Chlorine pentafluoride

Short description: Chemical compound

Chlorine pentafluoride  |  |

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Identifiers

CAS Number

* 13637-63-3 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 55559 N

PubChem CID

* 61654

RTECS number |

* FO2975000

UNII |

* O4RJ1HW01H Y

InChI

* InChI=1S/ClF5/c2-1(3,4,5)6 N

Key: KNSWNNXPAWSACI-UHFFFAOYSA-N N

SMILES

* FCl(F)(F)(F)F

Properties

Chemical formula

| ClF5
Molar mass | 130.445 g mol−1
Appearance  | colorless liquid
Density | 4.5 kg/m3 (g/L)
Melting point |  −103 °C (−153 °F; 170 K)
Boiling point |  −13.1 °C (8.4 °F; 260.0 K)

Solubility in water

| Hydrolyzes
Structure

Molecular shape

| Square pyramidal
Thermochemistry

Std molar
entropy (S ~~o~~ 298)

| 310.73 J K−1 mol−1

Std enthalpy of
formation (ΔfH⦵298)

| −238.49 kJ mol−1

Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

N verify (what is YN ?)
Infobox references

Tracking categories (test):

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Chlorine pentafluoride is an interhalogen compound with formula ClF5. This colourless liquid is a strong oxidant that was once a candidate oxidizer for rockets. The molecule adopts a square pyramidal structure with C4v symmetry,[1] as confirmed by its high-resolution 19F NMR spectrum.[2] It was first synthesized in 1963.[3]

## Contents

* 1 Preparation
* 2 Reactions
* 3 Uses
* 3.1 Rocket propellant
* 4 See also
* 5 References
* 6 External links

## Preparation

Some of the earliest research on the preparation was classified.[4][5] It was first prepared by fluorination of chlorine trifluoride at high temperatures and high pressures:[4]

ClF3 \+ F2 → ClF5
ClF + 2F2 → ClF5
Cl2 \+ 5F2 → 2ClF5
CsClF4 \+ F2 → CsF + ClF5

NiF2 catalyzes this reaction.[6]

Certain metal fluorides, MClF4 (i.e. KClF4, RbClF4, CsClF4), react with F2 to produce ClF5 and the corresponding alkali metal fluoride.[5]

## Reactions

In a highly exothermic reaction, ClF5 reacts with water to produce chloryl fluoride and hydrogen fluoride:[7]

ClF5 \+ 2 H2O → ClO2F \+ 4 HF

It is also a strong fluorinating agent. At room temperature it reacts readily with all elements (including otherwise "inert" elements like platinum and gold) except noble gases, nitrogen, oxygen and fluorine.[2]

## Uses

### Rocket propellant

Chlorine pentafluoride was once considered for use as an oxidizer for rockets. As a propellant, it has a higher maximum specific impulse than ClF3, but with the same difficulties in handling.[4] Due to the hazardous nature of chlorine pentafluoride, it has yet to be used in a large scale rocket propulsion system.

## See also

* Chlorine trifluoride
* Hypervalent molecule

## References

1. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 833. ISBN 978-0-08-037941-8.
2. ↑ 2.0 2.1 Pilipovich, D.; Maya, W.; Lawton, E.A.; Bauer, H.F.; Sheehan, D. F.; Ogimachi, N. N.; Wilson, R. D.; Gunderloy, F. C. et al. (1967). "Chlorine pentafluoride. Preparation and Properties". Inorganic Chemistry 6 (10): 1918. doi:10.1021/ic50056a036.
3. ↑ Smith D. F. (1963). "Chlorine Pentafluoride". Science 141 (3585): 1039–1040. doi:10.1126/science.141.3585.1039. PMID 17739492. Bibcode: 1963Sci...141.1039S.
4. ↑ 4.0 4.1 4.2 Clark, John D. (1972). Ignition! An Informal History of Liquid Rocket Propellants. Rutgers University Press. pp. 87–88. ISBN 0-8135-0725-1. http://www.sciencemadness.org/library/books/ignition.pdf.
5. ↑ 5.0 5.1 Smith D. F. (1963). "Chlorine Pentafluoride". Science 141 (3585): 1039–1040. doi:10.1126/science.141.3585.1039. PMID 17739492. Bibcode: 1963Sci...141.1039S.
6. ↑ "On the Synthesis of Chlorine Pentafluoride". Journal of Fluorine Chemistry 17 (4): 381–383. 1981. doi:10.1016/S0022-1139(00)81783-2.
7. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 834. ISBN 978-0-08-037941-8.

## External links

* National Pollutant Inventory - Fluoride and compounds fact sheet
* New Jersey Hazardous Substance Fact Sheet
* WebBook page for ClF5

* v
* t
* e

Chlorine compounds

* ClF
* ClF3
* ClF5
* ClNO3
* ClO
* ClOF3
* Cl2O2
* ClO2
* ClO2F
* ClO3F
* Cl2O
* Cl2O4
* Cl2O6
* Cl2O7
* HCl
* SiCl4

* v
* t
* e

Fluorine compounds

| HF |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  |  | He

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LiF | BeF2 |  |  |  |  |  |  |  |  |  |  | BF3
B2F4 | CF4 | NF3 | OF2 | F− | Ne
NaF | MgF2 |  |  |  |  |  |  |  |  |  |  | AlF3 | SiF4 | PF3
PF5 | SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF2 | ScF3 | TiF3
TiF4 | VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5 | MnF2
MnF3 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF3 | GeF4 | AsF3
AsF5 | SeF4
SeF6 | BrF3
BrF5 | KrF2
RbF | SrF2 | YF3 | ZrF4 | NbF4
NbF5 | MoF5
MoF6 | TcF6 | RuF3
RuF4
RuF5
RuF6 | RhF6 | PdF2 | AgF
AgF2
Ag2F | CdF2 | InF3 | SnF2
SnF4 | SbF3
SbF5 | TeF4 | IF
IF3
IF5
IF7 | XeF2
XeF4
XeF6
CsF | BaF2 | *  | HfF4 | TaF5 | WF4
WF6 | ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF3
IrF5
IrF6 | PtF4
PtF6 | AuF3
Au2F10
AuF5·F2
| HgF2
Hg2F2 | TlF
TlF3 | PbF2
PbF4 | BiF3
BiF5 | Po | At | RnF2
Fr | Ra | **  | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og
|  | ↓ |  |  |  |  |  |  |  |  |  |  |  |  |  |  |
| * | LaF3 | CeF3 | Pr | NdF3 | PmF3 | SmF3
| Eu | Gd | Tb | DyF3 | Ho | Er | Tm | YbF3
| Lu |
| ** | AcF3 | ThF4 | Pa | UF3
UF4
UF5
UF6 | NpF3
NpF4
NpF5
NpF6
| PuF3
PuF4
PuF5
PuF6 | AmF3
AmF4 | CmF3 | Bk | Cf | Es | Fm | Md | No | Lr |

Other|

* AgBF4
* AgPF6
* Cs2AlF5
* K3AlF6
* Na3AlF6
* KAsF6
* LiAsF6
* NaAsF6
* HBF4
* KBF4
* LiBF4
* NaBF4
* RbBF4
* Ba(BF4)2
* Ni(BF4)2
* Pb(BF4)2
* Sn(BF4)2
* BaClF
* BaSiF6
* BaGeF6
* BrOF3
* BrO2F
* CBrF3
* CBr2F2
* CBr3F
* CClF3
* CCl2F2
* CCl3F
* CFN
* CF2O
* CF3I
* CHF3
* CH2F2
* CH3F
* C2Cl3F3
* C2H3F
* C6H5F
* C7H5F3
* C15F33N
* ClFO2
* CrFO4
* CrF2O2
* CsBF4
* NH4F
* FNO
* FNO2
* FNO3
* KHF2
* NaHF2
* ThOF2
* NH5F2
* (NH4)2SiF6
* F2OS
* F3OP
* PSF3
* HPF6
* HSbF6
* NH4PF6
* KPF6
* KSbF6
* LiPF6
* NaPF6
* NaSbF6
* Na2SiF6
* Na2TiF6
* Na2ZrF6
* TlPF6
* IOF3
* K2NbF7
* K2TaF7
* IO3F
* UO2F2

Chemical formulas

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