub>4</sub>O<sub>6</sub> is the high temperature  (1560&nbsp;°C<!--seems high-->) gas.<ref name ="Wiberg&Holleman">{{ cite book |author1=Wiberg, E. |author2=Holleman, A. F. | year = 2001 | title = Inorganic Chemistry | publisher = Elsevier | isbn = 0-12-352651-5 }}</ref>  Sb<sub>4</sub>O<sub>6</sub> molecules are bicyclic cages, similar to the related oxide of phosphorus(III), [[phosphorus trioxide]].<ref name = "Wells">{{ cite book | author = Wells, A. F. | year = 1984 | title = Structural Inorganic Chemistry | location = Oxford | publisher = Clarendon Press | isbn = 0-19-855370-6 }}</ref>  The cage structure is retained in a solid that crystallizes in a cubic habit.  The Sb–O distance is 197.7&nbsp;pm and the O–Sb–O angle of 95.6°.<ref>{{ cite journal | author = Svensson, C. | title = Refinement of the crystal structure of cubic antimony(III) oxide, Sb<sub>2</sub>O<sub>3</sub> | journal = Acta Crystallographica B | year = 1975 | volume = 31 | issue = 8 | pages = 2016–2018 | doi = 10.1107/S0567740875006759 | doi-access =  }}</ref>  This form exists in nature as the [[mineral]] [[senarmontite]].<ref name = "Wells"/> Above 606&nbsp;°C, the more stable form is [[orthorhombic]], consisting of pairs of -Sb-O-Sb-O- chains that are linked by oxide bridges between the Sb centers.  This form exists in nature as the mineral [[valentinite]].<ref name = "Wells"/>
+{| class="wikitable" style="margin:1em auto; text-align:center;"
-<center>
+|[[File:Sb4O6-molecule-from-senarmontite-xtal-2004-3D-balls-B.png|100px]]||[[File:Antimony(III)-oxide-senarmontite-xtal-2004-3D-balls.png|200px]]||[[File:Antimony(III)-oxide-valentinite-xtal-2004-3D-balls.png|220px]]
-{|align="center"  class="wikitable"
-|<center>[[File:Sb4O6-molecule-from-senarmontite-xtal-2004-3D-balls-B.png|100px]]</center>||<center>[[File:Antimony(III)-oxide-senarmontite-xtal-2004-3D-balls.png|200px]]</center>||<center>[[File:Antimony(III)-oxide-valentinite-xtal-2004-3D-balls.png|220px]]</center>
 |-
-|<center>Sb<sub>4</sub>O<sub>6</sub></center>||<center>senarmontite</center>||<center>valentinite</center>
+|Sb<sub>4</sub>O<sub>6</sub>||senarmontite||valentinite
 |}
-</center>
 ==Uses==
-The annual consumption of antimony(III) oxide in the United States and Europe is approximately 10,000 and 25,000 [[tonne]]s, respectively. The main application is as flame retardant synergist in combination with halogenated materials. The combination of the halides and the antimony is key to the flame-retardant action for polymers, helping to form less flammable chars. Such flame retardants are found in electrical apparatuses, textiles, leather, and coatings.<ref name=Ullmann>{{ Ullmann | author = Grund, S. C. |author2=Hanusch, K. |author3=Breunig, H. J. |author4=Wolf, H. U. | title = Antimony and Antimony Compounds | doi = 10.1002/14356007.a03_055.pub2 }}</ref>
+The annual consumption of antimony(III) oxide in the United States and Europe is approximately 10,000 and 25,000 [[tonne]]s, respectively. The main application is as [[flame retardant]] synergist in combination with halogenated materials. The combination of the halides and the antimony is key to the flame-retardant action for polymers, helping to form less flammable chars. Such flame retardants are found in electrical apparatuses, textiles, leather, and coatings.<ref name=Ullmann>{{ Ullmann | author = Grund, S. C. |author2=Hanusch, K. |author3=Breunig, H. J. |author4=Wolf, H. U. | title = Antimony and Antimony Compounds | doi = 10.1002/14356007.a03_055.pub2 }}</ref>
 Other applications:
@@ Line 107: / Line 108: @@
 ==Safety==
-Antimony(III) oxide has suspected carcinogenic potential for humans.<ref name=Ullmann/>  Its [[Threshold Limit Value|TLV]] is 0.5&nbsp;mg/m<sup>3</sup>, as for most antimony compounds.<ref>{{ cite journal |author1=Newton, P. E. |author2=Schroeder, R. E. |author3=Zwick, L. |author4=Serex, T. | title = Inhalation Developmental Toxicity Studies In Rats With Antimony(III) oxide (Sb<sub>2</sub>O<sub>3</sub>) | journal = Toxicologist | year = 2004 | volume = 78 | issue = 1-S | pages = 38 }}</ref><br/>
+Antimony(III) oxide has suspected carcinogenic potential for humans.<ref name=Ullmann/> Its [[Threshold Limit Value|TLV]] is 0.5&nbsp;mg/m<sup>3</sup>, as for most antimony compounds.<ref>{{ cite journal |author1=Newton, P. E. |author2=Schroeder, R. E. |author3=Zwick, L. |author4=Serex, T. | title = Inhalation Developmental Toxicity Studies In Rats With Antimony(III) oxide (Sb<sub>2</sub>O<sub>3</sub>) | journal = Toxicologist | year = 2004 | volume = 78 | issue = 1–S | pages = 38 }}</ref> Before 2021, no other human health hazards were identified for antimony(III) oxide, and no risks to human health and the environment were identified from the production and use of antimony trioxide in daily life. However, the 15th Report on Carcinogens released on December 21, 2021, by the [[US Department of Health and Human Services]] categorised antimony(III) oxide as carcinogenic.<ref>{{Cite web |title=15th Report on Carcinogens |url=https://ntp.niehs.nih.gov/whatwestudy/assessments/cancer/roc |access-date=2023-06-15 |website=National Toxicology Program |language=en}}</ref>
-No other human health hazards were identified for antimony(III) oxide, and no risks to human health and the environment were identified from the production and use of antimony trioxide in daily life.
 ==References==
@@ Line 120: / Line 120: @@
 * [http://www.antimony.com/ International Antimony Association]
 * [http://www.inchem.org/documents/icsc/icsc/eics0012.htm International Chemical Safety Card 0012]
-* [http://www.manymetal.com/Antimony/ Antimony Market And Price]
+* [https://web.archive.org/web/20160819095940/http://www.manymetal.com/Antimony/ Antimony Market And Price]
 * [http://www.sica-chauny.com/ Société industrielle et chimique de l'Aisne]
@@ Line 127: / Line 127: @@
 {{DEFAULTSORT:Antimony Trioxide}}
-[[Category:Antimony compounds]]
+[[Category:Antimony(III) compounds]]
 [[Category:Oxides]]
 [[Category:Inorganic pigments]]
@@ Line 133: / Line 133: @@
 [[Category:Sesquioxides]]
 [[Category:Adamantane-like molecules]]
+[[Category:Flame retardants]]

v t e Oxides
Mixed oxidation states	Antimony tetroxide (Sb₂O₄) Boron suboxide (B₁₂O₂) Carbon suboxide (C₃O₂) Chlorine perchlorate (Cl₂O₄) Chloryl perchlorate (Cl₂O₆) Cobalt(II,III) oxide (Co₃O₄) Dichlorine pentoxide (Cl₂O₅) Iron(II,III) oxide (Fe₃O₄) Lead(II,IV) oxide (Pb₃O₄) Manganese(II,III) oxide (Mn₃O₄) Mellitic anhydride (C₁₂O₉) Praseodymium(III,IV) oxide (Pr₆O₁₁) Silver(I,III) oxide (Ag₂O₂) Terbium(III,IV) oxide (Tb₄O₇) Tribromine octoxide (Br₃O₈) Triuranium octoxide (U₃O₈)
+1 oxidation state	Aluminium(I) oxide (Al₂O) Copper(I) oxide (Cu₂O) Caesium monoxide (Cs₂O) Dicarbon monoxide (C₂O) Dichlorine monoxide (Cl₂O) Gallium(I) oxide (Ga₂O) Iodine(I) oxide (I₂O) Lithium oxide (Li₂O) Mercury(I) oxide (Hg₂O) Nitrous oxide (N₂O) Potassium oxide (K₂O) Rubidium oxide (Rb₂O) Silver oxide (Ag₂O) Thallium(I) oxide (Tl₂O) Sodium oxide (Na₂O) Water (hydrogen oxide) (H₂O)
+2 oxidation state	Aluminium(II) oxide (AlO) Barium oxide (BaO) Berkelium monoxide (BkO) Beryllium oxide (BeO) Bromine monoxide (BrO) Cadmium oxide (CdO) Calcium oxide (CaO) Carbon monoxide (CO) Chlorine monoxide (ClO) Chromium(II) oxide (CrO) Cobalt(II) oxide (CoO) Copper(II) oxide (CuO) Dinitrogen dioxide (N₂O₂) Europium(II) oxide (EuO) Germanium monoxide (GeO) Iron(II) oxide (FeO) Iodine monoxide (IO) Lead(II) oxide (PbO) Magnesium oxide (MgO) Manganese(II) oxide (MnO) Mercury(II) oxide (HgO) Nickel(II) oxide (NiO) Nitric oxide (NO) Palladium(II) oxide (PdO) Phosphorus monoxide (PO) Polonium monoxide (PoO) Protactinium monoxide (PaO) Radium oxide (RaO) Silicon monoxide (SiO) Strontium oxide (SrO) Sulfur monoxide (SO) Disulfur dioxide (S₂O₂) Thorium monoxide (ThO) Tin(II) oxide (SnO) Titanium(II) oxide (TiO) Vanadium(II) oxide (VO) Yttrium(II) oxide (YO) Zinc oxide (ZnO)
+3 oxidation state	Actinium(III) oxide (Ac₂O₃) Aluminium oxide (Al₂O₃) Americium(III) oxide (Am₂O₃) Antimony trioxide (Sb₂O₃) Arsenic trioxide (As₂O₃) Berkelium(III) oxide (Bk₂O₃) Bismuth(III) oxide (Bi₂O₃) Boron trioxide (B₂O₃) Caesium sesquioxide (Cs₂O₃) Californium(III) oxide (Cf₂O₃) Cerium(III) oxide (Ce₂O₃) Chromium(III) oxide (Cr₂O₃) Cobalt(III) oxide (Co₂O₃) Dinitrogen trioxide (N₂O₃) Dysprosium(III) oxide (Dy₂O₃) Einsteinium(III) oxide (Es₂O₃) Erbium(III) oxide (Er₂O₃) Europium(III) oxide (Eu₂O₃) Gadolinium(III) oxide (Gd₂O₃) Gallium(III) oxide (Ga₂O₃) Gold(III) oxide (Au₂O₃) Holmium(III) oxide (Ho₂O₃) Indium(III) oxide (In₂O₃) Iron(III) oxide (Fe₂O₃) Lanthanum oxide (La₂O₃) Lutetium(III) oxide (Lu₂O₃) Manganese(III) oxide (Mn₂O₃) Neodymium(III) oxide (Nd₂O₃) Nickel(III) oxide (Ni₂O₃) Phosphorus trioxide (P₄O₆) Praseodymium(III) oxide (Pr₂O₃) Promethium(III) oxide (Pm₂O₃) Rhodium(III) oxide (Rh₂O₃) Samarium(III) oxide (Sm₂O₃) Scandium oxide (Sc₂O₃) Terbium(III) oxide (Tb₂O₃) Thallium(III) oxide (Tl₂O₃) Thulium(III) oxide (Tm₂O₃) Titanium(III) oxide (Ti₂O₃) Tungsten(III) oxide (W₂O₃) Vanadium(III) oxide (V₂O₃) Ytterbium(III) oxide (Yb₂O₃) Yttrium(III) oxide (Y₂O₃)
+4 oxidation state	Americium dioxide (AmO₂) Berkelium(IV) oxide (BkO₂) Bromine dioxide (BrO₂) Californium dioxide (CfO₂) Carbon dioxide (CO₂) Carbon trioxide (CO₃) Cerium(IV) oxide (CeO₂) Chlorine dioxide (ClO₂) Chromium(IV) oxide (CrO₂) Curium(IV) oxide (CmO₂) Dinitrogen tetroxide (N₂O₄) Germanium dioxide (GeO₂) Iodine dioxide (IO₂) Iridium dioxide (IrO₂) Hafnium(IV) oxide (HfO₂) Lead dioxide (PbO₂) Manganese dioxide (MnO₂) Neptunium(IV) oxide (NpO₂) Nitrogen dioxide (NO₂) Osmium dioxide (OsO₂) Platinum dioxide (PtO₂) Plutonium(IV) oxide (PuO₂) Polonium dioxide (PoO₂) Praseodymium(IV) oxide (PrO₂) Protactinium(IV) oxide (PaO₂) Rhodium(IV) oxide (RhO₂) Ruthenium(IV) oxide (RuO₂) Selenium dioxide (SeO₂) Silicon dioxide (SiO₂) Sulfur dioxide (SO₂) Technetium(IV) oxide (TcO₂) Tellurium dioxide (TeO₂) Terbium(IV) oxide (TbO₂) Thorium dioxide (ThO₂) Tin dioxide (SnO₂) Titanium dioxide (TiO₂) Tungsten(IV) oxide (WO₂) Uranium dioxide (UO₂) Vanadium(IV) oxide (VO₂) Zirconium dioxide (ZrO₂)
+5 oxidation state	Antimony pentoxide (Sb₂O₅) Arsenic pentoxide (As₂O₅) Bismuth pentoxide (Bi₂O₅) Dinitrogen pentoxide (N₂O₅) Niobium pentoxide (Nb₂O₅) Phosphorus pentoxide (P₂O₅) Protactinium(V) oxide (Pa₂O₅) Tantalum pentoxide (Ta₂O₅) Vanadium(V) oxide (V₂O₅)
+6 oxidation state	Chromium trioxide (CrO₃) Molybdenum trioxide (MoO₃) Polonium trioxide (PoO₃) Rhenium trioxide (ReO₃) Selenium trioxide (SeO₃) Sulfur trioxide (SO₃) Tellurium trioxide (TeO₃) Tungsten trioxide (WO₃) Uranium trioxide (UO₃) Xenon trioxide (XeO₃)
+7 oxidation state	Dichlorine heptoxide (Cl₂O₇) Manganese heptoxide (Mn₂O₇) Rhenium(VII) oxide (Re₂O₇) Technetium(VII) oxide (Tc₂O₇)
+8 oxidation state	Iridium tetroxide (IrO₄) Osmium tetroxide (OsO₄) Ruthenium tetroxide (RuO₄) Xenon tetroxide (XeO₄) Hassium tetroxide (HsO₄)
Related	Oxocarbon Suboxide Oxyanion Ozonide Peroxide Superoxide Oxypnictide
Oxides are sorted by oxidation state. Category:Oxides