Iodine azide

Iodine azide (IN
3) is an explosive inorganic compound, which in ordinary conditions is a yellow solid.[1] Formally, it is an inter-pseudohalogen.

Not to be confused with Nitrogen triiodide (NI₃).

Iodine azide

Names
IUPAC name 3-Iodotriaza-1,2-dien-2-ium-1-ide
Identifiers
CAS Number	14696-82-3
3D model (JSmol)	Interactive image
ChemSpider	55652
PubChem CID	61763
CompTox Dashboard (EPA)	DTXSID70163550
InChI InChI=1S/IN3/c1-3-4-2
SMILES IN=[N+]=[N-]
Properties
Chemical formula	IN3
Molar mass	168.92 g/mol
Appearance	yellow solid
Solubility in water	decomposes
Vapor pressure	2 Torr
Structure
Crystal structure	orthorhombic
Space group	Pbam, No. 55
Related compounds
Related compounds	Fluorine azide Chlorine azide Bromine azide Hydrazoic acid
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

Preparation

Iodine azide can be prepared from the reaction between silver azide and elemental iodine:

${\displaystyle \mathrm {AgN_{3}+I_{2}\longrightarrow IN_{3}+AgI} }$

Since silver azide can only be handled safely while moist, but even small traces of water cause the iodine azide to decompose, this synthesis is done by suspending the silver azide in dichloromethane and adding a drying agent before reaction with the iodine. In this way, a pure solution of iodine azide results, which can then be carefully evaporated to form needle-shaped golden crystals.[2]

This reaction was used in the original synthesis of iodine azide in 1900, where it was obtained as unstable solutions in ether and impure crystals contaminated by iodine.[3]

Iodine azide can also be generated in situ by reacting iodine monochloride and sodium azide under conditions where it is not explosive.[4]

Properties

In the solid state, iodine azide exists as a one-dimensional polymeric structure,[5] forming two polymorphs, both of which crystallize in an orthorhombic lattice with the space group Pbam.[5] The gas phase exists as monomeric units.[6]

Iodine azide exhibits both high reactivitity and comparative stability, consequences of the polarity of the I–N bond. The N₃ group introduced by substitution with iodine azide can frequently undergo subsequent reactions due to its high energy content.

The isolated compound is strongly shock- and friction-sensitive.[7] Its explosivity has been characterized as follows:[1]

Normal gas volume	265 l·kg^−1
Heat of explosion	2091 kJ·kg^−1
Trauzl rating	14.0 cm^3·g^−1

These values lie significant lower in comparison to classical explosives like TNT or RDX, and also to acetone peroxide. Dilute solutions (< 3%) of the compound in dichloromethane can be handled safely.[2]

Uses

Despite its explosive character, iodine azide has many practical uses in chemical synthesis. Similar to bromine azide, it can add across an alkene double bond via both ionic and radical mechanisms, giving anti stereoselectivity. Addition of IN
3 to an alkene followed by reduction with lithium aluminium hydride is a convenient method of aziridine synthesis. Azirines can also be synthesized from the addition product by adding base to eliminate HI, giving a vinyl azide which undergoes thermolysis to form an azirine. Further radical modes of reactivity include radical substitutions on weak C-H bonds to form α‐azido ethers, benzal acetals, and aldehydes, and the conversion of aldehydes to acyl azides.[4][6]

External links

• Raman spectrum of iodine azide

References

1. Buzek, Peter; Klapötke, Thomas M.; von Ragué Schleyer, Paul; Tornieporth‐Oetting, Inis C.; White, Peter S. (1993). "Iodine Azide". Angewandte Chemie International Edition. 32 (2): 275–277. doi:10.1002/anie.199302751.
2. Dehnicke, Kurt (1979). "The Chemistry of Iodine Azide". Angewandte Chemie International Edition. 18 (7): 507–514. doi:10.1002/anie.197905071.
3. Hantzsch, Arthur (1900). "Ueber den Jodstickstoff N₃". Berichte der Deutschen Chemischen Gesellschaft. 33 (1): 522–527. doi:10.1002/cber.19000330182.
4. Marinescu, Lavinia; Thinggaard, Jacob; Thomsen, Ib B.; Bols, Mikael (2003). "Radical Azidonation of Aldehydes". Journal of Organic Chemistry. 68 (24): 9453–9455. doi:10.1021/jo035163v.
5. Lyhs, Benjamin; Bläser, Dieter; Wölper, Christoph; Schulz, Stephan; Jansen, Georg (2012). "A Comparison of the Solid‐State Structures of Halogen Azides XN₃ (X=Cl, Br, I)". Angewandte Chemie International Edition. 51 (51): 12859–12863. doi:10.1002/anie.201206028.
6. Hassner, Alfred; Marinescu, Lavinia; Bols, Mikael. "Iodine Azide". Encyclopedia of Reagents for Organic Synthesis. doi:10.1002/047084289X.ri007.
7. Urben, P. G. (1999). Bretherick’s Handbook of Reactive Chemical Hazards. 1 (6th ed.). Butterworth-Heinemann. ISBN 0-7506-3605-X.

 

Salts and covalent derivatives of the azide ion
HN3																	He
LiN3	Be(N3)2											B(N3)3	CH3N3, C(N3)4	N(N3)3,H2N—N3	O	FN3	Ne
NaN3	Mg(N3)2											Al(N3)3	Si(N3)4	P	SO2(N3)2	ClN3	Ar
KN3	Ca(N3)2	Sc(N3)3	Ti(N3)4	VO(N3)3	Cr(N3)3, CrO2(N3)2	Mn(N3)2	Fe(N3)2, Fe(N3)3	Co(N3)2, Co(N3)3	Ni(N3)2	CuN3, Cu(N3)2	Zn(N3)2	Ga(N3)3	Ge	As	Se(N3)4	BrN3	Kr
RbN3	Sr(N3)2	Y	Zr(N3)4	Nb	Mo	Tc	Ru(N3)6^3−	Rh(N3)6^3−	Pd(N3)2	AgN3	Cd(N3)2	In	Sn	Sb	Te	IN3	Xe(N3)2
CsN3	Ba(N3)2		Hf	Ta	W	Re	Os	Ir(N3)6^3−	Pt(N3)6^2−	Au(N3)4^−	Hg2(N3)2, Hg(N3)2	TlN3	Pb(N3)2	Bi(N3)3	Po	At	Rn
Fr	Ra(N3)2		Rf	Db	Sg	Bh	Hs	Mt	Ds	Rg	Cn	Nh	Fl	Mc	Lv	Ts	Og
		↓
		La	Ce(N3)3, Ce(N3)4	Pr	Nd	Pm	Sm	Eu	Gd(N3)3	Tb	Dy	Ho	Er	Tm	Yb	Lu
		Ac	Th	Pa	UO2(N3)2	Np	Pu	Am	Cm	Bk	Cf	Es	Fm	Md	No	Lr