Magnesium bromide Property

Melting point:

711 °C (lit.)

Boiling point:

1248.47°C (estimate)

Density 

3.72 g/mL at 25 °C (lit.)

solubility 

DMSO (Slightly, Heated), Methanol (Slightly), Water (Slightly)

form 

Powder

color 

off-white

Specific Gravity

3.72

Water Solubility 

g/100g H2O: 100.6 (25°C), 125.4 (100°C); solid phase, MgBr2 ·6H2O [KRU93]

Merck 

13,5681

Stability:

hygroscopic

CAS DataBase Reference

7789-48-2(CAS DataBase Reference)

NIST Chemistry Reference

Magnesium dibromide(7789-48-2)

EPA Substance Registry System

Magnesium bromide (MgBr2) (7789-48-2)

Safety

Hazard Codes 

Xi

Risk Statements 

36/37/38

Safety Statements 

26-36

WGK Germany 

1

HS Code 

28275900

Hazard and Precautionary Statements (GHS)

Symbol(GHS)

Signal word

Warning

Hazard statements

H315Causes skin irritation

H319Causes serious eye irritation

H335May cause respiratory irritation

Precautionary statements

P261Avoid breathing dust/fume/gas/mist/vapours/spray.

P271Use only outdoors or in a well-ventilated area.

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

Magnesium bromide Chemical Properties,Usage,Production

Chemical Properties

Magnesium Bromide is a colorless, very deliquescent crystals or white solid; bitter taste. Soluble in water; slightly soluble in alcohol. It formed by reaction of magnesium carbonate and hydrobromic acid.

Physical properties

The anhydrous MgBr2 is a white crystalline substance; hexagonal crystals; deliquescent; density 3.72 g/cm3; melts at 700°C; highly soluble in water (101.5g/100mL at 20°C); moderately soluble in methanol and ethanol (21.8 and 6.9 g/mL at 20°C, respectively).
The hexahydrate, MgBr2.6H2O consists of colorless monoclinic crystals; bitter taste; hygroscopic; fluoresce in x-rays; density 2.07 g/cm3; melts at 172.4°C; intensely soluble in water, 316 g/100 mL at 0°C; dissolves in methanol and ethanol; slightly soluble in ammonia solution.

Occurrence

Magnesium bromide occurs in seawater, some mineral springs, natural brines, inland seas and lakes such as the Dead Sea and the Great Salt Lake, and salt deposits such as the Stassfurt deposits. In seawater, it is the primary source of bromine. By the action of chlorine gas upon seawater or seawater bitterns, bromine is formed. It is an electrolyte component in certain dry cells. In medicine, it is a sedative and anticonvulsant for treatment of nervous disorder. It also is used in organic synthesis forming several addition compounds.

Uses

Magnesium Bromide is an inorganic salt used in the synthesis of superconductors and nanowires. Also present in polymer nanocomposites to improve conductivity.

Application

The major use of Magnesium bromide has been in the commercial production of bromine. The Dow process is an electrolytic method of bromine extraction from brine, and was Herbert Dow’s second revolutionary process for generating bromine commercially (1889).
Magnesium bromide has also been used in organic syntheses. An efficient and environmentally friendly procedure for the one-pot synthesis of tetrahydropyrimidines from aldehydes, a-diketones and urea/thiourea by using magnesium bromide as an inexpensive and easily available catalyst under solvent-free conditions has been described. Compared with the classical Biginelli reaction conditions, this new method has the advantage of good to excellent yields (74%–94%) and short reaction times (45–90 min). The structure of the Biginelli reaction product from a-diketone, salicylaldehyde and urea has been proposed to possess an oxygen bridge by cyclization (intramolecular Michael addition).

Preparation

Magnesium bromide is prepared by treating MgO with hydrobromic acid and then crystallization above 0.0°C in solution. The product is the hexahydrate salt:
MgO＋2HBr→MgBr2＋H2O→MgBr2·6H2O
The anhydrous form may also be prepared by heating the hexahydrate with dry HBr gas. This compound can also be formed directly from the elements:
Mg＋Br2→MgBr2

Synthesis

Magnesium bromide is prepared by treating magnesium oxide with hydrobromic acid and subsequent crystallization above 0°C. The product is hexahydrate, MgBr2.6H2O:
MgO + 2HBr → MgBr2 + H2O
The anhydrous MgBr2 may be obtained by heating the hexahydrate with dry hydrogen bromide gas. Magnesium bromide also can be made from its elements. Heating magnesium metal with bromine vapor yields the salt:
Mg + Br2 → MgBr2
Magnesium bromide, like the chloride salt, is obtained from sea water (see Magnesium and Magnesium chloride). In this process, magnesium hydroxide precipitated from sea water is neutralized with hydrobromic acid, and MgBr2 is obtained by crystallization.

Purification Methods

Crystallise it from EtOH or H2O (3.3g/mL). Dry it in a vacuum at ~150o, or heat the hydrate in a stream of HCl. It is very deliquescent. [Ehrlich in Handbook of Preparative Inorganic Chemistry (Ed. Brauer) Academic Press Vol I p 909 1963.]