Fluorine nitrate: Difference between revisions

| Watchedfields = changed

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| ImageAlt = Structural formulas of fluorine nitrate, showing its resonance structure

| ImageFile1 = Fluorine nitrate molecule ball.png

| ImageSize1 = 150

| ImageAlt1 = Ball-and-stick model of the fluorine nitrate molecule

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|Section1={{Chembox Identifiers

| CASNo_Ref = {{cascite|correct|??}}

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| ChemSpiderID = 109875

| UNII = 1Q6BYH7F2B

| StdInChI=1S/FNO3/c1-5-2(3)4

| StdInChIKey = VHFBTKQOIBRGQP-UHFFFAOYSA-N

| SMILES = (O)O }}

|Section2={{Chembox Properties

|F=1|N=1|O=3

| Density = 2.217&nbsp;g/L<ref name=Ruff1935>{{cite journal |title= The fluorination of nitric acid. The nitroxyfluoride, NO₃F |journal= Angewandte Chemie |first1= Otto |last1= Ruff |first2= Walter |last2= Kwasnik |year= 1935 |volume= 48 |pages= 238–240 |doi=10.1002/ange.19350481604}}</ref>

| = -175

| = -46

|Section3={{Chembox Thermochemistry

| DeltaHf = +10./mol }}

|Section4={{Chembox Hazards

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'''Fluorine nitrate''' is an unstable derivative of [[nitric acid]] with the formula {{chem|FNO|3}}. Due to its instability, it is often produced from [[chlorine nitrate]]. :

==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. <ref name=":0">{{Cite journal |last=Oberhammer |first=H. |date=2002-03-13 |title=The NO bond in covalent nitrates and nitrites |url=https://www.sciencedirect.com/science/article/pii/S0022286001007669 |journal=Journal of Molecular Structure |volume=605 |issue=2 |pages=177–185 |doi=10.1016/S0022-2860(01)00766-9 |issn=0022-2860}}</ref>

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.<ref name=":0" />

==Synthesis and properties==

Whilst not fully understood, it is thought that {{chem|FNO|3}} forms as a result of termolecular recombination of {{chem|FO|}} and {{chem|NO|2}} 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:<ref>{{Cite journal |last=Elliott |first=Scott |date=1983-01-01 |title=Ultraviolet absorption spectra of FNO3 and HOF |url=https://www.sciencedirect.com/science/article/pii/0004698183904249 |journal=Atmospheric Environment (1967) |volume=17 |issue=4 |pages=759–761 |doi=10.1016/0004-6981(83)90424-9 |issn=0004-6981}}</ref><ref name=":1">{{Cite journal |last=Dianxun |first=Wang |last2=Peng |first2=Jiang |last3=Qiyuan |first3=Zhang |date=1996-11-29 |title=HeI photoelectron spectrum (PES) of fluorine nitrate, FONO2 |url=https://www.sciencedirect.com/science/article/pii/S0009261496011542 |journal=Chemical Physics Letters |volume=262 |issue=6 |pages=771–775 |doi=10.1016/S0009-2614(96)01154-2 |issn=0009-2614}}</ref>

:{{chem2|F2 + HNO3 -> FNO3 + HF}}

:{{chem2|F2 + KNO3 -> FNO3 + KF}}

It decomposes in water to form [[oxygen]] gas, [[oxygen difluoride]], [[hydrofluoric acid]], and nitric acid.<ref name=Ruff1935/>

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, {{chem|FNO|3}} was determined to have a planar structure with a particularly long nitrogen-oxygen bond length.<ref>{{Cite journal |last=Casper |first=Bernd |last2=Mack |first2=Hans-Georg |last3=Oberhammer |first3=Heinz |date=1995-04-01 |title=Gas-phase structures of some hypofluorites: FOSF5, FOSO2F, FOClO3 and FONO2 |url=https://www.sciencedirect.com/science/article/pii/002211399406031G |journal=Journal of Fluorine Chemistry |series=Papers presented at the American Chemical Society - George H. Cady Memorial Symposium |volume=71 |issue=2 |pages=215 |doi=10.1016/0022-1139(94)06031-G |issn=0022-1139}}</ref>

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.<ref name=":1" />

==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.<ref name=":1" />

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.<ref name=":1" />

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.<ref name=":1" />

{{Greenwood&Earnshaw}}

{{nitrates}}

{{fluorine compounds}}

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