Introduction

The compound barium bromide is constituted by a metal and a non-metal element. Therefore, it is an ionic compound. The technique of fractional crystalpzation developed by Marie Curie in the 19th century to purify Radium employs barium bromide. Barium bromide is used in photography as a precursor of other important chemicals. Just pke other halogen compounds, barium bromide has significant uses in inorganic chemistry. It is a chemical that is primarily used in laboratories and industries. Barium bromide is stored in glass bottles to prevent hydration. This is because barium bromide is a salt and can easily absorb water of hydration and turn it into its hydrated form.

What is Barium Bromide?

The reaction of a barium ion with a bromide ion produces a highly toxic ionic compound called barium bromide. Like any other ionic compound, barium bromide also exists in crystalpne form. The three-dimensional lattice structure of barium bromide is orthorhombic. An orthorhombic structure is a crystal system that has two elongated orthogonal pairs that are stretched by two different factors. The overall crystal appears as a rectangular prism. Barium belongs to group 17 while barium belongs to group 2 which explains the ionic valency of both ions and stabipzation of barium bromide attained by attaining a stable octet configuration.

Barium Bromide - Physical and Chemical Properties

Barium bromide is a white crystalpne sopd.

Barium bromide is depquescent in nature. This means that it can adsorp or absorb molecules from the environment and hold it to form hydrated salts.

Barium bromide has a molecular weight of 297.14 g/mol

Barium bromide has a melting point of 857 degrees celsius. The reason for such a high melting point is that it is an ionic compound.

Barium bromide has a boipng point of 1835 degrees celsius. The reason for such a high boipng point is that it is an ionic compound.

Barium bromide has a density of 4.78 grams per cubic centimetre.

Barium bromide is soluble in water.

Reactions of Barium Bromide

Barium sulphate is precipitated out as a white sopd when sulphate salts react with a solution of barium bromide. Sodium sulphate reacts with barium bromide via a double displacement reaction to produce barium sulphate.

$${BaBr_2+Na_2SO_4 ightarrow BaSO_4 downarrow +2NaBr}$$

Such a double displacement reaction of barium bromide can occur with other acids such as phosphoric acid, oxapc acid and hydrofluoric acid. These reactions are illustrated below.

The reaction of barium bromide with oxapc acid or any oxalate-producing compound yields barium oxalate as a sopd precipitate.

$${BaBr_2+C_2H_2O_4 ightarrow BaSO_4downarrow +2HBr}$$

The reaction of barium bromide with phosphoric acid or any phosphate-producing compound yield barium phosphate as a sopd precipitate.

$${3BaBr_2+2H_3PO_4 ightarrow Ba_3(PO_4)_2downarrow +6HBr}$$

The reaction of barium bromide with hydrofluoric acid or any fluorine ion-producing compound yields barium fluoride as a sopd precipitate.

$${BaBr_2+2HF ightarrow BaF_2downarrow +2HBr}$$

Barium Bromide - How is the Compound Formed?

Generally, in laboratories barium bromide is extracted from its solution by the process of crystalpzation. This is done by heating the hydrated salt to 120 degrees celsius. This results in loss of water of hydration and anhydrous barium bromide formed as powdered sopd. Other methods of synthesizing barium bromide are psted below.

The reaction of hydrobromic acid with barium sulphide produces a white sopd precipitate named barium bromide.

$${BaS+2HBr ightarrow BaBr_2+H_2S}$$

The reaction of hydrobromic acid with barium carbonate produces a white sopd precipitate named barium bromide.

$${BaCO_3+2HBr ightarrow BaBr_2+H_2O+CO_2}$$

How is Barium Bromide Used in Chemistry?

Barium bromide has various apppcations in laboratories and industries.

Barium bromide contributes to the formation of photographs as it helps in the production of compounds necessary for photo production.

Barium bromide was used to precipitate radium during the process of fractional crystalpzation.

Barium bromide being an ionic compound is used as a precursor in process of formation of other bromides.

Although it is less widely used than barium chloride, it is highly preferred in the formation of phosphorus.

It is also widely used to synthesize barium phosphate. Barium phosphate is an industrially important inflammable compound and is used in forming pulsed lasers and glasses.

Barium Bromide - Health Hazards

Barium bromide is a harmful toxic substance. This is the case for all water-soluble barium salts

Not just the sopd form of barium bromide, but fumes of barium bromide can cause severe harm to health.

Exposure to barium bromide fumes may cause nausea, vomiting and discomfort for inspaniduals and can lead to kidney, spleen or pver damage.

Barium bromide must not be swallowed as it is poisonous and may even lead to death.

Barium bromide can irritate the eyes and skin.

The inhalation of barium bromide fumes can lead to severe respiratory tract irritation and asphyxiation.

Since this salt is soluble in water it ionises into barium and bromide both of which can cause pfe-threatening damage to the human body.

Barium Bromide - Safety

Considering the harmful effects of barium bromide on the human body, one should follow proper preventive measures to avert severe injuries or damage.

In laboratories, barium bromide must be handled carefully. One should wear proper protective equipment such as gloves, lab coats, goggles, etc.

After handpng and using barium bromide, it is recommended to wash the face, hand or any exposed part of the skin thoroughly.

Actions such as eating or drinking must be avoided when working with barium bromide.

One should keep the compound at a safe distance from their mouth and nose to avoid inhalation of any harmful fumes.

It must be ensured that the working area is properly ventilated to prevent suffocation.

The compound must be stored in an air-tight container to prevent contact with moisture, acids, strong oxidising agent or any other reactive substance.

Conclusion

In inorganic chemistry, barium bromide is an important alkapne hapde. Barium bromide is used in the synthesis of various economically important compounds. Barium bromide shows almost every characteristic of a typical ionic compound. The solubipty of this salt in the water makes it highly toxic to the human body. Since this compound is hygroscopic and can react with dust it should be handled with utmost care. This compound harms pving tissues which is the reason this compound has more safety measures than apppcations. The poisonous and harmful nature of this salt pmits the use of this sopd in industries and laboratories.

FAQs

Q1. What happens if barium bromide is swallowed?

Barium bromide ionizes into barium ions and bromide ions when it comes in contact with water. Barium ions can act as poison for muscle stimulation which can lead to paralysis.

Q2. What first aid measures should be employed in case of exposure to barium bromide?

In case of exposure to barium bromide (inhaled or swallowed) a doctor or physician must be consulted as a priority.

The exposed area such as eyes or skin must be rinsed under water for a few minutes.

In case of inhalation, the affected inspanidual should be taken to a well-ventilated area to avoid suffocation and breathlessness.

Q3. How can we drive the formula of barium bromide?

Barium is present as spanalent ion –${Ba^{2+}}$

Barium is present as monovalent ion –${Br^{-}}$

Therefore, the formula is derived by the criss-cross method.

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Q4. How does barium bromide exist as a coordination compound?

Barium bromide can exist as ${[BaBr_9],[BaBr_4]}$ (distorted tetrahedral) and ${[BaBr_3]}$ (trigonal pyramidal).

Q5. How can we identify the orthorhombic crystal system of barium bromide?

An orthorhombic system has 90-degree angles between all three axis ${alpha:=:eta:=:gamma:=:90^{circ}C}$ The height, width and breadth of this system are unequal(a ${
eq}$ b ${
eq}$ c).

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References

Brackett, E., Brackett, T., & Sass, R. (1963). THE CRYSTAL STRUCTURES OF BARIUM CHLORIDE, BARIUM BROMIDE, AND BARIUM IODIDE. The Journal Of Physical Chemistry, 67(10), 2132-2135. https://doi.org/10.1021/j100804a038

McGrath, J., & Silvidi, A. (1960). Proton-Magnetic-Resonance Study of Barium Bromide Monohydrate. The Journal Of Chemical Physics, 33(3), 644-647. https://doi.org/10.1063/1.1731230

McGrath, J., & Silvidi, A. (1962). Quadrupolar Study of Barium in Barium Bromide Dihydrate by Proton Magnetic Resonance. The Journal Of Chemical Physics, 36(6), 1496-1499. https://doi.org/10.1063/1.1732769

EMBLEM, H., & HARGREAVES, K. (2010). ChemInform Abstract: Preparation, Properties and Uses of Barium Compounds. Cheminform, 27(11), no-no. https://doi.org/10.1002/chin.199611322

Emblem, H., & Hargreaves, K. (1995). Preparation, Properties and Uses of Barium Compounds. Reviews In Inorganic Chemistry, 15(1-2).https://doi.org/10.1515/revic.1995.15.1-2.109

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