Barium Oxide (BaO): Properties, Structure, Production and Uses

Barium Oxide (BaO) is a thermally stable, hygroscopic compound. It is known by several names such as Barium Monoxide, Barium Protoxide or Calcined Baryta. Barium Oxide is highly insoluble and is suitable for glass, optic and ceramic applications. It is also used in the form of a drying agent for solvents, cathode ray tubes, catalysts and crown glass. 

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What is Barium Oxide?

Barium oxide is a highly insoluble thermally stable source of barium suitable for ceramic applications, optics, and glass. Barium oxide is represented by the symbol BaO. In nature, barium oxide is found to be white and is non-flammable. It is widely utilized in cathode ray tubes, catalysts, crown glass, and solvent-killing agents because of its cubic structure. However, consumption of barium oxide (BaO) can be lethal.

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Barium Oxide

Barium oxide reacts with water to form barium hydroxide. It reacts with water strongly because it is hygroscopic, which means it tends to absorb moisture or water vapors from the surrounding air or environment. While all other hydroxides are conductive to electricity, this compound is hardly conducive to electricity. On the other side, several perovskite structured oxides are good conductors of electricity that are used in the cathode of solid oxide fuel cells and oxygen generation technologies. At least one metallic cation and one oxygen anion are present in these compounds.

Barium Oxide

They are usually insoluble in aqueous solutions, like water, and highly stable, making them suitable for porcelain constructions ranging from simple clay bowls to advanced electronics. In addition, it is lighter, so engineers utilize it in aircraft and electrical and chemical applications like fuel cells, where it exhibits ionic conductivity. Other names of barium oxide are barium monoxide, barium protoxide and calcined baryta. Since barium oxide does not exist freely in nature, we always discover it mixed with other elements.

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Barium Oxide Formula

Barium oxide (BaO) is produced by the oxidation of barium salts like barium carbonate, in which the barium burns in oxygen. As a result, barium oxide's molecular formula is BaO.

The chemical reaction producing barium oxide is represented as:

2Ba + O₂ → 2BaO

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Structure of Barium Oxide

Barium oxide is known to have a cube-like structure, in which each barium ion participates in the reaction, and then both ions combine to produce barium oxide. As a result, barium oxidizes to generate barium oxide.

Barium Oxide Structure

Barium oxide has an overall monoisotopic mass of 153.9 g/mol. Because the number of hydrogen bond acceptors is one and the number of hydrogen bond donors is zero, the molecule contains just one covalently bound unit.

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Properties of Barium Oxide

These are a few of Barium oxide's characteristics (BaO):

1. When a barium salt is oxidized, it creates barium oxide, which is also known as baria. It is a non-flammable, white hygroscopic chemical.
2. Barium oxide Formula: Since barium salts are oxidized, the molecular formula for barium oxide is BaO. The following equation yields the formula for barium oxide: 2Ba + O₂ → 2BaO
3. Appearance: When a barium salt is oxidized to produce barium oxide, the barium oxide appears to be a white insoluble powdery substance.
4. Total Molar Mass: Barium oxide has a total molecular mass of 153.326 g/mol.
5. Chemical Names: Barium oxide is also known as barium monoxide, barium protoxide, and calcined baryta.

Barium Oxide Properties

6. Solubility in Water: At 20°C, barium oxide dissolves at 3.48 g/100 mL, while at 100°C, it dissolves at 90.8 g/100 mL.
7. Solubility: In ethanol, dilute mineral acids, and alkalies, barium oxide is soluble. Acetone and liquid ammonia do not dissolve.
8. Melting Point: The melting point of barium oxide is 1,923 degrees Celsius, 3,493 degrees Fahrenheit, or 2196 degrees Kelvin.
9. Boiling Point: Barium oxide boils at 2,000 degrees Celsius, 3,630 degrees Fahrenheit, or 2,270 degrees Kelvin.
10. Density: Barium oxide has a density of 5.72 grams per cubic centimeter.

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Barium Oxide Production

Heating barium carbonate produces barium oxide or barium monoxide (BaCO₃). The thermal breakdown of the barium nitrate (Ba (NO₃)₂) chemical can also be used to make it. In addition, decomposing different barium salts frequently make barium oxide. The following are the chemical processes that lead to the formation of barium oxide:

2Ba + O₂ → 2BaO

BaCO₃→ BaO + CO₂

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The barium carbonate (BaCO₃) is burned and degraded to produce barium oxide, while carbon dioxide is emitted throughout the reaction.

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Barium Oxide Uses

1. At ambient temperature, barium oxide is a distinctive white-colored chemical that absorbs moisture from the atmosphere. As a result, it is used as an absorbent in a variety of chemical reactions.
2. Barium oxide is also a supplier of pure oxygen due to heat fluctuation. It also oxidizes readily to BaO₂ by the production of peroxide ions. Additionally, complete peroxidation of BaO to BaO₂ occurs at an intermediate temperature. However, at high heat, the increased entropy of the O₂ molecule causes BaO₂ to break down into O₂ and BaO.
3. Hot cathodes, such as those used in cathode ray tubes, are coated with barium oxide.
4. Barium oxide is available in chunks, pellets, powder, tablets, nanopowder, and sputtering targets. It is ordinarily accessible in large quantities in nanopowder, high purity, submicron, and ultra-high purity.

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5. Optical crown glass is also made with barium oxide. Before barium oxide, lead oxide was used to make optical crown glass. But it was discovered that lead oxide increases dispersive power, causing trouble. Still, barium oxide increases the refractive index of the optical crown glass without altering dispersive power.
6. At the end of the twentieth century, this process was employed before air separation method became the primary approach to create oxygen. This is Brin’s process, named after its creator.
7. In the reaction between ethylene oxide and alcohols between 150 and 200 degrees Celsius, barium oxide is often utilized as an ethoxylation catalyst.

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Health Hazards

1. Severe burns or death can result from inhaling, swallowing, or coming into touch (with skin or eyes) with vapors, substances, or dust of barium oxide.
2. Barium oxide is a poisonous, corrosive, non-combustible, and water-sensitive substance.
3. When barium oxide burns, it releases irritating, poisonous, and corrosive fumes.
4. When it reacts with water, it produces heat, which raises the number of hydrogen fumes in the air.

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Things to Remember

1. Barium oxide is a highly insoluble thermally stable source of barium and has a cubic structure.
2. Barium oxide is non-flammable and hygroscopic.
3. Barium oxide does not exist freely in nature.
4. Barium oxide is produced by Brin’s process in large quantities.

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