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	{{chembox		{{Chembox
			| Watchedfields = changed
	| verifiedrevid = 443703841		| verifiedrevid = 454767937
	| Name = Ammonium fluoride
	| ImageFileL1 = Ammonium.svg		| Name = Ammonium fluoride
			| ImageFileL1 = Ammonium.svg
	| ImageSizeL1 = 90px
	| ImageNameL1 = The ammonium cation		| ImageSizeL1 = 90px
			| ImageNameL1 = The ammonium cation
	| ImageFileR1 = F-.svg		| ImageFileR1 = F-.svg
	| ImageSizeR1 = 30px		| ImageSizeR1 = 30px
	| ImageNameR1 = The fluoride anion		| ImageNameR1 = The fluoride anion
	| ImageFile2 = Ammonium-fluoride-3D-balls-ionic.png		| ImageFile2 = Ammonium-fluoride-3D-balls-ionic.png
	| ImageSize2 = 150px		| ImageSize2 = 150px
	| ImageName2 = ball-and-stick model of an ammonium cation (left) and an fluoride anion (right)		| ImageName2 = ball-and-stick model of an ammonium cation (left) and a fluoride anion (right)
	| ImageFile3 = Fluorid amonný.PNG		| ImageFile3 = Fluorid amonný.PNG
	| ImageName3 = Solid sample of ammonium fluoride		| ImageName3 = Solid sample of ammonium fluoride
	| IUPACName = Ammonium fluoride		| IUPACName = Ammonium fluoride
	| OtherNames = Neutral ammonium fluoride		| OtherNames = Neutral ammonium fluoride
	| Section1 = {{Chembox Identifiers		|Section1={{Chembox Identifiers
	| InChI = 1/FH.H3N/h1H;1H3		| InChI = 1/FH.H3N/h1H;1H3
	| SMILES = .		| SMILES = .
	| InChIKey = LDDQLRUQCUTJBB-UHFFFAOYAM		| InChIKey = LDDQLRUQCUTJBB-UHFFFAOYAM
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	| StdInChIKey = LDDQLRUQCUTJBB-UHFFFAOYSA-N		| StdInChIKey = LDDQLRUQCUTJBB-UHFFFAOYSA-N
	| CASNo = 12125-01-8		| CASNo = 12125-01-8
	| CASNo_Ref = {{cascite|correct|CAS}}		| CASNo_Ref = {{cascite|correct|CAS}}
	| RTECS = BQ6300000		| RTECS = BQ6300000
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID=23806		| ChemSpiderID =23806
	| EINECS = 235-185-9		| EINECS = 235-185-9
	| UNNumber = 2505		| UNNumber = 2505
			| ChEBI = 66871
			| PubChem = 25516
			| UNII = 4QT928IM0A
	}}		}}
	| Section2 = {{Chembox Properties		|Section2={{Chembox Properties
	| Formula = NH<sub>4</sub>F		| Formula = NH<sub>4</sub>F
	| MolarMass = 37.037 g/mol		| MolarMass = 37.037 g/mol
	| Appearance = White crystalline solid <br> ]		| Appearance = White crystalline solid <br> ]
	| Density = 1.009 g/cm<sup>3</sup>		| Density = 1.009 g/cm<sup>3</sup>
			| Solubility = 83.5 g/100 ml (25&nbsp;°C) <ref>{{cite web|title=Ammonium Fluoride|url=https://pubchem.ncbi.nlm.nih.gov/compound/ammonium_fluoride#section=Solubility|website=pubchem.ncbi.nlm.nih.gov|language=en}}</ref>
	| Solubility = 45.3 g/100 ml (25 °C)
	| SolubleOther = slightly soluble in alcohol, insoluble in liquid ammonia		| SolubleOther = slightly soluble in alcohol, insoluble in liquid ammonia
	| MeltingPt = 100 °C (decomp)		| MeltingPtC = 100
			| MeltingPt_notes = (decomposes)
			| MagSus = {{val|-23.0e-6|u=cm<sup>3</sup>/mol}}
	}}		}}
	| Section3 = {{Chembox Structure		|Section3={{Chembox Structure
	| CrystalStruct = ] (hexagonal)		| CrystalStruct = ] (hexagonal)
	}}		}}
	| Section7 = {{Chembox Hazards		|Section7={{Chembox Hazards
	| ExternalMSDS =		| ExternalSDS =
			| GHSPictograms = {{GHS05}} {{GHS06}}
	| EUIndex = 009-006-00-8
			| GHSSignalWord = Danger
	| EUClass = Toxic ('''T''')
			| HPhrases = {{H-phrases|301|311|314|330|331}}
	| RPhrases = {{R23/24/25}}
			| PPhrases = {{P-phrases|260|261|264|270|271|280|284|301+310|301+330+331|302+352|303+361+353|304+340|305+351+338|310|311|312|320|321|322|330|361|363|403+233|405|501}}
	| SPhrases = {{S1/2}}, {{S26}}, {{S45}}
			| GHS_ref = <ref>{{cite web|title=Ammonium Fluoride|url=https://pubchem.ncbi.nlm.nih.gov/compound/25516#section=Safety-and-Hazards|website=pubchem.ncbi.nlm.nih.gov|language=en}}</ref>
	| NFPA-H = 3
	| NFPA-F = 0		| NFPA-H = 3
	| NFPA-R = 0		| NFPA-F = 0
	| NFPA-O =		| NFPA-R = 0
	| FlashPt = Non-flammable		| NFPA-S =
			| FlashPt = Non-flammable
	}}		}}
	| Section8 = {{Chembox Related		|Section8={{Chembox Related
	| OtherAnions = ]<br/>]<br/>]		| OtherAnions = ]<br/>]<br/>]
	| OtherCations = ]<br/>]		| OtherCations = ]<br/>]
	| OtherCpds = ]		| OtherCompounds = ]
	}}		}}
	}}		}}
	'''Ammonium fluoride''' is the ] with the formula NH<sub>4</sub>F. It crystallizes as small colourless prisms, having a sharp saline taste, and is exceedingly soluble in water.		'''Ammonium fluoride''' is the ] with the formula NH<sub>4</sub>F. It crystallizes as small colourless prisms, having a sharp saline taste, and is highly soluble in water. Like all fluoride salts, it is moderately toxic in both acute and chronic overdose.<ref>{{cite web|title=Fluoride Toxicity - an overview {{!}} ScienceDirect Topics|url=https://www.sciencedirect.com/topics/pharmacology-toxicology-and-pharmaceutical-science/fluoride-toxicity|access-date=2020-12-16|website=www.sciencedirect.com}}</ref>
	==Crystal structure==		==Crystal structure==
	Ammonium fluoride adopts the ] crystal structure, in which both the ammonium cations and the fluoride anions are stacked in ABABAB... layers, each being tetrahedrally surrounded by four of the other. There are NH...F hydrogen bonds between the anions and cations.<ref>A. F. Wells, '''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984.</ref>. This structure is very similar to ], and ammonium fluoride is the only substance which can form mixed crystals with the water.<ref>{{cite journal|last=BRILL|first=R.|coauthors=ZAROMB, S.|title=Mixed Crystals of Ice and Ammonium Fluoride|journal=Nature|volume=173|issue=4398|pages=316–317|doi=10.1038/173316a0}}</ref>		Ammonium fluoride adopts the ] crystal structure, in which both the ammonium cations and the fluoride anions are stacked in ABABAB... layers, each being tetrahedrally surrounded by four of the other. There are N−H···F ]s between the anions and cations.<ref>A. F. Wells, ''Structural Inorganic Chemistry'', 5th ed., Oxford University Press, Oxford, UK, 1984.</ref> This structure is very similar to ], and ammonium fluoride is the only substance which can form mixed crystals with water.<ref>{{cite journal|last=Brill|first=R.|author2=Zaromb, S.|title=Mixed Crystals of Ice and Ammonium Fluoride|journal=Nature|year=1954 |volume=173|issue=4398|pages=316–317|doi=10.1038/173316a0|bibcode=1954Natur.173..316B |s2cid=4146351 }}</ref>
	==Reactions==		==Reactions==
	On passing ] gas (in excess) through the salt, ammonium fluoride absorbs the gas to form the ] ]. The reaction occurring is:		On passing ] gas (in excess) through the salt, ammonium fluoride absorbs the gas to form the ] ]. The reaction occurring is:
	:NH<sub>4</sub>F + HF → NH<sub>4</sub>HF<sub>2</sub>		:NH<sub>4</sub>F + HF → NH<sub>4</sub>HF<sub>2</sub>
	It sublimes when heated—a property common among ammonium salts. In the sublimation, the salt decomposes to ammonia and hydrogen fluoride , and the two gases recombine to give ammonium fluoride, ''i.e.'' the reaction is reversible:		Ammonium fluoride sublimes when heated—a property common among ammonium salts. In the sublimation, the salt decomposes to ammonia and hydrogen fluoride; the two gases can still recombine, ''i.e.'' the reaction is reversible:
	:F ↔ NH<sub>3</sub> + HF		:F ⇌ NH<sub>3</sub> + HF
	==Uses==		==Uses==
	This substance is commonly called "commercial ammonium fluoride". The word "neutral" is sometimes added to "ammonium fluoride" to represent the neutral salt - F vs the "acid salt" (NH<sub>4</sub>HF<sub>2</sub>). The acid salt is usually used in preference to the neutral salt in the ]ing of glass and related ]s. This property is shared among all soluble fluorides. For this reason it cannot be handled in glass test tubes or apparatus during laboratory work.		This substance is commonly called "commercial ammonium fluoride". The word "neutral" is sometimes added to "ammonium fluoride" to represent the neutral salt F as opposed to the "acid salt" (]). The acid salt is usually used in preference to the neutral salt in the ]ing of glass and related ]s. This property is shared among all soluble fluorides. For this reason it cannot be handled in glass test tubes or apparatus during laboratory work.
			Ammonium fluoride is a critical component of ] (BOE), a wet ] used in ]. It acts as the ] in a solution of concentrated ], creating an etchant with a more controllable rate of etching (than that of simple concentrated HF solutions).<ref name=Wolf>{{cite book | title = Silicon Processing for the VLSI Era: Volume 1 - Process Technology | last1 = Wolf | first1 = Stanley | last2 = Tauber | first2 = Richard | year = 1986 | pages = 532–533 | isbn = 978-0-9616721-3-3}}</ref>
⚫	It is also used for preserving wood, as a mothproofing agent, in printing and dying ]s, and as an ] in ].<ref name=Aigueperse>{{Cite book|first = Jean|last = Aigueperse|coauthors = Paul Mollard, Didier Devilliers, Marius Chemla, Robert Faron, Renée Romano, Jean Pierre Cuer|contribution = Fluorine Compounds, Inorganic|editor-last = Ullmann|title = Encyclopedia of Industrial Chemistry|year = 2005|publisher = Wiley-VCH|place = Weinheim|doi = 10.1002/14356007.a11_307}}</ref>
		⚫	It is also used for preserving wood, as a mothproofing agent, in printing and dyeing ]s, and as an ] in ].<ref name=Aigueperse>{{cite book|first = Jean|last = Aigueperse|author2=Paul Mollard |author3=Didier Devilliers |author4=Marius Chemla |author5=Robert Faron |author6=Renée Romano |author7=Jean Pierre Cuer |contribution = Fluorine Compounds, Inorganic|editor-last = Ullmann|title = Encyclopedia of Industrial Chemistry|year = 2005|publisher = Wiley-VCH|place = Weinheim|doi = 10.1002/14356007.a11_307| isbn=3-527-30673-0 }}</ref>
	==References==		==References==
	<references/>		<references/>
			{{Ammonium salts}}
			{{fluorine compounds}}
			{{Commons category}}
	]		]
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	]		]
	{{inorganic-compound-stub}}
	]
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