Oxygen difluoride

Names
IUPAC name

Oxygen difluoride

Other names

* Oxygen fluoride
* Hypofluorous anhydride

Identifiers

CAS Number

* 7783-41-7 Y

3D model (JSmol)

* Interactive image

ChEBI |

* CHEBI:30494 Y

ChemSpider |

* 22953 Y

EC Number |

* 231-996-7

PubChem CID

* 24547

RTECS number |

* RS2100000

UNII |

* 7BCS2CW398 Y

InChI

* InChI=1S/F2O/c1-3-2 Y

Key: UJMWVICAENGCRF-UHFFFAOYSA-N Y

* InChI=1/F2O/c1-3-2

Key: UJMWVICAENGCRF-UHFFFAOYAI

SMILES

* FOF

Properties

Chemical formula

| OF

Molar mass | 53.9962 g/mol
Appearance  | colorless gas, pale yellow liquid when condensed
Odor | peculiar, foul
Density |

* 1.90 g/cm3 (−224 °C, liquid)
* 1.719 g/cm3 (−183 °C, liquid)
* 1.521 g/cm3 (liquid at −145 °C)
* 1.88 g/L (gas at room temperature)

Melting point |  −223.8 °C (−370.8 °F; 49.3 K)
Boiling point |  −144.75 °C (−228.55 °F; 128.40 K)

Solubility in water

| hydrolyzes[1] slowly
Vapor pressure | 48.9 atm (at −58.0 °C or −72.4 °F or 215.2 K[lower-alpha 1])
Structure

Point group

| C2V
Thermochemistry

Heat capacity (C)

| 43.3 J/mol K

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

| 247.46 J/mol K

Std enthalpy of
formation (ΔfH⦵298)

| 24.5 kJ mol−1

Gibbs free energy (ΔfG˚)

| 41.8 kJ/mol
Hazards
GHS pictograms |
GHS Signal word | danger

GHS hazard statements

| HH270Script error: No such module "Preview warning".Category:GHS errors, HH314Script error: No such module "Preview warning".Category:GHS errors, HH330Script error: No such module "Preview warning".Category:GHS errors
NFPA 704 (fire diamond)  |

Lethal dose or concentration (LD, LC):

LC50 (median concentration)

* 2.6 ppm (rat, 1 hour)
* 1.5 ppm (mouse, 1 hour)
* 26 ppm (dog, 1 hour)
* 16 ppm (monkey, 1 hour)

[3]
NIOSH (US health exposure limits):

PEL (Permissible)

| TWA 0.05 ppm (0.1 mg/m3)[2]

REL (Recommended)

| C 0.05 ppm (0.1 mg/m3)[2]

IDLH (Immediate danger)

| 0.5 ppm[2]
Related compounds

Related compounds

* HFO
* O

* NHF

* NF

* SCl

* H

* Cl

* Br

* I

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

Y verify (what is YN ?)
Infobox references

Tracking categories (test):

* SizeSet

Oxygen difluoride is a chemical compound with the formula OF
2. As predicted by VSEPR theory, the molecule adopts a bent molecular geometry.[citation needed] It is a strong oxidizer and has attracted attention in rocketry for this reason.[5] With a boiling point of −144.75 °C, OF2 is the most volatile (isolable) triatomic compound.[6] The compound is one of many known oxygen fluorides.

## Contents

* 1 Preparation
* 2 Structure and bonding
* 3 Reactions
* 4 Safety
* 5 Popular culture
* 6 Notes
* 7 References
* 8 External links

## Preparation

Oxygen difluoride was first reported in 1929; it was obtained by the electrolysis of molten potassium fluoride and hydrofluoric acid containing small quantities of water.[7][8] The modern preparation entails the reaction of fluorine with a dilute aqueous solution of sodium hydroxide, with sodium fluoride as a side-product:

2 F
2 \+ 2 NaOH → OF
2 \+ 2 NaF + H

## Structure and bonding

It is a covalently bonded molecule with a bent molecular geometry and a F-O-F bond angle of 103 degrees. Its powerful oxidizing properties are suggested by the oxidation number of +2 for the oxygen atom instead of its normal −2.

## Reactions

Above 200 °C, OF
2 decomposes to oxygen and fluorine by a radical mechanism.

2 OF
2 → O
2 \+ 2 F

2 reacts with many metals to yield oxides and fluorides. Nonmetals also react: phosphorus reacts with OF
2 to form PF
5 and POF
3; sulfur gives SO
2 and SF
4; and unusually for a noble gas, xenon reacts (at elevated temperatures) yielding XeF
4 and xenon oxyfluorides.

Reactions of oxygen difluoride and hydrogen halides or halide salts produce the free halogen. For example:

> 4 HCl + OF
> 2 → 2 HF + H
> 2O + 2 Cl
> 2

Oxygen difluoride reacts with water to form hydrofluoric acid:

2 \+ H
2O → 2 HF + O

It can oxidize sulfur dioxide to sulfur trioxide and elemental fluorine:

2 \+ SO
2 → SO
3 \+ F

However, in the presence of UV radiation, the products are sulfuryl fluoride (SO

2) and pyrosulfuryl fluoride (S

2):

2 \+ 2 SO
2 → S

## Safety

Oxygen difluoride is considered an unsafe gas due to its oxidizing properties. It reacts explosively with water, hydrogen sulfide, diborane, and nitrogen oxides.[9] Hydrofluoric acid produced by the hydrolysis of OF
2 with water is highly corrosive and toxic, capable of causing necrosis, leaching calcium from the bones and causing cardiovascular damage, among a host of other highly toxic effects. Other acute poisoning effects include: pulmonary edema, bleeding lungs, headaches, etc.[10] Chronic exposure to oxygen difluoride, like that of other chemicals that release fluoride ions, can lead to fluorosis and other symptoms of chronic fluoride poisoning. Oxygen difluoride may be associated with kidney damage.[10] The maximum workplace exposure limit is 0.05 ppm.[11][10]

## Popular culture

In Robert L. Forward's science fiction novel Camelot 30K, oxygen difluoride was used as a biochemical solvent by fictional life forms living in the solar system's Kuiper belt. While OF
2 would be a solid at 30 K, the fictional alien lifeforms were described as endothermic, maintaining elevated body temperatures and liquid OF
2 blood by radiothermal heating.

## Notes

1. ↑ This is its critical temperature, which is below ordinary room temperature.

## References

1. ↑ "difluorine monoxide; oxygen difluoride, physical properties, suppliers, CAS, MSDS, structure, Molecular Formula, Molecular Weight, Solubility, boiling point, melting point". http://www.chemyq.com/En/xz/xz1/2818mqnrv.htm.
2. ↑ 2.0 2.1 2.2 NIOSH Pocket Guide to Chemical Hazards. "#0475". National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/npg/npgd0475.html.
3. ↑ "Oxygen difluoride". Immediately Dangerous to Life and Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH). https://www.cdc.gov/niosh/idlh/7783417.html.
4. ↑ GHS: GESTIS 570242
5. ↑ Forbes, Forrest S.; Van Splinter, Peter A. (2003). "Liquid Rocket Propellants". Encyclopedia of Physical Science and Technology. pp. 741–777. doi:10.1016/B0-12-227410-5/00385-9. ISBN 978-0-12-227410-7.
6. ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 819. ISBN 978-0-08-037941-8.
7. ↑ Lebeau, P.; Damiens, A. (1929). "Sur un nouveau mode de préparation du fluorure d'oxygène" (in fr). Comptes rendus hebdomadaires des séances de l'Académie des Sciences 188: 1253–1255. http://visualiseur.bnf.fr/CadresFenetre?O=NUMM-3141&I=1253&M=chemindefer. Retrieved February 21, 2013.
8. ↑ Lebeau, P.; Damiens, A. (1927). "Sur l'existence d'un composé oxygéné du fluor" (in fr). Comptes rendus hebdomadaires des séances de l'Académie des Sciences 185: 652–654. http://visualiseur.bnf.fr/CadresFenetre?O=NUMM-3138&I=652&M=tdm. Retrieved February 21, 2013.
9. ↑ "OXYGEN DIFLUORIDE | CAMEO Chemicals | NOAA". https://cameochemicals.noaa.gov/chemical/4148.
10. ↑ 10.0 10.1 10.2 "1449". https://www.kdocs.cn/singleSign4CST?cb=https://www.kdocs.cn/l/cn9j8vXb7Gq3?f=201&ts=1715699652.
11. ↑ "CDC - NIOSH Pocket Guide to Chemical Hazards - Oxygen difluoride". https://www.cdc.gov/niosh/npg/npgd0475.html.

## External links

* National Pollutant Inventory - Fluoride and compounds fact sheet
* WebBook page for OF

* CDC - NIOSH Pocket Guide to Chemical Hazards

* v
* t
* e

Salts and covalent derivatives of the fluoride ion

HF |  |  |  | He

|
|
|
|

LiF | BeF2 | BF
BF3
B2F4 | CF4
other compounds | NF3
FN3
N2F2
N2F4
NF5§  | F2O
F2O2
other compounds | F2 | Ne
NaF | MgF2 | AlF
AlF3 | SiF4 | P2F4
PF3
PF5 | S2F2
SF2
SF4
SF6 | ClF
ClF3
ClF5 | Ar
KF | CaF
CaF2 | ScF3 | TiF2
TiF3
TiF4 | VF2
VF3
VF4
VF5 | CrF2
CrF3
CrF4
CrF5
CrF6§  | MnF2 | FeF2
FeF3 | CoF2
CoF3 | NiF2 | CuF
CuF2 | ZnF2 | GaF2
GaF3 | GeF2
GeF4 | AsF3
AsF5 | Se2F2
SeF4
SeF6 | BrF
BrF3
BrF5 | KrF2
RbF | SrF
SrF2 | YF3 | ZrF3
ZrF4 | NbF4
NbF5 | MoF2
MoF3
MoF4
MoF5
MoF6 | TcF4
TcF6 | RuF3
RuF5
RuF6 | RhF3
RhF5
RhF6 | PdF2 | AgF | CdF2 | InF
InF2
InF3 | SnF2
SnF4 | SbF3
SbF5 | Te3F2
TeF4
TeF6 | IF
IF3</br>IF5</br>IF7 | XeF2
XeF4
XeF6
CsF | BaF2 |  | HfF4 | TaF5 | WF2
WF3
WF4
WF5
WF6 | Re3F9
ReF4
ReF5
ReF6
ReF7 | OsF4
OsF5
OsF6 | IrF2
IrF3
IrF4
IrF5
IrF6 | PtF2
PtF4
PtF5
PtF6 | AuF
AuF3
Au2F10
AuF5•F2 | Hg2F2
HgF2
HgF4 | TlF | PbF2
PbF4 | BiF3
BiF5 | PoF2
PoF4
PoF6 | AtF  | RnF2
FrF | RaF2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
LaF3 | CeF3
CeF4 | PrF3 | NdF2,
NdF3 | PmF3 | SmF2,
SmF3 | EuF2,
EuF3 | GdF3 | TbF3 | DyF2,
DyF3 | HoF3 | ErF3 | TmF2
TmF3 | YbF2
YbF3 | LuF3
AcF3 | ThF4 | PaF5 | UF3
UF4
UF5
UF6 | NpF4
NpF6 | PuF3
PuF6 | AmF2
AmF3 | CmF3 | BkF3 | CfF3 | EsF3 | Fm  | Md  | No  | LrF3

§ means the substance has not been made.

* v
* t
* e

Oxygen compounds

* AgO
* Al2O3
* AmO2
* Am2O3
* As2O3
* As2O5
* Au2O3
* B2O3
* BaO
* BeO
* Bi2O3
* BiO2
* Bi2O5
* BrO2
* Br2O3
* Br2O5
* CO
* CO2
* C2O3
* CaO
* CaO2
* CdO
* CeO2
* Ce3O4
* Ce2O3
* ClO2
* Cl2O
* Cl2O3
* Cl2O4
* Cl2O6
* Cl2O7
* CoO
* Co2O3
* Co3O4
* CrO3
* Cr2O3
* Cr2O5
* Cr5O12
* CsO2
* Cs2O3
* CuO
* D2O
* Dy2O3
* Er2O3
* Eu2O3
* FeO
* Fe2O3
* Fe3O4
* Ga2O
* Ga2O3
* GeO
* GeO2
* H2O
* H218O
* H2O2
* HfO2
* HgO
* Hg2O
* Ho2O3
* I2O4
* I2O5
* I2O6
* I4O9
* In2O3
* IrO2
* KO2
* K2O2
* La2O3
* Li2O
* Li2O2
* Lu2O3
* MgO
* Mg2O3
* MnO
* MnO2
* Mn2O3
* Mn2O7
* MoO2
* MoO3
* Mo2O3
* NO
* NO2
* N2O
* N2O3
* N2O4
* N2O5
* NaO2
* Na2O
* Na2O2
* NbO
* NbO2
* Nd2O3
* OF2
* O2F2
* O3F2
* O4F2
* O2PtF6

Chemical formulas

* v
* t
* e

Fluorine compounds

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

|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|
|

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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