Disilane
From Wikipedia, the free encyclopedia
| Disaline | |
|---|---|
 |
|
 |
|
| IUPAC name | disilicon hexahydride |
| Other names | disilane silicon hydride silicon(III) hydride |
| Identifiers | |
| CAS number | [1590-87-0] |
| Properties | |
| Molecular formula | Si2H6 |
| Molar mass | 62.219 g/mol |
| Appearance | Colourless, odourless flammable gas |
| Density | 2.7 kg/m3 |
| Melting point |
-132°C (141 K) |
| Boiling point |
-14°C (259 K) |
| Solubility in water | Insoluble |
| Structure | |
| Molecular shape | Tetrahedral |
| Dipole moment | 0 D |
| Hazards | |
| Main hazards | Flammable, Toxic, can cause burns when in contact with skin,
and can cause respiratory problems |
| Flash point | (Very flammable) |
| Related compounds | |
| Related covalent hydrides | ethane diborane |
| Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa) Infobox disclaimer and references |
|
Disilane is a poisonous silicon-hydrogen compound, existing as a gas at room temperature and pressure. It is analogous to ethane, though much more reactive than ethane, due to the larger size of the silicon atom and the weaker Si-Si bonding. Traces are formed during the hydrolysis of magnesium silicide, which produces mainly silane, siloxanes, and polysiloxanes.[1] The presence of traces of disilane is responsible for the spontaneous flammability of silane produced this way, as is diphosphine for phosphine.
[edit] Uses
Disilane is occasionally used as a source of hydrogen during reactions.[2] It is also utilized in the production of silicon wafers[3].
[edit] References
 |
This inorganic compound-related article is a stub. You can help Wikipedia by expanding it. |
