Magnesium peroxide

Last updated
Magnesium peroxide
FeS2structure.jpg
Names
IUPAC name
Magnesium peroxide
Other names
Magnesium dioxide, magnesium bioxide, UN 1476
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.034.928 OOjs UI icon edit-ltr-progressive.svg
EC Number
  • 238-438-1
PubChem CID
UNII
  • InChI=1S/Mg.O2/c;1-2/q+2;-2 Yes check.svgY
    Key: SPAGIJMPHSUYSE-UHFFFAOYSA-N Yes check.svgY
  • InChI=1/Mg.O2/c;1-2/q+2;-2
    Key: SPAGIJMPHSUYSE-UHFFFAOYAN
  • [Mg+2].[O-][O-]
Properties
MgO2
Molar mass 56.3038 g/mol
AppearanceWhite or off-white powder
Density 3 g/cm3
Melting point 223 °C (433 °F; 496 K)
Boiling point 350 °C (662 °F; 623 K) (decomposes)
insoluble
Structure
Cubic, cP12
Pa3, No. 205
Pharmacology
A02AA03 ( WHO ) A06AD03 ( WHO )
Hazards
GHS labelling:
GHS-pictogram-rondflam.svg
Warning
H272
P210, P220, P221, P280, P370+P378, P501
NFPA 704 (fire diamond)
NFPA 704.svgHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g. calciumSpecial hazard OX: Oxidizer. E.g. potassium perchlorate
2
0
1
OX
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
X mark.svgN  verify  (what is  Yes check.svgYX mark.svgN ?)

Magnesium peroxide (MgO2) is an odorless fine powder peroxide with a white to off-white color. It is similar to calcium peroxide because magnesium peroxide also releases oxygen by breaking down at a controlled rate with water. Commercially, magnesium peroxide often exists as a compound of magnesium peroxide and magnesium hydroxide.

Contents

Structure

O2, similarly to N2, has the ability to bind either side-on or end-on. The structure of MgO2 has been calculated as a triangular shape with the O2 molecule binding side-on to the magnesium. This arrangement is a result of the Mg+ donating charge to the oxygen and creating a Mg2+O22−. The bond between to O2 and the magnesium atom has an approximate dissociation energy of 90 kJ mol−1. [1]

In the solid state, MgO2 has a cubic pyrite-type crystal structure with 6-coordinate Mg2+ ions and O22− peroxide-groups, according to experimental data [2] and evolutionary crystal structure prediction, [3] the latter predicting a phase transition at the pressure of 53 GPa to a tetragonal structure with 8-coordinate Mg2+ ions. While at normal conditions MgO2 is a metastable compound (less stable than MgO + ½ O2), at pressures above 116 GPa it is predicted to become thermodynamically stable in the tetragonal phase. This theoretical prediction has been experimentally confirmed via synthesis in a laser-heated diamond anvil cell. [4]

Synthesis

MgO2 can be produced by mixing MgO with hydrogen peroxide to create magnesium peroxide and water. This being an exothermic reaction should be cooled and kept around 30–40 degrees Celsius. It is also important to remove as much iron from the reaction environment as possible due to iron's ability to catalyze the degradation of the peroxide. The addition of oxygen stabilizers such as sodium silicate can also be used to help prevent the premature degradation of the peroxide. Regardless, a good yield from this reaction is only about 35%. [5]

MgO + H2O2 → MgO2 + H2O

High yields are further complicated by the fact that MgO2 reacts with water to degrade the peroxide into magnesium hydroxide, also known as milk of magnesia.

Applications

Magnesium peroxide is a stable oxygen releasing compound, which is used in agricultural and environmental industries. It is used to reduce contaminant levels in groundwater. Magnesium peroxide is used in the bioremediation of contaminated soil and can improve the soil quality for plant growth and metabolism. It is also used in the aquaculture industry for bioremediation.

For sanitation purposes magnesium peroxide is often used as a source of oxygen for aerobic organisms in the treatment and disposal of biological waste. Since the breakdown of hydrocarbons in soil is usually quicker in aerobic conditions, MgO2 can also be added to compost piles or in soil to speed up the microbe activities and to reduce the odors produced in the process. [6]

In certain circumstances MgO2 has also been shown to inhibit growth of bacteria. In particular, the growth of sulfate-reducing bacteria can be inhibited in an environment containing magnesium peroxide. While the oxygen slowly dissociates, it is theorized that it may then act to displace the sulfate that normally acts as the terminal electron acceptor in their electron transport chain. [7]

Toxicity

Magnesium peroxide is an irritant that can cause redness, itching, swelling, and may burn the skin and eyes on contact. Inhalation can also cause irritation to the lungs, nose, and throat, as well as causing coughing. Long term exposure may lead to lung damage, shortness of breath, and tightening of the chest. Ingestion of MgO2 can cause numerous adverse effects including: bloating, belching, abdominal pain, irritation of the mouth and throat, nausea, vomiting, and diarrhea. [8] [9]

Environmentally, magnesium peroxide is not a naturally occurring compound and is not known to persist in the environment for prolonged times, in its complete state, or to bio-accumulate. The natural degradation of MgO2 leads to magnesium hydroxide, O2, and H2O. If spilled, MgO2 should be contained and isolated from any waterways, sewer drains, and it should be isolated from combustible materials or chemicals including paper, cloth, and wood. [6]

Common Environmental Reactions

Magnesium exists in the upper atmosphere in a variety of different molecular forms. Due to its ability to react with common oxygen and simple carbon-oxygen compounds the magnesium may exist in oxidized compounds including MgO2, OMgO2, MgO, and O2MgO2. [10]

MgCO3 + O → MgO2 + CO2
OMgO2 + O → MgO2 + O2
MgO + O3 → MgO2 + O2
MgO2 + O2 → O2MgO2
MgO2 + O → MgO + O2

In contact with water it decomposes by the reactions:

MgO2 + 2 H2O → Mg(OH)2 + H2O2
2 H2O2 → 2 H2O + O2

Related Research Articles

<span class="mw-page-title-main">Hydrogen peroxide</span> Chemical compound

Hydrogen peroxide is a chemical compound with the formula H2O2. In its pure form, it is a very pale blue liquid that is slightly more viscous than water. It is used as an oxidizer, bleaching agent, and antiseptic, usually as a dilute solution in water for consumer use and in higher concentrations for industrial use. Concentrated hydrogen peroxide, or "high-test peroxide", decomposes explosively when heated and has been used as both a monopropellant and an oxidizer in rocketry.

<span class="mw-page-title-main">Magnesium</span> Chemical element with atomic number 12 (Mg)

Magnesium is a chemical element; it has symbol Mg and atomic number 12. It is a shiny gray metal having a low density, low melting point and high chemical reactivity. Like the other alkaline earth metals it occurs naturally only in combination with other elements and almost always has an oxidation state of +2. It reacts readily with air to form a thin passivation coating of magnesium oxide that inhibits further corrosion of the metal. The free metal burns with a brilliant-white light. The metal is obtained mainly by electrolysis of magnesium salts obtained from brine. It is less dense than aluminium and is used primarily as a component in strong and lightweight alloys that contain aluminium.

In chemistry, a half reaction is either the oxidation or reduction reaction component of a redox reaction. A half reaction is obtained by considering the change in oxidation states of individual substances involved in the redox reaction. Often, the concept of half reactions is used to describe what occurs in an electrochemical cell, such as a Galvanic cell battery. Half reactions can be written to describe both the metal undergoing oxidation and the metal undergoing reduction.

<span class="mw-page-title-main">Magnesium oxide</span> Chemical compound naturally occurring as periclase

Magnesium oxide (MgO), or magnesia, is a white hygroscopic solid mineral that occurs naturally as periclase and is a source of magnesium (see also oxide). It has an empirical formula of MgO and consists of a lattice of Mg2+ ions and O2− ions held together by ionic bonding. Magnesium hydroxide forms in the presence of water (MgO + H2O → Mg(OH)2), but it can be reversed by heating it to remove moisture.

<span class="mw-page-title-main">Magnesium hydroxide</span> Inorganic compound of formula Mg(OH)2

Magnesium hydroxide is an inorganic compound with the chemical formula Mg(OH)2. It occurs in nature as the mineral brucite. It is a white solid with low solubility in water (Ksp = 5.61×10−12). Magnesium hydroxide is a common component of antacids, such as milk of magnesia.

<span class="mw-page-title-main">Bioremediation</span> Process used to treat contaminated media such as water and soil

Bioremediation broadly refers to any process wherein a biological system, living or dead, is employed for removing environmental pollutants from air, water, soil, flue gasses, industrial effluents etc., in natural or artificial settings. The natural ability of organisms to adsorb, accumulate, and degrade common and emerging pollutants has attracted the use of biological resources in treatment of contaminated environment. In comparison to conventional physicochemical treatment methods bioremediation may offer advantages as it aims to be sustainable, eco-friendly, cheap, and scalable.

<span class="mw-page-title-main">Magnesium chloride</span> Inorganic salt: MgCl2 and its hydrates

Magnesium chloride is an inorganic compound with the formula MgCl2. It forms hydrates MgCl2·nH2O, where n can range from 1 to 12. These salts are colorless or white solids that are highly soluble in water. These compounds and their solutions, both of which occur in nature, have a variety of practical uses. Anhydrous magnesium chloride is the principal precursor to magnesium metal, which is produced on a large scale. Hydrated magnesium chloride is the form most readily available.

<span class="mw-page-title-main">Calcium peroxide</span> Chemical compound

Calcium peroxide or calcium dioxide is the inorganic compound with the formula CaO2. It is the peroxide (O22−) salt of Ca2+. Commercial samples can be yellowish, but the pure compound is white. It is almost insoluble in water.

<span class="mw-page-title-main">Hypochlorite</span> Anion

In chemistry, hypochlorite, or chloroxide is an anion with the chemical formula ClO−. It combines with a number of cations to form hypochlorite salts. Common examples include sodium hypochlorite and calcium hypochlorite. The Cl-O distance in ClO− is 1.69 Å.

In chemistry, disproportionation, sometimes called dismutation, is a redox reaction in which one compound of intermediate oxidation state converts to two compounds, one of higher and one of lower oxidation state. The reverse of disproportionation, such as when a compound in an intermediate oxidation state is formed from precursors of lower and higher oxidation states, is called comproportionation, also known as symproportionation.

<span class="mw-page-title-main">Potassium superoxide</span> Chemical compound

Potassium superoxide is an inorganic compound with the formula KO2. It is a yellow paramagnetic solid that decomposes in moist air. It is a rare example of a stable salt of the superoxide anion. It is used as a CO2 scrubber, H2O dehumidifier, and O2 generator in rebreathers, spacecraft, submarines, and spacesuits.

<span class="mw-page-title-main">Sodium peroxide</span> Chemical compound

Sodium peroxide is an inorganic compound with the formula Na2O2. This yellowish solid is the product of sodium ignited in excess oxygen. It is a strong base. This metal peroxide exists in several hydrates and peroxyhydrates including Na2O2·2H2O2·4H2O, Na2O2·2H2O, Na2O2·2H2O2, and Na2O2·8H2O. The octahydrate, which is simple to prepare, is white, in contrast to the anhydrous material.

<span class="mw-page-title-main">Telluric acid</span> Chemical compound (Te(OH)6)

Telluric acid, or more accurately orthotelluric acid, is a chemical compound with the formula Te(OH)6, often written as H6TeO6. It is a white crystalline solid made up of octahedral Te(OH)6 molecules which persist in aqueous solution. In the solid state, there are two forms, rhombohedral and monoclinic, and both contain octahedral Te(OH)6 molecules, containing one hexavalent tellurium (Te) atom in the +6 oxidation state, attached to six hydroxyl (–OH) groups, thus, it can be called tellurium(VI) hydroxide. Telluric acid is a weak acid which is dibasic, forming tellurate salts with strong bases and hydrogen tellurate salts with weaker bases or upon hydrolysis of tellurates in water. It is used as tellurium-source in the synthesis of oxidation catalysts.

<span class="mw-page-title-main">Hydroperoxide</span> Class of chemical compounds

Hydroperoxides or peroxols are compounds of the form ROOH, where R stands for any group, typically organic, which contain the hydroperoxy functional group. Hydroperoxide also refers to the hydroperoxide anion and its salts, and the neutral hydroperoxyl radical (•OOH) consist of an unbond hydroperoxy group. When R is organic, the compounds are called organic hydroperoxides. Such compounds are a subset of organic peroxides, which have the formula ROOR. Organic hydroperoxides can either intentionally or unintentionally initiate explosive polymerisation in materials with unsaturated chemical bonds.

<span class="mw-page-title-main">Sodium formate</span> Chemical compound

Sodium formate, HCOONa, is the sodium salt of formic acid, HCOOH. It usually appears as a white deliquescent powder.

<span class="mw-page-title-main">Lithium peroxide</span> Chemical compound

Lithium peroxide is the inorganic compound with the formula Li2O2. Lithium peroxide is a white solid, and unlike most other alkali metal peroxides, it is nonhygroscopic. Because of its high oxygen:mass and oxygen:volume ratios, the solid has been used to remove CO2 from and release O2 to the atmosphere in spacecraft.

Zinc compounds are chemical compounds containing the element zinc which is a member of the group 12 of the periodic table. The oxidation state of zinc in most compounds is the group oxidation state of +2. Zinc may be classified as a post-transition main group element with zinc(II). Zinc compounds are noteworthy for their nondescript appearance and behavior: they are generally colorless, do not readily engage in redox reactions, and generally adopt symmetrical structures.

<span class="mw-page-title-main">Magnesium bicarbonate</span> Chemical compound

Magnesium bicarbonate or magnesium hydrogencarbonate, Mg(HCO3)2, is the bicarbonate salt of magnesium. It can be formed through the reaction of dilute solutions of carbonic acid (such as seltzer water) and magnesium hydroxide (milk of magnesia).

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<span class="mw-page-title-main">Metal peroxide</span> Metal-containing compounds with peroxide (O2) ions/groups

In chemistry, metal peroxides are metal-containing compounds with ionically- or covalently-bonded peroxide groups. This large family of compounds can be divided into ionic and covalent peroxide. The first class mostly contains the peroxides of the alkali and alkaline earth metals whereas the covalent peroxides are represented by such compounds as hydrogen peroxide and peroxymonosulfuric acid. In contrast to the purely ionic character of alkali metal peroxides, peroxides of transition metals have a more covalent character.

References

  1. ↑ Plowright, Richard J.; Thomas J. McDonnell; Timothy G. Wright; John M. C. Plane (28 July 2009). "Theoretical Study of Mg+−X and [X−Mg−Y]+Complexes Important in the Chemistry of Ionospheric Magnesium (X, Y = H2O, CO2, N2, O2, and O)". Journal of Physical Chemistry. 113 (33): 9354–9364. Bibcode:2009JPCA..113.9354P. doi:10.1021/jp905642h. PMID   19637880.
  2. ↑ Vannerberg N. (1959). "The formation and structure of magnesium peroxide". Ark. Kemi. 14: 99–105.
  3. ↑ Zhu, Qiang; Oganov, Artem R.; Lyakhov, Andriy O. (2013). "Novel stable compounds in the Mg–O system under high pressure". Physical Chemistry Chemical Physics. 15 (20): 7696–700. Bibcode:2013PCCP...15.7696Z. doi:10.1039/c3cp50678a. PMID   23595296.
  4. ↑ Lobanov, Sergey S.; Zhu, Qiang; Holtgrewe, Nicholas; Prescher, Clemens; Prakapenka, Vitali B.; Oganov, Artem R.; Goncharov, Alexander F. (1 September 2015). "Stable magnesium peroxide at high pressure". Scientific Reports. 5 (1): 13582. arXiv: 1502.07381 . Bibcode:2015NatSR...513582L. doi:10.1038/srep13582. PMC   4555032 . PMID   26323635.
  5. ↑ Shand, Mark A. (2006). The Chemistry and Technology of Magnesia. John Wiley & Sons. ISBN   978-0-471-98056-8.[ page needed ]
  6. 1 2 Vidali, M. (1 July 2001). "Bioremediation. An overview". Pure and Applied Chemistry. 73 (7): 1163–1172. doi: 10.1351/pac200173071163 . S2CID   18507182.
  7. ↑ Chang, Yu-Jie; Yi-Tang Chang; Chun-Hsiung Hung (2008). "The use of magnesium peroxide for the inhibition of sulfate-reducing bacteria under anoxic conditions". J Ind Microbiol Biotechnol. 35 (11): 1481–1491. doi: 10.1007/s10295-008-0450-6 . PMID   18712535. S2CID   13089863.
  8. ↑ "Product Safety Summary: Magnesium Peroxide" (PDF). Solvay America Inc. Retrieved 25 April 2012.
  9. ↑ Pohanish, Richard P. (2011). Sittig's Handbook of Toxic and Hazardous Chemicals and Carcinogens. William Andrew. pp. 1645–1646. ISBN   978-1437778700.
  10. ↑ Plane, John M. C.; Charlotte L. Whalley (2012). "A New Model for Magnesium Chemistry in the Upper Atmosphere". Journal of Physical Chemistry A. 116 (24): 6240–6252. Bibcode:2012JPCA..116.6240P. doi:10.1021/jp211526h. PMID   22229654.
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