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	{{chembox		{{chembox
			| Watchedfields = changed
	| verifiedrevid = 443022972
			| verifiedrevid = 451052860
	| ImageFile = Bismuth(III) oxide.jpg
			| ImageFile = Bismuth(III)_oxide_2.jpg
	| ImageSize = 200px
	| ImageName = Bismuth trioxide		| ImageSize =
			| ImageName = Bismuth trioxide
	| ImageFile2=AlfaBi2O3structure.jpg		| ImageFile2 =AlfaBi2O3structure.jpg
	| IUPACName = Bismuth trioxide<br />Bismuth(III) oxide<br />] (mineral)		| IUPACName = Bismuth trioxide<br />Bismuth(III) oxide<br />] (mineral)
	| OtherNames = Bismite, bismuth sesquioxide		| OtherNames = Bismuth oxide, bismuth sesquioxide
	| Section1 = {{Chembox Identifiers		|Section1={{Chembox Identifiers
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 14093		| ChemSpiderID = 14093
			| PubChem = 14776
	| UNII_Ref = {{fdacite|correct|FDA}}		| UNII_Ref = {{fdacite|correct|FDA}}
	| UNII = A6I4E79QF1		| UNII = A6I4E79QF1
			| EC_number = 215-134-7
	| InChI = 1/2Bi.3O/rBi2O3/c3-1-5-2-4		| InChI = 1/2Bi.3O/rBi2O3/c3-1-5-2-4
	| SMILES = O=O=O		| SMILES = O=O=O
Line 22:		Line 25:
	| CASNo = 1304-76-3		| CASNo = 1304-76-3
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
			| Bi=2|O=3
	| Formula = Bi<sub>2</sub>O<sub>3</sub>
			| Appearance = yellow crystals or powder
	| MolarMass = 465.96 g/mol
			| Odor = odorless
	| Appearance = yellow crystals or powder
	| Density = 8.90 g/cm<sup>3</sup>, solid		| Density = 8.90 g/cm<sup>3</sup>, solid
	| SolubleOther = soluble in ]s		| SolubleOther = soluble in ]s
	| Solubility = insoluble		| Solubility = insoluble
			| MeltingPtC = 817
	| MeltingPt = 817 °C , 1090 K, 1503 °F<ref name="handbook">{{cite book | last =Patnaik | first =Pradyot | year = 2003 | title =Handbook of Inorganic Chemical Compounds | publisher = McGraw-Hill | pages = | isbn =0070494398 | url= http://books.google.com/?id=Xqj-TTzkvTEC&pg=PA243 | accessdate = 2009-06-06}}
			| MeltingPt_ref = <ref name="handbook">{{cite book | last =Patnaik | first =Pradyot | year = 2003 | title =Handbook of Inorganic Chemical Compounds | publisher = McGraw-Hill | page = 243 | isbn =0-07-049439-8 | url= {{Google books|Xqj-TTzkvTEC|page=243|plainurl=yes}} | access-date = 2009-06-06}}
	</ref>		</ref>
	| BoilingPtC = 1890		| BoilingPtC = 1890
			| MagSus = -83.0·10<sup>−6</sup> cm<sup>3</sup>/mol
	}}		}}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| Coordination = pseudo-octahedral		| Coordination = pseudo-octahedral
	| CrystalStruct = ], ], <br>Space group P2<sub>1</sub>/c (No 14)		| CrystalStruct = ], ], <br>Space group P2<sub>1</sub>/c (No 14)
	}}		}}
	| Section7 = {{Chembox Hazards		|Section7={{Chembox Hazards
			| ExternalSDS =
	| ExternalMSDS =
	| EUClass = not listed		| NFPA-H = 1
	| NFPA-H = 0		| NFPA-F = 0
	| NFPA-F = 0		| NFPA-R = 0
			| FlashPt = Non-flammable
	| NFPA-R = 0
	| FlashPt = non-flammable
	}}		}}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherAnions = ]		| OtherAnions = ]<br> ] <br> ]
	| OtherCations = ]<br />]		| OtherCations = ]<br>]<br>]<br />]
	}}		}}
	}}		}}
	'''Bismuth(III) oxide''' is perhaps the most industrially important compound of ]. It is also a common starting point for bismuth chemistry. It is found naturally as the mineral ] (monoclinic) and sphaerobismoite (tetragonal, much more rare), but it is usually obtained as a by-product of the smelting of ] and ] ores. Bismuth trioxide is commonly used to produce the "]" effect in ], as a replacement of ].		'''Bismuth(III) oxide''' is a compound of ], and a common starting point for bismuth chemistry. It is found naturally as the mineral ] (monoclinic) and sphaerobismoite (tetragonal, much more rare), but it is usually obtained as a by-product of the smelting of ] and ] ores. Dibismuth trioxide is commonly used to produce the "]" effect in ], as a replacement of ].<ref name=handbook/>
			==Structure==
	==As a material for fuel cell electrolytes==
			The structures adopted by {{chem2|Bi2O3}} differ substantially from those of ], {{chem2|As2O3}}, and ], {{chem2|Sb2O3}}.<ref name="Wells">Wells, A.F. (1984) ''Structural Inorganic Chemistry''. 5th. London, England: Oxford University Press. p.890 {{ISBN|0-19-855370-6}}</ref>
	]
			]
			Bismuth oxide, {{chem2|Bi2O3}} has five crystallographic ]. The room temperature phase, α-{{chem2|Bi2O3}} has a ] crystal structure. There are three high temperature phases, a ] β-phase, a ] γ-phase, a ] δ-{{chem2|Bi2O3}} phase and an ε-phase.
	Bismuth oxide has seen interest as a material for ]s or SOFCs since it is an ionic conductor, i.e. oxygen atoms readily move through it. Pure bismuth oxide, Bi<sub>2</sub>O<sub>3</sub> has four crystallographic ]. It has a ] crystal structure, designated α- Bi<sub>2</sub>O<sub>3</sub>, at room temperature. This transforms to the ] fluorite-type crystal structure, δ-Bi<sub>2</sub>O<sub>3</sub>, when heated above 727°C, which remains the structure until the melting point, 824°C, is reached. The behaviour of Bi<sub>2</sub>O<sub>3</sub> on cooling from the δ-phase is more complex, with the possible formation of two intermediate ] phases; the ] β-phase or the ] γ-phase. The γ-phase can exist at room temperature with very slow cooling rates, but α- Bi<sub>2</sub>O<sub>3</sub> always forms on cooling the β-phase.
			The room temperature α-phase has a complex structure with layers of oxygen atoms with layers of bismuth atoms between them. The bismuth atoms are in two different environments which can be described as distorted 6 and 5 coordinate respectively.<ref name="MalmrosFernholt1970">{{cite journal |doi=10.3891/acta.chem.scand.24-0384 |title=The Crystal Structure of alpha-Bi2O2 |journal=Acta Chemica Scandinavica |volume=24 |pages=384–96 |year=1970 |last1=Malmros |first1=Gunnar |last2=Fernholt |first2=Liv |last3=Ballhausen |first3=C. J. |last4=Ragnarsson |first4=Ulf |last5=Rasmussen |first5=S. E. |last6=Sunde |first6=Erling |last7=Sørensen |first7=Nils Andreas |doi-access=free }}</ref>
			β-{{chem2|Bi2O3}} has a structure related to ].<ref name="Wells"/>
	δ- Bi<sub>2</sub>O<sub>3</sub> has the highest reported conductivity. At 750°C the conductivity of δ- Bi<sub>2</sub>O<sub>3</sub> is typically about 1 Scm<sup><nowiki>&minus;</nowiki>1</sup>, about three orders of magnitude greater than the intermediate phases and four orders greater than the ] phase. The conductivity in the β, γ and δ-phases is predominantly ionic with oxide ions being the main charge carrier. The α-phase exhibits p-type electronic conductivity (the charge is carried by positive holes) at room temperature which transforms to n-type conductivity (charge is carried by electrons) between 550°C and 650°C, depending on the oxygen partial pressure. It is therefore unsuitable for electrolyte applications. δ- Bi<sub>2</sub>O<sub>3</sub> has a defective fluorite-type crystal structure in which two of the eight oxygen sites in the unit cell are vacant. These intrinsic ] are highly mobile due to the high polarisability of the cation sub-lattice with the 6''s''<sup>2</sup> ] electrons of Bi<sup>3+</sup>. The Bi-O bonds have ] character and are therefore weaker than purely ionic bonds, so the oxygen ions can jump into ] more freely.
			γ-{{chem2|Bi2O3}} has a structure related to that of ] ({{chem2|Bi12SiO20}}), but in which a small fraction of the bismuth atoms occupy positions occupied by silicon atoms in sillenite, so the formula may be written as {{chem2|Bi12Bi0.8O19.2}}. The crystals are ] (] I23, or no. 197) with two {{chem2|Bi12Bi0.8O19.2}} formulas per unit cell.<ref name="RadaevSimonov1992">{{cite journal |doi=10.1107/S0108768192003847 |title=Structural features of γ-phase Bi<sub>2</sub>O<sub>3</sub> and its place in the sillenite family |journal=Acta Crystallographica Section B |volume=48 |issue=5 |pages=604–9 |year=1992 |last1=Radaev |first1=S. F. |last2=Simonov |first2=V. I. |last3=Kargin |first3=Yu. F. |doi-access=free }}</ref>
	The arrangement of oxygen atoms within the unit cell of δ- Bi<sub>2</sub>O<sub>3</sub> has been the subject of much debate in the past. Three different models have been proposed. Sillen (1937) used powder X-ray diffraction on quenched samples and reported the structure of Bi<sub>2</sub>O<sub>3</sub> was a simple ] phase with oxygen ] ordered along<111>, i.e. along the cube body diagonal (Figure 2a). Gattow and Schroder (1962) rejected this model, preferring to describe each oxygen site (8c site) in the unit cell as having 75% occupancy. In other words, the six oxygen atoms are randomly distributed over the eight possible oxygen sites in the unit cell. Currently, most experts seem to favour the latter description as a completely disordered oxygen sub-lattice accounts for the high conductivity in a better way.
			δ-{{chem2|Bi2O3}} has a defective ]-type crystal structure in which two of the eight oxygen sites in the unit cell are vacant.<ref name="Harwig1978">{{cite journal |doi=10.1002/zaac.19784440118 |title=On the Structure of Bismuthsesquioxide: The α, β, γ, and δ-phase |journal=Zeitschrift für anorganische und allgemeine Chemie |volume=444 |pages=151–66 |year=1978 |last1=Harwig |first1=H. A. }}</ref>
	Willis (1965) used ] to study the fluorite (CaF<sub>2</sub>) system. He determined that it could not be described by the ideal fluorite crystal structure, rather, the fluorine atoms were displaced from regular 8c positions towards the centres of the interstitial positions (Figure 2c). Shuk et al. (1996) and Sammes et al. (1999) suggest that because of the high degree of disorder in δ- Bi<sub>2</sub>O<sub>3</sub>, the Willis model could also be used to describe its structure.
			ε-{{chem2|Bi2O3}} has a structure related to the α- and β- phases but as the structure is fully ordered it is an ionic insulator. It can be prepared by hydrothermal means and transforms to the α- phase at 400&nbsp;°C.<ref name="RadaevSimonov1992"/>
			The ] α-phase transforms to the ] δ-{{chem2|Bi2O3}} when heated above 729&nbsp;°C, which remains the structure until the melting point, 824&nbsp;°C, is reached. The behaviour of {{chem2|Bi2O3}} on cooling from the δ-phase is more complex, with the possible formation of two intermediate ] phases; the ] β-phase or the ] γ-phase. The γ-phase can exist at room temperature with very slow cooling rates, but α-{{chem2|Bi2O3}} always forms on cooling the β-phase. Even though when formed by heat, it reverts to α-{{chem2|Bi2O3}} when the temperature drops back below 727&nbsp;°C, δ-{{chem2|Bi2O3}} can be formed directly through electrodeposition and remain relatively stable at room temperature, in an electrolyte of bismuth compounds that is also rich in sodium or potassium hydroxide so as to have a pH near 14.
	]
			==Conductivity==
	In addition to electrical properties, ] properties are very important when considering possible applications for solid electrolytes. High ] coefficients represent large dimensional variations under heating and cooling which would limit the performance of an electrolyte. The transition from the high-temperature δ- Bi<sub>2</sub>O<sub>3</sub> to the intermediate β- Bi<sub>2</sub>O<sub>3</sub> is accompanied by a large volume change and consequently, a deterioration of the mechanical properties of the material. This, combined with the very narrow stability range of the δ-phase (727-824<sup>o</sup>C), has led to studies on its stabilization to room temperature.
			The α-phase exhibits p-type electronic conductivity (the charge is carried by positive holes) at room temperature which transforms to n-type conductivity (charge is carried by electrons) between 550&nbsp;°C and 650&nbsp;°C, depending on the oxygen partial pressure.
			The conductivity in the β, γ and δ-phases is predominantly ]ic with oxide ions being the main charge carrier. Of these δ-{{chem2|Bi2O3}} has the highest reported conductivity. At 750&nbsp;°C the conductivity of δ-{{chem2|Bi2O3}} is typically about 1&nbsp;S&nbsp;cm<sup>−1</sup>, about three orders of magnitude greater than the intermediate phases and four orders greater than the ] phase.
			δ-{{chem2|Bi2O3}} has a defective fluorite-type crystal structure in which two of the eight oxygen sites in the unit cell are vacant. These intrinsic ] are highly mobile due to the high polarisability of the cation sub-lattice with the 6''s''<sup>2</sup> ] electrons of {{chem2|Bi(3+)}}. The Bi–O bonds have ] character and are therefore weaker than purely ionic bonds, so the oxygen ions can jump into ] more freely.
			The arrangement of ] atoms within the unit cell of δ-{{chem2|Bi2O3}} has been the subject of much debate in the past. Three different models have been proposed. Sillén (1937) used powder X-ray diffraction on quenched samples and reported the structure of {{chem2|Bi2O3}} was a simple ] phase with oxygen ] ordered along <111>, the cube body diagonal.<ref name=sillen>{{cite journal |last1=Sillén |first1=Lars Gunnar |year=1937 |title=X-Ray Studies on Bismuth Trioxide |journal=Arkiv för kemi, mineralogi och geologi |volume=12A |issue=1 |oclc=73018207 }}</ref> Gattow and Schroder (1962) rejected this model, preferring to describe each oxygen site (8c site) in the unit cell as having 75% occupancy. In other words, the six oxygen atoms are randomly distributed over the eight possible oxygen sites in the unit cell. Currently, most experts seem to favour the latter description as a completely disordered oxygen sub-lattice accounts for the high conductivity in a better way.<ref name=Gattow/>
	Bi<sub>2</sub>O<sub>3</sub> easily forms solid solutions with many other metal oxides. These doped systems exhibit a complex array of structures and properties dependent on the type of dopant, the dopant concentration and the thermal history of the sample. The most widely studied systems are those involving ] metal oxides, Ln<sub>2</sub>O<sub>3</sub>, including yttria, Y<sub>2</sub>O<sub>3</sub>. Rare earth metal cations are generally very stable, have similar chemical properties to one another and are similar in size to Bi<sup>3+</sup>, which has a radius of 1.03 Å, making them all excellent dopants. Furthermore, their ionic radii decrease fairly uniformly from La<sup>3</sup>+ (1.032 Å), through Nd<sup>3+</sup>, (0.983 Å), Gd<sup>3+</sup>, (0.938 Å), Dy<sup>3+</sup>, (0.912 Å) and Er<sup>3+</sup>, (0.89 Å), to Lu<sup>3+</sup>, (0.861 Å) (known as the ‘]’), making them useful to study the effect of dopant size on the stability of the Bi<sub>2</sub>O<sub>3</sub> phases.
			Willis (1965) used ] to study the fluorite ({{chem2|CaF2}}) system. He determined that it could not be described by the ideal fluorite crystal structure, rather, the fluorine atoms were displaced from regular 8c positions towards the centres of the interstitial positions.<ref name=Willis/> Shuk et al. (1996)<ref name=Shuk/> and Sammes et al. (1999)<ref name=Sammes/> suggest that because of the high degree of disorder in δ-{{chem2|Bi2O3}}, the Willis model could also be used to describe its structure.
			===Use in solid-oxide fuel cells (SOFCs)===
			Interest has centred on δ-{{chem2|Bi2O3}} as it is principally an ionic conductor. In addition to electrical properties, ] properties are very important when considering possible applications for solid electrolytes. High ] coefficients represent large dimensional variations under heating and cooling, which would limit the performance of an electrolyte. The transition from the high-temperature δ-{{chem2|Bi2O3}} to the intermediate β-{{chem2|Bi2O3}} is accompanied by a large volume change and consequently, a deterioration of the mechanical properties of the material. This, combined with the very narrow stability range of the δ-phase (727–824&nbsp;°C), has led to studies on its stabilization to room temperature.
			{{chem2|Bi2O3}} easily forms solid solutions with many other metal oxides. These doped systems exhibit a complex array of structures and properties dependent on the type of dopant, the dopant concentration and the thermal history of the sample. The most widely studied systems are those involving ] metal oxides, {{chem2|Ln2O3}}, including ], {{chem2|Y2O3}}. Rare earth metal cations are generally very stable, have similar chemical properties to one another and are similar in size to {{chem2|Bi(3+)}}, which has a radius of 1.03&nbsp;Å, making them all excellent dopants. Furthermore, their ionic radii decrease fairly uniformly from {{chem2|La(3+)}} (1.032&nbsp;Å), through {{chem2|Nd(3+)}} (0.983&nbsp;Å), {{chem2|Gd(3+)}} (0.938&nbsp;Å), {{chem2|Dy(3+)}} (0.912&nbsp;Å) and {{chem2|Er(3+)}} (0.89&nbsp;Å), to {{chem2|Lu(3+)}} (0.861&nbsp;Å) (known as the "]"), making them useful to study the effect of dopant size on the stability of the {{chem2|Bi2O3}} phases.
			{{chem2|Bi2O3}} has also been used as sintering additive in the {{chem2|Sc2O3}}-doped zirconia system for intermediate temperature SOFC.<ref>{{Cite journal |doi=10.1016/S0167-2738(02)00912-8 |title=Effect of Bi<sub>2</sub>O<sub>3</sub> additives in Sc stabilized zirconia electrolyte on a stability of crystal phase and electrolyte properties |journal=Solid State Ionics |volume=158 |issue=3–4 |pages=215–23 |year=2003 |last1=Hirano |first1=Masanori |last2=Oda |first2=Takayuki |last3=Ukai |first3=Kenji |last4=Mizutani |last5=Yasunobu }}</ref>
	==Preparation==		==Preparation==
	Bismuth trioxide is commercially made from ]. The latter is produced by dissolving bismuth in hot ]. Addition of excess ] followed by continuous heating of the mixture precipitates bismuth(III) oxide as a heavy yellow powder. Also, the trioxide can be prepared by ignition of ].<ref name=handbook/>
			The trioxide can be prepared by ignition of ].<ref name=handbook/> Bismuth trioxide can be also obtained by heating bismuth subcarbonate at approximately 400 °C.<ref name="Ortiz">{{cite journal |doi=10.1021/acs.inorgchem.6b02923 |title= Bismuth Oxide Nanoparticles Partially Substituted with Eu<sup>III</sup>, Mn<sup>IV</sup>, and Si<sup>IV</sup>: Structural, Spectroscopic, and Optical Findings |journal=Inorganic Chemistry |volume=56 |pages=3394–3403 |year=2017 |last1=Ortiz-Quiñonez |first1=Jose |last2=Zumeta-Dubé |first2=Inti |last3=Díaz |first3=David |last4=Nava-Etzana |first4=Noel |last5=Cruz-Zaragoza |first5=Epifanio |issue= 6 |pmid=28252972|s2cid= 3346966 }}</ref>
	==Reactions==		==Reactions==
	Oxidation with ] and dilute caustic soda gives ]. The same product can be obtained by using other oxidizing agents such as ] and concentrated caustic potash solution.
			Atmospheric carbon dioxide or {{chem2|CO2}} dissolved in water readily reacts with {{chem2|Bi2O3}} to generate ].<ref name=Ortiz/> Bismuth oxide is considered a basic oxide, which explains the high reactivity with {{chem2|CO2}}. However, when acidic cations such as Si(IV) are introduced within the structure of the bismuth oxide, the reaction with {{chem2|CO2}} do not occur.<ref name=Ortiz/>
	Electrolysis of bismuth(III) oxide in hot concentrated alkali solution gives a scarlet red precipitate of ]. Bismuth(III) oxide reacts with mineral acids to give the corresponding bismuth(III) salts.
			Bismuth(III) oxide reacts with a mixture of concentrated aqueous sodium hydroxide and bromine or aqueous potassium hydroxide and bromine to form ] or potassium bismuthate, respectively.<ref name="brauer1">{{Citation|last = Brauer|first = Georg|publication-date = 1963|year = 1963|title = Handbook of Preparative Inorganic Chemistry|edition = 2nd|volume = 1|location = New York|publisher = Academic Press Inc.|page = 628}}</ref>
	Reaction with ] and ] gives bismuth trioleate.
			==Usage==
			=== Medical devices ===
			Bismuth oxide is occasionally used in dental materials to make them more opaque to X-rays than the surrounding tooth structure. In particular, bismuth (III) oxide has been used in hydraulic silicate cements (HSC), originally in "]" (a trade name, standing for the chemically-meaningless "]") from 10 to 20% by mass with a mixture of mainly di- and tri-calcium silicate powders. Such HSC is used for dental treatments such as: apicoectomy, ], pulp capping, pulpotomy, pulp regeneration, internal repair of iatrogenic perforations, repair of resorption perforations, root canal sealing and obturation. MTA sets into a hard filling material when mixed with water. Some resin-based materials also include an HSC with bismuth oxide. Problems have allegedly arisen with bismuth oxide because it is claimed not to be inert at high pH, specifically that it slows the setting of the HSC, but also over time can lose color<ref>{{cite journal |pmid=23265162 |year=2012 |last1=Hutcheson |first1=C |title=Multi-surface composite vs stainless steel crown restorations after mineral trioxide aggregate pulpotomy: A randomized controlled trial |journal=Pediatric Dentistry |volume=34 |issue=7 |pages=460–7 |last2=Seale |first2=N. S. |last3=McWhorter |first3=A |last4=Kerins |first4=C |last5=Wright |first5=J }}</ref> by exposure to light or reaction with other materials that may have been used in the tooth treatment, such as sodium hypochlorite.<ref>{{cite journal |doi=10.1016/j.joen.2013.09.040 |pmid=24565667 |title=Color Stability of White Mineral Trioxide Aggregate in Contact with Hypochlorite Solution |journal=Journal of Endodontics |volume=40 |issue=3 |pages=436–40 |year=2014 |last1=Camilleri |first1=Josette }}</ref>
			=== Radiative cooling ===
			Bismuth oxide was used to develop a scalable colored surface high in ] and ] for ]. The paint was non-toxic and demonstrated a reflectance of 99% and emittance of 97%. In field tests the coating exhibited significant cooling power and reflected potential for the further development of colored surfaces practical for large-scale radiative cooling applications.<ref name=":16">{{Cite journal |last1=Zhai |first1=Huatian |last2=Fan |first2=Desong |last3=Li |first3=Qiang |date=September 2022 |title=Scalable and paint-format colored coatings for passive radiative cooling |url=https://www.sciencedirect.com/science/article/abs/pii/S0927024822002732 |journal=Solar Energy Materials and Solar Cells |volume=245 |page=111853 |doi=10.1016/j.solmat.2022.111853 |s2cid=249877164 |via=Elsevier Science Direct}}</ref>
	==References==		==References==
	<references/>
			{{Reflist|refs=
	*{{cite journal |last=Gattow |first=G. |authorlink= |coauthors=Schröder, H. |year=1962 |month= |title=Über Wismutoxide. III. Die Kristallstruktur der Hochtemperaturmodifikation von Wismut(III)-oxid (&delta;-Bi<sub>2</sub>O<sub>3</sub>) |journal=Zeitschrift für anorganische und allgemeine Chemie |volume=318 |issue=3–4 |pages=176–189 |doi=10.1002/zaac.19623180307 |url= |accessdate= |quote= }}
	*{{cite journal |last=Harwig |first=H. A. |authorlink= |coauthors= |year=1978 |month= |title=On the Structure of Bismuthsesquioxide: The &alpha;, &beta;, &gamma;, and &delta;-phase |journal=Zeitschrift für anorganische und allgemeine Chemie |volume=444 |issue=1 |pages=151–166 |doi=10.1002/zaac.19784440118 |url= |accessdate= |quote= }}		<ref name=Gattow>{{cite journal |doi=10.1002/zaac.19623180307 |title=Über Wismutoxide. III. Die Kristallstruktur der Hochtemperaturmodifikation von Wismut(III)-oxid (δ-Bi2O3) |trans-title=About bismuth oxides. III. The crystal structure of the high-temperature modification of bismuth (III) oxide (δ-Bi2O3) |language=de |journal=Zeitschrift für anorganische und allgemeine Chemie |volume=318 |issue=3–4 |pages=176–89 |year=1962 |last1=Gattow |first1=G. |last2=Schröder |first2=H. }}</ref>
	*{{cite journal |last=Harwig |first=H. A. |authorlink= |coauthors=Gerards, A. G. |year=1978 |month= |title=Electrical properties of the &alpha;, &beta;, &gamma; and &delta; phases of bismuth sesquioxide |journal=Journal of Solid State Chemistry |volume=26 |issue=3 |pages=265–274 |doi=10.1016/0022-4596(78)90161-5 |url= |accessdate= |quote= }}
	*{{cite journal |last=Sammes |first=N. M. |authorlink= |coauthors=Tompsett, G. A.; Cai, Z. H. |year=1999 |month= |title=The chemical reaction between ceria and fully stabilised zirconia |journal=Solid State Ionics |volume=121 |issue=1 |pages=121–125 |doi=10.1016/S0167-2738(98)00538-4 |url= |accessdate= |quote= }}		<ref name=Sammes>{{cite journal |doi=10.1016/S0167-2738(98)00538-4 |title=The chemical reaction between ceria and fully stabilised zirconia |journal=Solid State Ionics |volume=121–5 |pages=121–5 |year=1999 |last1=Sammes |first1=N |last2=Tompsett |first2=G.A |last3=Cai |first3=Zhihong |issue=1–4 }}</ref>
	*{{cite journal |last=Shannon |first=R. D. |authorlink= |coauthors= |year=1976 |month= |title= |journal=Acta Crystallographica A |volume=32 |issue= |pages=751 |id= |url= |accessdate= |quote= }}
	*{{cite journal |last=Shuk |first=P. |authorlink= |coauthors=Wiemhofer, H. D.; Guth, U.; Gopel, W.; Greenblatt, M.; |year=1996 |month= |title=Oxide ion conducting solid electrolytes based on Bi<sub>2</sub>O<sub>3</sub> |journal=Solid State Ionics |volume=89 |issue=3 |pages=179–196 |doi=10.1016/0167-2738(96)00348-7 |url= |accessdate= |quote= }}		<ref name=Shuk>{{cite journal |doi=10.1016/0167-2738(96)00348-7 |title=Oxide ion conducting solid electrolytes based on Bi<sub>2</sub>O<sub>3</sub> |journal=Solid State Ionics |volume=89 |issue=3–4 |pages=179–96 |year=1996 |last1=Shuk |first1=P |last2=Wiemhöfer |first2=H.-D. |last3=Guth |first3=U. |last4=Göpel |first4=W. |last5=Greenblatt |first5=M. }}</ref>
	*{{cite journal |last=Sillen |first=L. G. |authorlink= |coauthors= |year=1937 |month= |title= |journal=Ark. Kemi. Mineral. Geol. |volume=12A |issue=1 |pages= |id= |url= |accessdate= |quote= }}
			<ref name=Willis>{{cite journal |doi=10.1107/S0365110X65000130 |title=The anomalous behaviour of the neutron reflexion of fluorite |journal=Acta Crystallographica |volume=18 |pages=75–6 |year=1965 |last1=Willis |first1=B. T. M. |issue=1 |doi-access=free |bibcode=1965AcCry..18...75W }}</ref>
	*{{cite journal |last=Vannier |first=R. N. |authorlink= |coauthors=Mairesse, G.; Abraham, F.; Nowogrocki, G. |year=1993 |month= |title=Incommensurate Superlattice in Mo-Substituted Bi<sub>4</sub>V<sub>2</sub>O<sub>11</sub> |journal=Journal of Solid State Chemistry |volume=103 |issue=2 |pages=441–446 |doi=10.1006/jssc.1993.1120 |url= |accessdate= |quote= }}
			}}
	*{{cite journal |doi=10.1107/S0365110X65000130 |last=Willis |first=B. T. M. |authorlink= |coauthors= |year=1965 |month= |title= The anomalous behaviour of the neutron reflexion of fluorite|journal=Acta Crystallographica |volume=18 |issue= 1|pages=75 |id= |url= |accessdate= |quote= }}
			==Further reading==
			*{{cite journal |doi=10.1107/S0567739476001551 |title=Revised effective ionic radii and systematic studies of interatomic distances in halides and chalcogenides |journal=Acta Crystallographica Section A |volume=32 |issue=5 |pages=751–67 |year=1976 |last1=Shannon |first1=R. D. |bibcode=1976AcCrA..32..751S |doi-access=free }}
			*{{cite journal |doi=10.1006/jssc.1993.1120 |title=Incommensurate Superlattice in Mo-Substituted Bi<sub>4</sub>V<sub>2</sub>O<sub>11</sub> |journal=Journal of Solid State Chemistry |volume=103 |issue=2 |pages=441–6 |year=1993 |last1=Vannier |first1=R.N. |last2=Mairesse |first2=G. |last3=Abraham |first3=F. |last4=Nowogrocki |first4=G. |bibcode=1993JSSCh.103..441V }}
	{{Bismuth compounds}}		{{Bismuth compounds}}
			{{Oxides}}
			{{Authority control}}
	{{DEFAULTSORT:Bismuth(Iii) Oxide}}		{{DEFAULTSORT:Bismuth(Iii) Oxide}}
	]		]
	]
			]
	]		]
	]
	]		]
	]
	]
	]
	]
	]
	]
	]
	]
	]