Fluorine nitrate

Names
Other names

Nitryl hypofluorite

Identifiers

CAS Number

* 7789-26-6 Y

3D model (JSmol)

* Interactive image

ChemSpider |

* 109875

PubChem CID

* 123262

UNII |

* 1Q6BYH7F2B

InChI

* InChI=1S/FNO3/c1-5-2(3)4

Key: VHFBTKQOIBRGQP-UHFFFAOYSA-N

SMILES

* FO[N+](=O)[O-]

Properties

Chemical formula

| FNO3
Molar mass | 81.002 g·mol−1
Density | 2.217 g/L[1]
Melting point |  −175 °C (−283.0 °F; 98.1 K)
Boiling point |  −46 °C (−51 °F; 227 K)
Thermochemistry

Std enthalpy of
formation (ΔfH⦵298)

| +10.46 kJ/mol
Hazards
Main hazards | Explosive gas

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

Fluorine nitrate is an unstable derivative of nitric acid with the formula FNO3. It is shock-sensitive.[1] Due to its instability, it is often produced from chlorine nitrate as needed[citation needed]. Fluorine Nitrate is an inert molecule thought to play a significant role in atmospheric chemistry.[2]

## Contents

* 1 History
* 2 Synthesis and properties
* 3 Applications
* 4 References

## History

In 1935, professor George H. Cady was first to synthesize fluorine nitrate and has since maintained a long and controversial history. In 1937, American chemist and biochemist Linus Pauling and one of his first graduate students, Lawrence O. Brockway, utilized electron diffraction intensities to determine the structure of the oxygen and fluorine bond perpendicular to the NO2 plane to be a non-planar structure. This would later be confirmed in 1963 and 1966 utilizing infrared spectra. [3]

In a 1995 study performed by Universität Tubingen in Germany, found through electron diffraction that the nitrogen–oxygen bond is surprisingly long at about a length of 150.7 ppm. This length is likely the result of the presence of electronegative atoms compared to other similar structures such as nitric acid.[3]

## Synthesis and properties

Whilst not fully understood, it is thought that FNO3 forms as a result of termolecular recombination of FO and NO2 radicals. Fluorine Nitrate is prepared through the agitation of fluorine in its gaseous form, which will bubble through nitric acid or solid KNO3. Due to the shock sensitive nature of the compound, it is necessary to handle it with extreme caution:[4][5]

2 \+ HNO
3 → FNO
3 \+ HF

2 \+ KNO
3 → FNO
3 \+ KF

It decomposes in water to form oxygen gas, oxygen difluoride, hydrofluoric acid, and nitric acid.[1]

In fluorine nitrate, the oxygen atom bridging nitrogen and fluorine is in a rare oxidation state of 0 due to its electronegativity being lower than that of fluorine but higher than that of nitrogen. The role of electronegativity also is significant in the structure of fluorine nitrate. Through electron diffraction analysis, FNO3 was determined to have a planar structure with a particularly long nitrogen-oxygen bond length.[6]

Fluorine nitrate has been linked to higher ionization potential due to the centrality of fluorine. This higher ionization potential is indicative of electron ionization of deeper shell orbitals.[5]

## Applications

Since the 1990s, fluorine nitrate has been studied as a critical factor of atmospheric chemistry. It was in this period that fluorine nitrate began to be labeled as a reservoir species in the atmosphere.[5]

The relationship between the ionization potential and the highest occupied molecular orbital (HOMO) in fluorine nitrate was determined to be large. In a 1996 study, researchers asserted that the ionization potential of the HOMO in a molecule is a reflection of the electron-donating capacities of a molecule and as the ionization potential of the HOMO is lowered, subsequently the electron donating capacities of the molecule increase and become stronger.[5]

Despite the molecule’s inert nature, it is asserted by the 1996 study that fluorine nitrate may be the best possible reservoir species in the process of ozone depletion.[5]

## References

1. ↑ 1.0 1.1 1.2 Ruff, Otto; Kwasnik, Walter (1935). "The fluorination of nitric acid. The nitroxyfluoride, NO3F". Angewandte Chemie 48: 238–240. doi:10.1002/ange.19350481604.
2. ↑ Jensen, James O. (2005-03-07). "Vibrational frequencies and structural determination of fluorine nitrate". Journal of Molecular Structure: THEOCHEM 716 (1): 11–17. doi:10.1016/j.theochem.2004.10.041. ISSN 0166-1280. https://www.sciencedirect.com/science/article/pii/S0166128004008486.
3. ↑ 3.0 3.1 Oberhammer, H. (2002-03-13). "The NO bond in covalent nitrates and nitrites". Journal of Molecular Structure 605 (2): 177–185. doi:10.1016/S0022-2860(01)00766-9. ISSN 0022-2860. https://www.sciencedirect.com/science/article/pii/S0022286001007669.
4. ↑ Elliott, Scott (1983-01-01). "Ultraviolet absorption spectra of FNO3 and HOF". Atmospheric Environment (1967) 17 (4): 759–761. doi:10.1016/0004-6981(83)90424-9. ISSN 0004-6981. https://www.sciencedirect.com/science/article/pii/0004698183904249.
5. ↑ 5.0 5.1 5.2 5.3 5.4 Dianxun, Wang; Peng, Jiang; Qiyuan, Zhang (1996-11-29). "HeI photoelectron spectrum (PES) of fluorine nitrate, FONO2". Chemical Physics Letters 262 (6): 771–775. doi:10.1016/S0009-2614(96)01154-2. ISSN 0009-2614. https://www.sciencedirect.com/science/article/pii/S0009261496011542.
6. ↑ Casper, Bernd; Mack, Hans-Georg; Oberhammer, Heinz (1995-04-01). "Gas-phase structures of some hypofluorites: FOSF5, FOSO2F, FOClO3 and FONO2". Journal of Fluorine Chemistry. Papers presented at the American Chemical Society - George H. Cady Memorial Symposium 71 (2): 215. doi:10.1016/0022-1139(94)06031-G. ISSN 0022-1139. https://www.sciencedirect.com/science/article/pii/002211399406031G.

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Salts and covalent derivatives of the nitrate ion

HNO3 |  |  |  | He

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LiNO3 | Be(NO3)2 | B(NO3)−4 | C  | NO−3,
NH4NO3 | O  | FNO3 | Ne
NaNO3 | Mg(NO3)2 | Al(NO3)3 | Si  | P  | S  | ClONO2 | Ar
KNO3 | Ca(NO3)2 | Sc(NO3)3 | Ti(NO3)4 | VO(NO3)3 | Cr(NO3)3 | Mn(NO3)2 | Fe(NO3)3,
Fe(NO3)2 | Co(NO3)2,
Co(NO3)3 | Ni(NO3)2 | Cu(NO3)2 | Zn(NO3)2 | Ga(NO3)3 | Ge  | As  | Se  | Br  | Kr
RbNO3 | Sr(NO3)2 | Y(NO3)3 | Zr(NO3)4 | Nb  | Mo  | Tc  | Ru  | Rh  | Pd(NO3)2 | AgNO3 | Cd(NO3)2 | In  | Sn  | Sb(NO3)3 | Te  | I  | Xe(NO3)2
CsNO3 | Ba(NO3)2 |  | Hf  | Ta  | W  | Re  | Os  | Ir  | Pt  | Au  | Hg2(NO3)2,
Hg(NO3)2 | Tl(NO3)3,
TlNO3 | Pb(NO3)2 | Bi(NO3)3
BiO(NO3) | Po  | At  | Rn
FrNO3 | Ra(NO3)2 |  | Rf  | Db  | Sg  | Bh  | Hs  | Mt  | Ds  | Rg  | Cn  | Nh  | Fl  | Mc  | Lv  | Ts  | Og
| ↓  |  |
La(NO3)3 | Ce(NO3)3,
Ce(NO3)4 | Pr  | Nd(NO3)3 | Pm  | Sm  | Eu(NO3)3 | Gd(NO3)3 | Tb(NO3)3 | Dy  | Ho  | Er  | Tm  | Yb  | Lu
Ac(NO3)3 | Th(NO3)4 | Pa  | UO2(NO3)2 | Np  | Pu  | Am  | Cm  | Bk  | Cf  | Es  | Fm  | Md  | No  | Lr

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* 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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