zinc peroxide

In another modality, a 'secondary' explosive is mixed with zinc peroxide.

Next, zinc peroxide is applied, also in solution.

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

In the 1980s the discovery of zinc peroxide's ability to complement pyrotechnical mixtures was discovered.

Zinc peroxide (ZnO) appears as a bright yellow powder at room temperature.

More recently zinc peroxide has also been used as an oxidant in explosives and pyrotechnic mixtures.

Zinc peroxide forms a cubic crystalline structure similar to that of FeS.

Zinc peroxide is scarcely soluble in water.

Zinc peroxide is very hazardous in case of skin contact, of eye contact, ingestion, or inhalation.

Zinc peroxide can be synthesized through the reaction of zinc chloride and hydrogen peroxide.

Aryl alkyl (E)-enones have been epoxidized with high enantioselectivity using stoichiometric zinc peroxide systems.

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.

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.

The mechanism of this action involves the application of a metal salt (such as iron chloride) and the zinc peroxide to the substrate material (wood or wood-like material, i.e. bamboo, paper, cloths, and cellulose products).