| IUPAC name
| Preferred IUPAC name
| Systematic IUPAC name
| Other names
|Molar mass||103.619 g/mol|
|Melting point||2,531 °C (4,588 °F; 2,804 K)|
|Boiling point||3,200 °C (5,790 °F; 3,470 K) (decomposes)|
|Solubility||Insoluble in organic solvents|
|Vapor pressure||~0 mmHg|
Std enthalpy of
|Safety data sheet||Sigma-Aldrich|
| Magnesium oxide|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Strontium oxide, strontia or SrO, is formed when strontium metal reacts with oxygen. Burning strontium in air results in a mixture of strontium oxide and strontium nitride. It also forms from the decomposition of strontium carbonate SrCO3. It is a strongly basic oxide.
SrO reacts with water, releasing heat and producing strontium hydroxide. In open air, it reacts with water vapor and carbon dioxide, slowly converting to strontium carbonate over time.
It will react with many acids to form strontium salts and water.
- SrO + 2 HNO3 → Sr(NO3)2 + H2O
SrO is a white solid, usually in powder form. Strontium oxide will react in contact with water. It is slightly soluble in ethanol, but insoluble in acetone and ether. It has a very high melting and boiling point (2,531 °C and 3,200 °C respectively).
Strontium oxide can be purchased from chemical suppliers, although it's easier to find strontium carbonate and hydroxide than the simple oxide, as they're less reactive.
- Make strontium metal (reducing with aluminium in inert atmosphere or vacuum)
- Make strontium salts
- Red colored fireworks
Strontium oxide is extremely corrosive to the human tissue as it reacts vigorously with the water from them, and releases heat which causes severe burns. Gloves must be worn at all times while handling SrO.
Strontium ions, being similar to the calcium ones, pose little danger to health when consumed. In fact, many studies on both animals and humans have shown that strontium supplements can increase the density and strength of bones. However it is advised to avoid consuming lab-grade strontium compounds, as they are unfit for consumption.
Contact with damp air must be kept to a minimal to prevent it from reacting with water and oxides of carbon and nitrogen and other reactive gases.
Strontium oxide can be neutralized with water or a cheap acid. Since most of strontium compounds are similar to calcium compounds, it can be dumped without any special precautions. However, as strontium is rarer than calcium, it's best to try to recycle the compound when possible.