Zinc peroxide

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Zinc peroxide
Zinc peroxide
CAS number 1314-22-3 YesY
PubChem 10129902
Molecular formula ZnO2
Molar mass 97.408 g/mol
Appearance white-yellowish powder
Density 1.57 g/cm3
Melting point 212°C (decomposes)
Acidity (pKa) ~7 (3% solution)
Band gap 3.8 eV (indirect) [1]
Crystal structure Cubic
Space group Pa-3
EU classification not listed
NFPA 704
Flammability code 0: Will not burn. E.g., water Health code 3: Short exposure could cause serious temporary or residual injury. E.g., chlorine gas Reactivity code 1: Normally stable, but can become unstable at elevated temperatures and pressures. E.g., calcium Special hazards (white): no codeNFPA 704 four-colored diamond
Except where noted otherwise, data are given for materials in their standard state (at 25 °C (77 °F), 100 kPa)
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Infobox references

Zinc peroxide (ZnO2) appears as a bright yellow powder at room temperature. It was historically used as a surgical antiseptic. More recently zinc peroxide has also been used as an oxidant in explosives and pyrotechnic mixtures. Its properties have been described as a transition between ionic and covalent peroxides.[2] Zinc peroxide can be synthesized through the reaction of zinc chloride and hydrogen peroxide.[3]


Zinc peroxide forms a cubic crystalline structure similar to that of FeS2. Zinc peroxide is scarcely soluble in water. In the presence of other inorganic compounds or metal ions, it decomposes rapidly above room temperature. One oxygen atom tends to split off at temperatures exceeding 150°C.[4]


Since the 1930s Zinc peroxide has been applied in a variety of settings, from medicine to aesthetics and even fireworks.[3]

Medical Use[edit]

The treatment of burrowing ulcers in the abdominal wall with Zinc Peroxide was first recorded in 1933 and throughout the 1940s ZnO2 was used as a disinfectant in surgical infections.[5] Zinc Peroxide was, however, deemed ineffective against certain bacterial strains, such as Streptococcus viridans, staphylococcus aureus, E. coli, B. proteus, and B. pyocyoneus. One aspect of the compound’s microorganism toxicity is the resultant stagnation of microbial populations upon administration. This effect was hypothesized to depend upon the compound’s penchant for oxygen donation. It has been suggested that the increase in oxygen concentration associated with the presence of ZnO2 interferes with the replicative processes of anaerobic and micro-aerophillic organisms, both of which require low oxygen environments for their survival.[6] While this mechanism was sufficient to explain the stagnation of microbe populations, it did not account for the active reduction in colony size. As to the microbicidal function, the Zinc ion itself has been postulated to have antibacterial properties, facilitated by the binding of the Zn ion to the bacterial cell wall, which allows for the exertion of cytotoxic effects. Zn has been observed to be more effective in the elimination of gram-positive bacteria than gram-negative bacteria. This difference has been attributed to a difference in the protein composition of the respective cell walls, with the gram-positive wall providing a composition more conducive to binding.[7]

Mineral stain[edit]

Recently the compound has found use as a mineral stain for wood and other substances. The mechanism of this action involves the application of a metal salt (such as iron chloride[disambiguation needed]) and the zinc peroxide to the substrate material (wood or wood-like material, i.e. bamboo, paper, cloths, and cellulose products). The metal salt is applied in solution and allowed to dry for up to 30 minutes. Next, zinc peroxide is applied, also in solution. Color change is immediately visible. The two solutions soak into the material, and react, thereby becoming ingrained in the matrix of the substrate. While these stains can produce a variety of colors ranging from a reddish brown to a yellow hue, they are generally used to mimic the look of endangered wood species in cheaper and more commonly available stock.[8]


In the 1980s the discovery of zinc peroxide’s ability to complement pyrotechnical mixtures was discovered. It was noted that ZnO2 was preferable to the usage of barium compounds, as it was deemed to be less toxic. The zinc compound proves an effective component in explosives because of its oxidizing properties. Many chemical explosives rely on rapid oxidation reactions, for this reason ZnO2 is an ideal candidate for use in pyrotechnics. Another advantage of ZnO2 was, as compared to the barium and strontium pyroingredients, it effects less corrosion in the metallic materials which contain the compounds in the pyrotechnic instrument. In one modality it is necessary for zinc peroxide to act in conjunction with a reducer like calcium silicate, to create the necessary red/ox reaction. In another modality, a ‘secondary’ explosive is mixed with zinc peroxide. Secondary explosives include nitrocellulose, pentaerythritol tetranitrate (PETN), as well as a variety of compounds, like trinitrobenzene, which provide powerful negative charge balance.[9] These secondary explosives are relatively insensitive to stimuli such as physical impact, heat or charge. The explosive mixture would be comprised, in bulk, of the secondary explosive with a much smaller fraction of Zinc Peroxide, present to initiate the reaction.


Zinc peroxide is very hazardous in case of skin contact, of eye contact, ingestion, or inhalation. It has been shown to be corrosive to skin. Prolonged exposure may result in skin burns and ulcerations. Over-exposure by inhalation may cause respiratory irritation. Skin inflammation is characterized by itching, scaling, reddening, or, occasionally, blistering. Zinc Peroxide is toxic to lungs and mucous membranes. Repeated or prolonged exposure can produce organ damage. Repeated or prolonged inhalation of vapors may lead to chronic respiratory irritation.[10]


  1. ^ A.L. Companion (1962). "The diffuse reflectance spectra of zinc oxide and zinc peroxide". Journal of Physics and Chemistry of Solids 23 (12): 1685. doi:10.1016/0022-3697(62)90205-6. 
  2. ^ R.D. Ayengar (1971). "ESR Studies on Zinc Peroxide and Zinc Oxide Obtained from a Decomposition of Zinc Peroxide". J. Phys. Chem. 75 (20): 3089. doi:10.1021/j100689a009. 
  3. ^ a b W. Chen (2009). "Synthesis, Thermal Stability and Properties of Zinc Peroxide Nanoparticles". J. Phys. Chem. 113 (4): 1320. 
  4. ^ M. Eagleson (1993). Concise Encyclopedia Chemistry. Walter de Gruyter & Co. 
  5. ^ F. Meleney (1941). "Zinc Peroxide in Surgical Infections". The American Journal of Nursing. 41 (6): 645. doi:10.1097/00000446-194106000-00004. 
  6. ^ B. Johnson, et al (1939). "The Antiseptic and Detoxifying Actions of Zinc Peroxide on Certain Aerobic, Anaerobic and Micro-aerophilic Bacteria". Annals of Surgery 109 (6): 595. doi:10.1097/00000658-193906000-00001. 
  7. ^ S. Atmaca, et al (1998). "The Effect of Zinc on Microbial Growth". Turkish J. of Medical Science 28: 595. 
  8. ^ ["http://osdir.com/patents/Dyeing-textiles/Mineral-stains-wood-substrates-06905520.html" "Peroxide Mineral Stain"]. Retrieved 2012-05-27. 
  9. ^ ["http://ip.com/patent/US4363679" "Zinc Peroxide Pyrotechnic Patent"]. Retrieved 2012-05-27. 
  10. ^ "Zinc Peroxide Material Safety Sheet". Retrieved 2012-05-27.