Transition metal azide complex

Structure of [Fe2(N3)10]4-.[1]

Transition metal azide complexes are coordination complexes containing one or more azide (N3−) ligands.[2] In addition to coordination complexes, this article summarizes homoleptic transition metal azides, which are often coordination polymers.

Structure and bonding

Azide is a pseudohalide but more nucleophilic than chloride, as reflected by the higher pKa of hydrazoic acid (4.6) vs hydrochloric acid (-5.9). As a monodentate ligand, azide binds through one of the two terminal nitrogen atoms, i.e. M-N=N=N. The N3 unit is linear or nearly so. The M-N-N angles are quite bent. Azide functions as a bridging ligand via two bonding modes. Commonly the metals share the same nitrogen ("N-diazonium" mode). Less common is the motif M-N=N=N-M, illustrated by [Cu(N3)(PPh3)2]2.[2]

General synthetic methods

Traditionally, metal azide complexes are prepared by salt metathesis, e.g. the reaction of metal chlorides with sodium azide. In some cases, trimethylsilyl azide is employed as the azide source. Another popular route include acid-base reactions hydrazoic acid HN3 and either hydrido or lewis base complexes. Still other methods rely on halide-azide exchange with trimethylsilyl azide SiMe3N3 with the metal fluorides as incomplete halide/azide exchange is often seen when using the chloride derivatives.[3]

Homoleptic complexes

Structure of [Nb(N3)7]2-.[4]-

Many homoleptic complexes (with only one kind of ligand) are known. Coordination numbers range from 2 (e.g., [Au(N3)2]−) to 7 (e.g., [W(N3)7]−). Many homoleptic complexes are octahedral anions of the type [M(N3)6]n-:

  • dianions for tetravalent metals V, Pt, Ti, Zr, Hf
  • trianions for trivalent metals Cr, Fe, Ru, Rh, Ir
  • tetraanions for the divalent Ni

For some metals, homoleptic complexes exist in two oxidation states: [Au(N3)2]− vs [Au(N3)4]− and [Pt(N3)6]2- vs [Pt(N3)4]2-.[2]

Binary azide compounds can take on several structures including discrete compounds, or one- two, and three-dimensional nets, leading some to dub them as "polyazides".[5]  Reactivity studies of azide compounds are relatively limited due to how sensitive they can be.

Group 3

Neutral unsolvated group 3 polyazide is only known for divalent europium(II) compound, Eu(N3)2.[6] Attempts to react lanthanide hydroxides with HN3 result in their basic azides, Ln(OH)(N3)2 or Ln(OH)2N3.[7]

Group 4

Group 4 polyazides of the formula M(N3)4 are predicted to have linear or near linear M-N-N angles unlike their main group counterparts which are predicted to have bent M-N-N angles.[8] This couldn’t be proved in the case of Ti(N3)4, owing to difficulty in crystallization.[9] However, incorporation of large spacer counterions or N-donor adducts makes the compounds far easier to work with. In the cases of [PPh4]2[M(N3)6] (M=Ti, Zr, Hf), only the axial ligands exhibit near linear M-N-N angles whereas the equatorial ligands are closer to bent angles.[9][10] This deviation in theory is also seen in the N-donor adducts.[11]

Highest Occupied Molecular Orbital (HOMO) of Ti(N3)4

The main hypothesis given for why these compounds do not have linear M-N-N angles despite theoretical calculations is that these adducts are not tetrahedral.[9] In the homoleptic tetrahedral compounds, the nitrogen closest to the (+IV) metal center is positioned in such a way that the three valence electron pairs can donate to the vacant d orbitals on the metal and therefore the azido can act as a tridentate donor ligand in which case the expected coordination would be linear. Since the adduct compounds are not tetrahedral, the azido group can only act as a monodentate donor with two sterically active electron pairs which result in a bent M-N-N bond angles.

Group 5

The neutral binary V(IV) azide as well as V(III), V(IV), and V(V) azido ions are known.[12][13] Similar to the neutral Ti(IV) azide, V(N3)4 is difficult to study due to high shock and temperature instability.[12] However, [V(N3)6]2- paired with a large, inert counterion is relatively stable and crystalizeses as a near perfect octahedral. In contrast to V(IV), the neutral binary V(V) could not be synthesized and attempts result in the reduction of V(V) to V(IV) with the elimination of N2 gas. Fortunately, the oxidation potentials of anions are lower than that of their parent compounds so [V(N3)6]- can be formed. Unlike [V(N3)6]2-, [V(N3)6]- is highly shock sensitive and distorted from octahedral symmetry with three long and three short M-N bonds in mer positions.

The neutral binary Nb(N3)5 and Ta(N3)5 also exist, and the acetonitrile adducts of these compounds contain a nearly linear azido trans to the coordinating acetonitrile.[14] They represent the first evidence of linear M-N-N bonding. The corresponding anions [Nb(N3)6]-, [Nb(N3)7]2-, [Ta(N3)6]-, and [Ta(N3)7]2- are known and accordingly are much less shock sensitive.[14][15] The structure of the hexaazido monoanions are similar to other heptaazido monoanions with bent azido ligands despite being predicted to have perfect S6 symmetry in the gas phase for [Nb(N3)6].[14] The heptaazido dianions possess monocapped triangular-prismatic 1/4/2 structures unlike the actinide trianion [U(N3)7]3- which crystallizes as a monocapped octahedron or pentagonal bipyramid.[15] Several N-donor adducts are known to exist as well.[16] Reactions of the neutral binary NbF5 and TaF5 in the presence of Me3SiN3 with N-donors containing small bite angles such as 2,2’-bipyridine or 1,10-phenanthroline result in self ionization products of the type [M(N3)4L2]+[M(N3)6]- (L= N-donor) whereas N-donors containing large bite angles such as 3,3’-bipryidine or 4,4’-bipyridine produces the neutral pentaazide adducts M(N3)5•L (L=N-donor).

Group 6

Both Mo(N3)6 and W(N3)6 have been synthesized, and W(N3)6 is stable enough to grow single crystals.[17] Contrary to group 4 and group 5 binary azido compounds, the anionic [Mo(N3)7]- and [W(N3)7]- are less stable and more sensitive to handle than their neutral parent compounds.  Upon warming solutions of the heptaazido anions in either MeCN or SO2 to room temperature, the tetraazido nitrido ions [NMo(N3)4]- and [NW(N3)4]- are formed with elimination of N2.

Group 7

End-on (EO) [left] and end-to-end (EE) [right] binding modes of the azido ligand

The first Mn polyazide compound was prepared by Wöhler et al. in 1917 by reaction of MnCO3 with HN3 to form Mn(N3)2.[18] Many divalent Mn azide salts have been synthesized.[5][19] 1D chains are formed when 2,2’-bipyridine, a bidentate ligand, is used as the counter ion in the reaction between Mn(ClO4)2 • 6H2O and excess NaN3.[20] This results in a chain with alternating EE and EO bridges which predictably gives alternating antiferromagnetic-ferromagnetic coupling.[21][22] Another 2D structure is accessed via the reaction of (PPh4)2MnCl2 with AgN3 to form the [PPh4]2[Mn(N3)4].[23]  

The first example of a 3D azido compound was [N(CH3)4][Mn(N3)3].[24] This compound has a pseudo-perovskite structure with [N(CH3)4]+ ions in the cavities between the Mn centers. The azido moieties are arranged in an EE fashion, and indeed, this compound exhibits the expected antiferromagnetic behavior.[21] The cesium analogue Cs[Mn(N3)3] is synthesized in a similar manner.[19] For each 6 coordinate Mn, four of the azido linkages are EE and two are EO instead of all six being EE. This arrangement results in a honeycomb-like shape and a rare example of alternating ferro-antiferromagnetic interactions in 3D solid.

Examples of manganese azido compounds in higher oxidation states are rare. The triazide acetonitrile adduct can be prepared using the fluoride exchange route to give Mn(N3)3CN as a dark red shock sensitive compound.[25] Upon addition of PPh4N3 the compound disproportionates into an insensitive mixture of [PPh4]2[Mn(N3)2] and [PPh4]2[Mn(N3)6]. The Mn(IV) salt can be prepared on its own by using Cs2MnF6 as the starting material to give the highly explosive Cs2[Mn(N3)6].

Group 8

Anti-Markovnikov addition of an azide to an alkene using Fe(N3)3

Pentaazidoiron (III) ion [Fe(N3)5]2- can be made by treating iron(III) salts with sodium azide.[26][27] An iron azide reagent can be generated in situ.[28] NaN3 and iron (III) sulfate Fe2(SO4)3 are combined in methanol and added to an organoborane followed by slow addition of 30% hydrogen peroxide, presumably forming Fe(N3)3. When combined with alkenes, the equivalent of hydrogen azide add in an anti-Markovnikov fashion.[29]

[n-Bu4N]3[Ru(N3)6] is prepared by treating K2[RuIVCl6] with NaN3.[30] N2 gas is liberated in this reaction, which involves reduction of Ru(IV) to Ru(III).

Group 9

Tetraazido cobalt(II) compounds have been isolated as both the tetraphenylphosphonium and tetraphenylarsonium salts from solutions of cobalt sulfate with a 15 time sexcess of NaN3 to yield [Ph4P]2[Co(N3)4] and [Ph4As]2[Co(N3)4] respectively.[31] The autooxidation of solutions of  [Co(N3)4]2- can be used as a colorimetric spot test for the presence of sulfite ions.[32]

Tetrabutylammonium salts of rhodium(III) and iridium(III) azides are known and are prepared by reacting a large excess of NaN3 in an aqueous solution with the corresponding Na3[MCl6] • 12H2O metal chloride salt to form [n-Bu4N]3[Rh(N3)6] and [n-Bu4N]3[Ir(N3)6].[30]

Group 10

The binary nickel azide Ni(N3)2 has been prepared by distilling HN3 onto nickel carbonate.[33] Samples of Ni(N3)2 decompose upon heating .

[Pd(N3)4]2- anions are square planar and the degree of interaction between the anion and its corresponding cation can be determined by the amount of deviation in the torsion angles from the ideal geometry.[34] Various platinates [Pt(N3)4]2- and [Pt(N3)6]4- are known and are prepared from Pt chloride salts with NaN3.[30] Pt(II) salts tend to be far less stable than the Pt(IV) versions, and they either decompose fairly rapidly upon standing or explode.[35] Their sensitivity in part has been explained by poor crystal packing.[34]

Group 11

Both copper(I) and copper(II) azides are known. The binary copper(I) azide, CuN3, which is white, is a one-dimensional polymer.[36] Molecular Copper (II) azides include salts of [Cu(N3)4]2- and [Cu(N3)6]2-.[26][37] {[Cu(N3)3]-}n forms 1D chains wherein octahedral Cu(II) centers are linked by both EE and EO bridging azides.[21] All copper azides are explosive but their sensitivities vary widely from the parent azides CuN3 and Cu(N3)2 which are extremely sensitive to the ions paired with large countercations that are practically insensitive.[38]

Silver (I) azide is a well known explosive compound and has been demonstrated to form a 2D coordination polymer with square planar Ag+ ions surrounded by azido ligands in an EE fashion.[39] Slow ramping of temperature from 150°C to 251°C results in melting and slow decomposition but rapid heating to 300°C results in an explosion.[38]

Gold(III) azide is known as the tetraethylammonium salt [Et4N][Au(N3)4] and also adopts a square planar structure.[30] However unlike the silver azide, the gold azide is not stable at room temperature and will decompose after a few days and its metal azide bonds have significant covalent character.

Group 12

While Zn(N3)2 has been known since the late 1890s, solvent free Zn(N3)2 was isolated for the first time in 2016 from a dry ethereal solution of HN3 and Et2Zn in n-hexane. Zn(N3)2 crystallizes in three different polymorphs α-Zn(N3)2 and the labile β-Zn(N3)2 and γ-Zn(N3)2 forms.[40]

The first mercury (I) azide was realized by Curtius in 1890 by combining aqueous mercury(I) salts with alkali metal azides and by combining HN3 with elemental mercury to produce Hg2(N3)2.[41][42] Both mercury (I) and mercury(II) azides can be easily prepared by mixing the respective mercury nitrates with sodium azide in aqueous solution at roomtemperature.[42] The mercury (II) azide Hg(N3)2 exists in two polymorphs α-Hg(N3)2 and β-Hg(N3)2. The β form is very labile and quickly turns into the α polymorphs at room temperature. However, the β polymorph can prepared in analogy to β-Pb(N3)2 by slow diffusion of aqueous NaN3 into a solution of Hg(NO3)2 separated by a layer of aqueous NaNO3, but crystals nearly always explode during formation leading to a mixture of α and β polymorphs.

Binary cadmium azide Cd(N3)2 can be prepared from CdCO3 and aqueous HN3.[43] However, it is structural unrelated to the mercury or zinc anaolgues and is based on repeat units of Cd2(N3)10 double octahedrals.

Mixed ligand complexes

Structure of trans-PdN3(CH3)(PMe3)2. Distances are in picometers.[44]

Azide forms myriad mixed ligand complexes. Examples include Zn(N3)2(NH3)2 and (C5H5)2Ti(N3)2.[11]

Reactions

A characteristic reaction of azide complexes and compounds) is degradation via loss of nitrogen gas. The stoichiometry for a diazide compound is:

M(N3)2 → 2 M + 3 N2

The process often occurs explosively.

Azide ligands are react with nitrosonium to give nitrous oxide. This reaction is used to generate coordinatively unsaturated complexes.[45]

[Co(NH3)5N3]2+ + NO+ + H2O → [Co(NH3)5(H2O)]3+ + N2O + N2

This approach was used to prepare the previously elusive dicationic complex pentamminecobalt(III) perchlorate, [Co(NH3)5(OClO3)]2+.[46]

See also

References

  1. ^ De Munno, Giovanni; Poerio, Teresa; Viau, Guillaume; Julve, Miguel; Lloret, Francesc (1997). "Ferromagnetic Coupling in the Bis(μ-end-on-azido)iron(III) Dinuclear Complex Anion of[FeII(bpym)3]2[Fe2III(N3)10]·2H2O". Angewandte Chemie International Edition in English. 36 (1314): 1459–1461. doi:10.1002/anie.199714591.
  2. ^ a b c Fehlhammer, Wolf Peter; Beck, Wolfgang (2013). "Azide Chemistry - an Inorganic Perspective, Part I Metal Azides: Overview, General Trends and Recent Developments". Zeitschrift für Anorganische und Allgemeine Chemie. 639 (7): 1053–1082. doi:10.1002/zaac.201300162.
  3. ^ Portius, Peter; Davis, Martin (2013-03-01). "Recent developments in the chemistry of homoleptic azido complexes of the main group elements". Coordination Chemistry Reviews. Recent Developments in Main Group Chemistry. 257 (5): 1011–1025. doi:10.1016/j.ccr.2012.09.019. ISSN 0010-8545.
  4. ^ Haiges, Ralf; Boatz, Jerry A.; Yousufuddin, Muhammed; Christe, Karl O. (2007). "Monocapped Trigonal-Prismatic Transition-Metal Heptaazides: Syntheses, Properties, and Structures of [Nb(N3)7]2− and [Ta(N3)7]2−". Angewandte Chemie International Edition. 46 (16): 2869–2874. doi:10.1002/anie.200604520. PMID 17348060.
  5. ^ a b Ribas, Joan; Escuer, Albert; Monfort, Montserrat; Vicente, Ramon; Cortés, Roberto; Lezama, Luis; Rojo, Teófilo (1999-10-01). "Polynuclear NiII and MnII azido bridging complexes. Structural trends and magnetic behavior". Coordination Chemistry Reviews. 193–195: 1027–1068. doi:10.1016/S0010-8545(99)00051-X. ISSN 0010-8545.
  6. ^ Thomas G. Müller; Friedrich Karau; Wolfgang Schnick; Florian Kraus. A New Route to Metal Azides. Angewandte Chemie International Edition. 2014. doi:10.1002/anie.201404561
  7. ^ Kati Rosenstengel, Axel Schulz, Oliver Niehaus, Oliver Janka, Rainer Pöttgen, Alexander Villinger. Binary Polyazides of Cerium and Gadolinium. European Journal of Inorganic Chemistry. 2017. doi:10.1002/ejic.201701408.
  8. ^ Li, Qian Shu; Duan, Hong Xia (2005-10-01). "Density Functional Theoretical Study of a Series of Binary Azides M(N 3 ) n ( n = 3, 4)". The Journal of Physical Chemistry A. 109 (40): 9089–9094. Bibcode:2005JPCA..109.9089L. doi:10.1021/jp052726t. ISSN 1089-5639. PMID 16332016.
  9. ^ a b c Haiges, Ralf; Boatz, Jerry A.; Schneider, Stefan; Schroer, Thorsten; Yousufuddin, Muhammed; Christe, Karl O. (2004-06-14). "The Binary Group 4 Azides[Ti(N3)4],[P(C6H5)4][Ti(N3)5], and[P(C6H5)4]2[Ti(N3)6] and on Linear TiNNN Coordination". Angewandte Chemie International Edition. 43 (24): 3148–3152. doi:10.1002/anie.200454156. ISSN 1433-7851. PMID 15199563.
  10. ^ Deokar, Piyush; Vasiliu, Monica; Dixon, David A.; Christe, Karl O.; Haiges, Ralf (2016-11-07). "The Binary Group 4 Azides [PPh 4 ] 2 [Zr(N 3 ) 6 ] and [PPh 4 ] 2 [Hf(N 3 ) 6 ]". Angewandte Chemie International Edition. 55 (46): 14350–14354. doi:10.1002/anie.201609195. PMID 27735115.
  11. ^ a b Saal, Thomas; Deokar, Piyush; Christe, Karl O.; Haiges, Ralf (2019-05-15). "The Binary Group 4 Azide Adducts [(bpy)Ti(N3)4], [(phen)Ti(N3)4], [(bpy)2Zr(N3)4]2·bpy, and [(bpy)2Hf(N3)4]2·bpy". European Journal of Inorganic Chemistry. 2019 (18): 2388–2391. doi:10.1002/ejic.201900334. ISSN 1434-1948. S2CID 132294068.
  12. ^ a b Haiges, Ralf; Boatz, Jerry A.; Christe, Karl O. (2010-10-18). "The Syntheses and Structure of the Vanadium(IV) and Vanadium(V) Binary Azides V(N3)4, [V(N3)6]2−, and [V(N3)6]−". Angewandte Chemie International Edition. 49 (43): 8008–8012. doi:10.1002/anie.200906537. PMID 20715219.
  13. ^ Gutmann, V.; Leitmann, O.; Scherhaufer, A.; Czuba, H. (1967-01-01). "Azidokomplexe in nichtwäßrigen Lösungsmitteln, 3. Mitt.: Ti(III), V(III) und Cr(III) in Acetonitril, Propandiol-1,2-carbonat und Trimethylphosphat". Monatshefte für Chemie und verwandte Teile anderer Wissenschaften (in German). 98 (1): 188–199. doi:10.1007/BF00901117. ISSN 1434-4475.
  14. ^ a b c Haiges, Ralf; Boatz, Jerry A.; Schroer, Thorsten; Yousufuddin, Muhammed; Christe, Karl O. (2006-07-17). "Experimental Evidence for Linear Metal–Azido Coordination: The Binary Group 5 Azides [Nb(N3)5], [Ta(N3)5], [Nb(N3)6]−, and [Ta(N3)6]−, and 1:1 Acetonitrile Adducts [Nb(N3)5(CH3CN)] and [Ta(N3)5(CH3CN)]". Angewandte Chemie International Edition. 45 (29): 4830–4835. doi:10.1002/anie.200601060. ISSN 1433-7851. PMID 16795097.
  15. ^ a b Haiges, Ralf; Boatz, Jerry A.; Yousufuddin, Muhammed; Christe, Karl O. (2007-04-13). "Monocapped Trigonal-Prismatic Transition-Metal Heptaazides: Syntheses, Properties, and Structures of [Nb(N3)7]2− and [Ta(N3)7]2−". Angewandte Chemie International Edition. 46 (16): 2869–2874. doi:10.1002/anie.200604520. PMID 17348060.
  16. ^ Haiges, Ralf; Deokar, Piyush; Christe, Karl O. (2014-05-19). "Coordination Adducts of Niobium(V) and Tantalum(V) Azide M(N 3 ) 5 (M=Nb, Ta) with Nitrogen Donor Ligands and their Self-Ionization". Angewandte Chemie International Edition. 53 (21): 5431–5434. doi:10.1002/anie.201402775. PMID 24756882.
  17. ^ Haiges, Ralf; Boatz, Jerry A.; Bau, Robert; Schneider, Stefan; Schroer, Thorsten; Yousufuddin, Muhammed; Christe, Karl O. (2005-03-11). "Polyazide Chemistry: The First Binary Group 6 Azides, Mo(N3)6, W(N3)6, [Mo(N3)7]?, and [W(N3)7]?, and the [NW(N3)4]? and [NMo(N3)4]? Ions". Angewandte Chemie International Edition. 44 (12): 1860–1865. doi:10.1002/anie.200462740. ISSN 1433-7851. PMID 15723363.
  18. ^ Dehnicke, K.; Dubgen, R. (1978). "Die Reaktionen des Jodazids mit Metallcarbonylen". Zeitschrift für anorganische und allgemeine Chemie (in German). 444 (1): 61–70. doi:10.1002/zaac.19784440106. ISSN 0044-2313.
  19. ^ a b Goher, Mohamed A. S.; Cano, Joan; Journaux, Yves; Abu-Youssef, Morsy A. M.; Mautner, Franz A.; Escuer, Albert; Vicente, Ramon (2000-03-03). "Synthesis, Structural Characterisation, and Monte Carlo Simulation of the Magnetic Properties of the 3D-Stacked Honeycomb Csn[{Mn(N3)3}n] and the Irregular Double Chain [{N(C2H5)4}n][{Mn2(N3)5(H2O)}n]". Chemistry - A European Journal. 6 (5): 778–784. doi:10.1002/(SICI)1521-3765(20000303)6:5<778::AID-CHEM778>3.0.CO;2-P. ISSN 0947-6539. PMID 10826599.
  20. ^ Cortés, Roberto; Lezama, Luis; Rojo, Teófilo; Arriortua, M. Isabel; Pizarro, J. Luis; Solans, Xavier (1995-01-03). "Alternating Ferro- and Antiferromagnetic Interactions in a MnII Chain with Alternating End-On and End-to-End Bridging Azido Ligands". Angewandte Chemie International Edition in English. 33 (2324): 2488–2489. doi:10.1002/anie.199424881. ISSN 0570-0833.
  21. ^ a b c Mautner, Franz A.; Hanna, Samy; Cortés, Roberto; Lezama, Luis; Barandika, M. Gotzone; Rojo, Teófilo (1999-10-01). "Crystal Structure and Spectroscopic and Magnetic Properties of the Manganese(II) and Copper(II) Azido−Tetramethylammonium Systems". Inorganic Chemistry. 38 (21): 4647–4652. doi:10.1021/ic981373s. ISSN 0020-1669. PMID 11671186.
  22. ^ Ma, Yu; Cheng, Ai-Ling; Sun, Wei-Wei; Zhang, Jiang-Yong; Gao, En-Qing (2009-05-01). "Homoleptic manganese(II)–azide layer: Synthesis, structural characterization and magnetic properties". Inorganic Chemistry Communications. 12 (5): 412–416. doi:10.1016/j.inoche.2009.03.005. ISSN 1387-7003.
  23. ^ Steiner, Klaus; Willing, Wolfgang; Müller, Ulrich; Dehnicke, Kurt (1987). "Azidokomplexe von Mangan(II) und Cobalt(II) Die Kristallstrukturen von (PPh4)2[Mn(N3)4] und (PPh4)2[Co(N3)3Cl]". Zeitschrift für anorganische und allgemeine Chemie (in German). 555 (12): 7–15. doi:10.1002/zaac.19875551202. ISSN 0044-2313.
  24. ^ Mautner, Franz A.; Cortés, Roberto; Lezama, Luis; Rojo, Teófilo (1996-01-19). "[N(CH3)4][Mn(N3)3]: A Compound with a Distorted Perovskite Structure through Azido Ligands". Angewandte Chemie International Edition in English. 35 (1): 78–80. doi:10.1002/anie.199600781. ISSN 0570-0833.
  25. ^ Haiges, Ralf; Buszek, Robert J.; Boatz, Jerry A.; Christe, Karl O. (2014-07-28). "Preparation of the First Manganese(III) and Manganese(IV) Azides". Angewandte Chemie International Edition. 53 (31): 8200–8205. doi:10.1002/anie.201404735. PMID 25044947.
  26. ^ a b Beck, Wolfgang; Fehlhammer, Wolf Peter; Pöllmann, Peter; Schuierer, Erich; Feldl, Klaus (1967). "Darstellung, IR- und Elektronenspektren von Azido-Metall-Komplexen". Chemische Berichte. 100 (7): 2335–2361. doi:10.1002/cber.19671000731. ISSN 0009-2940.
  27. ^ Drummond, J.; Wood, J. S. (1969). "The Structure of a Five-Co-ordinate Complex of Iron; the Penta-Azidoiron(III) Ion, Fe(N3)52-". Journal of the Chemical Society D: Chemical Communications (23): 1373. doi:10.1039/c29690001373. ISSN 0577-6171.
  28. ^ Suzuki, Akira; IShidoya, Masahiro; Tabata, Masayoshi (1976). "Reaction of Organoboranes with Iron(III) Azide in the Presence of Hydrogen Peroxide. A Novel Synthesis of Azidoalkanes from Alkenes via Hydroboration". Synthesis. 1976 (10): 687–689. doi:10.1055/s-1976-24160. ISSN 0039-7881.
  29. ^ White, Andrew D. (2001-04-15), "Iron(III) Azide", Encyclopedia of Reagents for Organic Synthesis, Chichester, UK: John Wiley & Sons, Ltd, doi:10.1002/047084289x.ri053, ISBN 0471936235, retrieved 2022-12-13
  30. ^ a b c d Schmidtke, Hans-Herbert.; Garthoff, Dieter. (1967). "The Electronic Spectra of Some Noble Metal Azide Complexes". Journal of the American Chemical Society. 89 (6): 1317–1321. doi:10.1021/ja00982a007. ISSN 0002-7863.
  31. ^ Senise, Paschoal (1959). "On the Reaction between Cobalt(II) and Azide Ions in Aqueous and Aqueous-organic Solutions1". Journal of the American Chemical Society. 81 (16): 4196–4199. doi:10.1021/ja01525a020. ISSN 0002-7863.
  32. ^ Senise, Paschoal (1957-09-01). "Spot test for sulfites based on the induced oxidation of cobalt-azide solutions". Microchimica Acta. 45 (5): 640–643. doi:10.1007/BF01236544. ISSN 1436-5073. S2CID 98339990.
  33. ^ Sood, R. K.; Nya, A. E.; Etim, E. S. (1981). "Thermal decomposition of nickel azide". Journal of Thermal Analysis. 22 (2): 231–237. doi:10.1007/bf01915269. ISSN 0022-5215. S2CID 95478362.
  34. ^ a b Beck, Wolfgang; Fehlhammer, Wolf Peter; Feldl, Klaus; Klpötke, Thomas M.; Kramer, Gernot; Mayer, Peter; Piotrowski, Holger; Pöllman, Peter; Ponikwar, Walter; Schütt, Thomas; Schuierer, Erich; Vogt, Martin (2001). <1751::AID-ZAAC1751>3.0.CO;2-5 "Crystal Structures of (PPh3)2Pd(N3)2, (AsPh3)2Pd(N3)2, (2-Chloropyridine)2Pd(N3)2, [(AsPh4)2][Pd2(N3)4Cl2], [(PNP)2][Pd(N3)4], [(AsPh4)2][Pt(N3)4] 2H2O, and [(AsPh4)2][Pt(N3)6]". Zeitschrift für anorganische und allgemeine Chemie. 627 (8): 1751–1758. doi:10.1002/1521-3749(200108)627:8<1751::AID-ZAAC1751>3.0.CO;2-5. ISSN 0044-2313.
  35. ^ Neumüller, Bernhard; Schmock, Fritjof; Schlecht, Sabine; Dehnicke, Kurt (2000). <1792::AID-ZAAC1792>3.0.CO;2-U "Die Kristallstrukturen der Azido-Platinate (AsPh4)2[Pt(N3)4] und (AsPh4)2[Pt(N3)6]". Zeitschrift für anorganische und allgemeine Chemie. 626 (8): 1792–1796. doi:10.1002/1521-3749(200008)626:8<1792::AID-ZAAC1792>3.0.CO;2-U.
  36. ^ Wilsdorf, H. (1948-07-02). "Die Kristallstruktur des einwertigen Kupferazids, CuN3". Acta Crystallographica (in German). 1 (3): 115–118. Bibcode:1948AcCry...1..115W. doi:10.1107/S0365110X48000314. ISSN 0365-110X.
  37. ^ Goher, Mohamed A. S.; Abdou, Azza E. H.; Abu-Youssef, Morsy A. M.; Mautner, Franz A. (2001-02-01). "Bis-(tetraethylammonium)[tetraazidocuprate(II)] and catena-di-μ-1,1-azido-[di-μ-1,1-azido-bis-(2,4-dimethylpyridine)dicopper(II)]". Transition Metal Chemistry. 26 (1): 39–43. doi:10.1023/A:1007195015645. ISSN 1572-901X. S2CID 92350747.
  38. ^ a b Harry David Fair; Raymond F. Walker, eds. (1977). Physics and chemistry of the inorganic azides. New York: Plenum Press. ISBN 0-306-37076-X. OCLC 2985662.
  39. ^ Schmidt, Carsten L.; Dinnebier, Robert; Wedig, Ulrich; Jansen, Martin (2007-02-01). "Crystal Structure and Chemical Bonding of the High-Temperature Phase of AgN 3". Inorganic Chemistry. 46 (3): 907–916. doi:10.1021/ic061963n. ISSN 0020-1669. PMID 17257034.
  40. ^ Schulz, Axel; Villinger, Alexander (2016-01-08). "Binary Zinc Azides". Chemistry - A European Journal. 22 (6): 2032–2038. doi:10.1002/chem.201504524. ISSN 0947-6539. PMID 26749253.
  41. ^ Nockemann, Peter; Meyer, Gerd (2002). <2709::aid-zaac2709>3.0.co;2-p "Bildung von NH4[Hg3(NH)2](NO3)3 und Umwandlung in [Hg2N](NO3)". Zeitschrift für anorganische und allgemeine Chemie. 628 (12): 2709–2714. doi:10.1002/1521-3749(200212)628:12<2709::aid-zaac2709>3.0.co;2-p. ISSN 0044-2313.
  42. ^ a b Lund, Henrik; Oeckler, Oliver; Schröder, Thorsten; Schulz, Axel; Villinger, Alexander (2013-08-26). "Mercury Azides and the Azide of Millon's Base". Angewandte Chemie International Edition. 52 (41): 10900–10904. doi:10.1002/anie.201305545. ISSN 1433-7851. PMID 24038779.
  43. ^ Karau, Friedrich; Schnick, Wolfgang (2005). "Darstellung und Kristallstruktur von Cadmiumazid Cd(N3)2". Zeitschrift für anorganische und allgemeine Chemie. 631 (12): 2315–2320. doi:10.1002/zaac.200500226. ISSN 0044-2313.
  44. ^ Kim, Yong-Joo; Kim, Dae-Hun; Lee, Jae-Young; Lee, Soon-W. (1997). "Preparation and Reactions of Methylpalladium(II) and -Platinum(II) Azido Complexes. The Crystal Structure of trans-PdMe(N3)(PMe3)2 and trans-PdMe[CN4(C6H11)](PMe3)2". Journal of Organometallic Chemistry. 538 (1–2): 189–197. doi:10.1016/S0022-328X(96)06908-2.
  45. ^ Buckingham, David A.; Olsen, I. I.; Sargeson, Alan M.; Satrapa, H. (1967). "The Mechanism of Substitution Reactions of Pentamminecobalt(III) Complexes. Product Distributions in the Induced Aquation of Some [Co(NH3)5X]2+ Ions in the Presence of Added Anions". Inorganic Chemistry. 6 (5): 1027–1032. doi:10.1021/ic50051a038.
  46. ^ Harrowfield, J. Macb.; Sargeson, A. M.; Singh, B.; Sullivan, J. C. (1975). "Trapping of Labile Cobalt(III) Complexes. Characterization of the Perchloratopentaamminecobalt(III) Ion". Inorganic Chemistry. 14 (11): 2864–2865. doi:10.1021/ic50153a059.