What is Barium Oxide?
Barium oxide, BaO, is a hygroscopic or moisture-absorbing compound that is non-flammable in nature. It is also known as barium monoxide, barium protoxide, and calcined baryta. It has a cubic structure and is widely used in Cathode ray tubes, crown glass, catalysts, and as a solvent dye. Consumption of barium oxide (BaO) can be fatal. The symbol for Barium Oxide is BaO.
Barium Oxide (BaO) is produced by oxidising barium salts such as barium carbonate, in which the barium burns in oxygen to produce barium oxide. As a result, Barium Oxide has the chemical formula BaO. The chemical reaction for producing Barium Oxide is as follows:
${{2}{Ba} {+} {O}_{2}\to {2}{Ba}{O}}$
Structure of Barium
Barium Oxide has a cubic structure; the image below depicts the barium oxide structure (BaO), in which one ion of barium participates in the reaction and both ions combine to form barium oxide. As a result, barium is oxidised to form barium oxide. Barium oxide has a total 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 compound has one covalently bonded unit.
Properties of Barium Oxide (BaO)
When a barium salt is oxidised, barium oxide, also known as baria, is formed. It is a non-flammable, white hygroscopic compound. Here, are some of the characteristics of Barium oxide (BaO).
Barium Oxide Formula: Because barium oxide is formed by the oxidation of barium salts, its chemical formula is BaO. The following equation yields the formula for barium oxide.
$${{2}{Ba} {+} {O}_{2}\to {2}{Ba}{O}}$$
Molar Mass: Barium oxide has a total molecular mass of 153.326 g/mol.
Appearance: When a barium salt is oxidised to produce barium oxide, it appears as a white solid powdered substance.
Density: The density of barium oxide is 5.72 g/$${{cm}_{3}}$$.
Chemical Name: Barium oxide is also known as barium monoxide, barium protoxide, and calcined baryta.
Melting Point: The melting point of barium oxide is 1,923 degrees Celsius, 3,493 degrees Fahrenheit, or 2196 degrees Kelvin.
Boiling Point: The boiling point of barium oxide is 2,000 degrees Celsius, 3,630 degrees Fahrenheit, or 2,270 degrees Kelvin.
Solubility in Water: At 20°C, barium oxide dissolves in water at a rate of 3.48 g/100 mL and at 100°C, it dissolves at a rate of 90.8 gm/100 mL.
Solubility: In ethanol, dilute mineral acids, and alkalies, barium oxide is soluble. Acetone and liquid ammonia are not soluble in it.
Production of Barium Oxide
Heating barium carbonate produces barium oxide or barium monoxide (BaCO3). It can also be made by thermally decomposing the compound Barium Nitrate Ba(NO3). It is frequently formed through the decomposition of other Barium salts. The following are the chemical reactions that result in the compound barium oxide.
$${{2}{Ba} {+} {O}_{2}\to {2}{Ba}{O}}$$
$${{Ba}{C}{O}_{3}\to {Ba}{O} {+} {C}{O}_{2}}$$
The barium carbonate BaCO3 is heated and decomposed to obtain barium oxide, and carbon dioxide is released during the reaction.
Uses of Barium Oxide
At room temperature, Barium Oxide is a unique white compound that has the ability to absorb moisture from its surroundings. As a result, it is used as an absorbent in a variety of chemical reactions. Let us now look at the applications of BaO (Barium oxide).
Barium oxide is used to coat hot cathodes, such as those found in cathode ray tubes.
Barium oxide is also used to make optical crown glass. Prior to the use of Barium oxide in the production of optical crown glass, lead oxide was used, but it was discovered that lead oxide raised the dispersive power, which caused difficulty, whereas barium oxide raised the refractive index of the optical crown glass without affecting the dispersive power.
Barium Oxide is widely used as an ethoxylation catalyst in the reaction of ethylene oxide and alcohols, which typically occurs between 150 and 200 degrees Celsius.
It is used as a source of pure oxygen via heat fluctuation because it decomposes easily to BaO2 via the formation of a peroxide ion.
It is used in the isomer separation process.
It is widely used in the production of fuel and as a reducing agent.
It is a fantastic oxidising agent.
Important Questions
1. What is the element barium used for?
Ans: The amount of barium found in food and water is usually not high enough to be a health concern. Those who work in the barium industry are at the greatest risk of additional health effects from barium exposure. The majority of the health risks they face are caused by breathing in air containing barium sulphate or barium carbonate. Certain amounts of barium can be found in many hazardous waste sites. People who live nearby may be exposed to dangerous levels. The exposure will then be caused by breathing dust, eating barium-contaminated soil or plants, or drinking barium-contaminated water. Skin contact is also possible.
2. What is the History of Barium Oxide?
Ans: Some barium minerals were known to alchemists in the early Middle Ages. Smooth pebble-like stones of the mineral barite were discovered in volcanic rock near Bologna, Italy, and became known as "Bologna stones." Alchemists were drawn to them because they glowed for years after being exposed to light. V. Casciorolus described the phosphorescent properties of barite heated with organics in 1602.
In 1774, Carl Scheele discovered that baryte contained a new element, but he was unable to isolate barium, only barium oxide. Johan Gottlieb Gahn isolated barium oxide in similar studies two years later. Guyton de Morveau named oxidised barium "barote," which was later changed to baryta by Antonie Lavoisier. In the $${{1}{8}^{th}}$$ century, English mineralogist William Withering discovered a heavy mineral called witherite in the Cumberland lead mines. Sir Humphry Davy of England was the first to isolate barium by electrolysis of molten barium salts in 1808.
Multiple Choice Questions
1. What is the pH value of Barium?
a)10
b)12
c)9
d)13
Answer: (d)
2. Barium is used for
a)Checking blood group
b)X-ray of alimentary canal
c)X-ray of brain
d)None of these
Answer: (b)
Conclusion
Barium Oxide is also known as barium monoxide (Mono means one) and calcined baryta. In this article, we have learned that Barium oxide is a white, one-of-a-kind chemical compound that, at room temperature, can absorb water molecules from its surroundings. The formula for barium oxide is BaO. It is formed when barium salts, such as barium carbonate, are heated. It is also used as a solvent drying agent.
FAQs on Barium Oxide
1. What are the safety issues for Barium Oxide?
Barium oxide is a hazardous and toxic compound that causes irritation if it comes in contact with the skin or eyes. Inhalation or swallowing of barium oxide fumes can cause nausea, diarrhea, or skin infection. It can also cause muscle paralysis, which can eventually cause death. Suppose a person ingests or comes in contact with barium oxide, he should immediately be given medical attention, or else it may cause various other health issues leading to death. Barium oxide should never be released into the environment as it is harmful to plants and animals.
2. What are the Chemical properties of Barium Oxide?
The chemical properties of Barium oxide are as follows.
What is the Chemical name for Barium oxide? | Baria, Calcined baryta or Barium monoxide or Barium protoxide. |
What is the Chemical formula for Barium Oxide? | The chemical formula barium oxide is BaO. |
What is the molecular weight of Barium Oxide? | The molecular weight is 5.72 g/cm3. |
What is the Boiling point of BaO? | The boiling point is ~ 2,000ᣞC. |
What is the Melting point of BaO? | The melting point is 1,923 ᐤC. |
3. What is barium titanate used for?
With dielectric constant values as high as 7,000, barium titanate is a dielectric ceramic used in capacitors. Values as high as 15,000 are possible over a narrow temperature range; most common ceramic and polymer materials have values less than 10, while others, such as titanium dioxide $${({Ti}{O}_{2})}$$, have values between 20 and 70.
It's a piezoelectric material that's commonly found in microphones and other transducers. At room temperature, the spontaneous polarisation of barium titanate single crystals ranges between 0.15 C/$${{m}_{2}}$$ in earlier studies and 0.26 C/m2 in more recent publications, with a Curie temperature between 120 and 130°C. The differences are due to the growth technique, with earlier crystals being less pure than current crystals grown with the Czochralski process, which have a higher Curie temperature and a larger spontaneous polarisation.
4. What type of bonding is found in Barium oxide?
One barium cation $${{Ba}^{2+}}$$ and one oxide anion $${{O}^{2-}}$$ combine to form the molecule. One ionic bond connects both ions. Ionic bond, also known as electrovalent bond, is a type of linkage formed in a chemical compound by the electrostatic attraction of oppositely charged ions. When the valence electrons of one atom are permanently transferred to another, a bond is formed. The atom that loses electrons becomes a positively charged ion (cation) whereas the atom that gains electrons becomes a negatively charged ion (anion).
5. Why can barium not reduce to a lower oxidation state?
We should return to the oxidation state general rule. Free elements have an oxidation state of 0. Because it does not form chemical bonds with other elements, barium metal is a free element. Because barium cannot form a negative ion, it cannot be reduced to a lower oxidation state. In Barium Oxide, the oxidation number of barium is +2.
6. What is the origin of barium oxide?
Barium is a naturally occurring component of minerals that are found in small but widely distributed amounts in the earth's crust, especially in igneous rocks, sandstone, shale, and coal (Kunesh 1978; Miner 1969a). Barium enters the environment naturally through the weathering of rocks and minerals.
