Sodium hypobromite

Sodium hypobromite
Names

IUPAC name Sodium hypobromite
Identifiers
CAS Number	13824-96-9^Y
3D model (JSmol)	Interactive image
ChemSpider	146053
ECHA InfoCard	100.034.096
EC Number	237-520-4
PubChem CID	23673712
UNII	ZU61C4V8RA^Y
CompTox Dashboard (EPA)	DTXSID40930039
InChI InChI=1S/BrO.Na/c1-2;/q-1;+1 Key: CRWJEUDFKNYSBX-UHFFFAOYSA-N
SMILES [O-]Br.[Na+]
Properties
Chemical formula	NaOBr
Molar mass	118.893 g·mol⁻¹
Appearance	orange solid
Related compounds
Other anions	Sodium bromide Sodium bromite Sodium bromate Sodium perbromate
Related compounds	Hypobromous acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). Infobox references

Chemical compound

Sodium hypobromite is an inorganic compound with the chemical formula Na O Br. It is a sodium salt of hypobromous acid. It consists of sodium cations Na⁺ and hypobromite anions ⁻OBr. It is usually obtained as the pentahydrate, so the compound that is usually called sodium hypobromite actually has the formula NaOBr·5H₂O. It is a yellow-orange solid that is soluble in water. It adopts a monoclinic crystal structure with a Br–O bond length of 1.820 Å.^[1] It is the bromine analogue of sodium hypochlorite, the active ingredient in common bleach. In practice the salt is usually encountered as an aqueous solution.

Sodium hypobromite arises by treatment of aqueous solution of bromine with base:^[2]

Br₂ + 2 NaOH → NaBr + NaOBr + H₂O

It can be prepared in situ for use as a reagent, such as in the synthesis of 3-aminopyridine from nicotinamide^[3] (Hofmann rearrangement).

References

^ Topić, Filip; Marrett, Joseph M.; Borchers, Tristan H.; Titi, Hatem M.; Barrett, Christopher J.; Friščić, Tomislav (2021). "After 200 Years: The Structure of Bleach and Characterization of Hypohalite Ions by Single-Crystal X-Ray Diffraction". Angew. Chem. Int. Ed. 60 (46): 24400–24405. doi:10.1002/anie.202108843. PMID 34293249. S2CID 236199263.
^ Schmeisser, M. (1963). "Sodium Hypobromite". In Brauer, Georg (ed.). Handbook of Preparative Inorganic Chemistry. Vol. 1 (2nd ed.). New York: Academic Press. pp. 310–311. ISBN 9780323161275.
^ Allen, C. F. H.; Wolf, Calvin N. (1950). "3-Aminopyridine". Organic Syntheses. 30: 3. doi:10.15227/orgsyn.030.0003; Collected Volumes, vol. 4, p. 45.

Sodium compounds

Inorganic

Halides	NaF NaHF₂ NaCl NaBr NaI NaAt
Chalcogenides	NaO₃ NaO₂ Na₂O Na₂O₂ NaOH NaOD Na₂S NaSH Na₂Se NaSeH Na₂Te NaHTe Na₂Po
Pnictogenides	Na₃N NaN₃ NaNH₂ Na₃P Na₃As
Oxyhalides	NaClO NaClO₂ NaClO₃ NaClO₄ NaBrO NaBrO₂ NaBrO₃ NaBrO₄ NaIO₃ NaIO₄
Oxychalcogenides	Na₂SO₃ Na₂SO₄ NaHSO₃ NaHSO₄ Na₂S₂O₃ Na₂S₂O₄ Na₂S₂O₅ Na₂S₂O₆ Na₂S₂O₇ Na₂S₂O₈ Na₂SeO₃ Na₂SeO₄ NaHSeO₃ Na₂TeO₃
Oxypnictogenides	NaNO₂ NaNO₃ Na₂N₂O₂ NaH₂PO₄ NaPO₂H₂ Na₂HPO₃ Na₂PO₃F Na₃PS₂O₂ Na₃PO₄ Na₅P₃O₁₀ Na₄P₂O₇ Na₂H₂P₂O₇ Na₃AsO₃ Na₃AsO₄ Na₂HAsO₄ NaH₂AsO₄ NaSbO₃
Others	NaAlH₄ NaAlO₂ Na₃AlF₆ NaAl(SO₄)₂ NaAuCl₄ Na₂TiF₆ NaBH₄ NaBH₃(CN) NaBO₂ Na₂B₄O₇ Na₂B₂O₉ Na₂B₈O₁₃ NaBiO₃ NaCN NaCNO NaCoO₂ NaH NaHCO₃ Na₄XeO₆ NaHXeO₄ NaMnO₄ NaOCN NaReO₄ NaSCN NaTcO₃ NaTcO₄ NaVO₃ Na₂CO₃ Na₂C₂O₄ Na₂C₃S₅ Na₂CrO₄ Na₂Cr₂O₇ Na₂Cr₃O₁₀ Na₂GeO₃ Na₂He Na₂[Fe(CO)₄] Na₂MnO₄ Na₂MoO₄ Na₃IrCl₆ Na₂PtCl₆ Na₂O(UO₃)₂ Na₂S₄O₆ Na₂SiO₃ Na₂TiO₃ Na₂U₂O₇ Na₂WO₄ Na₂Zn(OH)₄ Na₃VO₄ Na₆V₁₀O₂₈ Na₄Fe(CN)₆ Na₃Fe(CN)₆ Na₃Fe(C₂O₄)₃ Na₄SiO₄ Na₂SiF₆ Na₃[Co(NO₂)₆] NaNSi₆ Na₂PdCl₄