Difference between revisions of "Dibromine monoxide"
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| MolarMass = 175.81 g mol<sup>−1</sup> | | MolarMass = 175.81 g mol<sup>−1</sup> | ||
| MeltingPt = −17.5 °C (255.7 K) ''decomp.'' | | MeltingPt = −17.5 °C (255.7 K) ''decomp.'' | ||
| − | | Density = | + | | Density = 4.10 g cm<sup>−3</sup> |
| Appearance = dark brown solid | | Appearance = dark brown solid | ||
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==Structure== | ==Structure== | ||
| − | Dibromine monoxide has a bent ''C''<sub>2v</sub> structure in the vapour phase, with ''r''(Br–O) = 184.29(20) pm, ''θ''(Br–O–Br) = 112.24(20)°.<ref>{{citation | first1 = Holger S. P. | last1 = Müller | first2 = Edward A. | last2 = Cohen | title = Dibromine monoxide, Br<sub>2</sub>O: The rotational spectrum and molecular properties | journal = J. Chem. Phys. | volume = 106 | issue = 20 | pages = 8344–54 | year = 1997 | doi = 10.1063/1.473920}}.</ref> In the solid state, the symmetry is lower, with slightly different Br–O distances and ''θ''(Br–O–Br) = 114.2(2)°.<ref name="Xstal"/> Solid Br<sub>2</sub>O has also been studied by [[EXAFS]].<ref>{{citation | first1 = William | last1 = Levason | first2 = J. Steven | last2 = Ogden | first3 = Mark D. | last3 = Spicer | first4 = Nigel A. | last4 = Young | title = Characterization of dibromine monoxide (Br<sub>2</sub>O) by bromine K-edge EXAFS and IR spectroscopy | journal = J. Am. Chem. Soc. | year = 1990 | volume = 112 | issue = 3 | pages = 1019–22 | doi = 10.1021/ja00159a019}}.</ref> | + | Dibromine monoxide has a bent ''C''<sub>2v</sub> structure in the vapour phase, with ''r''(Br–O) = 184.29(20) pm, ''θ''(Br–O–Br) = 112.24(20)°.<ref>{{citation | first1 = Holger S. P. | last1 = Müller | first2 = Edward A. | last2 = Cohen | title = Dibromine monoxide, Br<sub>2</sub>O: The rotational spectrum and molecular properties | journal = J. Chem. Phys. | volume = 106 | issue = 20 | pages = 8344–54 | year = 1997 | doi = 10.1063/1.473920}}.</ref> In the solid state, the symmetry is lower, with slightly different Br–O distances (185.7(5), 187.5(5) pm) and ''θ''(Br–O–Br) = 114.2(2)°.<ref name="Xstal"/> Solid Br<sub>2</sub>O has also been studied by [[EXAFS]].<ref>{{citation | first1 = William | last1 = Levason | first2 = J. Steven | last2 = Ogden | first3 = Mark D. | last3 = Spicer | first4 = Nigel A. | last4 = Young | title = Characterization of dibromine monoxide (Br<sub>2</sub>O) by bromine K-edge EXAFS and IR spectroscopy | journal = J. Am. Chem. Soc. | year = 1990 | volume = 112 | issue = 3 | pages = 1019–22 | doi = 10.1021/ja00159a019}}.</ref> |
==Notes and references== | ==Notes and references== | ||
Revision as of 09:52, 1 January 2011
| Dibromine monoxide | |
|---|---|
| IUPAC name | Oxygen dibromide |
| Other names | Hypobromous anhydride |
| Identifiers | |
| InChI | InChI=1/Br2O/c1-3-2 |
| InChIKey | HJCMMOODWZOXML-UHFFFAOYAD |
| Standard InChI | InChI=1S/Br2O/c1-3-2 |
| Standard InChIKey | HJCMMOODWZOXML-UHFFFAOYSA-N |
| CAS number | [] |
| ChemSpider | |
| Properties[1][2][3] | |
| Chemical formula | Br2O |
| Molar mass | 175.81 g mol−1 |
| Appearance | dark brown solid |
| Density | 4.10 g cm−3 |
| Melting point |
−17.5 °C (255.7 K) decomp. |
| Structure[3] | |
| Space group | Pc21n (No. 33) |
| Lattice constant | a = 390.4(1) pm, b = 686.2(1) pm, c = 1062.2(2) pm |
| Thermochemistry[4] | |
| Std enthalpy of formation ΔfH |
+107.1(35) kJ mol−1 |
| Related compounds | |
| Other cations | Difluorine monoxide Dichlorine monoxide |
| Other oxides of bromine | Bromine dioxide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Dibromine monoxide, Br2O, is a binary compound of bromine and oxygen. It is prepared by the reaction of bromine with mercury(II) oxide[5][6] or by the low temperature decomposition of bromine dioxide in vacuo.[7][8]
Structure
Dibromine monoxide has a bent C2v structure in the vapour phase, with r(Br–O) = 184.29(20) pm, θ(Br–O–Br) = 112.24(20)°.[9] In the solid state, the symmetry is lower, with slightly different Br–O distances (185.7(5), 187.5(5) pm) and θ(Br–O–Br) = 114.2(2)°.[3] Solid Br2O has also been studied by EXAFS.[10]
Notes and references
Notes
References
- ↑ Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 996–97. ISBN 0-08-022057-6.
- ↑ Cotton, F. Albert; Wilkinson, Geoffrey Advanced Inorganic Chemistry, 5th ed.; Wiley-Interscience: New York, 1988; p 562. ISBN 0-471-84997-9.
- ↑ 3.0 3.1 3.2 Hwang, In-Chur; Kuschel, Raimund; Seppelt, Konrad Structures of Bromine Oxygen Compounds. Z. Anorg. Allg. Chem., 623 (1–6), 379–83. DOI: 10.1002/zaac.19976230160.
- ↑ Thorn, R. Peyton, Jr.; Monks, Paul S.; Stief, Louis J.; Kuo, Szu-Cherng; Zhang, Zhengyu; Klemm, R. Bruce Photoionization Efficiency Spectrum, Ionization Energy, and Heat of Formation of Br2O. J. Phys. Chem. 1996, 100 (30), 12199–203. DOI: 10.1021/jp960405z.
- ↑ Zintl, E.; Rienäcker, G. Über die Existenz eines flüchtigen Bromoxyds. Ber. Dtsch. Chem. Ges. B 1930, 63 (5), 1098–1104. DOI: 10.1002/cber.19300630516.
- ↑ Brenschede, W.; Schumacher, H.-J. Über die Darstellung und einige Eigenschaften eines Bromoxyds von der Formel Br2O. Z. Anorg. Allg. Chem. 1936, 226 (4), 370–84. DOI: 10.1002/zaac.19362260409.
- ↑ Schwarz, R.; Wiele, H. Über das Bromoxyd Br2O. Naturwissenschaften 1938, 26 (45), 742. DOI: 10.1007/BF01774152.
- ↑ Schwarz, Robert; Wiele, Heinz Zur Kenntnis der Bromoxyde (II. Mitteilung). J. Prakt. Chem. 1938, 152 (3–6), 157–76. DOI: 10.1002/prac.19391520306.
- ↑ Müller, Holger S. P.; Cohen, Edward A. Dibromine monoxide, Br2O: The rotational spectrum and molecular properties. J. Chem. Phys. 1997, 106 (20), 8344–54. DOI: 10.1063/1.473920.
- ↑ Levason, William; Ogden, J. Steven; Spicer, Mark D.; Young, Nigel A. Characterization of dibromine monoxide (Br2O) by bromine K-edge EXAFS and IR spectroscopy. J. Am. Chem. Soc. 1990, 112 (3), 1019–22. DOI: 10.1021/ja00159a019.
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