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			{{Chembox
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	* Parameters work only in their own section.
		⚫	| verifiedrevid = 446277962
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			| ImageFile1 = Nitrogen-iodide-2D.png
	* When a section is really not needed, delete the whole section.
			| ImageSize1 = 120px
	For more information, see ]. -->
			| ImageName1 = Nitrogen triiodide (structural formula)
	{{chembox
		⚫	| ImageFileL2 = Nitrogen-triiodide-3D-balls.png
⚫	| verifiedrevid = 400328418
	| ImageFileL1 = Nitrogen-iodide-2D.png		| ImageNameL2 = Nitrogen triiodide
		⚫	| ImageFileR2 = Nitrogen-triiodide-3D-vdW.png
	| ImageSizeL1 = 120px
	| ImageNameL1 = Nitrogen triiodide (structural formula)		| ImageNameR2 = Nitrogen triiodide
			| IUPACNames = Nitrogen triiodide<ref name="redbook2005-NF3">''per analogiam'', see NF<sub>3</sub> names, IUPAC Red Book 2005, p. 314</ref><br>Triiodoazane<ref name="redbook2005-NF3"/><br>Triiodidonitrogen<ref name="redbook2005-NF3"/>
⚫	| ImageFileR1 = Nitrogen-triiodide-3D-balls.png
			| OtherNames = Nitrogen iodide<br>Ammonia triiodide<br>Touch Powder<br>Triiodine nitride<br>Triiodine mononitride<br>Triiodamine{{Citation needed|date=September 2020}}<br>Triiodoamine{{citation needed|date=June 2018}}<br>Iodine nitride
	| ImageSizeR1 = 120px
		⚫	| Section1 = {{Chembox Identifiers
⚫	| ImageNameR1 = Nitrogen triiodide
		⚫	| Abbreviations =
	| IUPACName = triiodoamine
	| OtherNames = nitrogen iodide, triiodine nitride
⚫	| Section1 = {{Chembox Identifiers
⚫	| Abbreviations =
	| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}		| ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}}
	| ChemSpiderID = 55511		| ChemSpiderID = 55511
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	| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}		| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}}
	| StdInChIKey = FZIONDGWZAKCEX-UHFFFAOYSA-N		| StdInChIKey = FZIONDGWZAKCEX-UHFFFAOYSA-N
			| CASNo_Ref = {{cascite|correct|??}}
	| CASNo = 13444-85-4		| CASNo = 13444-85-4
	| EC-number =		| EC_number =
	| PubChem = 61603		| PubChem = 61603
	| SMILES = IN(I)I		| SMILES = IN(I)I
	| InChI =
	| RTECS =		| RTECS =
	| MeSHName =		| MeSHName =
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	| ChEBI =		| ChEBI =
	| KEGG_Ref = {{keggcite|correct|kegg}}		| KEGG_Ref = {{keggcite|correct|kegg}}
	| KEGG =		| KEGG =
			}}
	| ATCCode_prefix =
		⚫	| Section2 = {{Chembox Properties
	| ATCCode_suffix =
	| ATC_Supplemental =}}
⚫	| Section2 = {{Chembox Properties
	| Formula = NI<sub>3</sub>		| Formula = NI<sub>3</sub>
	| MolarMass = 394.719 g/mol		| MolarMass = 394.719 g/mol
	| Appearance = red solid		| Appearance = dark solid
	| Density =		| Density =
	| MeltingPt =		| MeltingPt =
	| Melting_notes =		| MeltingPt_notes =
	| BoilingPt =		| BoilingPt =
	| Boiling_notes = sublimes at -20 °C		| BoilingPt_notes = sublimes at −20 °C
	| Solubility = no		| Solubility = Insoluble
			| SolubleOther = organic solvents,<ref>. acornusers.org</ref> such as ]
	| SolubleOther =
	| Solvent =		| pKa =
	| pKa =		| pKb =
			}}
	| pKb = }}
	| Section7 = {{Chembox Hazards		| Section7 = {{Chembox Hazards
			| MainHazards = Extremely explosive and unstable
	| EUClass =
	| EUIndex =		| NFPA-H = 3
	| MainHazards =		| NFPA-F = 0
	| NFPA-H =		| NFPA-R = 4
	| NFPA-F =		| NFPA-S =
	| NFPA-R =		| FlashPt =
	| NFPA-O =		| AutoignitionPt =
	| RPhrases =		| ExploLimits =
	| SPhrases =		| PEL =
			}}
	| RSPhrases =
	| FlashPt =
	| Autoignition =
	| ExploLimits =
	| PEL = }}
	}}<!-- Text starts below-->		}}<!-- Text starts below-->
	'''Nitrogen triiodide''' is the ] with the formula ]]<sub>3</sub>. It is an extremely sensitive ]: small quantities explode with a gunpowder-like snap when touched even lightly, releasing a purple cloud of iodine vapor. NI<sub>3</sub> has a complex structural chemistry that is difficult to study because of the instability of the derivatives.		'''Nitrogen triiodide''' is an ] with the formula ]]<sub>3</sub>. It is an extremely sensitive ]: small quantities explode with a loud, sharp snap when touched even lightly, releasing a purple cloud of ] vapor; it can even be detonated by ]. NI<sub>3</sub> has a complex structural chemistry that is difficult to study because of the instability of the derivatives.
	==Structure of NI<sub>3</sub> and its derivatives==		==Structure of NI<sub>3</sub> and its derivatives==
	Nitrogen triiodide was first characterized by ] in 1990 when it was prepared by an ammonia-free route. ] reacts with ] in ] at −30 °C to produce pure NI<sub>3</sub> in low yield:<ref>{{cite journal |author = Tornieporth-Oetting, I.; Klapötke, T. | journal = Angewandte Chemie International Edition |year = 1990 | volume = 29| page =677–679| doi = 10.1002/anie.199006771 |title = Nitrogen Triiodide}}</ref>		Nitrogen triiodide was first characterized by ] in 1990, when it was prepared by an ammonia-free route. ] reacts with ] in ] at −30&nbsp;°C to produce pure NI<sub>3</sub> in low yield:<ref>{{ cite journal |author1=Tornieporth-Oetting, I. |author2=Klapötke, T. | title = Nitrogen Triiodide | journal = Angewandte Chemie International Edition | year = 1990 | volume = 29 | issue = 6 | pages = 677–679 | doi = 10.1002/anie.199006771 }}</ref>
	:BN + 3IF → NI<sub>3</sub> + BF<sub>3</sub>		:BN + 3 IF → NI<sub>3</sub> + BF<sub>3</sub>
	NI<sub>3</sub> is pyramidal (C<sub>3v</sub> ]), as are the other nitrogen trihalides as well as ].<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>		NI<sub>3</sub> is pyramidal (C<sub>3v</sub> ]), as are the other nitrogen trihalides and ].<ref name=Holleman>{{ cite book |author1=Holleman, A. F. |author2=Wiberg, E. | title = Inorganic Chemistry | publisher = Academic Press | location = San Diego | year = 2001 | isbn = 0-12-352651-5 }}</ref>
	The material that is usually called "nitrogen triiodide" is prepared by the reaction of iodine with ]. When this reaction is conducted at low temperatures in anhydrous ammonia, the initial product is NI<sub>3</sub>·(NH<sub>3</sub>)<sub>5</sub>, but this material loses some ammonia upon warming to give the 1:1 ] NI<sub>3</sub>·(NH<sub>3</sub>). This adduct was first reported by ] in 1812, and its formula was finally determined in 1905 by Silberrad.<ref>Silberrad, O. "On the Constitution of Nitrogen Triiodide" ''Journal of the Chemistry Society'' 1905, volume 87, pages 55-66. {{DOI|10.1039/CT9058700055}}</ref> Its solid state structure consists of chains of -NI<sub>2</sub>-I-NI<sub>2</sub>-I-NI<sub>2</sub>-I-... Ammonia molecules are situated between the chains. When kept cold in the dark and damp with ammonia, NI<sub>3</sub>·(NH<sub>3</sub>) is stable.		The material that is usually called "nitrogen triiodide" is prepared by the reaction of iodine with ]. When this reaction is conducted at low temperatures in anhydrous ammonia, the initial product is NI<sub>3</sub> · (NH<sub>3</sub>)<sub>5</sub>, but this material loses some ammonia upon warming to give the 1:1 ] NI<sub>3</sub> · NH<sub>3</sub>. This adduct was first reported by ] in 1812, and its formula was finally determined in 1905 by ].<ref>{{ cite journal | author = Silberrad, O. | title = The Constitution of Nitrogen Triiodide | journal = Journal of the Chemical Society, Transactions | year = 1905 | volume = 87 | pages = 55–66 | doi = 10.1039/CT9058700055 | url = https://zenodo.org/record/1429707 }}</ref> Its solid state structure consists of chains of -NI<sub>2</sub>-I-NI<sub>2</sub>-I-NI<sub>2</sub>-I-.<ref>{{ cite journal | first1 = H. | last1 = Hart | first2 = H. | last2 = Bärnighausen | first3 = J. | last3 = Jander | title = Die Kristallstruktur von Stickstofftrijodid-1-Ammoniak NJ<sub>3</sub> · NH<sub>3</sub> | issue = 4–6 | journal = ] | year = 1968 | volume = 357 | pages = 225–237 | doi = 10.1002/zaac.19683570410 }}</ref> Ammonia molecules are situated between the chains. When kept cold in the dark and damp with ammonia, NI<sub>3</sub> · NH<sub>3</sub> is stable.
			]
	==Decomposition and explosiveness==		==Decomposition and explosiveness==
			]
⚫	The instability of NI<sub>3</sub> and NI<sub>3</sub>NH<sub>3</sub> can be attributed to the great stability of N<sub>2</sub>. Nitrogen triiodide has no practical commercial value due to its extreme shock sensitivity, making it impossible to store, transport, and utilize for controlled explosions. Whereas pure ] is also highly shock-sensitive (although not nearly as much so as nitrogen triiodide, which can be set off with the touch of a feather) and powerful, it was only due to ] that its shock sensitivity was reduced and it became safer to handle and transport as ].
		⚫	The instability of NI<sub>3</sub> and NI<sub>3</sub> · NH<sub>3</sub> can be attributed to the large ] caused by the three large iodine atoms being held in proximity to each other around the relatively tiny nitrogen atom. This results in a very low ] for its decomposition, a reaction made even more favorable due to the great stability of N<sub>2</sub>. Nitrogen triiodide has no practical commercial value due to its extreme shock sensitivity, making it impossible to store, transport, and utilize for controlled explosions. Whereas pure ] is powerful and also greatly shock-sensitive (although not nearly as much so as nitrogen triiodide, which can be set off with the touch of a feather), it was only due to ] that nitroglycerin's shock sensitivity was reduced and it became safer to handle and transport in the form of ].
	The decomposition of NI<sub>3</sub> proceeds as follows to give nitrogen gas and iodine:		The decomposition of NI<sub>3</sub> proceeds as follows to give nitrogen gas and iodine:
	:2 NI<sub>3</sub> (s) → N<sub>2</sub> (g) + 3 I<sub>2</sub> (g) (–290 kJ/mol)		:2 NI<sub>3</sub> (s) → N<sub>2</sub> (g) + 3 I<sub>2</sub> (g) (−290 kJ/mol)
	However, the dry material is a contact explosive, decomposing approximately as follows:<ref name=Holleman/>		However, the dry material is a contact explosive, decomposing approximately as follows:<ref name=Holleman/>
	: 8 NI<sub>3</sub>NH<sub>3</sub> → 5 N<sub>2</sub> + 6 NH<sub>4</sub>I + 9 I<sub>2</sub>		: 8 NI<sub>3</sub> · NH<sub>3</sub> → 5 N<sub>2</sub> + 6 ] + 9 I<sub>2</sub>
	Consistent with this equation, these explosions leave orange-to-purple stains of iodine, which can be removed with ] solution. An alternate method of stain removal is to simply allow the iodine time to sublime.		Consistent with this equation, these explosions leave orange-to-purple stains of iodine, which can be removed with ] solution. An alternate method of stain removal is to simply allow the iodine time to sublime.
	Small amounts of nitrogen triiodide are sometimes synthesized as a demonstration to high school chemistry students or as an act of "chemical magic".<ref>Ford, L. A. and Grundmeier, E. W. ''Chemical Magic''. Dover, '''1993''', p. 76. ISBN 0486676285</ref> To highlight the sensitivity of the compound, it is usually detonated by touching it with a feather but even the slightest air current or other movement can cause ]. Nitrogen triiodide is also notable for being the only known chemical explosive that detonates when exposed to ] and ] products.<ref>Bowden, F. P. Initiation of explosion by neutrons, α-particles, and fission products. ''Proc. Roy. Soc.'' (London) '''1958''', ''A246'', 216-19.</ref>		Small amounts of nitrogen triiodide are sometimes synthesized as a demonstration to high school chemistry students or as an act of "chemical magic."<ref>{{cite book | author1 = Ford, L. A. | author2 = Grundmeier, E. W. | title = Chemical Magic | publisher = Dover | year = 1993 | page = | isbn = 0-486-67628-5 | url-access = registration | url = https://archive.org/details/chemicalmagic00ford_0/page/76 }}</ref> To highlight the sensitivity of the compound, it is usually detonated by touching it with a feather, but even the slightest air current, laser light, or other movement can cause ]. Nitrogen triiodide is also notable for being the only known chemical explosive that detonates when exposed to ] and ] products.<ref>{{ cite journal | author = Bowden, F. P. | title = Initiation of Explosion by Neutrons, α-Particles, and Fission Products | journal = Proceedings of the Royal Society of London A | year = 1958 | volume = 246 | issue = 1245 | pages = 216–219 | doi = 10.1098/rspa.1958.0123 | bibcode = 1958RSPSA.246..216B | s2cid = 137728239 }}</ref>
	==References==		==References==
	{{reflist}}		{{reflist|30em}}
	==External links==		==External links==
	*		*
	*		*
	*		*
			{{iodides}}
			{{Nitrides}}
			{{Nitrogen compounds}}
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