Sodium borohydride

Sodium borohydride
Wireframe model of sodium borohydride
Names
IUPAC name
Sodium tetrahydridoborate(1–)
Systematic IUPAC name
Sodium boranuide
Identifiers
3D model (JSmol)
ChEBI
ChemSpider
ECHA InfoCard 100.037.262 Edit this at Wikidata
EC Number
  • 241-004-4
23167
MeSH Sodium+borohydride
RTECS number
  • ED3325000
UNII
UN number 1426
  • InChI=1S/BH4.Na/h1H4;/q-1;+1 checkY
    Key: YOQDYZUWIQVZSF-UHFFFAOYSA-N checkY
  • InChI=1S/BH4.Na/h1H4;/q-1;+1
  • Key: YOQDYZUWIQVZSF-UHFFF
  • [Na+].[BH4-]
Properties
Na[BH4]
Molar mass 37.83 g·mol−1
Appearance white crystals
hygroscopic
Density 1.07 g/cm3[1]
Melting point 400 °C (752 °F; 673 K)(decomposes)[1]
550 g/L[1]
Solubility soluble in liquid ammonia, amines, pyridine
Structure[2]
Cubic (NaCl), cF8
Fm3m, No. 225
a = 0.6157 nm
Thermochemistry[3]
86.8 J·mol−1·K−1
101.3 J·mol−1·K−1
−188.6 kJ·mol−1
−123.9 kJ·mol−1
Hazards
GHS labelling:[4]
GHS02: FlammableGHS06: ToxicGHS08: Health hazardGHS05: Corrosive
Danger
H260, H301, H314, H360F
P201, P231+P232, P280, P308+P313, P370+P378, P402+P404
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 1: Must be pre-heated before ignition can occur. Flash point over 93 °C (200 °F). E.g. canola oilInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
1
2
Flash point 70 °C (158 °F; 343 K)
ca. 220 °C (428 °F; 493 K)
Explosive limits 3%
Lethal dose or concentration (LD, LC):
160 mg/kg (Oral – Rat)
230 mg/kg (Dermal – Rabbit)
Related compounds
Other anions
Sodium cyanoborohydride
Sodium hydride
Sodium borate
Borax
Sodium aluminum hydride
Other cations
Lithium borohydride
Related compounds
Lithium aluminium hydride
Sodium triacetoxyborohydride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate,[5] is an inorganic compound with the formula NaBH4 (sometimes written as Na[BH4]). It is a white crystalline solid, usually encountered as an aqueous basic solution. Sodium borohydride is a reducing agent that finds application in papermaking and dye industries. It is also used as a reagent in organic synthesis.[6]

The compound was discovered in the 1940s by H. I. Schlesinger, who led a team seeking volatile uranium compounds.[7][8] Results of this wartime research were declassified and published in 1953.

  1. ^ a b c Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.89. ISBN 978-1439855119.
  2. ^ Ford, P. T. and Powell, H. M. (1954). "The unit cell of potassium borohydride, KBH4, at 90° K". Acta Crystallogr. 7 (8): 604–605. Bibcode:1954AcCry...7..604F. doi:10.1107/S0365110X54002034.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  3. ^ CRC handbook of chemistry and physics : a ready-reference book of chemical and physical data. William M. Haynes, David R. Lide, Thomas J. Bruno (2016-2017, 97th ed.). Boca Raton, Florida. 2016. ISBN 978-1-4987-5428-6. OCLC 930681942.{{cite book}}: CS1 maint: location missing publisher (link) CS1 maint: others (link)
  4. ^ Record of Sodium borohydride in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2023-11-09.
  5. ^ Busch, D.H. (2009). Inorganic Syntheses. Vol. 20. Wiley. p. 137. ISBN 9780470132869. Retrieved 20 May 2015.
  6. ^ Banfi, Luca; Narisano, Enrica; Riva, Renata; Stiasni, Nikola; Hiersemann, Martin; Yamada, Tohru; Tsubo, Tatsuyuki (2014). "Sodium Borohydride". Encyclopedia of Reagents for Organic Synthesis. pp. 1–13. doi:10.1002/047084289X.rs052.pub3. ISBN 9780470842898.
  7. ^ Schlesinger, H. I.; Brown, H. C.; Abraham, B.; Bond, A. C.; Davidson, N.; Finholt, A. E.; Gilbreath, J. R.; Hoekstra, H.; Horvitz, L.; Hyde, E. K.; Katz, J. J.; Knight, J.; Lad, R. A.; Mayfield, D. L.; Rapp, L.; Ritter, D. M.; Schwartz, A. M.; Sheft, I.; Tuck, L. D.; Walker, A. O. (1953). "New developments in the chemistry of diborane and the borohydrides. General summary". J. Am. Chem. Soc. 75: 186–90. doi:10.1021/ja01097a049.
  8. ^ Hermann I Schlesinger and Herbert C Brown (1945) "Preparation of alkali metal compounds". US Patent 2461661. Granted on 1949-02-15; expired on 1966-02-15.