12031-80-0

Basic information

• Product Name: Lithium peroxide
• Synonyms: Li2O2;Lithium peroxide (Li2(O2));lithiumoxide(li2o2);lithiumperoxide(li2(o2));dilithium peroxide;LITHIUM PEROXIDE, TECH., 90%;Lithium peroxide, 90% min;Peroxydilithium
• CAS NO: 12031-80-0
• Molecular Formula: Li₂O₂
• Molecular Weight: 45.88
• EINECS: 234-758-0
• Product Categories: LithiumSynthetic Reagents;Metal and Ceramic Science;Oxidation;Oxides;Peroxides
• Mol File: 12031-80-0.mol
• Article Data: 4

Chemical Properties

• Melting Point: 340°C (dec.)
• Boiling Point: 150.2°Cat760mmHg
• Flash Point: °C
• Appearance: White to pale yellow/Powder
• Density: 2.310
• Solubility: Soluble in anhydrous acetic acid. Insoluble in alcohol.
• Water Solubility: solubility in H2O is 8% (20°C); solubility in acetic acid is 5.6% (20°C); insoluble absolute alcohol (20°C) [HAW93]
• Sensitive: Air & Moisture Sensitive
• CAS DataBase Reference: Lithium peroxide(CAS DataBase Reference)
• NIST Chemistry Reference: Lithium peroxide(12031-80-0)
• EPA Substance Registry System: Lithium peroxide(12031-80-0)

Safety Data

• Hazard Codes: O,C
• Statements: 8-35
• Safety Statements: 8-26-27-28-36/37/39-45
• RIDADR: UN 1472 5.1/PG 2
• WGK Germany: 3
• F: 3-10-23
• TSCA: Yes
• HazardClass: 5.1
• PackingGroup: II
• Hazardous Substances Data: 12031-80-0(Hazardous Substances Data)

Usage

Description

Lithium peroxide, also known as lithium dioxide, is a white crystalline solid or pale yellow powder with a chemical formula of Li2O2. It is thermodynamically stable at room temperature and has an active oxygen content of 34.8%, which is the highest among all metal peroxides. Lithium peroxide is used to produce a supply of high-purity oxygen and is known for its potential applications in atmosphere regeneration for undersea and space applications.

Uses

Used in Air Purifiers:
Lithium peroxide is used as an air purifier to produce high-purity oxygen, making it suitable for various applications where clean air is required.
Used in Oxygen Production:
Lithium peroxide is used as a source of high-purity oxygen, which can be utilized in various industries and applications where oxygen is needed.
Used in Polymerization Catalysts:
Lithium peroxide acts as a catalyst for the polymerization of styrene to polystyrene, a process that is essential in the production of various plastics and materials.
Used in Curing Agents for Special Polymers:
Lithium peroxide serves as a curing agent for special polymers, enhancing their properties and performance in specific applications.
Used in Sealed Spaces:
Lithium peroxide is used as a source of oxygen in sealed spaces such as submarines and in breathing apparatus, providing a reliable supply of oxygen in confined environments.
Used in Atmosphere Regeneration:
One interesting potential application of lithium peroxide is in the field of atmosphere regeneration for undersea and space applications. The compound reacts with carbon dioxide to release oxygen, making it a promising candidate for life support systems in extreme environments.
Used in Chemical Preparation:
The decomposition of lithium peroxide forms the basis for the preparation of lithium oxide, which is used in various chemical processes and applications.

Preparation

Lithium peroxide is prepared industrially by the reaction of lithium hydroxide monohydrate with hydrogen peroxide which yields lithium hydroperoxide monohydrate. LiOH·H20 + H202 → LiOOH·H20+H20 The hydroperoxide may be dehydrated by heating in a vacuum to yield the peroxide. 2LiOOH·H20 → Li202+H202 + 2H20

Air & Water Reactions

Contact with water or moist air generates a large amount of heat and corrosive, alkaline lithium hydroxide [AAR 1991].

Reactivity Profile

Lithium peroxide is strongly basic and an extremely powerful oxidizing agent. Accelerates the combustion of other materials, especially organic materials, involved in a fire. Can ignite wood, paper, oil, clothing, etc. on contact. May react explosively with hydrocarbons (fuels). Exposure to heat in a closed container may result in a vigorous reaction that violently ruptures the container.

Health Hazard

TOXIC; inhalation, ingestion or contact (skin, eyes) with vapors, dusts or substance may cause severe injury, burns or death. Fire may produce irritating and/or toxic gases. Toxic fumes or dust may accumulate in confined areas (basement, tanks, hopper/tank cars, etc.). Runoff from fire control or dilution water may cause pollution.

Fire Hazard

May explode from friction, heat or contamination. These substances will accelerate burning when involved in a fire. May ignite combustibles (wood, paper, oil, clothing, etc.). Some will react explosively with hydrocarbons (fuels). Containers may explode when heated. Runoff may create fire or explosion hazard.

Flammability and Explosibility

Notclassified

Safety Profile

A powerful oxidizer and irritant to skin, eyes, and mucous membranes. A very dangerous fire hazard because it is an extremely powerful oxidizing agent. Will react with water or steam to produce heat; on contact with reducing materials, can react vigorously. See also LITHIUM COMPOUNDS, PEROXIDES, and PEROXIDES, INORGANIC.

InChI:InChI=1/2Li.2O/rLi2O2/c1-3-2-4-1

Synthetic route

oxygen (80937-33-3) + bis(trifluoromethane)sulfonimide lithium (90076-65-6) → lithium peroxide (12031-80-0)

Conditions	Yield
With 1-butyl-methylpyrrolidinium bis(trifluoromethylsulfonyl)amide Electrochemical reaction;

lithium perchlorate + tetramethylammonium superoxide (62205-77-0) → lithium peroxide (12031-80-0)

Conditions	Yield
In acetonitrile at 20℃; for 1h; Glovebox; Inert atmosphere;

oxygen (80937-33-3) + lithium perchlorate → lithium peroxide (12031-80-0)

Conditions	Yield
With ruthenium oxide nanoparticle decorated mesoporous boron doped carbon nitride electrode In dimethyl sulfoxide at 80℃; for 48h; Mitsunobu Displacement; Electrochemical reaction; Glovebox;

lithium hydroxide monohydrate (1310-66-3) + dihydrogen peroxide (7722-84-1) → lithium peroxide (12031-80-0)

Conditions	Yield
for 1h;

hydrogenchloride (7647-01-0) + lithium peroxide (12031-80-0) + lithium chloride + lithium hydroxide (1310-65-2) + ruthenium (7440-18-8) → Li8Ru2OCl14

Conditions	Yield
Stage #1: lithium peroxide; lithium hydroxide; ruthenium In melt at 600℃; for 0.5h; Stage #2: hydrogenchloride; lithium chloride	60%

lithium peroxide (12031-80-0) + neptunium(IV) dioxide → NpO6(5-)*5Li(1+)=Li5NpO6

Conditions	Yield
In solid NpO2 and Li2O2 ground together, heated at 400°C for 24-72 h under O2; cooled, analyzed, reground, reheated until const. Np(VII) content (about 80-85%), not pure material(!);

lithium peroxide (12031-80-0) + cesium oxo terbate (IV) → cesium oxide + Cs2Li14{Tb3O14} + octalithium oxo terbate (IV)

Conditions	Yield
In neat (no solvent) byproducts: O2; tempering (ratio Tb:Li 1:5, 550°C, closed Au-tube, 3 weeks, heating rate 10°C/h);

lithium peroxide (12031-80-0) + terbium oxide + cesium oxo terbate (IV) → Cs2Li14{Tb3O14}

Conditions	Yield
In neat (no solvent) byproducts: O2; tempering (560°C, closed Au-tube, 10 d or 8 weeks);

lithium peroxide (12031-80-0) + copper(II) oxide → lithium cuprate (12527-46-7)

Conditions	Yield
With oxygen heating (platinum crucible, oxygen flow, 500°C, 5 d);
450°C for 5 d;

nickel(II) oxide (1313-99-1) + lithium peroxide (12031-80-0) → lithium nickelate(III)

Conditions	Yield
educts were ground together in an argon grove box and were pelletized, pellets were heated to 850°C very slowly under a stream of pure dried O2 passed through liquid N2 (24-48 h); cooling to room temp. very slowly;

lithium peroxide (12031-80-0) → oxygen (7782-44-7)

Conditions	Yield
With hydrogenchloride In neat (no solvent) solid peroxide exposured to gaseous haloid acid; not isolated, detected by emission spectroscopy;

lithium peroxide (12031-80-0) → octalithium oxo terbate (IV)

Conditions	Yield
With TbO(x) In neat (no solvent) in a sealed Ag-bomb, 700°C for 7 d, excess of Li2O2;;

lithium peroxide (12031-80-0) → octalithium oxo praseodymate (IV)

Conditions	Yield
With PrO(x) In neat (no solvent) sealed Ag-bomb, 700°C for 7 d, excess of Li2O2;;

cobalt(II,III) oxide + lithium peroxide (12031-80-0) → lithium cobalt(III) oxide

Conditions	Yield
In neat (no solvent) mixt. of Li2O2 and Co3O4 ball milled for 30 min and heated at 800°C for 5 h under air flow; detn. by induced coupled plasma (ICP) anal. and XRD;
Stage #1: cobalt(II,III) oxide; lithium peroxide With oxygen at 750℃; for 16h; Glovebox; Stage #2: With oxygen at 700℃; for 16h;

lithium peroxide (12031-80-0) + curium oxide → Cm(x)Li(x)O(x)

Conditions	Yield
Grounding the oxides in an agate mortar, heating the mixt. (ratio Li:Cm=8:1) for 10 min at 600°C.;

lithium peroxide (12031-80-0) + lithium arsenite → lithium arsenate

Conditions	Yield
With dihydrogen peroxide In water soln. of LiAsO2 in distd. H2O, continually stirred (10 min), addn. of Li2O2, exothermic reaction, kept 20 min, addn. of 30% H2O2; filtration, evapn. (on a water bath), crystn., crystals dried in a drying cupboard at 160-170°C to constant mass (5 h); elem. anal.;	99.3-99.8

lithium peroxide (12031-80-0) + tellurium oxide (13451-18-8) + lithium oxide → Li6TeO6

Conditions	Yield
In neat (no solvent) heating (700-800°C, closed Au- or Ag-tubes);

lithium peroxide (12031-80-0) + manganese(II) oxide → lithium manganate + LiMnO3

lithium peroxide (12031-80-0) + manganese(II) oxide → Li0.33Mn0.67O

Conditions	Yield
at 600°C;

lithium peroxide (12031-80-0) + manganese(II) oxide → Li0.35Mn0.65O + Li0.6Mn0.4O + Li0257Mn0743O

Conditions	Yield
at 900°C, tempering at 750°C;

lithium peroxide (12031-80-0) + manganese(II) oxide → lithium manganate

Conditions	Yield
in vac. for 5 h;

lithium peroxide (12031-80-0) + manganese(II) oxide → Li0135Mn0865O

Conditions	Yield
at 700°C;

lithium peroxide (12031-80-0) + manganese(II) oxide → Li0046Mn0954O

Conditions	Yield
at 600°C;

lithium peroxide (12031-80-0) + manganese(II) oxide → (x)LiMn2O4*(y)α-Mn2O3

Conditions	Yield
sintering for 24 h in a Pt vessel at 600 - 900°C under 0.3 atm Ar;

lithium peroxide (12031-80-0) + manganese(II) oxide → Li0308Mn0692O

Conditions	Yield
at 800°C;

lithium peroxide (12031-80-0) + uranium oxide → Li6O6U, α

Conditions	Yield
heating at 600°C for 7 days;;
heating at 910°C for 3 days; at 800°C for 5 days; at 660°C for 7 days; cooling;;

nickel(II) oxide (1313-99-1) + lithium peroxide (12031-80-0) → Li0.96Ni1.04O2

Conditions	Yield
In neat (no solvent) (Ar), mixing, pelletizing, heating (flowing O2, 850°C, 48 h);

nickel(II) oxide (1313-99-1) + lithium peroxide (12031-80-0) → Li0.92Ni1.08O2

Conditions	Yield
In neat (no solvent) (Ar), mixing, pelletizing, heating (flowing O2, 900°C, 48 h);

sodium oxide + lithium peroxide (12031-80-0) + terbium(III, IV) oxide + palladium (7440-05-3) → Li2PdO2

Conditions	Yield
In neat (no solvent) byproducts: Na2TbO3, TbO2; annealing a mixt. of Na2O, Li2O2, and "active" Tb4O7 (Na:Li:Tb = 6:2:1)in a sealed Pd tube (1100°C, 7 d);

lithium peroxide (12031-80-0) + rubidium oxide + arsenic(III) trioxide → 2Rb(1+)*Li(1+)*AsO4(3-)=Rb2Li{AsO4}

Conditions	Yield
In neat (no solvent) heating of well-grounded mixtures of the binary oxide, Ni-tube, 550°C, 21d, Ar;; single crystals;;

cesium oxide + lithium peroxide (12031-80-0) + arsenic(III) trioxide → 2Cs(1+)*Li(1+)*AsO4(3-)=Cs2(Li[AsO4])

Conditions	Yield
In neat (no solvent) heating of well-grounded mixtures of the binary oxide, Ni-tube, 550°C, 21d, Ar;; single crystals;;

lithium peroxide (12031-80-0) + potassium oxo cerate (III) → octalithium oxo cerate (IV)

Conditions	Yield
In neat (no solvent) byproducts: K2O; annealing a mixt. of Li2O2, and KCeO2 (Li:K:Ce = 9:1:1) in a sealed butnot complete tight Ag bomb tube (sealed in a Supremax glass tube, 650°C, 63 d or <600°C, 90 d);

lithium peroxide (12031-80-0) + copper (12775-96-1, 15158-11-9, 15721-63-8, 16941-75-6, 17493-86-6, 19498-52-3, 20499-83-6, 20499-84-7, 20499-85-8, 20499-86-9, 20573-10-8, 20573-11-9, 21595-51-7, 21595-52-8, 22206-52-6, 26445-28-3, 28959-95-7, 37362-93-9, 39417-05-5, 54603-16-6, 54603-23-5, 54603-32-6, 54603-40-6, 54603-48-4, 54603-81-5, 54603-89-3, 56316-56-4, 95985-91-4, 122297-32-9, 7440-50-8) → Li4{Cu4O4}

Conditions	Yield
In neat (no solvent, solid phase) heating of the oxide in a Cu-bomb under Ar at 680°C;

lithium peroxide (12031-80-0) + rubidium oxide + terbium(III, IV) oxide → Li6Tb2O7

Conditions	Yield
In neat (no solvent) heating (sealed Au tube, 750°C, 13 d or 850°C, 22 d);

Upstream product

• 80937-33-3 oxygen 
• 90076-65-6 bis(trifluoromethane)sulfonimide lithium 
• 62205-77-0 tetramethylammonium superoxide 
• 1310-66-3 lithium hydroxide monohydrate 
• 7722-84-1 dihydrogen peroxide 

Downstream Products

• 1313-99-1 nickel(II) oxide 
• 12162-79-7 Li₀₃₀₈Mn₀₆₉₂O 
• 12162-79-7 Li₀₀₄₆Mn₀₉₅₄O 
• 12162-79-7 Li₀₁₃₅Mn₀₈₆₅O 
• 12162-79-7 Li_0.35Mn_0.65O 
• 12162-79-7 Li_0.6Mn_0.4O 
• 12162-79-7 Li₀₂₅₇Mn₀₇₄₃O 
• 12162-79-7 Li_0.33Mn_0.67O 
• 20281-00-9 cesium oxide 

Related news

Morphology control of Lithium peroxide (cas 12031-80-0) using Pd3Co as an additive in aprotic Li-O2 batteries07/27/2019

During discharge in aprotic Li-O2 batteries, lithium peroxide (Li2O2) can be formed by a surface- or solution-mediated route. In the surface-mediated process, a Li2O2 film is formed electrochemically on the cathode surface, leading to low capacity and rate capability. In contrast, in high donor ...detailed

Relevant articles and documents

Thermal decomposition study on Li2O2 for Li2NiO2 synthesis as a sacrificing positive additive of lithium-ion batteries

Herein, thermal decomposition experiments of lithium peroxide (Li2O2) were performed to prepare a precursor (Li2O) for sacrificing cathode material, Li2NiO2. The Li2O2 was prepared by a hydrometallurgical reaction between LiOH·H2O and H2O2. The overall reaction during annealing was found to involve the following three steps: (1) dehydration of LiOH·H2O, (2) decomposition of Li2O2, and (3) pyrolysis of the remaining anhydrous LiOH. This stepwise reaction was elucidated by thermal gravimetric and quantitative X-ray diffraction analyses. Furthermore, over-lithiated lithium nickel oxide (Li2NiO2) using our lithium precursor was synthesized, which exhibited a larger yield of 90.9% and higher irreversible capacity of 261 to 265 mAh g?1 than the sample prepared by commercially purchased Li2O (45.6% and 177 to 185 mAh g?1, respectively) due to optimal powder preparation conditions.

Amorphous Li2O2: Chemical Synthesis and Electrochemical Properties

When aprotic Li–O2batteries discharge, the product phase formed in the cathode often contains two different morphologies, that is, crystalline and amorphous Li2O2. The morphology of Li2O2impacts strongly on the electrochemical performance of Li–O2cells in terms of energy efficiency and rate capability. Crystalline Li2O2is readily available and its properties have been studied in depth for Li–O2batteries. However, little is known about the amorphous Li2O2because of its rarity in high purity. Herein, amorphous Li2O2has been synthesized by a rapid reaction of tetramethylammonium superoxide and LiClO4in solution, and its amorphous nature has been confirmed by a range of techniques. Compared with its crystalline siblings, amorphous Li2O2demonstrates enhanced charge-transport properties and increased electro-oxidation kinetics, manifesting itself a desirable discharge phase for high-performance Li–O2batteries.