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Inorganic imide

The inorganic imide is an inorganic chemical compound containing

  • an anion with the chemical formula HN2−, in which nitrogen atom is covalently bonded to one hydrogen atom (as in lithium imide Li2NH and calcium imide CaNH). The other name of that anion is monohydrogen nitride.
  • functional groups with the chemical formulas −NH− or =NH, in which nitrogen atom is also covalently bonded to one hydrogen atom, with two covalent single bonds or one covalent double bond from the nitrogen atom to other atoms, respectively (as in heptasulfur imide S7NH, sulfur diimide S(=NH)2 and nitroxyl O=NH).

Organic imides have the functional groups −NH− or =NH as well.

The imides are related to the inorganic amides, containing the H2N− anions, the nitrides, containing the N3− anions and the nitridohydrides or nitride hydrides, containing both nitride N3− and hydride H− anions.

In addition to solid state imides, molecular imides are also known in dilute gases, where their spectrum can be studied.

When covalently bound to a metal, an imide ligand produces a transition metal imido complex.

When the hydrogen of the imide group is substituted by an organic group, an organoimide results. Complexes of actinide and rare earth elements with organoimides are known.[1]

Properties

Lithium imide undergoes a phase transition at 87 °C where it goes from an ordered to a more symmetric disordered state.[2]

Structure

Many imides have a cubic rock salt structure, with the metal and nitrogen occupying the main positions. The position of the hydrogen atom is hard to determine, but is disordered.

Many of the heavy metal simple imide molecules are linear. This is due to the filled 2p orbital of nitrogen donating electrons to an empty d orbital on the metal.[3]

Imides in coordination chemistry

In coordination chemistry transition metal imido complexes feature the NR2- ligand. They are similar to oxo ligands in some respects. In some the M-N-C angle is 180º but often the angle is decidedly bent. The parent imide (NH2-) is an intermediate in nitrogen fixation by synthetic catalysts.[4]

Structure of a representative imido complex (py = pyridine, CMe3 = tert-butyl)[5]

Formation

Heating lithium amide with lithium hydride yields lithium imide and hydrogen gas. This reaction takes place as released ammonia reacts with lithium hydride.[2]

Heating magnesium amide to about 400 °C yields magnesium imide with the loss of ammonia. Magnesium imide itself decomposes if heated between 455 and 490 °C.[6]

Beryllium imide forms from beryllium amide when heated to 230 °C in a vacuum.[7]

When strontium metal is heated with ammonia at 750 °C, the dark yellow strontium imide forms.[8]

When barium vapour is heated with ammonia in an electrical discharge, the gaseous, molecular BaNH is formed.[9] Molecules ScNH, YNH, and LaNH are also known.[10][11]

Hydrogen storage

Inorganic imides are of interest because they can reversibly store hydrogen, which may be important for the hydrogen economy. For example, calcium imide can store 2.1% mass of hydrogen. Li2Ca(NH)2 reversibly stores hydrogen and release it at temperatures between 140 and 206 °C. It can reversibly hold 2.3% hydrogen.[12] When hydrogen is added to the imide, amides and hydrides are produced. When imides are heated, they can yield hydridonitrides or nitrides, but these may not easily reabsorb hydrogen.

List

Ionic

name formula structure space group unit cell references
Lithium imide Li2NH cubic Fm3m a=5.0742 [2]
Beryllium imide BeNH [7]
Magnesium imide MgNH hexagonal P6/m a = 11.567 Å c = 3.683Å Z=12 [6]
Dilithium magnesium imide Li2Mg(NH)2 [12]
Disilicon dinitride imide Si2N2(NH) [13]
K2Si(NH)3 amourphous [14]
K2Si2(NH)5 amourphous [14]
K2Si3(NH)7 amourphous [14]
potassium imido nitrido silicate K3Si6N5(NH)6 cubic P4332 a = 10.789 [13]
Calcium imide CaNH hexagonal Fm3m [12]
Dilithium calcium imide Li2Ca(NH)2 hexagonal [12]
Magnesium calcium diimide MgCa(NH)2 cubic [15]
Lithium calcium magnesium imide Li4CaMg(NH)4 [12]
Strontium imide SrNH orthorhombic Pmna a =7.5770 b =3.92260 c =5.69652 Z=4 [8]
Tin(IV) diamide imide Sn(NH2)2NH [16][17]
Barium imide BaNH tetragonal I4/mmm a=4.062 c=6.072 Z=2 [18]
Lanthanum imide La2(NH)3 rock salt a=5.32 [19]
Cerium(II) imide CeNH [20]
Ytterbium(II) imide YbNH cubic a=4.85 [21]
[NH4][Hg3(NH)2](NO3)3 cubic P4132 a = 10.304, Z = 4 [22]
Thorium(IV) dinitride imide Th2N2(NH) hexagonal P3m1 a = 3.886 c = 6.185 Å [23]

Molecular

name formula structure symmetry CAS references
Boron imide B2(NH)3 polymer [24]
HNO bent 14332-28-6
Aluminium amide imide Al(NH2)(NH) polymer [24]
Silicon dimide Si(NH)2
  • Thionitrosyl hydride
  • Azanethial
  • Azanethione
 HNS bent 14616-59-2 [25]
Sulfur diimide S(NH)2
Heptasulfur imide S7NH 293-42-5 [26]
  • 1,2,3,4,5,7,6,8-Hexathiadiazocane
  • 1,3-Hexasulfurdiimide
  • 1,3-Diazacyclooctasulfane
 H2N2S6 1003-75-4
  • 1,2,3,4,6,7,5,8-Hexathiadiazocane
  • 1,4-Hexasulfurdiimide
  • 1,4-Diazacyclooctasulfane
 H2N2S6 1003-76-5
  • 1,2,3,5,6,7,4,8-Hexathiadiazocane
  • 1,5-Hexasulfurdiimide
  • 1,5-Diazacyclooctasulfane
 H2N2S6
  • 1,2,3,5,7,4,6,8-Pentathiatriazocane
  • 1,3,5-Pentasulfurtriimide
  • 1,3,5-Triazacyclooctasulfane
 H3N3S5 638-50-6
Scandium(II) imide ScNH [10]
Gallium(III) imide Ga2(NH)3 polymer [24]
Yttrium(II) imide YNH [10]
Barium imide BaNH linear [3]
Lanthanum(II) imide LaNH linear C∞v [11][27]
Cerium(II) imide CeNH linear C∞v [27]
Uranimine nitride N≡U=N−H [28]
Uranimine dihydride HN=UH2 [28]

Molecular imines of other actinides called neptunimine and plutonimine have been postulated to exist in the gas phase or noble gas matrix.[29]

References

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  2. ^ a b c Lowton, Rebecca L. (1999). Structural and thermogravimetric studies of alkali metal amides and imides (PhD thesis). Oxford University, UK.
  3. ^ a b Janczyk, Alexandra; Lichtenberger, Dennis L.; Ziurys, Lucy M. (February 2006). "Competition between Metal-Amido and Metal-Imido Chemistries in the Alkaline Earth Series: An Experimental and Theoretical Study of BaNH". Journal of the American Chemical Society. 128 (4): 1109–1118. doi:10.1021/ja053473k. ISSN 0002-7863. PMID 16433526.
  4. ^ Nugent, W. A.; Mayer, J. M., "Metal-Ligand Multiple Bonds," J. Wiley: New York, 1988.
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  7. ^ a b Jacobs, Herbert; Juza, Robert (November 1969). "Darstellung und Eigenschaften von Berylliumamid und -imid". Zeitschrift für anorganische und allgemeine Chemie (in German). 370 (5–6): 248–253. doi:10.1002/zaac.19693700507. ISSN 0044-2313.
  8. ^ a b Schultz‐Coulon, Verena; Irran, Elisabeth; Putz, Bernd; Schnick, Wolfgang (1999). "β-SrNH und β-SrND – Synthese und Kristallstrukturbestimmung mittels Röntgen- und Neutronenbeugung an Pulvern". Zeitschrift für anorganische und allgemeine Chemie. 625 (7): 1086–1092. doi:10.1002/(SICI)1521-3749(199907)625:7<1086::AID-ZAAC1086>3.0.CO;2-B.
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  18. ^ Wegner, B.; Essmann, R.; Jacobs, H.; Fischer, P. (December 1990). "Synthesis of barium imide from the elements and orientational disorder of anions in BaND studied by neutron diffraction from 8 to 294 K". Journal of the Less Common Metals. 167 (1): 81–90. doi:10.1016/0022-5088(90)90291-Q.
  19. ^ Jacobs, H; Gieger, B; Hadenfeldt, C (March 1979). "Über das system kalium/lanthan/ammoniak". Journal of the Less Common Metals (in German). 64 (1): 91–99. doi:10.1016/0022-5088(79)90136-X.
  20. ^ Imamura, Hayao; Kawasoe, Masahiro; Imayoshi, Kyouya; Sakata, Yoshihisa (2015). "Preparation and Some Properties of Nanostructural Rare Earth Nitrides by Using the Reaction of Hydrides with Ammonia". International Journal of Theoretical and Applied Nanotechnology. 3: 1–8. doi:10.11159/ijtan.2015.001.
  21. ^ Imamura, Hayao (2000), "Chapter 182 The metals and alloys (prepared utilizing liquid ammonia solutions) in catalysis II", The Role of Rare Earths in Catalysis, Handbook on the Physics and Chemistry of Rare Earths, vol. 29, Elsevier, pp. 45–74, doi:10.1016/s0168-1273(00)29005-3, ISBN 978-0-444-50472-2, retrieved 2020-11-10
  22. ^ Nockemann, Peter; Meyer, Gerd (2002). "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.
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  24. ^ a b c Janik, Jerzy F.; Wells, Richard L. (January 1996). "Gallium Imide, {Ga(NH) 3/2 } n , a New Polymeric Precursor for Gallium Nitride Powders". Chemistry of Materials. 8 (12): 2708–2711. doi:10.1021/cm960419h. ISSN 0897-4756.
  25. ^ Nguyen, Minh Tho; Vanquickenborne, L.G.; Plisnier, Michel; Flammang, Robert (January 1993). "A mass spectrometric and ab initio molecular orbital characterization of thionitrosyl hydride (H-N=S)". Molecular Physics. 78 (1): 111–119. Bibcode:1993MolPh..78..111N. doi:10.1080/00268979300100111. ISSN 0026-8976.
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  29. ^ Li, Peng; Niu, Wenxia; Gao, Tao (2015-11-25). "Systematic analysis of structural and spectroscopic properties of neptunimine (HN=NpH2) and plutonimine (HN=PuH2)". Journal of Molecular Modeling. 21 (12): 316. doi:10.1007/s00894-015-2856-1. ISSN 0948-5023. PMID 26608606. S2CID 7587370.
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