Chlorine trifluoride
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| Names | |||
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Systematic IUPAC name
Trifluoro-λ3-chlorane(substitutive)
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| Other names
Chlorotrifluoride
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| Identifiers | |||
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3D model (Jmol)
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| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.029.301 | ||
| EC Number | 232-230-4 | ||
| 1439 | |||
| MeSH | chlorine+trifluoride | ||
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PubChem CID
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| RTECS number | FO2800000 | ||
| UN number | 1749 | ||
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| Properties | |||
| ClF3 | |||
| Molar mass | 92.45 g·mol−1 | ||
| Appearance | Colourless gas or greenish-yellow liquid | ||
| Odor | sweet, pungent, irritating, suffocating | ||
| Density | 4 mg cm−3 | ||
| Melting point | −76.34 °C (−105.41 °F; 196.81 K) | ||
| Boiling point | 11.75 °C (53.15 °F; 284.90 K) (decomposes @ 180 °C (356 °F; 453 K)) | ||
| Reacts violently | |||
| Solubility | reacts violently with benzene, toluene, ether, alcohol, acetic acid, selenium tetrafluoride, nitric acid, sulfuric acid, alkali, hexane. Forms shock-sensitive explosive solution in CCl4 | ||
| Vapor pressure | 175 kPa | ||
| -26.5·10−6 cm3/mol | |||
| Viscosity | 91.82 μPa s | ||
| Structure | |||
| T-shaped | |||
| Thermochemistry | |||
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Std molar
entropy (S |
281.59 J K−1mol−1 | ||
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Std enthalpy of
formation (ΔfH |
−158.87 kJ mol−1 | ||
| Hazards | |||
| Main hazards | explosive when exposed to organics, reacts violently with water | ||
| Safety data sheet | natlex.ilo.ch | ||
| GHS pictograms |
   
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| GHS signal word | Danger | ||
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EU classification (DSD)
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 O (O) T+ (T+) N (N) C (C) |
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| R-phrases | R8, R14, R39/26/27/28, R35, R49, R46, R60, R61 | ||
| S-phrases | (S1/2), S17, S30, S38, S45, S53, S60, S61 | ||
| NFPA 704 | |||
| Flash point | noncombustible | ||
| Lethal dose or concentration (LD, LC): | |||
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LC50 (median concentration)
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95 ppm (rat, 4 hr) 178 ppm (mouse, 1 hr) 230 ppm (monkey, 1 hr) 299 ppm (rat, 1 hr) |
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| US health exposure limits (NIOSH): | |||
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PEL (Permissible)
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C 0.1 ppm (0.4 mg/m3) | ||
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REL (Recommended)
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C 0.1 ppm (0.4 mg/m3) | ||
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IDLH (Immediate danger)
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20 ppm | ||
| Related compounds | |||
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Related compounds
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Chlorine pentafluoride |
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Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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| Infobox references | |||
Chlorine monofluoride
Bromine trifluoride
Iodine trifluoride
Chlorine trifluoride is an interhalogen compound with the formula ClF3. This colourless, poisonous, corrosive, and extremely reactive gas condenses to a pale-greenish yellow liquid, the form in which it is most often sold (pressurized at room temperature). The compound is primarily of interest as a component in rocket fuels, in plasmaless cleaning and etching operations in the semiconductor industry, in nuclear reactor fuel processing, and other industrial operations.
It was first reported in 1930 by Ruff and Krug who prepared it by fluorination of chlorine; this also produced ClF and the mixture was separated by distillation.
ClF3 is approximately T-shaped, with one short bond (1.598 Å) and two long bonds (1.698 Å). This structure agrees with the prediction of VSEPR theory, which predicts lone pairs of electrons as occupying two equatorial positions of a hypothetic trigonal bipyramid. The elongated Cl-F axial bonds are consistent with hypervalent bonding.
Pure ClF3 is stable to 180 °C in quartz vessels; above this temperature it decomposes by a free radical mechanism to the elements.
Reaction with several metals give chlorides and fluorides; phosphorus yields phosphorus trichloride (PCl3) and phosphorus pentafluoride (PF5); and sulfur yields sulfur dichloride (SCl2) and sulfur tetrafluoride (SF4). ClF3 also reacts explosively with water, in which it oxidizes water to give oxygen or in controlled quantities, oxygen difluoride (OF2), as well as hydrogen fluoride and hydrogen chloride. Metal oxides will react to form metal halides and oxygen or oxygen difluoride.
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