Perchloryl fluoride
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Perchloryl fluoride[6] is a reactive gas with the chemical formula ClO
3F. It has a characteristic sweet odor[7] that resembles gasoline and kerosene. It is toxic and is a powerful oxidizing and fluorinating agent. It is the acid fluoride of perchloric acid.
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Names | |||
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IUPAC name
Perchloryl fluoride | |||
Other names
Chlorine oxyfluoride, Perchlorofluoride, Chlorine fluorine oxide, Trioxychlorofluoride, Perchloric acid fluoride | |||
Identifiers | |||
3D model (JSmol) |
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ChemSpider |
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ECHA InfoCard | 100.028.660 | ||
EC Number |
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PubChem CID |
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RTECS number |
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UNII | |||
CompTox Dashboard (EPA) |
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Properties | |||
ClO3F | |||
Molar mass | 102.4496 g/mol | ||
Appearance | Colorless gas | ||
Odor | sweet odor | ||
Density | 1.434 g/cm3 | ||
Melting point | −147.8 °C (−234.0 °F; 125.3 K) | ||
Boiling point | −46.7 °C (−52.1 °F; 226.5 K) | ||
Critical point (T, P) | 95.2 °C (203.4 °F; 368.3 K), 53 standard atmospheres (5,400 kPa; 780 psi)[1] | ||
0.06 g/100 ml (20 °C), slow hydrolysis | |||
Vapor pressure | 10.5 atm (20°C)[2] | ||
Viscosity | 3.91 x 10−3 Pa.s (@ melting point) | ||
Structure | |||
Tetrahedral[3]: 373 | |||
Thermochemistry | |||
Std molar entropy (S⦵298) |
278.97 J/(mol*K) | ||
Std enthalpy of formation (ΔfH⦵298) |
-21.42 kJ/mol [4]: 380 | ||
Hazards | |||
Occupational safety and health (OHS/OSH): | |||
Main hazards |
oxidizing, toxic. Non-corrosive. | ||
NFPA 704 (fire diamond) | |||
Threshold limit value (TLV) |
3 ppm | ||
Lethal dose or concentration (LD, LC): | |||
LC50 (median concentration) |
385 ppm (rat, 4 hr) 451 ppm (dog, 4 hr)[5] | ||
LCLo (lowest published) |
2000 ppm (rat, 40 min) 451 ppm (dog, 4 hr)[5] | ||
NIOSH (US health exposure limits): | |||
PEL (Permissible) |
TWA 3 ppm (13.5 mg/m3)[2] | ||
REL (Recommended) |
TWA 3 ppm (14 mg/m3) ST 6 ppm (28 mg/m3)[2] | ||
IDLH (Immediate danger) |
100 ppm[2] | ||
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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In spite of its small enthalpy of formation (ΔfH° = −5.2 kcal/mol (−22 kJ/mol)), it is kinetically stable, decomposing only at 400 °C.[3]: 380 It is quite reactive towards reducing agents and anions, however, with the chlorine atom acting as an electrophile.[3]: 382 It reacts explosively with reducing agents such as metal amides, metals, hydrides, etc.[7] Its hydrolysis in water occurs very slowly, unlike that of chloryl fluoride.