Nitrogen triiodide

Galal-Gorchev and Morris reported that they prepared nitrogen tribromide by reaction of aqueous bromine with ammonia and they confirmed the formation of NBr3 by extraction into chloroform and analyzed the chloroform solution by UV spectroscopy [41]. Jander [40] reports that the first preparation of nitrogen tribromide was achieved by Thiedemann by reaction of an acidic aqueous ammonia salt solution (pH = 4) with bromine. The UV spectroscopy is mentioned as the method of the product analysis. The isolation of pure nitrogen tribromide from these aqueous solutions was done by extraction with ether and subsequent precipitation in Freon 12 at —110 °C. 

Some other methods of preparation of NBrs by direct bromination of ammonia are further summarized by Jander [40]. Another possible way for preparation of pure solid NBr3 is by reaction of bromine or hypobromus acid with an aqueous solution of ammonia [41, 45]. The crmcentration of reaction products is a function of temperature, acidity, and bromine to ammonia ratio. Nitrogen tribromide, NBr3 forms from neutral solutions when the molar ratio of bromine to ammonia is greater than 1.5 [45]. 

Pure solid nitrogen tribromide may be prepared by reaction of bistrimethylsilyl-bromamine and bromine chloride at —87 °C in pentane according to Jander [40]  

According to some more recent investigations by Klapbtke, nitrogen tribromide also forms by reaction of bromine azide and elemental bromine in gaseous form [42]  

Nitrogen triiodide adduct with one molecule of ammonia (NI3-NH3) was first prepared by Bernard Courtois, discoverer of iodine, in 1813. It was among the first derivatives of iodine ever made [46, 47]. The history of the investigation of nitrogen triiodide during the nineteenth century is summarized in review by Chattaway [47]. 

In the observation of phenomena, the conduct of analyses, and other determinations, one is urgently warned against being influenced in any way by theories or other miscellaneous preconceived opinions. 

As early as 1813 B. Courtois reported Ann. Chim. 1813, 88, 309) that a black powder is formed when aqueous ammonia reacts with iodine. This so-called iodure d azote (nitrogen iodide) is not a single homogeneous compound, but a mixture of nitrogen triiodide and addition compounds between ammonia and iodoamincs. Other authors later obtained a compound of the composition NI3 NH3 using various methods.  

This experiment may only be carried out by experienced chemists. Nitrogen iodide is extremely explosive. Safety glasses and protective gloves must be 

Large test tube, stand, funnel containing a fluted filter paper, 500-mL Erlcn-meyer flask, stick 2 meters in length, safety glasses, protective gloves. 

Iodine, concentrated aqueous ammonia solution, ethanol, diethyl ether. Experimental Procedure 

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Nitrogen triiodide Acids, bromine, chlorine, hydrogen sulflde, ozone... 

Nitrogen Triiodide. NI3, mw 394.77, N 3.55%, blk powd, mp (explds), bp (subl in vac). Insol in cold w, decomps in hot w sol in aq Na2S203 and KCNS. Prepd by the action of gaseous NH3 on solid KIBr2, foilowed by rapid w washing (Refs 1,4, 10 11). NI3 must be kept ether wet. When dry, the slightest shock, vibration, temp rise, air draft, etc, will cause it to detonate (Refs 14 15). Under vac, dry NI3 detonates at pressures under 2xlG 3cm. Over this press simple decompn occurs with the evolution of I2 (Refs 7-9)... 

Nitrogen Triiodide, NI3, mw 394.77, N 3.5% a black powd, detons when dry, exposed to light, or an elec spark (Refs 8 10) Qf 35kcal/mole (Ref 7). It is formed by the interaction of free 1 or I3" on liq, gaseous, or aq ammonia (Refs 1, 8 10). N triiodide forms a series of solvates with excess ammonia NI3.NH3) bright red needles, explds when dry (Ref 2). 

D.6 Write the formula of (a) dinitrogen tetroxide (b) hydrogen sulfide (c) dichlorine heptoxide (d) nitrogen triiodide (e) sulfur dioxide (f) hydrogen fluoride (g) diiodine hexachloride. 

Recent Chemistry and Structure Investigation of Nitrogen Triiodide, Tribromide, Trichloride, and Related Compounds... 

Write formulas for each of the following compounds (a) nitrogen monoxide, (b) nitrogen tribromide, and (c) nitrogen triiodide. 

Explosive, formed on prolonged contact of nitrogen triiodide with water. 

See Nitrogen triiodide-ammonia See other A -iia login compounds... 

During the reductive cleavage of cyclopolyenes with potassium in liquid ammonia, the intermediate anionic species are quenched with iodine-pentane mixtures. The possibility of formation of explosive nitrogen triiodide and the need for precautions are stressed. 

Ammonia solutions react with iodine (or potassium iodide) to produce highly explosive addition compounds of nitrogen triiodide and ammonia. 

Reaction of iodine with the lithium heptynide in liquid ammonia to give (explosive) 1-iodoheptyne may lead to formation of nitrogen triiodide as a black precipitate. Low temperatures minimise the formation, and it may be destroyed by adding sodium ethoxide solution. 

Nitrogen triiodide a-Nitroguanidine Nitromethane Acids, bromine, chlorine, hydrogen sulfide, ozone Complex salts of mercury and silver Acids, alkylmetal halides, hydroxides, hydrocarbons, organic amines, formaldehyde, nitric acid, perchlorates... 

Nitrogen trilluoride, 4336 Nitrogen triodide, 4633 Nitrogen triiodide-silver amide, 4634 Nitrogen triiodide-ammonia, 4635 Nitrosyl chloride, 4023 Nitrosyl fluoride, 4302 Nitryl chloride, 4025 Nitryl fluoride, 4303... 

Mercury(II) /V-pcrchlory lbcnzylamidc. 3651 Monopotassium perchlorylamide, 3994 Nitrogen triiodide-silver amide, 4634 Nitrosylruthenium trichloride, 4144 Pentaamminedinitrogenruthenium(II) salts, 4596 Pentakis(dimethylamino)tantalum, 3384 Pentasilver diamidophosphate, 0046 Pentasilver orthodiamidophosphate, 0044 Plutonium nitride, 4726 Poly (dimercury immonium hydroxide), 4422... 

Reaction with hypochlorite solution also produces chloramine. Ammonia reacts with iodine to form nitrogen triiodide, which further combines with a molecule of NH3 to form an adduct NI3 NH3, an insoluble brown-black sohd which decomposes upon exposure to light in the presence of NH3 ... 

Most reactions of bromine are highly exothermic which can cause incandescence or sudden increase in pressure and rupture of reaction flasks. There are a number of cases of explosions documented in the literature. (NFPA. 1986. Fire Protection Guide on Hazardous Materials, 9th ed. Quincy, MA National Fire Protection Association) Reactions of liquid bromine with most metals (or any metal in finely divided state), metal hydrides, carbonyls and nitrides can be explosive. Many oxides and halides of nonmetals, such as nitrogen triiodide or phosphorus trioxide, react explosively or burst into flame in contact with liquid bromine. 

The case with which highly expl Xe03 may be formed at room temp by reaction of Xe fluorides with moisture has been strongly emphasized (Refs 2, 3 4). Xenon trioxide, Xe03, is a wh sol comparable in deton sensitivity to nitrogen triiodide and in expl force to TNT Refs 1) N. Bartlett P.R. Rao, Science 139, 506 (1963) 2) D.F. Smith, JACS 85, 816... 

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