Tin(II) oxide
Tin(II) oxide, also known as stannous oxide, is a chemical compound. Its chemical formula is SnO. It has tin in an oxidation state of +2. It also has oxide ions in it.
| Tin(II) oxide | |
|---|---|
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_oxide_hydrate_(2).JPG)
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| IUPAC name | Tin(II) oxide |
| Other names | Stannous oxide, tin monoxide |
| Identifiers | |
| CAS number | |
| PubChem | |
| EC number | 244-499-5 |
| RTECS number | XQ3700000 |
| SMILES | O=[Sn] |
| Properties | |
| Molecular formula | SnO |
| Molar mass | 134.709 g/mol |
| Appearance | black or red powder when anhydrous, white when hydrated |
| Density | 6.45 g/cm3 |
| Melting point |
1080 °C, 1353 K, 1976 °F |
| Solubility in water | insoluble |
| −19.0·10−6 cm3/mol | |
| Structure | |
| Crystal structure | tetragonal |
| Thermochemistry | |
| Std enthalpy of formation ΔfH |
−285 kJ·mol−1[1] |
| Standard molar entropy S |
56 J·mol−1·K−1[1] |
| Hazards | |
| Flash point | Non-flammable |
| U.S. Permissible exposure limit (PEL) |
none |
| Related compounds | |
| Other anions | Tin sulfide Tin selenide Tin telluride |
| Other cations | Carbon monoxide Silicon monoxide Germanium(II) oxide Lead(II) oxide |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) | |
Properties
It is normally a blue-black solid. It can be red but the red form is more unstable. It burns in air with a green flame to make tin(IV) oxide. It is a reducing agent. It is rarer than tin(IV) oxide. It dissolves in acids to make a colorless solution.
Preparation
It can be made by reacting sulfuric acid with tin and reacting the tin(II) sulfate made with sodium hydroxide to make the tin(II) oxide hydrate. This is heated to get the tin(II) oxide.
Uses
It is used in touchscreens. It is used to make a glass with gold in it called ruby glass.
Tin(II) Oxide Media
Tin(II) oxide burning in an aluminium foil tray. The dim green flame in the aluminium foil is the flame produced by the burning tin(II) oxide. The orange flames are produced by the aluminium and are not unique to any metal.
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Related pages
References
- ↑ 1.0 1.1 Zumdahl, Steven S. (2009). Chemical Principles 6th Ed. Houghton Mifflin Company. p. A23. ISBN 978-0-618-94690-7.