What is sodium oxide

Sodium peroxide N / A2O2 
Light yellow powder
or light yellow beads
molar mass 77.979 g / mol

AGW not specified
density 2.805 g / cm3   
Melting point +675 ° C
Water solubility 
reacts violently with water

GHS 03
GHS 05
Hazard classes + category  
Oxidising solids 1
Corrosive / irritant effect. on the skin 1A

HP rates (see note)    
H 271, 314 P 210, 221, 280.1-4, 301 + 330 + 331, 305 + 351 + 338, 309 + 310
disposal Collect separately in a container or in a fume cupboard in a water disposal

German nameEnglish name
CAS1313-60-6Sodium peroxideSodium peroxide
Note for schools: Sodium peroxide is highly corrosive and can react violently with water and all flammable substances. Safety glasses, goggles, protective gloves and a face shield must be worn. You may only work in the fume cupboard. It is stored in a separate mini chemical cabinet over a glass pan.

Light yellow spheres are commercially available, which in this form are more stable and chemically not quite as reactive as the powder. Pure sodium peroxide would be completely white, the yellow coloration is caused by sodium hyperoxide NaO2 caused. Sodium peroxide eagerly absorbs moisture and carbon dioxide from the air and reacts with them spontaneously. Sodium carbonate and oxygen are formed with carbon dioxide.

Sodium peroxide comes on the market as light yellow globules.

Sodium peroxide reacts with water with bubbles and strong heat generation, forming sodium hydroxide and hydrogen peroxide. If it is not cooled with ice at the same time, the hydrogen peroxide immediately breaks down further into water and oxygen:

N / A2O2 + 2 H.2O 2 NaOH + H2O2
2 H2O2 2 H2O + O2
Sodium peroxide can trigger explosive reactions on contact with flammable substances such as aluminum and magnesium powder or phosphorus. Flammable organic liquids can ignite by themselves. A mixture of paper or wood wool and sodium peroxide will also ignite by itself if little water is added.
Sodium peroxide is produced when sodium is burned in an oxygen atmosphere. At the same time, sodium oxide Na is also formed2O. How much of each of the two oxides is produced during combustion depends on the moisture present, the oxygen content and the combustion temperature. At higher combustion temperatures, sodium peroxide is more likely to form.
4 Na + O2  2 Well2O     ΔHR. = −418 kJ / mol
2 Na + O2  N / A2O2     ΔHR. = −513 kJ / mol
Sodium peroxide is used in the chemical industry as a bleaching agent for plant and animal products. It has not been used in laundry detergents since 1939. The detergents used at the time caused fires again and again. In fire brigade breathing apparatus or in submarines, it is used as a very efficient absorbent for carbon dioxide. Sodium peroxide is also a raw material for making other peroxo compounds.