Sodium borohydride

Sodium borohydride
Names
	IUPAC name Sodium tetrahydridoborate(1–)
	Systematic IUPAC name Sodium boranuide
Identifiers
CAS Number	16940-66-2 ; 15681-89-7 (2D4) ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:50985 ;
ChemSpider	26189 ; 9052313 (2D4) ; 9312193 (3T4) ;
ECHA InfoCard	100.037.262
EC Number	241-004-4;
Gmelin Reference	23167
MeSH	Sodium+borohydride
PubChem CID	4311764; 23673181 (2D4); 23671303 (3T4);
RTECS number	ED3325000;
UNII	87L0B9CPPA ;
UN number	1426
CompTox Dashboard (EPA)	DTXSID80893977 ;
	InChI InChI=1S/BH4.Na/h1H4;/q-1;+1 Key: YOQDYZUWIQVZSF-UHFFFAOYSA-N ; InChI=1S/BH4.Na/h1H4;/q-1;+1; Key: YOQDYZUWIQVZSF-UHFFF;
	SMILES [Na+].[BH4-];
Properties
Chemical formula	Na[BH4]
Molar mass	37.83 g·mol−1
Appearance	white crystals ; hygroscopic
Density	1.07 g/cm3
Melting point	400 °C (752 °F; 673 K)(decomposes)
Solubility in water	550 g/L
Solubility	soluble in liquid ammonia, amines, pyridine
Structure
Crystal structure	Cubic (NaCl), cF8
Space group	Fm3m, No. 225
Lattice constant	a = 0.6157 nm
Thermochemistry
Heat capacity (C)	86.8 J·mol−1·K−1
Std molar; entropy (S⦵298)	101.3 J·mol−1·K−1
Std enthalpy of; formation (ΔfH⦵298)	−188.6 kJ·mol−1
Gibbs free energy (ΔfG⦵)	−123.9 kJ·mol−1
Hazards
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H260, H301, H314, H360F
Precautionary statements	P201, P231+P232, P280, P308+P313, P370+P378, P402+P404
NFPA 704 (fire diamond)	3 1 2 W
Flash point	70 °C (158 °F; 343 K)
Autoignition; temperature	ca. 220 °C (428 °F; 493 K)
Explosive limits	3%
	Lethal dose or concentration (LD, LC):
LD50 (median dose)	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). verify (what is ?) Infobox references

Sodium borohydride, also known as sodium tetrahydridoborate and sodium tetrahydroborate,^[5] is an inorganic compound with the formula Na B H₄ (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.

^ ^a ^b ^c Haynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). CRC Press. p. 4.89. ISBN 978-1439855119.
^ 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)
^ 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)
^ Record of Sodium borohydride in the GESTIS Substance Database of the Institute for Occupational Safety and Health, accessed on 2023-11-09.
^ Busch, D.H. (2009). Inorganic Syntheses. Vol. 20. Wiley. p. 137. ISBN 9780470132869. Retrieved 20 May 2015.
^ 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.
^ 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.
^ 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.

[crc-1] 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.

[google-5] Busch, D.H. (2009). Inorganic Syntheses. Vol. 20. Wiley. p. 137. ISBN 9780470132869. Retrieved 20 May 2015.

[eros-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.

[sch1945-8] 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.

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