Difference between revisions of "Perbromate"
Physchim62 (talk | contribs) (Created page with "{{chembox | OtherNames = Tetraoxidobromate(1−) | Section1 = {{Chembox Identifiers | ChemSpiderID = 4574125 | InChI=1/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | InChIKey = | S...") |
Physchim62 (talk | contribs) |
||
| Line 4: | Line 4: | ||
| ChemSpiderID = 4574125 | | ChemSpiderID = 4574125 | ||
| InChI=1/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | | InChI=1/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | ||
| − | | InChIKey = | + | | InChIKey = LLYCMZGLHLKPPU-REWHXWOFAT |
| StdInChI=1S/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | | StdInChI=1S/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 | ||
| StdInChIKey = LLYCMZGLHLKPPU-UHFFFAOYSA-M | | StdInChIKey = LLYCMZGLHLKPPU-UHFFFAOYSA-M | ||
| Line 17: | Line 17: | ||
}} | }} | ||
}} | }} | ||
| − | A '''perbromate''' is a [[salt]] or [[ester]] of [[perbromic acid]]. | + | A '''perbromate''' is a [[salt]] or [[ester]] of [[perbromic acid]]. Perbromates, including perbromic acid,<ref group=note>[[Perbromic acid]] is fully dissociated in solution. By analogy with [[perchloric acid]], the solid HBrO<sub>4</sub>·2H<sub>2</sub>O is expected to contain [(H<sub>2</sub>O)<sub>2</sub>H]</sup>+</sup>[BrO<sub>4</sub>]<sup>−</sup>.</ref> are the only well-characterized compounds of bromine in the +7 [[oxidation state]]. |
| + | |||
| + | Perbromates are thermodynamically more oxidizing than [[perchlorate]]s or [[periodate]]s, and eluded preparation for more than 100 years until 1968.<ref name="1st">{{citation | title = The Synthesis of perbromates | first = Evan H. | last = Appelman | journal = J. Am. Chem. Soc. | year = 1968 | volume = 90 | issue = 7 | pages = 1900–1 | doi = 10.1021/ja01009a040}}.</ref><ref name="G&E">{{Greenwood&Earnshaw1st|pages=1020–22}}.</ref> However, they are kinetically quite inert, especially in dilute solution.<ref name="G&E"/> | ||
==Notes and references== | ==Notes and references== | ||
| Line 27: | Line 29: | ||
===Further reading=== | ===Further reading=== | ||
| + | *{{citation | first = E. H. | last = Appelman | journal = Inorg. Chem. | volume = 8 | pages = 223 | year = 1969}}. | ||
| + | *{{citation | first1 = G. K. | last1 = Johnson | first2 = P. N. | last2 = Smith | first3 = E. H. | last3 = Appelman | first4 = W. N. | last4 = Hubbard | journal = Inorg. Chem. | volume = 9 | pages = 119 | year = 1970}}. | ||
| + | *{{citation | first1 = V. K. | last1 = Klaening | first2 = K. J. | last2 = Olsen | first3 = E. H. | last3 = Appelman | journal = J. Chem. Soc., Faraday Trans. 1 | volume = 71 | pages = 473 | year = 1975}}. | ||
| + | *{{citation | first1 = K. J. | last1 = Olsen | first2 = K. | last2 = Sehested | first3 = E. H. | last3 = Appelman | journal = Chem. Phys. Lett. | volume = 19 | pages = 213 | year = 1973}}. | ||
| + | *{{citation | title = Preparation of an alkyl perbromate | first1 = Kurt | last1 = Baum | first2 = Charles D. | last2 = Beard | first3 = Vytautas | last3 = Grakauskas | journal = J. Am. Chem. Soc. | year = 1975 | volume = 97 | issue = 2 | pages = 267–68 | doi = 10.1021/ja00835a005}}. | ||
==External links== | ==External links== | ||
Revision as of 18:44, 4 January 2011
| Perbromate | |
|---|---|
| Other names | Tetraoxidobromate(1−) |
| Identifiers | |
| InChI | InChI=1/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 |
| InChIKey | LLYCMZGLHLKPPU-REWHXWOFAT |
| Standard InChI | InChI=1S/BrHO4/c2-1(3,4)5/h(H,2,3,4,5)/p-1 |
| Standard InChIKey | LLYCMZGLHLKPPU-UHFFFAOYSA-M |
| CAS number | [] |
| ChemSpider | |
| Structure[1] | |
| Molecular geometry | r(Br–O) = 161 pm |
| Related compounds | |
| Other anions | Perchlorate Periodate |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
A perbromate is a salt or ester of perbromic acid. Perbromates, including perbromic acid,[note 1] are the only well-characterized compounds of bromine in the +7 oxidation state.
Perbromates are thermodynamically more oxidizing than perchlorates or periodates, and eluded preparation for more than 100 years until 1968.[2][3] However, they are kinetically quite inert, especially in dilute solution.[3]
Notes and references
Notes
- ↑ Perbromic acid is fully dissociated in solution. By analogy with perchloric acid, the solid HBrO4·2H2O is expected to contain [(H2O)2H]+[BrO4]−.
References
- ↑ Levason, William; Ogden, J. Steven; Spicer, Mark D.; Young, Nigel A. Characterisation of the oxo-anions of bromine BrOx− (x = 1–4) by infrared, Raman, nuclear magnetic resonance, and bromine K-edge extended X-ray absorption fine structure techniques. J. Chem. Soc., Dalton Trans. 1990 (1), 349–53. DOI: 10.1039/DT9900000349.
- ↑ Appelman, Evan H. The Synthesis of perbromates. J. Am. Chem. Soc. 1968, 90 (7), 1900–1. DOI: 10.1021/ja01009a040.
- ↑ 3.0 3.1 Greenwood, Norman N.; Earnshaw, A. Chemistry of the Elements; Pergamon: Oxford, 1984; pp 1020–22. ISBN 0-08-022057-6.
Further reading
- Appelman, E. H. Inorg. Chem. 1969, 8, 223.
- Johnson, G. K.; Smith, P. N.; Appelman, E. H.; Hubbard, W. N. Inorg. Chem. 1970, 9, 119.
- Klaening, V. K.; Olsen, K. J.; Appelman, E. H. J. Chem. Soc., Faraday Trans. 1 1975, 71, 473.
- Olsen, K. J.; Sehested, K.; Appelman, E. H. Chem. Phys. Lett. 1973, 19, 213.
- Baum, Kurt; Beard, Charles D.; Grakauskas, Vytautas Preparation of an alkyl perbromate. J. Am. Chem. Soc. 1975, 97 (2), 267–68. DOI: 10.1021/ja00835a005.
External links
 |
See also the corresponding article on Wikipedia. |
| 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. |
