Nitrogen triiodide: Difference between revisions

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| verifiedrevid = 400328418

| ImageFileL1 = Nitrogen-iodide-2D.png

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| ImageNameL1 = Nitrogen triiodide (structural formula)

| ImageFileR1 = Nitrogen-triiodide-3D-balls.png

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| ImageNameR1 = Nitrogen triiodide

| IUPACName = triiodoamine

| OtherNames = nitrogen iodide, triiodine nitride

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'''Nitrogen triiodide''' is the [[inorganic compound]] with the formula [[nitrogen|N]][[Iodine|I]]₃. It is an extremely sensitive [[contact explosive]]: small quantities explode with a gunpowder-like snap when touched even lightly, releasing a purple cloud of iodine vapor. NI₃ has a complex structural chemistry that is difficult to study because of the instability of the derivatives.

Nitrogen triiodide was first characterized by [[X-ray crystallography]] in 1990 when it was prepared by an ammonia-free route. [[Boron nitride]] reacts with [[iodine fluoride]] in [[trichlorofluoromethane]] at −30 °C to produce pure NI₃ 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>

:BN + 3IF → NI₃ + BF₃

NI₃ is pyramidal (C_3v [[molecular symmetry]]), as are the other nitrogen trihalides as well as [[ammonia]].<ref name=Holleman>Holleman, A. F.; Wiberg, E. "Inorganic Chemistry" Academic Press: San Diego, 2001. ISBN 0-12-352651-5.</ref>

The material that is usually called "nitrogen triiodide" is prepared by the reaction of iodine with [[ammonia]]. When this reaction is conducted at low temperatures in anhydrous ammonia, the initial product is NI₃·(NH₃)₅, but this material loses some ammonia upon warming to give the 1:1 [[adduct]] NI₃·(NH₃). This adduct was first reported by [[Bernard Courtois]] 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 -NI₂-I-NI₂-I-NI₂-I-... Ammonia molecules are situated between the chains. When kept cold in the dark and damp with ammonia, NI₃·(NH₃) is stable.

The instability of NI₃ and NI₃NH₃ can be attributed to the great stability of N₂. 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 [[nitroglycerin]] 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 [[phlegmatizers]] that its shock sensitivity was reduced and it became safer to handle and transport as [[dynamite]].

:2 NI₃ (s) → N₂ (g) + 3 I₂ (g) (–290 kJ/mol)

: 8 NI₃NH₃ → 5 N₂ + 6 NH₄I + 9 I₂

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 [[detonation]]. Nitrogen triiodide is also notable for being the only known chemical explosive that detonates when exposed to [[alpha particles]] and [[nuclear fission]] products.<ref>Bowden, F. P. Initiation of explosion by neutrons, α-particles, and fission products. ''Proc. Roy. Soc.'' (London) '''1958''', ''A246'', 216-19.</ref>

{{reflist}}

*[http://jchemed.chem.wisc.edu/JCESoft/CCA/CCA0/MOVIES/NI3IOD.html See the explosion (requires the Quicktime plugin)]

*[http://www.chm.bris.ac.uk/motm/ni3/ni3j.htm Nitrogen Tri-Iodide - explains why the compound is explosive]

*[http://www.youtube.com/watch?v=2KlAf936E90 Nitrogen Tri-Iodide Detonation on Youtube]

[[cs:Jodid dusitý]]

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