Silicon tetrafluoride

Silicon tetrafluoride
Silicon tetrafluoride
Silicon tetrafluoride
Names
IUPAC names
Tetrafluorosilane
Silicon tetrafluoride
Other names
Silicon fluoride
Fluoro acid air
Identifiers
3D model (JSmol)
ECHA InfoCard 100.029.104 Edit this at Wikidata
RTECS number
  • VW2327000
UNII
UN number 1859
  • F[Si](F)(F)F
Properties
SiF4
Molar mass 104.0791 g/mol
Appearance colourless gas, fumes in moist air
Density 1.66 g/cm3, solid (−95 °C)
4.69 g/L (gas)
Melting point −95.0 °C (−139.0 °F; 178.2 K)[2][3]
Boiling point −90.3 °C (−130.5 °F; 182.8 K)[2]
Critical point (T, P) −14.15 °C (6.5 °F; 259.0 K), 36.71 standard atmospheres (3,719.6 kPa; 539.5 psi)[1]
decomposes
Structure
tetrahedral
0 D
Hazards
Occupational safety and health (OHS/OSH):
Main hazards
toxic, corrosive
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 3: Short exposure could cause serious temporary or residual injury. E.g. chlorine gasFlammability 0: Will not burn. E.g. waterInstability 2: Undergoes violent chemical change at elevated temperatures and pressures, reacts violently with water, or may form explosive mixtures with water. E.g. white phosphorusSpecial hazard W: Reacts with water in an unusual or dangerous manner. E.g. sodium, sulfuric acid
3
0
2
Lethal dose or concentration (LD, LC):
69.220 mg/m3 (rat, 4 hr)[4]
Safety data sheet (SDS) ICSC 0576
Related compounds
Other anions
Silicon tetrachloride
Silicon tetrabromide
Silicon tetraiodide
Other cations
Carbon tetrafluoride
Germanium tetrafluoride
Tin tetrafluoride
Lead tetrafluoride
Related compounds
Hexafluorosilicic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Silicon tetrafluoride or tetrafluorosilane is a chemical compound with the formula SiF4. This colorless gas is notable for having a narrow liquid range: its boiling point is only 4 °C above its melting point. It was first prepared in 1771 by Carl Wilhelm Scheele by dissolving silica in hydrofluoric acid,[5] and later synthesized by John Davy in 1812.[6] It is a tetrahedral molecule and is corrosive.[7]

  1. ^ Lide, David R.; Kehiaian, Henry V. (1994). CRC Handbook of Thermophysical and Themochemical Data (PDF). CRC Press. p. 28.
  2. ^ a b Silicon Compounds, Silicon Halides. Collins, W.: Kirk-Othmer Encyclopedia of Chemical Technology; John Wiley & Sons, Inc, 2001.
  3. ^ Cite error: The named reference :1 was invoked but never defined (see the help page).
  4. ^ "Fluorides (as F)". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
  5. ^ Greenwood & Earnshaw 1997, p. 328.
  6. ^ John Davy (1812). "An Account of Some Experiments on Different Combinations of Fluoric Acid". Philosophical Transactions of the Royal Society of London. 102: 352–369. doi:10.1098/rstl.1812.0020. ISSN 0261-0523. JSTOR 107324.
  7. ^ "Hazardous Substance Fact Sheet" (PDF). New Jersey Department of Health and Senior services. November 2001.