Difference between revisions of "Oxides of bromine"

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The '''oxides of bromine''' are far less stable than their [[Oxides of chlorine|chlorine]] or [[Oxides of iodine|iodine]] analogues. Of the seventeen binary species that have been described, none is stable at room temperature and pressure: the reality of many of these species is dubious.<ref name="JANAF">{{citation | first = Malcolm W. | last = Chase | title = NIST–JANAF Thermochemical Tables for the Bromine Oxides | journal = J. Phys. Chem. Ref. Data | volume = 25 | issue = 4 | year = 1996 | pages = 1069–1111 | url = http://www.nist.gov/data/PDFfiles/jpcrd508.pdf}}.</ref>
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The '''oxides of bromine''' are far less stable than their [[Oxides of chlorine|chlorine]] or [[Oxides of iodine|iodine]] analogues. Of the seventeen binary species that have been described, none is stable at room temperature and pressure: the existence of many of these species is doubtful.<ref name="JANAF">{{citation | first = Malcolm W. | last = Chase | title = NIST–JANAF Thermochemical Tables for the Bromine Oxides | journal = J. Phys. Chem. Ref. Data | volume = 25 | issue = 4 | year = 1996 | pages = 1069–1111 | url = http://www.nist.gov/data/PDFfiles/jpcrd508.pdf}}.</ref><ref>{{citation | first1 = Martin | last1 = Jansen | first2 = Thorsten | last2 = Kraft | title = The Structural Chemistry of Binary Halogen Oxides in the Solid State | journal = Chem. Ber. | volume = 130 | issue = 3 | pages = 307–16 | year = 1997 | doi = 10.1002/cber.19971300302}}.</ref><ref>{{citation | title = Bromine Oxides | first = Konrad | last = Seppelt | journal = Acc. Chem. Res. | year = 1997 | volume = 30 | issue = 3 | pages = 111–13 | doi = 10.1021/ar950236l}}.</ref>
  
 
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{| class="wikitable"
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! Ref.
 
! Ref.
 
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| BrO || 23878-08-2 || || || || || || || ||
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| BrO || 15656-19-6 || || || || || || || ||
 
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|-
 
| BrO<sub>2</sub> || 21255-83-4 || OBrO || || || || || || ||
 
| BrO<sub>2</sub> || 21255-83-4 || OBrO || || || || || || ||
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| BrO<sub>4</sub> || 11092-92-5 || || || || || || || ||
 
| BrO<sub>4</sub> || 11092-92-5 || || || || || || || ||
 
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| [[Dibromine monoxide|Br<sub>2</sub>O]] || 21308-80-5 || BrOBr || align=center | 184.3<br/>185.7, 187.5 || || || align=center | <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><br/><ref>{{citation | first1 = In-Chur | last1 = Hwang | first2 = Raimund | last2 = Kuschel | first3 = Konrad | last3 = Seppelt | title = Structures of Bromine Oxygen Compounds | journal = Z. Anorg. Allg. Chem. | volume = 623 | issue = 1–6 | pages = 379–83 | doi = 10.1002/zaac.19976230160}}.</ref> || +107.1 || <ref>{{citation | title = Photoionization Efficiency Spectrum, Ionization Energy, and Heat of Formation of Br<sub>2</sub>O | first1 = R. Peyton, Jr. | last1 = Thorn | first2 = Paul S. | last2 = Monks | first3 = Louis J. | last3 = Stief | first4 = Szu-Cherng | last4 = Kuo | first5 = Zhengyu | last5 = Zhang | first6 = R. Bruce | last6 = Klemm | journal = J. Phys. Chem. | year = 1996 | volume = 100 | issue = 30 | pages = 12199–203 | doi = 10.1021/jp960405z}}.</ref> ||
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| [[Dibromine monoxide|Br<sub>2</sub>O]] || 21308-80-5 || BrOBr || align=center | 184.3<br/>185.7, 187.5 || || || align=center | <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><br/><ref>{{citation | first1 = In-Chur | last1 = Hwang | first2 = Raimund | last2 = Kuschel | first3 = Konrad | last3 = Seppelt | title = Structures of Bromine Oxygen Compounds | journal = Z. Anorg. Allg. Chem. | volume = 623 | issue = 1–6 | pages = 379–83 | doi = 10.1002/zaac.19976230160}}.</ref> || align=center | +107.1 || align=center | <ref>{{citation | title = Photoionization Efficiency Spectrum, Ionization Energy, and Heat of Formation of Br<sub>2</sub>O | first1 = R. Peyton, Jr. | last1 = Thorn | first2 = Paul S. | last2 = Monks | first3 = Louis J. | last3 = Stief | first4 = Szu-Cherng | last4 = Kuo | first5 = Zhengyu | last5 = Zhang | first6 = R. Bruce | last6 = Klemm | journal = J. Phys. Chem. | year = 1996 | volume = 100 | issue = 30 | pages = 12199–203 | doi = 10.1021/jp960405z}}.</ref> ||
 
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| Br<sub>2</sub>O || 68322-97-4 || BrBrO || || || || || || ||
 
| Br<sub>2</sub>O || 68322-97-4 || BrBrO || || || || || || ||
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==References==
 
==References==
 
{{reflist}}
 
{{reflist}}
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==Further reading==
 
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*{{citation | first1 = Martin | last1 = Jansen | first2 = Thorsten | last2 = Kraft | title = The Structural Chemistry of Binary Halogen Oxides in the Solid State | journal = Chem. Ber. | volume = 130 | issue = 3 | pages = 307–16 | year = 1997 | doi = 10.1002/cber.19971300302}}.
 
  
 
[[Category:Oxides|Bromine]]
 
[[Category:Oxides|Bromine]]

Latest revision as of 07:02, 3 January 2011

The oxides of bromine are far less stable than their chlorine or iodine analogues. Of the seventeen binary species that have been described, none is stable at room temperature and pressure: the existence of many of these species is doubtful.[1][2][3]

Formula CAS
number 		Structure Thermochemistry Notes
  r(Br–O)/pm r(Br–Br)/pm r(O–O)/pm Ref. ΔfHo298/kJ mol−1 Ref.
BrO 15656-19-6
BrO2 21255-83-4 OBrO
BrO2 67177-47-3 BrOO
BrO3 32062-14-9 C3v
BrO4 11092-92-5
Br2O 21308-80-5 BrOBr 184.3
185.7, 187.5		 [4]
[5]		 +107.1 [6]
Br2O 68322-97-4 BrBrO
Br2O2 96028-01-2 BrOOBr
Br2O3 53809-75-9 OBrOBrO
Br2O3 152172-79-7 BrOBrO2
Br2O4 141438-65-5 BrOBrO3 161(2), 186(2) [7] bromine perbromate
Br2O4 53723-86-7 O2BrBrO2
Br2O4 55589-64-5 O2BrOBrO
Br2O5 58572-43-3 O2BrOBrO2 [8]
Br2O6
Br2O7
Br3O8 121992-88-0

References

  1. ↑ Chase, Malcolm W. NIST–JANAF Thermochemical Tables for the Bromine Oxides. J. Phys. Chem. Ref. Data 1996, 25 (4), 1069–1111, <http://www.nist.gov/data/PDFfiles/jpcrd508.pdf>.
  2. ↑ Jansen, Martin; Kraft, Thorsten The Structural Chemistry of Binary Halogen Oxides in the Solid State. Chem. Ber. 1997, 130 (3), 307–16. DOI: 10.1002/cber.19971300302.
  3. ↑ Seppelt, Konrad Bromine Oxides. Acc. Chem. Res. 1997, 30 (3), 111–13. DOI: 10.1021/ar950236l.
  4. ↑ 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.
  5. ↑ 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.
  6. ↑ 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.
  7. ↑ Gilson, Trevor R.; Levason, William; Ogden, J. Steven; Spicer, Mark D.; Young, Nigel A. Bromine perbromate: synthesis and bromine K-edge EXAFS studies. J. Am. Chem. Soc. 1992, 114 (13), 5469–70. DOI: 10.1021/ja00039a093.
  8. ↑ Leopold, Dieter; Seppelt, Konrad Dibromine Pentoxide Br2O5. Angew. Chem., Int. Ed. Engl. 1994, 33 (9), 975–76. DOI: 10.1002/anie.199409751.
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