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词条 Sodium bromide
释义

  1. Synthesis, structure, reactions

  2. Applications

     Medicine  Preparation of other bromine compounds  Disinfectant  Petroleum industry 

  3. Safety

  4. References

  5. External links

{{chembox
| Verifiedfields = changed
| Watchedfields = changed
| verifiedrevid = 422030388
| Name = Sodium bromide
| ImageFile = Sodium-bromide-3D-ionic.png
| ImageSize = 150px
| ImageName = 3D model of sodium bromide
| ImageFile1 = Sodium bromide.jpg
| ImageSize1 = 200px
| ImageName1 = Sodium bromide powder
| IUPACName = Sodium bromide
| OtherNames =
|Section1={{Chembox Identifiers
| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
| ChemSpiderID = 22712
| ChEMBL_Ref = {{ebicite|changed|EBI}}
| ChEMBL = 1644694
| UNII_Ref = {{fdacite|correct|FDA}}
| UNII = LC1V549NOM
| InChI = 1/BrH.Na/h1H;/q;+1/p-1
| InChIKey = JHJLBTNAGRQEKS-REWHXWOFAR
| SMILES = [Na+].[Br-]
| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
| StdInChI = 1S/BrH.Na/h1H;/q;+1/p-1
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
| StdInChIKey = JHJLBTNAGRQEKS-UHFFFAOYSA-M
| CASNo = 7647-15-6
| CASNo_Ref = {{cascite|correct|CAS}}
| CASNo1 = 13466-08-5
| CASNo1_Comment = (dihydrate)
| CASNo1_Ref = {{cascite|changed|CAS}}
| PubChem = 253881
| RTECS = VZ3150000
|Section2={{Chembox Properties
| Na=1|Br=1
| Appearance = White powder, hygroscopic
| Density = 3.21 g/cm3 (anhydrous)
2.18 g/cm3 (dihydrate)
| Solubility = 71.35 g/100 mL (−20 °C)
79.52 g/100 mL (0 °C)
94.32 g/100 mL (25 °C)[1]
104.9 g/100 mL (40 °C)
116.2 g/100 mL (100 °C)[2]
| Solubility1 = 17.3 g/100 g (0 °C)
16.8 g/100 g (20 °C)
16.1 g/100 g (40 °C)
15.3 g/100 g (60 °C)[1]
| Solvent1 = methanol
| Solubility2 = 2.45 g/100 g (0 °C)
2.32 g/100 g (20 °C)
2.29 g/100 g (30 °C)
2.35 g/100 g (70 °C)[1]
| Solvent2 = ethanol
| Solubility3 = 19.3 g/100 g (18 °C)
19.4 g/100 g (25 °C)[1]
| Solvent3 = formic acid
| Solubility4 = 38.7 g/100 g (20 °C)[1]
| Solvent4 = glycerol
| Solubility5 = 3.2 g/100 g (10.3 °C)[1]
| Solvent5 = dimethylformamide
| SolubleOther = Soluble in alcohol, liquid ammonia, pyridine, hydrazine, SO2, amine
Insoluble in acetone, acetonitrile[1]
| MeltingPtC = 747
| MeltingPt_notes =
(anhydrous)
{{convert|36|C|F K}}
(dihydrate) decomposes[3]
| BoilingPtC = 1390
| BoilingPt_notes = [3]
| RefractIndex = 1.6428 (24 °C)
nKrF = 1.8467 (24 °C)
nHe–Ne = 1.6389 (24 °C)[4]
| Viscosity = 1.42 cP (762 °C)
1.08 cP (857 °C)
0.96 cP (937 °C)[1]
| VaporPressure = 1 torr (806 °C)
5 torr (903 °C)[3]
| ThermalConductivity = 5.6 W/m·K (150 K)[5]
| MagSus = −41.0·10−6 cm3/mol
|Section4={{Chembox Structure
| CrystalStruct = Cubic
| LattConst_a = 5.97 Å[5]
|Section5={{Chembox Thermochemistry
| DeltaHf = −361.41 kJ/mol[1]
| DeltaGf = −349.3 kJ/mol[1]
| Entropy = 86.82 J/mol·K[1]
| HeatCapacity = 51.4 J/mol·K[1]
|Section7={{Chembox Hazards
| ExternalSDS = External MSDS
| FlashPtC = 800
| LD50 = 3500 mg/kg (rats, oral)
| NFPA-H = 2
| NFPA-F = 0
| NFPA-R = 0
| NFPA_ref = [20]
|Section8={{Chembox Related
| OtherAnions = Sodium fluoride
Sodium chloride
Sodium iodide
Sodium astatide
| OtherCations = Lithium bromide
Potassium bromide
Rubidium bromide
Caesium bromide
Francium bromide
}}Sodium bromide is an inorganic compound with the formula NaBr. It is a high-melting white, crystalline solid that resembles sodium chloride. It is a widely used source of the bromide ion and has many applications.[6]

Synthesis, structure, reactions

NaBr crystallizes in the same cubic motif as NaCl, NaF and NaI. The anhydrous salt crystallizes above 50.7 °C.[6] Dihydrate salts (NaBr·2H2O) crystallize out of water solution below 50.7 °C.[7]

NaBr is produced by treating sodium hydroxide with hydrogen bromide.

Sodium bromide can be used as a source of the chemical element bromine. This can be accomplished by treating an aqueous solution of NaBr with chlorine gas:

2 NaBr + Cl2 → Br2 + 2 NaCl

Applications

Sodium bromide is the most useful inorganic bromide in industry.[6] It is also used as a catalyst in TEMPO-mediated oxidation reactions.[8]

Medicine

{{see also|Potassium bromide#Medical and Veterinary}}

Also known as Sedoneural, sodium bromide has been used as a hypnotic, anticonvulsant, and sedative in medicine, widely used as an anticonvulsant and a sedative in the late 19th and early 20th centuries. Its action is due to the bromide ion, and for this reason potassium bromide is equally effective. In 1975, bromides were removed from drugs in the U.S. such as Bromo-Seltzer due to toxicity.[9]

Preparation of other bromine compounds

Sodium bromide is widely used for the preparation of other bromides in organic synthesis and other areas. It is a source of the bromide nucleophile to convert alkyl chlorides to more reactive alkyl bromides by the Finkelstein reaction:

NaBr + RCl → RBr + NaCl (R = alkyl)

Once a large need in photography, but now shrinking, the photosensitive salt silver bromide is prepared using NaBr.

Disinfectant

Sodium bromide is used in conjunction with chlorine as a disinfectant for hot tubs and swimming pools.

Petroleum industry

Sodium bromide is used to prepare dense fluids used in oil wells.

Safety

NaBr has a very low toxicity with an oral {{LD50}} estimated at 3.5 g/kg for rats.[10] However, this is a single-dose value. Bromide ion is a cumulative toxin with a relatively long half life (in excess of a week in humans): see potassium bromide.

References

1. ^1 2 3 4 5 6 7 8 9 10 11 {{Cite web | url=http://chemister.ru/Database/properties-en.php?dbid=1&id=714 | title=Sodium bromide}}
2. ^{{cite book|last = Seidell|first = Atherton|last2 = Linke|first2 = William F.|year = 1919|title = Solubilities of Inorganic and Organic Compounds|publisher = D. Van Nostrand Company|edition = 2nd}}
3. ^1 2 {{cite book|last = Pradyot|first = Patnaik|year = 2003|title = Handbook of Inorganic Chemicals|publisher = The McGraw-Hill Companies, Inc.|isbn = 978-0-07-049439-8}}
4. ^{{cite web|url = http://refractiveindex.info/?shelf=main&book=NaBr&page=Li|title = Refractive index of NaBr (Sodium bromide) - Li|website = refractiveindex.info|first = Mikhail|last = Polyanskiy|accessdate = 2014-06-11}}
5. ^1 {{cite web|url = http://www.korth.de/index.php/162/items/23.html|title = Sodium Bromide (NaBr)|website = korth.de|publisher = Korth Kristalle GmbH|accessdate = 2014-06-11}}
6. ^1 2 Michael J. Dagani, Henry J. Barda, Theodore J. Benya, David C. Sanders "Bromine Compounds" in Ullmann's Encyclopedia of Industrial Chemistry Wiley-VCH, Weinheim, 2000. {{DOI|10.1002/14356007.a04_405}}
7. ^{{cite book|last=Eagleson|first=Mary (translated by)|title=Concise Encyclopedia Chemistry|date=1994|publisher=Walter De Gruyter|location=Berlin [u.a.]|isbn=9783110114515|pages=996|edition=Illustrated, revised, English language}}
8. ^{{cite journal | doi=10.1007/s10570-009-9381-2 | volume=17 | issue=2 | title=Water dispersion of cellulose II nanocrystals prepared by TEMPO-mediated oxidation of mercerized cellulose at pH 4.8 | journal=Cellulose | pages=279–288|year = 2010|last1 = Hirota|first1 = Masayuki| last2=Tamura | first2=Naoyuki | last3=Saito | first3=Tsuguyuki | last4=Isogai | first4=Akira }}
9. ^{{cite web|url = http://www.canine-epilepsy.com/Bromide.html|title = Bromide: Potassium & Sodium|website = canine-epilepsy.com|publisher = Canine-Epilepsy Resources|date = 2011-05-31|accessdate = 2014-06-11}}
10. ^1 {{cite web|url = http://www.sciencelab.com/msds.php?msdsId=9927262|title = Sodium bromide MSDS|website = sciencelab.com|publisher = Sciencelab.com, Inc.|date = 2013-05-21|accessdate = 2014-06-11|format = PDF}}

External links

{{Commons category|Sodium bromide}}
  • Information about NaBr.
  • Bromide Poisoning in Angola
{{Sodium compounds}}{{Inorganic bromides}}{{Hypnotics and sedatives}}{{Anticonvulsants}}{{GABAAR PAMs}}{{bromine compounds}}{{Authority control}}{{DEFAULTSORT:Sodium Bromide}}

5 : Sodium compounds|Bromides|GABAA receptor positive allosteric modulators|Sedatives|Alkali metal bromides
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