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BARIUM PEROXIDE

Barium peroxide is a grayish-white or pale yellow powder known for its strong oxidizing properties and is primarily used as a source of pure oxygen in chemical processes and pyrotechnics, producing vibrant green colors in fireworks.
Barium peroxide is relatively stable under standard conditions but decomposes when heated, releasing oxygen gas, and reacts vigorously with water and acids, making it hazardous if improperly handled.
Barium peroxide has important industrial applications, including its use as a bleaching agent, a precursor in hydrogen peroxide production, and in glass and ceramics manufacturing, while requiring strict safety protocols due to its toxicity and reactivity.

CAS Number: 1304-29-6
EC Number: 215-128-4
Molceular Formula: BaO2
Molar Mass: 169.34 g/mol

Synonyms: BARIUM PEROXIDE, 1304-29-6, barium(2+);peroxide, Barium dioxide, MFCD00003454, Barium binoxide, Barium superoxide, Barium oxide, per-, Bario (perossido di), Bariumperoxid, Bariumperoxid [German], Bariumperoxyde, Bariumperoxyde [Dutch], Dioxyde de baryum, Dioxyde de baryum [French], Peroxyde de baryum, Barium peroxide (Ba(O2)), Peroxyde de baryum [French], HSDB 396, Bario (perossido di) [Italian], EINECS 215-128-4, UN1449, Bariumsuperoxyd, UNII-T892KY013Y, Barium peroxide, anhydrous, Ba(O2), T892KY013Y, Barium peroxide [UN1449] [Oxidizer], Barium dioxide, Barium binoxide, Barium superoxide, Barium(II) peroxide, Barium oxide(II, I), Barium peroxide hydrate, Peroxide of barium, Barium peroxyhydrate, Barium oxygen compound, BaO₂ (chemical formula), Barium (II) oxide, Barium peroxide anhydrous, Barium peroxide solid, Barium superoxide salt, Barium bisperoxide, Barium dioxygen, Barium oxydioxide, BaO₂ salt, Barium oxygenate, Barium peroxides, Barium peroxide compound, Barium oxoperoxide, Barium peroxide solution, Barium peroxide crystals, Oxidized barium compound

Barium peroxide is an inorganic compound that appears as a grayish-white or pale yellow powder.
Barium peroxide is primarily known for its use as a source of pure oxygen in chemical processes and in pyrotechnics.

Barium peroxide has a crystalline structure and is relatively stable under standard conditions.
However, Barium peroxide can decompose when exposed to heat, releasing oxygen gas.

Barium peroxide has strong oxidizing properties and reacts vigorously with water or acids, producing hydrogen peroxide and other compounds.
In pyrotechnics, barium peroxide serves as an oxidizer, playing a role in the production of vibrant green colors in fireworks displays due to the emission spectra of barium.

Barium peroxide's industrial applications extend to being a bleaching agent for textiles, a precursor in the manufacture of hydrogen peroxide, and a component in certain types of batteries.
Although valuable in these areas, barium peroxide can be hazardous if improperly handled, as it is toxic to humans and the environment.

Proper safety protocols, such as wearing protective gear and handling Barium peroxide in well-ventilated areas, are essential when working with Barium peroxide.
Barium peroxide's production typically involves the reaction of barium salts with oxygen under controlled conditions.
In historical contexts, barium peroxide was also used to produce oxygen in early experiments with oxygen generation and has been a part of various chemical reactions involving the synthesis of other barium compounds.

Barium peroxide is an inorganic compound with the formula BaO2.
This white solid (gray when impure) is one of the most common inorganic peroxides, and Barium peroxide was the first peroxide compound discovered.
Being an oxidizer and giving a vivid green colour upon ignition (as do all barium compounds), Barium peroxide finds some use in fireworks; historically, it was also used as a precursor for hydrogen peroxide.

Barium peroxide is registered under the REACH Regulation and is manufactured in and / or imported to the European Economic Area, at ≥ 10 to < 100 tonnes per annum.
Barium peroxide is used by professional workers (widespread uses), in formulation or re-packing, at industrial sites and in manufacturing.

Barium peroxide appears as a grayish-white granular solid.
Barium peroxide is insoluble in water.

Barium peroxide is noncombustible, but accelerates the burning of combustible material.
Barium peroxide is mixture with finely divided combustible material may be explosive.
Barium peroxide is mixtures with combustible material may be ignited by friction or contact with moisture.

Barium peroxide is an oxide of barium.
Barium peroxide is used in bleaching and to produce a green color in fireworks.

Barium peroxide is a metallic alkaline earth metal with the symbol Ba, and atomic number 56.
Barium peroxide never occurs in nature in its pure form due to its reactivity with air, but combines with other chemicals such as sulfur or carbon and oxygen to form barium compounds that may be found as minerals.

Barium peroxide is a highly reactive, crystalline solid primarily used as an oxidizing agent in various industrial and chemical applications.
Barium peroxide is commonly encountered as a pale yellow or grayish-white powder due to its ability to absorb moisture from the air, although Barium peroxide is anhydrous in Barium peroxide's pure form.

Barium peroxide is notable for its strong oxidizing properties, making it useful in applications that require the release of oxygen.
One of Barium peroxide's key characteristics is its ability to decompose at elevated temperatures (around 800°C), releasing oxygen gas, which makes it valuable for oxygen generation in various chemical processes.

Barium peroxide was historically important in the production of hydrogen peroxide (H₂O₂), as it reacts with sulfuric acid to yield this important industrial chemical.
Barium peroxide's high reactivity also lends itself to uses in pyrotechnics, where it is responsible for producing the bright green colors seen in fireworks.

This green hue is the result of the emission spectra of barium ions when excited by the heat of combustion.
Additionally, Barium peroxide has been utilized in the glass and ceramics industries to introduce barium into the mix, which helps modify the refractive index and thermal stability of glass products.

In terms of safety and handling, barium peroxide is classified as a hazardous material due to Barium peroxide's strong oxidizing nature and toxicity.
Barium peroxide can pose serious health risks if inhaled, ingested, or if it comes into contact with skin.

Inhalation of barium peroxide dust can irritate the respiratory tract, while ingestion can lead to barium poisoning, affecting the cardiovascular and nervous systems.
Barium peroxide reacts violently with organic materials, water, and acids, potentially leading to the formation of hydrogen peroxide or other reactive oxygen species, which can pose further risks of combustion or explosion in improper conditions.
As such, Barium peroxide must be handled with strict safety protocols, including the use of personal protective equipment (PPE) like gloves, goggles, and protective clothing, and Barium peroxide should be stored in tightly sealed containers to avoid exposure to moisture and incompatible substances.

The synthesis of barium peroxide typically involves the reaction of barium oxide (BaO) with oxygen at high temperatures.
This process was historically significant in the early development of oxygen production methods before more efficient technologies were developed.

Today, while its use in oxygen generation has diminished, barium peroxide remains a key chemical in niche applications such as the synthesis of other barium compounds, the production of explosives, and specialized oxidation reactions.
In some batteries, Barium peroxide has been investigated as a potential component for enhancing the electrochemical performance, although it is not widely used in modern battery technologies.
Barium peroxide's versatility in industrial chemistry, along with its reactivity, ensures that barium peroxide continues to be a valuable chemical in controlled environments.

Uses of Barium Peroxide:
Barium peroxide is used for bleaching (animal and plant fibers), decolorizing glass, dyeing and printing textiles, and drying agent for lithographics.
Barium peroxide is also used with powdered aluminum in welding, in igniter compositions, and in cathodes of fluorescent lamps.

Barium peroxide is used in cathodes of fluorescent lamps; as a drying agent for lithographic inks.
Barium peroxide is used in bleaching and to produce a green color in fireworks.

Barium peroxide is used for bleaching (animal and plant fibers), decolorizing glass, dyeing and printing textiles, and drying agent for lithographics.
Barium peroxide is also used with powdered aluminum in welding, in igniter compositions, and in cathodes of fluorescent lamps.

Barium peroxide has several important industrial and chemical applications due to its strong oxidizing properties.
One of its primary uses is in the production of hydrogen peroxide (H₂O₂), where Barium peroxide reacts with acids to generate this compound, widely used as a bleaching agent, disinfectant, and in chemical synthesis.

In the pyrotechnics industry, barium peroxide is valued for Barium peroxide's role in producing the bright green flames seen in fireworks and flares, thanks to the characteristic emission spectra of barium ions.
Barium peroxide is also employed in oxygen generation due to its ability to release oxygen when decomposed at high temperatures, a property once used in early oxygen production methods.

Additionally, Barium peroxide serves as a bleaching agent in the textile industry, assisting in the whitening of fabrics.
Barium peroxide is also used in the glass and ceramics industries, where it helps to improve the refractive index and durability of certain glass products.

In niche applications, Barium peroxide is involved in oxidation reactions and is occasionally explored as a component in specialized battery technologies.
Despite its diverse uses, Barium peroxide must be handled with care due to its toxicity and reactivity, especially when exposed to moisture or organic materials.

Uses at industrial sites:
Barium peroxide is used in the following products: laboratory chemicals and pH regulators and water treatment products.
Barium peroxide is used in the following areas: scientific research and development.

Barium peroxide is used for the manufacture of: chemicals.
Release to the environment of Barium peroxide can occur from industrial use: in processing aids at industrial sites, as an intermediate step in further manufacturing of another substance (use of intermediates) and as processing aid.

Industry Uses:
Oxidizing/reducing agents

Consumer Uses:
Not Known or Reasonably Ascertainable

Applications of Barium Peroxide:
Barium peroxide finds applications across several industries due to its oxidizing properties and reactivity.

Here are some of Barium peroxide's key applications:

Hydrogen Peroxide Production:
Barium peroxide is used to produce hydrogen peroxide (H₂O₂) by reacting with dilute acids.
Hydrogen peroxide is essential in a variety of industries, including textiles, paper, and chemical synthesis.

Pyrotechnics:
In fireworks and flares, barium peroxide acts as an oxidizer, producing the characteristic bright green color when burned, due to the emission spectra of barium ions.

Oxygen Generation:
Historically, barium peroxide was used as a source of oxygen.
When heated, Barium peroxide decomposes and releases oxygen, which was significant in early oxygen production technologies.

Textile Bleaching:
Barium peroxide is used as a bleaching agent in the textile industry, helping to whiten fabrics by breaking down pigments and dyes.

Glass and Ceramics Industry:
Barium peroxide is used in the manufacturing of certain types of glass and ceramics, where it enhances the refractive index and thermal stability of the final product.

Oxidation Reactions:
Barium peroxide serves as an oxidizing agent in chemical synthesis, where it is involved in various oxidation reactions in organic and inorganic chemistry.

Explosives:
Due to its strong oxidizing properties, barium peroxide is used in the formulation of explosives and propellants.

Batteries:
In some experimental applications, barium peroxide has been explored as a potential component in batteries, though Barium peroxide is not widely used in modern battery technology.

Preparation and Use:
Barium peroxide arises by the reversible reaction of O2 with barium oxide.
The peroxide forms around 500 °C and oxygen is released above 820 °C.

2 BaO + O2 ⇌ 2 BaO2

This reaction is the basis for the now-obsolete Brin process for separating oxygen from the atmosphere.
Other oxides, e.g. Na2O and SrO, behave similarly.

In another obsolete application, barium peroxide was once used to produce hydrogen peroxide via its reaction with sulfuric acid:
BaO2 + H2SO4 → H2O2 + BaSO4

The insoluble barium sulfate is filtered from the mixture.

Manufacturing Methods of Barium Peroxide:
Barium peroxide is manufactured by the oxidation of barium oxide with air at 1000°F (537°C).
Barium hydroxide is reacted with hydrogen peroxide to produce barium peroxide monohydrate.

General Manufacturing Information:

Industry Processing Sectors:
Primary Metal Manufacturing

Production of Barium Peroxide:
The production of barium peroxide typically involves the reaction of barium oxide (BaO) with oxygen (O₂) under controlled conditions.
This process requires elevated temperatures to promote the formation of BaO₂ from BaO.

The general production method can be broken down into the following steps:

Preparation of Barium Oxide (BaO):
Barium peroxide is generally synthesized from barium oxide, which itself is produced by heating barium carbonate (BaCO₃) in a furnace.

When barium carbonate is heated at high temperatures (above 1000°C), Barium peroxide decomposes into barium oxide and carbon dioxide (CO₂):
BaCO₃ (s)→BaO (s)+CO₂ (g)

Oxidation of Barium Oxide:
The barium oxide is then reacted with oxygen gas at a temperature of around 500-600°C to produce barium peroxide.

The reaction is conducted in an environment where the temperature is carefully controlled to encourage the formation of BaO₂:
2BaO (s)+O₂ (g)→2BaO₂ (s)

The reaction is exothermic, meaning Barium peroxide releases heat, but it needs to be closely monitored to avoid decomposition of the peroxide back into barium oxide.

Purification:
After the oxidation reaction, the barium peroxide produced is cooled and purified.
Any remaining barium oxide or unreacted materials are separated through processes such as filtration or washing, ensuring the final product is mostly composed of BaO₂.

Drying and Packaging:
Once purified, the barium peroxide is dried to remove any moisture, which is important because Barium peroxide is hygroscopic (Barium peroxide can absorb water from the air).
The dried barium peroxide is then packaged and stored in sealed containers to maintain its stability and prevent degradation from moisture and air exposure.

This production method is used to create barium peroxide for various industrial uses.
The reaction conditions (such as temperature and pressure) must be precisely controlled to maximize yield and prevent the formation of unwanted by-products.
Historically, this method was also important in the early development of oxygen generation techniques.

Structure of Barium Peroxide:
Barium peroxide is a peroxide, containing O2− 2 subunits.
The solid is isomorphous to calcium carbide, CaC2.

Pharmacology and Biochemistry of Barium Peroxide:

Metabolism / Metabolites:
Barium peroxide compounds are absorbed via ingestion and inhalation, the extent of which depends on the individual compound.
In the body, the majority of the barium is found in the bone, while small amounts exists in the muscle, adipose, skin, and connective tissue. 

Barium peroxide is not metabolized in the body, but it may be transported or incorporated into complexes or tissues.
Barium peroxide is excreted in the urine and faeces.

History of Barium Peroxide:
Barium peroxide was first discovered in 1799 by the German chemist Johann Bartholomäus Trommsdorff.
He was experimenting with various barium salts and noted that barium oxide, when exposed to air, formed a compound which he identified as barium peroxide.
In the 19th century, barium peroxide gained industrial significance due to its role in the production of hydrogen peroxide, which was not easily accessible until then.

Barium peroxide was later used by German chemist Justus von Liebig to synthesize hydrogen peroxide (H₂O₂) in 1818 by treating BaO₂ with acid.
This method became one of the earliest ways to produce hydrogen peroxide on a commercial scale.

Occurrence of Barium Peroxide:
Barium peroxide does not occur naturally in large quantities due to its relatively unstable nature under normal environmental conditions.
Barium peroxide is typically synthesized from barium oxide (BaO) through oxidation.
In industrial settings, Barium peroxide is produced by heating barium oxide in air or oxygen at high temperatures.

Due to its oxidative properties, barium peroxide is used in a variety of applications, including:
As an oxidizing agent in pyrotechnics and fireworks, where Barium peroxide imparts a green color to flames.
In the production of hydrogen peroxide, where Barium peroxide served as a primary source before modern methods were developed.
In the glass and ceramics industry, where Barium peroxide is sometimes added to improve the characteristics of certain glass formulations.

Though barium peroxide was more prominent in historical industrial chemistry, its use has declined with the advent of more efficient ways to produce hydrogen peroxide and other oxidizing agents.

Handling and Storage of Barium Peroxide:

Handling:
Handle barium peroxide in a well-ventilated area.
Avoid generating dust; use protective equipment (gloves, safety goggles, dust masks) to prevent exposure.

Keep away from incompatible materials such as reducing agents, organic materials, and acids.
Avoid contact with skin, eyes, and clothing, and do not inhale dust.
Wash hands thoroughly after handling.

Storage:
Store in a cool, dry, well-ventilated place away from sources of ignition.
Store in tightly closed containers, away from organic materials, acids, combustibles, and moisture.

Containers should be clearly labeled and kept in a segregated area due to Barium peroxide's reactive nature.
Keep away from light and heat sources.

Stability and Reactivity of Barium Peroxide:

Stability:
Barium peroxide is stable under normal conditions of storage and handling.
However, Barium peroxide decomposes at elevated temperatures.

Reactivity:

Incompatible materials:
Acids (which can release oxygen), organic materials, and reducing agents.

Decomposition:
When heated or exposed to moisture, Barium peroxide may release oxygen, which could intensify fires.

Hazardous reactions:
Reacts violently with acids and combustible materials.

First Aid Measures of Barium Peroxide:

Inhalation:
Move the exposed person to fresh air immediately.
If breathing is difficult, give oxygen, and seek medical attention.

Skin Contact:
Wash affected area with plenty of water for at least 15 minutes.
Remove contaminated clothing and wash Barium peroxide before reuse.
Seek medical attention if irritation persists.

Eye Contact:
Flush eyes with water for at least 15 minutes, holding eyelids apart.
Seek immediate medical attention.

Ingestion:
Do not induce vomiting.
Rinse mouth thoroughly with water.

Seek immediate medical attention.
Barium compounds can be toxic if ingested, and professional treatment may include giving the person a solution containing sulfate to precipitate barium as barium sulfate.

Firefighting Measures of Barium Peroxide:

Extinguishing Media:
Use water spray, alcohol-resistant foam, or carbon dioxide (CO₂).
Do not use dry chemical extinguishers as these can react with barium peroxide.

Firefighting Instructions:
Firefighters should wear self-contained breathing apparatus (SCBA) and full protective gear.
Keep cool containers that are exposed to flames using water spray to prevent rupture.

As barium peroxide releases oxygen when heated, it can intensify fires.
Water is preferred as an extinguishing medium, but avoid using water directly on the material unless cooling containers.

Hazards:
The decomposition of barium peroxide can release oxygen, increasing the risk of fire or explosion when in contact with flammable materials.

Accidental Release Measures of Barium Peroxide:

Personal Protection:
Evacuate the area and ventilate Barium peroxide properly.
Wear protective gear including gloves, goggles, and respirators to avoid contact with the material.

Environmental Precautions:
Prevent the release of barium peroxide into water sources or sewers, as it is hazardous to aquatic life.

Cleanup:
Sweep up the spilled material using non-sparking tools and place Barium peroxide in a suitable, labeled container for proper disposal.
Avoid creating dust and do not allow contact with organic materials or acids.

Disposal:
Dispose of the waste in accordance with local, state, and federal regulations, typically as hazardous waste.

Exposure Controls/Personal Protective Equipment of Barium Peroxide:

Exposure Controls:

Ventilation:
Use local exhaust ventilation or a fume hood to keep exposure levels below regulatory limits (e.g., OSHA PEL).

Exposure Limits:
Follow guidelines like ACGIH TLV and OSHA PEL for barium compounds.

Personal Protective Equipment (PPE):

Respiratory Protection:
If exposure levels exceed regulatory limits, use an approved respirator.

Hand Protection:
Wear protective gloves (rubber, neoprene, or nitrile) resistant to chemical agents.

Eye Protection:
Safety goggles or a full face shield to protect against dust or splashes.

Skin Protection:
Wear appropriate protective clothing to prevent skin exposure.

Hygiene:
Wash hands, face, and exposed skin thoroughly after handling.
Do not eat, drink, or smoke while handling the material.

Identifiers of Barium Peroxide:
CAS Number: 1304-29-6
ChemSpider: 14090
ECHA InfoCard: 100.013.754
EC Number: 215-128-4
PubChem CID: 14773
RTECS number: CR0175000
UNII: T892KY013Y
UN number: 1449
CompTox Dashboard (EPA): DTXSID9051294
InChI: InChI=1S/Ba.O2/c;1-2/q+2;-2
Key: ZJRXSAYFZMGQFP-UHFFFAOYSA-N
InChI=1/Ba.O2/c;1-2/q+2;-2
Key: ZJRXSAYFZMGQFP-UHFFFAOYAZ
SMILES: [Ba+2].[O-][O-]

CAS number: 1304-29-6
EC index number: 056-001-00-1
EC number: 215-128-4
Hill Formula: BaO₂
Molar Mass: 169.34 g/mol
HS Code: 2816 40 00
Quality Level: MQ200

Linear Formula: BaO2
MDL Number: MFCD00003454
EC No.: 215-128-4
Beilstein/Reaxys No.: N/A
Pubchem CID: 14773
IUPAC Name: barium(2+); peroxide
SMILES: [Ba+2].[O-][O-]
InchI Identifier: InChI=1S/Ba.O2/c;1-2/q+2;-2
InchI Key: ZJRXSAYFZMGQFP-UHFFFAOYSA-N

Properties of Barium Peroxide:
Chemical formula: BaO2
Molar mass: 169.33 g/mol (anhydrous)
313.45 (octahydrate)
Appearance: Grey-white crystalline (anhydrous)
colorless solid (octahydrate)
Odor: odorless
Density: 5.68 g/cm3 (anhydrous) 2.292 g/cm3 (octahydrate)
Melting point: 450 °C (842 °F; 723 K)
Boiling point: 800 °C (1,470 °F; 1,070 K) (decomposes to BaO & O2.[1])
Solubility in water: anhydrous
0.091 g/100 mL (20 °C)
octahydrate
0.168 g/cm3
Solubility: dissolves with decomposition in acid
Magnetic susceptibility (χ): -40.6·10−6 cm3/mol

Density: 4.96 g/cm3 (20 °C)
Melting Point: 450 °C
pH value: 12 (10 g/l, H₂O, 20 °C) (slurry)
Bulk density: 1700 - 2000 kg/m3

Molecular Weight: 169.33 g/mol
Hydrogen Bond Donor Count: 0
Hydrogen Bond Acceptor Count: 2
Rotatable Bond Count: 0
Exact Mass: 169.895076 g/mol
Monoisotopic Mass: 169.895076 g/mol
Topological Polar Surface Area: 46.1Ų
Heavy Atom Count: 3
Complexity: 2.8
Isotope Atom Count: 0
Defined Atom Stereocenter Count: 0
Undefined Atom Stereocenter Count: 0
Defined Bond Stereocenter Count: 0
Undefined Bond Stereocenter Count: 0
Covalently-Bonded Unit Count: 2
Compound Is Canonicalized: Yes

Structure of Barium Peroxide:
Crystal structure: Tetragonal
Space group: D174h, I4/mmm, tI6
Coordination geometry: 6

Specifications of Barium Peroxide:
Assay of peroxide (as BaO2): Min. 95 %
Insoluble in HCl: Max. 0.5 %
Loss on drying (105°C): Max. 1 %
Iron (Fe): Max. 0.005 %
Heavy metals (as Pb): Max. 0.01 %
Chloride (Cl): Max. 0.01 %
Substances not precipitated by H2SO4 (as SO4): Max. 1 %

Names of Barium Peroxide:

Regulatory process names:
Barium peroxide
BARIUM PEROXIDE
barium peroxide
Barium peroxide (Ba(O2))

Translated names:
Baariumperoksiid (et)
barijev peroksid (hr)
barijev peroksid (sl)
bario peroksidas (lt)
bariumperoksid (no)
Bariumperoksidi (fi)
bariumperoxid (da)
Bariumperoxid (de)
bariumperoxid (sv)
bariumperoxide (nl)
bárium-peroxid (hu)
bārija peroksīds (lv)
nadtlenek baru(II) (pl)
perossido di bario bario perossido (it)
peroxid barnatý (cs)
peroxid bárnatý (sk)
peroxide de bariu (ro)
peroxyde de baryum peroxyde de baryum (fr)
peróxido de bario dióxido de bario (es)
peróxido de bário (pt)
υπεροξείδιο του βαρίου (el)
бариев пероксид (bg)

IUPAC names:
Barium Peroxide
barium peroxide
Barium peroxide
barium(2+) ion dioxidanediide
barium(2+);peroxide
barium-peroxide-

Trade names:
Barium peroxide

Other names:
Barium binoxide
Barium dioxide

Other identifiers:
056-001-00-1
1304-29-6
16678-58-3
55396-27-5
61233-09-8

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