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| CAS No.: | 1313-60-6 |
|---|---|
| Name: | Sodium peroxide |
| Molecular Structure: | |
|
|
|
| Formula: | Na2O2 |
| Molecular Weight: | 77.98 |
| Synonyms: | Disodiumdioxide;Disodium peroxide;Sodium oxide (Na2O2); |
| EINECS: | 215-209-4 |
| Density: | 2.805 g/cm3 |
| Melting Point: | 460 °C (dec.)(lit.) |
| Boiling Point: | 150.2 °C at 760 mmHg |
| Flash Point: | 657 °C |
| Solubility: | Soluble in water, forming NaOH and H{2}O{2}. Soluble in acid. Insoluble in alkali. |
| Appearance: | light yellow granular powder |
| Hazard Symbols: |
 O, C
|
| Risk Codes: | 8-35 |
| Safety: | 8-27-39-45 |
| Transport Information: | UN 1504 5.1/PG 1 |
| PSA: | 46.12000 |
| LogP: | -0.23760 |
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Consensus Reports
Reported in EPA TSCA Inventory.
Standards and Recommendations
DOT Classification: 5.1; Label: Oxidizer
Specification
The Sodium peroxide, with the CAS registry number 1313-60-6, is also known as Natrium peroxydatum. It belongs to the product category of Inorganics. Its EINECS registry number is 215-209-4. This chemical's molecular formula is Na2O2 and molecular weight is 77.98. Its systematic name is called sodioperoxysodium. This chemical is light yellow granular powder. Sodium peroxide is the inorganic compound with the formula Na2O2. This solid is the product when sodium is burned with oxygen.
Physical properties of Sodium peroxide: (1)#H bond acceptors: 2; (2)#H bond donors: 0; (3)#Freely Rotating Bonds: 3; (4)Polar Surface Area: 18.46 Å2.
Preparation: Sodium peroxide formerly was prepared on a large scale by the reaction with sodium with oxygen at 130–200 °C, a process that generates sodium oxide, which in a separate stage absorbs oxygen:
4 Na + O2 → 2 Na2O
2 Na2O + O2 → 2 Na2O2
More specialized routes have been developed. At ambient temperatures (0–20 °C), O2 reacts with a dilute (0.1–5.0 mole percent) sodium amalgam. It may also be produced by passing ozone gas over solid sodium iodide inside a platinum or palladium tube. The ozone oxidizes the sodium to form sodium peroxide. The iodine is freed into iodine crystals, which can be sublimed by mild heating. The platinum or palladium catalyzes the reaction and is not attacked by the sodium peroxide.
Sodium peroxide was used to bleach wood pulp for the production of paper and textiles. Presently it is mainly used for specialized laboratory operations, e.g. the extraction of minerals from various ores. Sodium peroxide may go by the commercial names of Solozone and Flocool. In chemistry preparations, sodium peroxide is used as an oxidising agent. It is also used as an oxygen source by reacting it with carbon dioxide to produce oxygen and sodium carbonate; it is thus particularly useful in scuba gear, submarines, etc. Lithium peroxide has similar uses. It is also used for the preparation of samples by peroxide fusion and later analysis by AA or ICP.
When you are using this chemical, please be cautious about it as the following:
This chemical will react exothermically with other chemicals. It may destroy living tissue on contact. Contact with combustible material, it may cause fire. In addition, this chemical can cause severe burns. You should keep its container dry. Whenever you will contact it, please wear eye/face protection. In case of accident or if you feel unwell seek medical advice immediately (show the label where possible).
You can still convert the following datas into molecular structure:
(1)SMILES: [Na]OO[Na]
(2)InChI: InChI=1/2Na.O2/c;;1-2/q2*+1;-2/rNa2O2/c1-3-4-2
(3)InChIKey: PFUVRDFDKPNGAV-YWDPWCALAC