Lithium borohydride Property

Melting point:

280 °C

Boiling point:

66°C/760mmHg

Density 

0.896 g/mL at 25 °C

Flash point:

−1 °F

storage temp. 

water-free area

solubility 

Soluble in ether, THF, and aliphatic aminesSoluble in ether, tetrahydrofuran, aliphatic amines and ethanol.

form 

Powder

color 

White

Specific Gravity

0.66

explosive limit

4.00-75.60%(V)

Water Solubility 

soluble H2O above pH 7, ether, tetrahydrofuran, aliphatic amines [MER06]

Sensitive 

Air & Moisture Sensitive

Merck 

14,5525

CAS DataBase Reference

16949-15-8(CAS DataBase Reference)

NIST Chemistry Reference

Lithium tetrahydroborate(16949-15-8)

EPA Substance Registry System

Borate(1-), tetrahydro-, lithium (16949-15-8)

Safety

Hazard Codes 

F,T,C,Xn,F+

Risk Statements 

14/15-23/24/25-34-20/21/22-11-40-36/37/38-19-67-66-22-12

Safety Statements 

26-36/37/39-43-45-36/37-16

RIDADR 

UN 3399 4.3/PG 1

WGK Germany 

2

RTECS 

ED2725000

F 

10-21

TSCA 

Yes

HS Code 

2850 00 20

HazardClass 

4.3

PackingGroup 

I

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Danger

Hazard statements

H260In contact with water releases flammable gases which may ignite spontaneously

H301Toxic if swalloed

H314Causes severe skin burns and eye damage

Precautionary statements

P231+P232Handle under inert gas. Protect from moisture.

P260Do not breathe dust/fume/gas/mist/vapours/spray.

P280Wear protective gloves/protective clothing/eye protection/face protection.

P303+P361+P353IF ON SKIN (or hair): Remove/Take off Immediately all contaminated clothing. Rinse SKIN with water/shower.

P305+P351+P338IF IN EYES: Rinse cautiously with water for several minutes. Remove contact lenses, if present and easy to do. Continuerinsing.

Lithium borohydride Chemical Properties,Usage,Production

Physical Properties

White orthorhombic crystals; density 0.67 g/cm3; decomposes in moist air; melts at 268°C; decomposes at 380°C; reacts with water; dissolves in ether, tetrahydrofuran, and diethylamine; solubility in ether, 25g/L at 25°C.

Uses

Lithium borohydride is used as a strong reducing agent. Its principal applications are in organic syntheses for reducing carbonyl groups such as aldehydes, ketones, and esters. It also is used for selectively reducing a carbonyl group in the presence of a nitrile group. Such selective reduction cannot be achieved with lithium aluminum hydride, which is a much stronger reducing agent. The compound also is used to detect free carbonyl groups in proteins and peptides.

Preparation

Lithium borohydride is prepared by reacting ethyllithium with aluminum borohydride:
C2H5Li + Al(BH4)3→3LiBH4 + Al(C2H5)3
Alternatively, the compound may be obtained by the reaction of ethyllithium with diborane:
C2H5Li + B2H6→LiBH4 + C2H5BH2

Reactions

Lithium borohydride reacts with water with liberation of hydrogen:
LiBH4 + 2H2O → LiBO2 + 4H2
Reaction with methanol yields lithium boromethoxide and hydrogen:
LiBH4 + 2CH3OH → LiB(OCH3)2 + 3H2
Reaction with hydrogen chloride yields diborane, lithium chloride and hydrogen:
2LiBH4 + 2HCl → 2LiCl + B2H6 + 2H2
Reactions with oxidizing agents are violent.

Chemical Properties

WHITE POWDER

Physical properties

White orthorhombic crystals; density 0.67 g/cm³; decomposes in moist air; melts at 268°C; decomposes at 380°C; reacts with water; dissolves in ether, tetrahydrofuran, and diethylamine; solubility in ether, 25g/L at 25°C.

Uses

Strong reducing agent. Used to reduce compounds containing ketones, aldehydes, ester carbonyls, acid chlorides, lactones, and epoxidesLithium borohydride is a versatile reducing agent for aldehydes, ketones, nitriles, primary amides, acid chlorides, lactones, epoxides, and esters. It is involved in the preparation of intercalation compounds and nanocomposites. It is used as a precursor for other borohydrides and acts as a catalyst in hydroboration reactions. It is known to be good reversible storage compound for anhydrous ammonia and hydrogen.

Uses

Lithium borohydride (LiBH₄) is a complex hydride with a high hydrogen density. It is a strong reducing agent and an electrode material. It has a high gravimetric (18.4 wt%) and volumetric (121 kg/m³) hydrogen storage capacities. It can also be used in lithium-ion batteries.

Uses

Strong reducing agent. Used in the reduction of Compounds contg ketonic, aldehydic, or ester carbonyls and a nitrile group, where reduction of the carbonyl, but not of the nitrile group, is wanted. In the determination of free carboxyl groups in peptides and proteins; after esterification and acetylation, only the ester groups, and none of the peptide bonds are reduced.

General Description

A white to grayish crystalline powder.

Air & Water Reactions

Likely to ignite when moistened with water [Lab. Gov. Chemist 1965].

Reactivity Profile

Lithium borohydride is a strong reducing agent. Is easily ignited and burns vigorously once ignited. Reacts on contact with water or acids to form hydrogen gas and corrosive products. Reaction with limited amounts of water or moisture may cause ignition after a delay [Gaylord, 1965, p. 22].

Health Hazard

Inhalation or contact with vapors, substance or decomposition products may cause severe injury or death. May produce corrosive solutions on contact with water. Fire will produce irritating, corrosive and/or toxic gases. Runoff from fire control may cause pollution.

Fire Hazard

Produce flammable gases on contact with water. May ignite on contact with water or moist air. Some react vigorously or explosively on contact with water. May be ignited by heat, sparks or flames. May re-ignite after fire is extinguished. Some are transported in highly flammable liquids. Runoff may create fire or explosion hazard.

Safety Profile

Poison by ingestion, inhalation, and skin contact. Flammable; can liberate H2. Incompatible with H20 as moisture on fibers of cellulose or as liquid. See also LITHIUM, BORON COMPOUNDS, and HYDRIDES.

Purification Methods

It is crystallised from Et2O, and pumped free of ether at 90-100o during 2hours [Schaeffer et al. J Am Chem Soc 78 729 1956]. Store it dry as it decomposes slowly in moist air. [Becher in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 775 1963.]