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			{{short description|Chemical compound}}{{One source|date=October 2023}}{{Chembox
	{{chembox
			| Watchedfields = changed
	| verifiedrevid = 400328723		| verifiedrevid = 441981882
⚫	| Name = Nitrosyl fluoride
	| ImageFile = Nitrosyl-fluoride-2D-dimensions.png		| ImageFile = Nitrosyl-fluoride-2D-dimensions.png
			| ImageFile_Ref = {{chemboximage|correct|??}}
	<!-- | ImageSize = 200px -->		| ImageSize = 100
	| ImageName = Nitrosyl fluoride
			| ImageName = Skeletal formula of nitrosyl fluoride with measurements
	| ImageFile1 = Nitrosyl-fluoride-3D-balls.png
		⚫	| ImageFile1 = Nitrosyl-fluoride-3D-balls.png
⚫	<!-- | ImageSize1 = 200px -->
			| ImageFile1_Ref = {{chemboximage|correct|??}}
⚫	| ImageName1 = Nitrosyl fluoride
		⚫	| ImageSize1 = 100
⚫	| IUPACName = Nitrosyl fluoride
		⚫	| ImageName1 = Ball and stick model of nitrosyl fluoride
⚫	| OtherNames = NOF<br />Nitrogen oxyfluoride
		⚫	| IUPACName = Nitrosyl fluoride{{Citation needed|date=April 2012}}
⚫	| Section1 = {{Chembox Identifiers
		⚫	| OtherNames = Nitrogen oxyfluoride{{Citation needed|date=April 2012}}
⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
		⚫	|Section1={{Chembox Identifiers
⚫	| ChemSpiderID = 109874
			| Abbreviations = NOF{{Citation needed|date=April 2012}}
		⚫	| CASNo = 7789-25-5
			| CASNo_Ref = {{cascite|correct|??}}
			| UNII_Ref = {{fdacite|correct|FDA}}
			| UNII = 9FXL2Q69DQ
	| PubChem = 123261		| PubChem = 123261
		⚫	| ChemSpiderID = 109874
	| InChI = 1/FNO/c1-2-3
		⚫	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| InChIKey = ZEIYBPGWHWECHV-UHFFFAOYAP
			| EINECS = 232-153-6
	| SMILES = FN=O		| SMILES = FN=O
⚫	| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChI = 1S/FNO/c1-2-3		| StdInChI = 1S/FNO/c1-2-3
	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChI_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = ZEIYBPGWHWECHV-UHFFFAOYSA-N		| StdInChIKey = ZEIYBPGWHWECHV-UHFFFAOYSA-N
		⚫	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
⚫	| CASNo = 7789-25-5
		⚫	}}
	| RTECS =
		⚫	|Section2={{Chembox Properties
⚫	}}
		⚫	| Formula = NOF
⚫	| Section2 = {{Chembox Properties
		⚫	| MolarMass = 49.0045 g mol<sup>−1</sup>
⚫	| Formula = NOF
			| Appearance = Colourless gas
⚫	| MolarMass = 49.0045 g/mol
		⚫	| Density = 2.657 mg mL<sup>−1</sup>(gas) 1.326 g/cm<sup>3</sup>(liquid)
	| Appearance = colourless gas <br> bluish with impurities
			| Solubility = Reacts
⚫	| Density = 1.719 g/cm<sup>3</sup> (solid) <br> 1.326 g/mL (liquid) <br> 2.657 g/L (gas)
	| Solubility = Reacts.		| MeltingPtC = -166
	| MeltingPt = -166°C (107.15 K)		| BoilingPtC = -72.4
		⚫	}}
	| BoilingPt = -72.4°C (200.75 K)
		⚫	|Section3={{Chembox Related
⚫	}}
			| OtherCompounds = {{Unbulleted list|]|]|]}}
	| Section3 = {{Chembox Structure
		⚫	}}
	| MolShape =
	| CrystalStruct =
	| Dipole =
⚫	}}
	| Section7 = {{Chembox Hazards
	| ExternalMSDS =
	| MainHazards =
	| FlashPt =
	| RPhrases =
	| SPhrases =
	}}
⚫	| Section8 = {{Chembox Related
	| OtherAnions = ]<br/>]
	| OtherCations = ], ]
	}}
	}}		}}
		⚫	'''Nitrosyl fluoride''' (''']]]''') is a ] ] compound.
			== Physical properties ==
⚫	'''Nitrosyl fluoride''', ]]], is a ] ] compound.
			The compound is a ] gas, with ].<ref name=":0">{{Greenwood&Earnshaw1st|page=507}}</ref> The ] explains this geometry via a ] on the nitrogen atom.
	==Reactions==		==Chemistry==
	NOF is a highly reactive ] that converts many ]s to their ]s, releasing ]:		Nitrosyl fluoride is typically produced by direct reaction of ] and ], although halogenation with a perfluorinated metal salt is also possible. The compound is a highly reactive ] that converts many ]s to their ]s, releasing ] in the process:
	:''n'' NOF + M → MF<sub>''n''</sub> + ''n'' NO		:''n'' NOF + M → MF<sub>''n''</sub> + ''n'' NO
			For this reason, aqueous NOF solutions are, like ], powerful solvents for metals.<ref name=":0" />
	NOF also fluorinates ]s to form ]s that have a ]-like character, such as ].
	Aqueous solutions of NOF are powerful solvents for metals, by a mechanism similar to that seen in ]. Nitrosyl fluoride reacts with ] to form ], which then forms ]:		Absent an oxidizable metal, NOF reacts with ] to form ], which then disproportionates to ]:
	:NOF + H<sub>2</sub>O → HNO<sub>2</sub> + HF		:NOF + H<sub>2</sub>O → HNO<sub>2</sub> + HF
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	:3 HNO<sub>2</sub> → HNO<sub>3</sub> + 2 NO + H<sub>2</sub>O		:3 HNO<sub>2</sub> → HNO<sub>3</sub> + 2 NO + H<sub>2</sub>O
			These reactions occur in both acidic and basic solutions.<ref name=":0" />
	Nitrosyl fluoride can also convert ]s to ]:
			Nitrosyl fluoride also forms ]-like ]s with ] ]s; for example, ] reacts to give ]. Similarly, the compound nitrosylates compounds with a free proton; thus ]s convert to ]:<ref name=":0" />
	:ROH + NOF → RONO + HF		:ROH + NOF → RONO + HF
	==Uses==		==Uses==
	Nitrosyl fluoride is used as a ]{{Fact|date=March 2007}} and as a ] and ] agent in ].{{Fact|date=March 2007}} It is also used as an oxidizer in ]s.		Nitrosyl fluoride is used as a ] and as a ] and ]{{dubious|reason=More likely to nitrosate|date=November 2024}} agent in ].{{cn|date=November 2024}}
	==References==		==References==
			<references />
	{{Greenwood&Earnshaw}}
	==External links==		==External links==
	*		*
	*		*
	]		]
	]		]
	]		]
			]
			]
			{{Fluorine compounds}}
	]
	]
	]