Бор триоксид

Бор триоксид
Имена
	IUPAC name Diboron trioxide
	Other names boron oxide, diboron trioxide, boron sesquioxide, boric oxide, boria; Boric anhydride
Identifiers
CAS Number	1303-86-2 ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:30163 ;
ChemSpider	452485 ;
ECHA InfoCard	100.013.751
EC Number	215-125-8;
Gmelin Reference	11108
PubChem CID	518682;
RTECS number	ED7900000;
UNII	483W67CPF4 ;
CompTox Dashboard (EPA)	DTXSID7034387 ;
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Properties
Chemical formula	B2O3
Molar mass	69.6182 g/mol
Appearance	white, glassy solid
Density	2.460 g/cm3, liquid;; 2.55 g/cm3, trigonal;; 3.11–3.146 g/cm3, monoclinic
Melting point	450 °C (842 °F; 723 K) (trigonal) ; 510 °C (tetrahedral)
Boiling point	1,860 °C (3,380 °F; 2,130 K) , sublimes at 1500 °C
Solubility in water	1.1 g/100mL (10 °C) ; 3.3 g/100mL (20 °C) ; 15.7 g/100mL (100 °C)
Solubility	partially soluble in methanol
Acidity (pKa)	~ 4
Magnetic susceptibility (χ)	−39.0·10−6 cm3/mol
Thermochemistry
Heat capacity (C)	66.9 J/(mol⋅K)
Std molar; entropy (S⦵298)	80.8 J/(mol⋅K)
Std enthalpy of; formation (ΔfH⦵298)	−1254 kJ/mol
Gibbs free energy (ΔfG⦵)	−832 kJ/mol
Hazards
	Occupational safety and health (OHS/OSH):
Main hazards	Irritant
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H360FD
Precautionary statements	P201, P202, P281, P308+P313, P405, P501
NFPA 704 (fire diamond)	2 0 0
Flash point	noncombustible
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	3163 mg/kg (oral, mouse)
	NIOSH (US health exposure limits):
PEL (Permissible)	TWA 15 mg/m3
REL (Recommended)	TWA 10 mg/m3
IDLH (Immediate danger)	2000 mg/m3
Supplementary data page
	Boron 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

Триоксид бора или триоксид дибурона является оксидом бора с формулой B ₂ O ₃ . Это бесцветный прозрачный твердый, почти всегда стеклянный (аморфный), который может быть кристаллизован только с большим трудом. Это также называется оксидом борика ^{[ 6 ]} или Бория . ^{[ 7 ]} Он имеет много важных промышленных применений, главным образом в керамике, в качестве потока для глазури и эмалей, а также в производстве очков .

Структура

Триоксид бора имеет три известные формы: одна аморфная и два кристаллических.

Аморфная форма

The amorphous form (g-B ₂ O ₃ ), безусловно, наиболее распространен. Считается, что он состоит из кольцевых колец , которые представляют собой шестичленные кольца, состоящие из чередующегося 3-координатного бора и 2-координатного кислорода.

Because of the difficulty of building disordered models at the correct density with many boroxol rings, this view was initially controversial, but such models have recently been constructed and exhibit properties in excellent agreement with experiment.^[8]^[9] It is now recognized, from experimental and theoretical studies,^[10]^[11]^[12]^[13]^[14] that the fraction of boron atoms belonging to boroxol rings in glassy B₂O₃ is somewhere between 0.73 and 0.83, with 0.75 = 3/4 corresponding to a 1:1 ratio between ring and non-ring units. The number of boroxol rings decays in the liquid state with increasing temperature.^[15]

Crystalline α form

The crystalline form (α-B₂O₃) is exclusively composed of BO₃ triangles. It crystal structure was initially believed to be the enantiomorphic space groups P3₁(#144) and P3₂(#145), like γ-glycine;^[16]^[17] but was later revised to the enantiomorphic space groups P3₁21(#152) and P3₂21(#154) in the trigonal crystal system, like α-quartz^[18]

Crystallization of α-B₂O₃ from the molten state at ambient pressure is strongly kinetically disfavored (compare liquid and crystal densities). It can be obtained with prologued annealing of the amorphous solid ~200 °C under at least 10 kbar of pressure.^[19]^[1]

Crystalline β form

The trigonal network undergoes a coesite-like transformation to monoclinic β-B₂O₃ at several gigapascals (9.5 GPa).^[20]

Preparation

Boron trioxide is produced by treating borax with sulfuric acid in a fusion furnace. At temperatures above 750 °C, the molten boron oxide layer separates out from sodium sulfate. It is then decanted, cooled and obtained in 96–97% purity.^[3]

Another method is heating boric acid above ~300 °C. Boric acid will initially decompose into steam, (H₂O_(g)) and metaboric acid (HBO₂) at around 170 °C, and further heating above 300 °C will produce more steam and diboron trioxide. The reactions are:

H₃BO₃ → HBO₂ + H₂O

2 HBO₂ → B₂O₃ + H₂O

Boric acid goes to anhydrous microcrystalline B₂O₃ in a heated fluidized bed.^[21] Carefully controlled heating rate avoids gumming as water evolves.

Boron oxide will also form when diborane (B₂H₆) reacts with oxygen in the air or trace amounts of moisture:

2B₂H₆(g) + 3O₂(g) → 2B₂O₃(s) + 6H₂(g)

B₂H₆(g) + 3H₂O(g) → B₂O₃(s) + 6H₂(g)^[22]

Reactions

Molten boron oxide attacks silicates. Containers can be passivated internally with a graphitized carbon layer obtained by thermal decomposition of acetylene.^[23]

Applications

Major component of borosilicate glass
Fluxing agent for glass and enamels^{[citation needed]}
An additive used in glass fibres (optical fibres)
The inert capping layer in the Liquid Encapsulation Czochralski process for the production of gallium arsenide single crystal
As an acid catalyst in organic synthesis
As a starting material for the production of other boron compounds, such as boron carbide

References

^ Jump up to: ^a ^b Gurr, G. E.; Montgomery, P. W.; Knutson, C. D.; Gorres, B. T. (1970). "The Crystal Structure of Trigonal Diboron Trioxide". Acta Crystallographica B. 26 (7): 906–915. doi:10.1107/S0567740870003369.
^ High temperature corrosion and materials chemistry: proceedings of the Per Kofstad Memorial Symposium. Proceedings of the Electrochemical Society. The Electrochemical Society. 2000. p. 496. ISBN 978-1-56677-261-7.
^ Jump up to: ^a ^b Patnaik, P. (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 119. ISBN 978-0-07-049439-8. Retrieved 2009-06-06.
^ Jump up to: ^a ^b ^c ^d NIOSH Pocket Guide to Chemical Hazards. "#0060". National Institute for Occupational Safety and Health (NIOSH).
^ "Boron oxide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
^ L. McCulloch (1937): "A Crystalline Boric Oxide". Journal of the American Chemical Society, volume 59, issue 12, pages 2650–2652. doi:10.1021/ja01291a05
^ I.Vishnevetsky and M.Epstein (2015): "Solar carbothermic reduction of alumina, magnesia and boria under vacuum". Solar Energy, volume 111, pages 236-251 doi:10.1016/j.solener.2014.10.039
^ Ferlat, G.; Charpentier, T.; Seitsonen, A. P.; Takada, A.; Lazzeri, M.; Cormier, L.; Calas, G.; Mauri. F. (2008). "Boroxol Rings in Liquid and Vitreous B₂O₃ from First Principles". Phys. Rev. Lett. 101 (6): 065504. Bibcode:2008PhRvL.101f5504F. doi:10.1103/PhysRevLett.101.065504. PMID 18764473.
^ Ferlat, G.; Seitsonen, A. P.; Lazzeri, M.; Mauri, F. (2012). "Hidden polymorphs drive vitrification in B₂O₃". Nature Materials Letters. 11 (11): 925–929. arXiv:1209.3482. Bibcode:2012NatMa..11..925F. doi:10.1038/NMAT3416. PMID 22941329. S2CID 11567458.
^ Hung, I.; et al. (2009). "Determination of the bond-angle distribution in vitreous B₂O₃ by rotation (DOR) NMR spectroscopy". Journal of Solid State Chemistry. 182 (9): 2402–2408. Bibcode:2009JSSCh.182.2402H. doi:10.1016/j.jssc.2009.06.025.
^ Soper, A. K. (2011). "Boroxol rings from diffraction data on vitreous boron trioxide". J. Phys.: Condens. Matter. 23 (36): 365402. Bibcode:2011JPCM...23.5402S. doi:10.1088/0953-8984/23/36/365402. PMID 21865633. S2CID 5291179.
^ Joo, C.; et al. (2000). "The ring structure of boron trioxide glass". Journal of Non-Crystalline Solids. 261 (1–3): 282–286. Bibcode:2000JNCS..261..282J. doi:10.1016/s0022-3093(99)00609-2.
^ Zwanziger, J. W. (2005). "The NMR response of boroxol rings: a density functional theory study". Solid State Nuclear Magnetic Resonance. 27 (1–2): 5–9. doi:10.1016/j.ssnmr.2004.08.004. PMID 15589722.
^ Micoulaut, M. (1997). "The structure of vitreous B₂O₃ obtained from a thermostatistical model of agglomeration". Journal of Molecular Liquids. 71 (2–3): 107–114. doi:10.1016/s0167-7322(97)00003-2.
^ Alderman, O. L. G. Ferlat, G. Baroni, A. Salanne, M. Micoulaut, M. Benmore, C. J. Lin, A. Tamalonis, A. Weber, J. K. R. (2015). "Liquid B2O3 up to 1700K: X-ray diffraction and boroxol ring dissolution" (PDF). Journal of Physics: Condensed Matter. 27 (45): 455104. Bibcode:2015JPCM...27S5104A. doi:10.1088/0953-8984/27/45/455104. PMID 26499978. S2CID 21783488.{{cite journal}}: CS1 maint: multiple names: authors list (link)
^ Gurr, G. E.; Montgomery, P. W.; Knutson, C. D.; Gorres, B. T. (1970). "The crystal structure of trigonal diboron trioxide". Acta Crystallographica B. 26 (7): 906–915. doi:10.1107/S0567740870003369.
^ Strong, S. L.; Wells, A. F.; Kaplow, R. (1971). "On the crystal structure of B₂O₃". Acta Crystallographica B. 27 (8): 1662–1663. doi:10.1107/S0567740871004515.
^ Effenberger, H.; Lengauer, C. L.; Parthé, E. (2001). "Trigonal B₂O₃ with Higher Space-Group Symmetry: Results of a Reevaluation". Monatshefte für Chemie. 132 (12): 1515–1517. doi:10.1007/s007060170008. S2CID 97795834.
^ Aziz, M. J.; Nygren, E.; Hays, J. F.; Turnbull, D. (1985). "Crystal Growth Kinetics of Boron Oxide Under Pressure". Journal of Applied Physics. 57 (6): 2233. Bibcode:1985JAP....57.2233A. doi:10.1063/1.334368.
^ Brazhkin, V. V.; Katayama, Y.; Inamura, Y.; Kondrin, M. V.; Lyapin, A. G.; Popova, S. V.; Voloshin, R. N. (2003). "Structural transformations in liquid, crystalline and glassy B₂O₃ under high pressure". JETP Letters. 78 (6): 393–397. Bibcode:2003JETPL..78..393B. doi:10.1134/1.1630134. S2CID 189764568.
^ Kocakuşak, S.; Akçay, K.; Ayok, T.; Koöroğlu, H. J.; Koral, M.; Savaşçi, Ö. T.; Tolun, R. (1996). "Production of anhydrous, crystalline boron oxide in fluidized bed reactor". Chemical Engineering and Processing. 35 (4): 311–317. doi:10.1016/0255-2701(95)04142-7.
^ AirProducts (2011). "Diborane Storage & Delivery" (PDF). Archived from the original (PDF) on 2015-02-04. Retrieved 2013-08-21. {{cite journal}}: Cite journal requires |journal= (help)
^ Morelock, C. R. (1961). "Research Laboratory Report #61-RL-2672M". General Electric. {{cite journal}}: Cite journal requires |journal= (help)

Внешние ссылки

[a1-1] Jump up to: ^a ^b Gurr, G. E.; Montgomery, P. W.; Knutson, C. D.; Gorres, B. T. (1970). "The Crystal Structure of Trigonal Diboron Trioxide". Acta Crystallographica B. 26 (7): 906–915. doi:10.1107/S0567740870003369.

[2] High temperature corrosion and materials chemistry: proceedings of the Per Kofstad Memorial Symposium. Proceedings of the Electrochemical Society. The Electrochemical Society. 2000. p. 496. ISBN 978-1-56677-261-7.

[patnaik-3] Jump up to: ^a ^b Patnaik, P. (2003). Handbook of Inorganic Chemical Compounds. McGraw-Hill. p. 119. ISBN 978-0-07-049439-8. Retrieved 2009-06-06.

[PGCH-4] Jump up to: ^a ^b ^c ^d NIOSH Pocket Guide to Chemical Hazards. "#0060". National Institute for Occupational Safety and Health (NIOSH).

[5] "Boron oxide". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).

[mccu1937-6] L. McCulloch (1937): "A Crystalline Boric Oxide". Journal of the American Chemical Society, volume 59, issue 12, pages 2650–2652. doi:10.1021/ja01291a05

[vish2015-7] I.Vishnevetsky and M.Epstein (2015): "Solar carbothermic reduction of alumina, magnesia and boria under vacuum". Solar Energy, volume 111, pages 236-251 doi:10.1016/j.solener.2014.10.039

[ferl2008-8] Ferlat, G.; Charpentier, T.; Seitsonen, A. P.; Takada, A.; Lazzeri, M.; Cormier, L.; Calas, G.; Mauri. F. (2008). "Boroxol Rings in Liquid and Vitreous B₂O₃ from First Principles". Phys. Rev. Lett. 101 (6): 065504. Bibcode:2008PhRvL.101f5504F. doi:10.1103/PhysRevLett.101.065504. PMID 18764473.

[ferl2012-9] Ferlat, G.; Seitsonen, A. P.; Lazzeri, M.; Mauri, F. (2012). "Hidden polymorphs drive vitrification in B₂O₃". Nature Materials Letters. 11 (11): 925–929. arXiv:1209.3482. Bibcode:2012NatMa..11..925F. doi:10.1038/NMAT3416. PMID 22941329. S2CID 11567458.

[hung2009-10] Hung, I.; et al. (2009). "Determination of the bond-angle distribution in vitreous B₂O₃ by rotation (DOR) NMR spectroscopy". Journal of Solid State Chemistry. 182 (9): 2402–2408. Bibcode:2009JSSCh.182.2402H. doi:10.1016/j.jssc.2009.06.025.

[soper2011-11] Soper, A. K. (2011). "Boroxol rings from diffraction data on vitreous boron trioxide". J. Phys.: Condens. Matter. 23 (36): 365402. Bibcode:2011JPCM...23.5402S. doi:10.1088/0953-8984/23/36/365402. PMID 21865633. S2CID 5291179.

[jooc2000-12] Joo, C.; et al. (2000). "The ring structure of boron trioxide glass". Journal of Non-Crystalline Solids. 261 (1–3): 282–286. Bibcode:2000JNCS..261..282J. doi:10.1016/s0022-3093(99)00609-2.

[zwan2005-13] Zwanziger, J. W. (2005). "The NMR response of boroxol rings: a density functional theory study". Solid State Nuclear Magnetic Resonance. 27 (1–2): 5–9. doi:10.1016/j.ssnmr.2004.08.004. PMID 15589722.

[mico1997-14] Micoulaut, M. (1997). "The structure of vitreous B₂O₃ obtained from a thermostatistical model of agglomeration". Journal of Molecular Liquids. 71 (2–3): 107–114. doi:10.1016/s0167-7322(97)00003-2.

[alde2015-15] Alderman, O. L. G. Ferlat, G. Baroni, A. Salanne, M. Micoulaut, M. Benmore, C. J. Lin, A. Tamalonis, A. Weber, J. K. R. (2015). "Liquid B2O3 up to 1700K: X-ray diffraction and boroxol ring dissolution" (PDF). Journal of Physics: Condensed Matter. 27 (45): 455104. Bibcode:2015JPCM...27S5104A. doi:10.1088/0953-8984/27/45/455104. PMID 26499978. S2CID 21783488.{{cite journal}}: CS1 maint: multiple names: authors list (link)

[gurr1970-16] Gurr, G. E.; Montgomery, P. W.; Knutson, C. D.; Gorres, B. T. (1970). "The crystal structure of trigonal diboron trioxide". Acta Crystallographica B. 26 (7): 906–915. doi:10.1107/S0567740870003369.

[stro1971-17] Strong, S. L.; Wells, A. F.; Kaplow, R. (1971). "On the crystal structure of B₂O₃". Acta Crystallographica B. 27 (8): 1662–1663. doi:10.1107/S0567740871004515.

[effe2001-18] Effenberger, H.; Lengauer, C. L.; Parthé, E. (2001). "Trigonal B₂O₃ with Higher Space-Group Symmetry: Results of a Reevaluation". Monatshefte für Chemie. 132 (12): 1515–1517. doi:10.1007/s007060170008. S2CID 97795834.

[aziz1985-19] Aziz, M. J.; Nygren, E.; Hays, J. F.; Turnbull, D. (1985). "Crystal Growth Kinetics of Boron Oxide Under Pressure". Journal of Applied Physics. 57 (6): 2233. Bibcode:1985JAP....57.2233A. doi:10.1063/1.334368.

[braz2003-20] Brazhkin, V. V.; Katayama, Y.; Inamura, Y.; Kondrin, M. V.; Lyapin, A. G.; Popova, S. V.; Voloshin, R. N. (2003). "Structural transformations in liquid, crystalline and glassy B₂O₃ under high pressure". JETP Letters. 78 (6): 393–397. Bibcode:2003JETPL..78..393B. doi:10.1134/1.1630134. S2CID 189764568.

[akca1996-21] Kocakuşak, S.; Akçay, K.; Ayok, T.; Koöroğlu, H. J.; Koral, M.; Savaşçi, Ö. T.; Tolun, R. (1996). "Production of anhydrous, crystalline boron oxide in fluidized bed reactor". Chemical Engineering and Processing. 35 (4): 311–317. doi:10.1016/0255-2701(95)04142-7.

[AIRP2011-22] AirProducts (2011). "Diborane Storage & Delivery" (PDF). Archived from the original (PDF) on 2015-02-04. Retrieved 2013-08-21. {{cite journal}}: Cite journal requires |journal= (help)

[more1961-23] Morelock, C. R. (1961). "Research Laboratory Report #61-RL-2672M". General Electric. {{cite journal}}: Cite journal requires |journal= (help)

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[5]

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[9]

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v Т и Бор соединения
Boron pnictogenides	BAs BN BP
Boron halides	BBr₃ BCl₃ BF BFO BF₃ BI₃ B₂F₄ B₂Cl₄
Acids	B(NO₃)₃ B(OH)₃ BPO₄ BH₃O
Boranes	BH₃ B₂H₄ B₂H₆ BH₃NH₃ B₄H₁₀ B₅H₉ B₅H₁₁ B₆H₁₀ B₆H₁₂ B₁₀H₁₄ B₁₈H₂₂
Boron oxides and sulfides	B₂O B₂O₃ B₂S₃ B₆O
Carbides	B₄C
Organoboron compounds	(BH₂Me)₂ BMe₃ BEt₃ Ac₄(BO₃)₂ COBH₃

v Т и Оксиды
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