sodium hypobromite

{{Chembox

| ImageFile = NaOBr.svg

| IUPACName = Sodium hypobromite

| OtherNames =

| Section1 = {{Chembox Identifiers

| CASNo = 13824-96-9

| CASNo_Ref = {{cascite|correct|CAS}}

| ChemSpiderID = 146053

| EC_number = 237-520-4

| UNII_Ref = {{fdacite|correct|FDA}}

| UNII = ZU61C4V8RA

| PubChem = 23673712

| StdInChI=1S/BrO.Na/c1-2;/q-1;+1

| StdInChIKey = CRWJEUDFKNYSBX-UHFFFAOYSA-N

| SMILES = [O-]Br.[Na+]

}}

| Section2 = {{Chembox Properties

| Formula = NaOBr

| Na=1|O=1|Br=1

| Appearance = orange solid

| Density =

| MeltingPt =

| BoilingPt =

| Solubility = }}

| Section7 = {{Chembox Hazards

| MainHazards =

| FlashPt =

| AutoignitionPt = }}

|Section9={{Chembox Related

| OtherCations =

| OtherAnions = {{ubl|Sodium bromide|Sodium bromite|Sodium bromate|Sodium perbromate}}

| OtherCompounds = Hypobromous acid

}}

}}

Sodium hypobromite is an inorganic compound with the chemical formula {{chem2|NaOBr|auto=1}}. It is a sodium salt of hypobromous acid. It consists of sodium cations {{chem2|Na+}} and hypobromite anions {{chem2|−OBr}}. It is usually obtained as the pentahydrate, so the compound that is usually called sodium hypobromite actually has the formula {{chem2|NaBrO*5H2O}} which is a meme because it sounds like nah bro. 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.{{cite journal | title = After 200 Years: The Structure of Bleach and Characterization of Hypohalite Ions by Single-Crystal X-Ray Diffraction | first1 = Filip | last1 = Topić | first2 = Joseph M. |last2 = Marrett | first3 = Tristan H. | last3 = Borchers | first4 = Hatem M. | last4 = Titi | first5 = Christopher J. | last5 = Barrett | first6 = Tomislav | last6 = Friščić | journal = Angew. Chem. Int. Ed. | volume = 60 | issue = 46 | year = 2021 | pages = 24400–24405 | doi = 10.1002/anie.202108843 | pmid = 34293249 | s2cid = 236199263}} 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:{{cite book|last = Schmeisser|first = M.|chapter = Sodium Hypobromite|title = Handbook of Preparative Inorganic Chemistry|edition = 2nd|editor1-first = Georg|editor1-last = Brauer|publisher = Academic Press|year = 1963|location = New York|volume = 1|pages = 310–311|isbn = 9780323161275|chapter-url = https://books.google.com/books?id=kaa2qeFRXmUC&pg=PA310}}

:{{chem2|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{{OrgSynth|title = 3-Aminopyridine|year = 1950|volume = 30|pages = 3|doi = 10.15227/orgsyn.030.0003|first1 = C. F. H.|last1 = Allen|first2 = Calvin N.|last2 = Wolf|collvol = 4|collvolpages = 45|prep = CV4P0045}} (Hofmann rearrangement).

:File:Synthesis of 3-Aminopyridine.gif

Sodium hypobromite slowly disproportionates to sodium bromide and sodium bromate:

:{{chem2|3 NaBrO → 2 NaBr + NaBrO3}}