liitiumperoksiidi

Lithium peroxide (chemical formula Li₂O₂) is a white, crystalline solid that functions as a strong oxidizing agent. It belongs to the class of alkali‑metal peroxides and is typically obtained by reacting lithium hydroxide or lithium oxide with hydrogen peroxide. The reaction is highly exothermic and must be conducted under controlled conditions to avoid rapid decomposition and evolution of oxygen gas. In the laboratory, Li₂O₂ can be produced by passing a dry lithium metal solution over a stream of hydrogen peroxide at low temperature, or by electrolytic oxidation of lithium in an aqueous solution.

The material has a melting point of 801 °C and a density of 1.49 g cm⁻³. It is highly hygroscopic, absorbing moisture from the air to form lithium hydroxide and hydrogen peroxide. Lithium peroxide decomposes when heated, liberating oxygen and leaving lithium oxide as a residue. Because it is a potent oxidizer, Li₂O₂ can intensify combustion and must be stored away from organic materials and reducing agents.

Lithium peroxide is of particular interest in energy storage research. In lithium‑air battery concepts, Li₂O₂ forms at the negative electrode during discharge and is subsequently re‑reduced on recharge, thereby enabling high theoretical energy densities. It also finds use as an oxidizer in propellant mixtures for aerospace applications and as a component in some sterilization agents due to its ability to generate reactive oxygen species.

Handling of lithium peroxide requires strict safety measures: use of closed‑system containers, ventilation to prevent accumulation of oxygen, and protective equipment to mitigate skin and eye contact. Disposal guidelines recommend neutralization with a mild base followed by safe removal of metal ions. Regulatory agencies classify Li₂O₂ as a hazardous material, and its transport is governed by international regulations for oxidizing substances.