Difference between revisions of "Oxides of bromine"

From WikiChem
Jump to: navigation, search
(Created page with "The '''oxides of bromine''' are far less stable than their chlorine or iodine analogues. Of the seventeen binary species that have bee...")
 
Line 1: Line 1:
 
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>
 
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>
 +
 +
{| class="wikitable"
 +
|-
 +
! rowspan=2 | Formula
 +
! colspan=5 | Structure
 +
! colspan=2 | Thermochemistry
 +
! rowspan=2 | Notes
 +
|-
 +
! &nbsp;
 +
! ''r''(Br–O)
 +
! ''r''(Br–Br)
 +
! ''r''(O–O)
 +
! Ref.
 +
! Δ<sub>f</sub>''H''{{su|p=<s>o</s>|b=298}}/kJ mol<sup>−1</sup>
 +
! Ref.
 +
|-
 +
| BrO || || || || || || || ||
 +
|-
 +
| BrO<sub>2</sub> || OBrO || || || || || || ||
 +
|-
 +
| BrO<sub>2</sub> || BrOO || || || || || || ||
 +
|-
 +
| BrO<sub>3</sub> || ''C''<sub>3v</sub> || || || || || || ||
 +
|-
 +
| BrO<sub>4</sub> || || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O || BrOBr || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O || BrBrO || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>2</sub> || BrOOBr || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>3</sub> || OBrOBrO || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>4</sub> || BrOBrO<sub>3</sub> || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>4</sub> || O<sub>2</sub>BrBrO<sub>2</sub> || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>4</sub> || O<sub>2</sub>BrOBrO || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>5</sub> || O<sub>2</sub>BrOBrO<sub>2</sub> || || || || || || ||
 +
|-
 +
| Br<sub>2</sub>O<sub>6</sub> ||
 +
|-
 +
| Br<sub>2</sub>O<sub>7</sub> ||
 +
|-
 +
| Br<sub>2</sub>O<sub>3</sub> || || || || || || || ||
 +
|-
 +
|}
  
 
==References==
 
==References==

Revision as of 18:08, 2 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 reality of many of these species is dubious.[1]

Formula Structure Thermochemistry Notes
  r(Br–O) r(Br–Br) r(O–O) Ref. ΔfHo298/kJ mol−1 Ref.
BrO
BrO2 OBrO
BrO2 BrOO
BrO3 C3v
BrO4
Br2O BrOBr
Br2O BrBrO
Br2O2 BrOOBr
Br2O3 OBrOBrO
Br2O4 BrOBrO3
Br2O4 O2BrBrO2
Br2O4 O2BrOBrO
Br2O5 O2BrOBrO2
Br2O6
Br2O7
Br2O3

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>.
Error creating thumbnail: Unable to save thumbnail to destination
 This page is currently licensed under the Creative Commons Attribution 3.0 Unported license and any later versions of that license.
Retrieved from "https://wiki.potsdam.edu/wikichem/index.php?title=Oxides_of_bromine&oldid=11396"