Indium halides

There are three sets of indium halides, the trihalides, the monohalides, and several intermediate halides. In the monohalides the oxidation state of indium is +1 and their proper names are indium(I) fluoride, indium(I) chloride, indium(I) bromide and indium(I) iodide.

The intermediate halides contain indium with oxidation states, +1, +2 and +3.

Indium trihalides

In all of the trihalides the oxidation state of indium is +3, and their proper names are indium(III) fluoride, indium(III) chloride, indium(III) bromide, and indium(III) iodide. The trihalides are Lewis acidic. Indium trichloride is a starting point in the production of trimethylindium which is used in the semiconductor industry.

Indium(III) fluoride

InF3 is a white crystalline solid with mp 1170 °C. Its structure contains 6 coordinate indium.

Indium(III) chloride

InCl3 is a white crystalline solid mp 586 °C. It has the same structure as AlCl3.

Indium(III) bromide

InBr3 is a pale yellow crystalline solid, m.p. 435 °C. It has the same structure as AlCl3. InBr3 is finding some use in organic synthesis as a water tolerant Lewis acid.[1]

Indium(III) iodide

Ball-and-stick model of the In2I6 molecule

InI3 is a coloured crystalline solid, usually described as orange. Distinct yellow and a red forms are known. The red form undergoes a transition to the yellow at 57 °C. The structure of the red form has not been determined by X-ray crystallography, however spectroscopic evidence indicates that indium may be six coordinate.[2] The yellow form consists of In2I6 with 4 coordinate indium centres. It is used as an "iodide getter" in the Cativa process.

Intermediate halides

A surprising number of intermediate chlorides and bromides are known, but only one iodide, and no difluoride. Rather than the apparent oxidation state of +2, these compounds contain indium in the +1 and +3 oxidation states. Thus the diiodide is described as InIInIIIX4. It was some time later that the existence of compounds containing the anion In2
Br2−
 were confirmed which contains an indium-indium bond. Early work on the chlorides and bromides involved investigations of the binary phase diagrams of the trihalides and the related monohalide. Many of the compounds were initially misidentified as many of them are incongruent and decompose before melting. The majority of the previously reported chlorides and bromides have now either had their existence and structures confirmed by X Ray diffraction studies or have been consigned to history. Perhaps the most unexpected case of mistaken identity was the surprising result that a careful reinvestigation of the InCl/InCl3 binary phase diagram did not find InCl2.[3]
The reason for this abundance of compounds is that indium forms 4 and 6 coordinate anions containing indium(III) e.g. In
Br−
, In
Cl3−
 as well as the anion In2
Br2−
 that surprisingly contains an indium-indium bond.

In7Cl9 and In7Br9

In7Cl9 is yellow solid stable up to 250oC that is formulated InI6 (InIIICl6)Cl3[4]

In7Br9 has a similar structure to In7Cl9 and can be formulated as InI6 (InIIIBr6)Br3[5]

In5Br7

In5Br7 is a pale yellow solid. It is formulated InI3 (InII2Br6)Br. The InII2Br6 anion has an eclipsed ethane like structure with a metal-metal bond length of 270 pm.[6]

In2Cl3 and In2Br3

In2Cl3 is colourless and is formulated InI3 InIIICl6[7] In contrast In2Br3 contains the In2Br6 anion as present in In5Br7, and is formulated InI(InII2Br6) with a structure similar to Ga2Br3.[8]

In4Br7

In4Br7 is near colourless with a pale greenish yellow tint. It is light sensitive (like TlCl and TlBr) decaying to InBr2 and In metal. It is a mixed salt containing the In
Br−
 and In
Br3−
 anions balanced by In+ cations. It is formulated InI5 (InIIIBr4)2 (InIIIBr6) The reasons for the distorted lattice have been ascribed to an antibonding combination between doubly filled, non-directional indium 5s orbitals and neighboring bromine 4p hybrid orbitals.[9]

In5Cl9

In5Cl9 is formulated as InI3InIII2Cl9. The In2
Cl3−
 anion has two 6 coordinate indium atoms with 3 bridging chlorine atoms, face sharing bioctahedra, with a similar structure to Cr2
Cl2−
 and Tl2
Cl2−
.[10]

InBr2

InBr2 is a greenish white crystalline solid, which is formulated InIInIII Br4. It has the same structure as GaCl2. InBr2 is soluble in aromatic solvents and some compounds containing η6-arene In(I) complexes have been identified. (See hapticity for an explanation of the bonding in such arene-metal ion complexes). With some ligands InBr2 forms neutral complexes containing an indium-indium bond.[11]

InI2

InI2 is a yellow solid that is formulated InIInIIII4.

Monohalides

The solid monohalides InCl, InBr and InI are all unstable with respect to water, decomposing to the metal and indium(III) species. They fall between gallium(I) compounds, which are more reactive and thallium(I) that are stable with respect to water. InI is the most stable. Up until relatively recently the monohalides have been scientific curiosities, however with the discovery that they can be used to prepare indium cluster and chain compounds they are now attracting much more interest.

InF

InF only known as an unstable gaseous compound.

InCl

The room temperature form of InCl is yellow, with a cubic distorted NaCl structure.[12] The red high temperature (>390oC) has the structure.[13]

InBr

InBr is a red crystalline solid, mp 285oC. It has the same structure as , with an orthorhombic distorted rock salt structure. It can be prepared from indium metal and InBr3.

InI

InI is a deep red purple crystalline solid. It has the same structure as . It can be made by direct combination of its constituent elements at high temperature. Alternatively it can be prepared from InI3 and indium metal in refluxing xylenes.[14] It is the most stable of the solid monohalides and is soluble in some organic solvents. Solutions of InI in a pyridine/m-xylene mixture are stable below 243 K.[15]

Anionic halide complexes of In(III)

The trihalides are Lewis Acids and form addition compounds with ligands. For InF3 there are few examples known however for the other halides addition compounds with tetrahedral, trigonal bipyramidal and octahedral coordination geometries are known. With halide ions there are examples of all of these geometries along with some anions with octahedrally coordinated indium and with bridging halogen atoms, In2
X3−
 with three bridging halogen atoms and In2
X−
 with just one. Additionally there are examples of indium with square planar geometry in the InX52− ion. The square planar geometry of In
Cl2−
 was the first found for a main group element.

In
X−
 and In
X3−

Salts of In
Cl−
, In
Br−
 and I
Ni−
 are known. The salt LiInF4 has been prepared [16] however it does not contain tetrahedral anions but has an unusual layer structure with octahedrally coordinated Indium atoms. Salts of InF63−, In
Cl3−
 and In
Br3−
 [17] have all been made.

In
Cl2−
 and In
Br2−

The In
Cl2−
 ion has been found to be square pyramidal in the salt (NEt4)2 InCl5, with the same structure as (NEt4)2 TlCl5, but is trigonal bipyramidal in tetraphenylphosphonium pentachloroindate acetonitrile solvate.[18]

The In
Br2−
 ion has similarly been found square pyramidal, albeit distorted, in the Bis(4-chloropyridinium) salt [19] and trigonal bipyramidal [20] in Bi37InBr48.

In2
X−

The In2
X−
 ions contain a single bridging halogen atom. Whether the bridge is bent or linear cannot be determined from the spectra. The chloride and bromide have been detected using electrospray mass spectrometry. The In2
I−
 ion has been prepared in the salt CsIn2I7.[21]

In2
X3−

The caesium salts of In2
Cl3−
 and In2
Br3−
 both contain binuclear anions with octahedrally coordinated Indium atoms.[22]

Anionic halide complexes of In(I) and In(II)

InI
X−
 and InI
X2−

InIX2− is produced when the In2X62− ion disproportionates. Salts containing the InI
X2−
 ions have been made and their vibrational spectra interpreted as showing that they have C3v symmetry, trigonal pyramidal geometry, with structures similar to the isoelectronic Sn
X−
 ions.

In2
Cl2−
, In2
Br2−
 and In2
I2−

Salts of the chloride, bromide and iodide ions ( Bu4N)2In2X6 have been prepared. In non aqueous solvents this ion disproportionates to give InI
X−
 and InIII
X−
.

Neutral Indium(II) halide adducts

Following the discovery of the In2Br62− a number of related neutral compounds containing the InII2X4 kernel have been formed from the reaction of indium dihalides with neutral ligands.[23] Some chemists refer to these adducts, when used as the starting point for the synthesis of cluster compounds as ‘In2X4’ e.g. the TMEDA adduct.[24]

References

  • WebElements Periodic Table » Indium » compounds information
  • Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 0-08-037941-9.
  • Cotton, F. Albert; Wilkinson, Geoffrey; Murillo, Carlos A.; Bochmann, Manfred (1999), Advanced Inorganic Chemistry (6th ed.), New York: Wiley-Interscience, ISBN 0-471-19957-5
  1. ↑ Zhan-Hui Zhang Thieme Connect Synlett 2005 711
  2. ↑ Taylor M. J., Kloo L. A. Journal of Raman Spectroscopy 31, 6, (2000), 465
  3. ↑ Meyer G., Blachnik R.Z. Anorg. Allg. Chem. 1983, 503, 126
  4. ↑ H.P. Beck D. Wilhelm Angew. Chem. Int. Ed. Engl., 30 (7) (1991) 824-25
  5. ↑ Dronskowski R Z Kristallogr. 210 (1995) 920
  6. ↑ M Ruck , H Bärnighausen Z. Anorg. allg. Chem. 625, Issue 4, (1999), 577
  7. ↑ Meyer. G. Z. Anorg. Allgem. Chem. 479 (1981) 7 39
  8. ↑ Staffel. T., Meyer. G.,Z Anorg Allgem Chem 552 9 113
  9. ↑ R.Dronskowski, Angew. Chem. Int. Ed. Engl. 34 (1995) 1126.
  10. ↑ Meyer. G. Z. Anorg. Allgem. Chem. 1978 445 140,
  11. ↑ Sinclair I., Worrall I.J Can. J. Chem./Rev. can. chim. 60(6): 695-698 (1982)
  12. ↑ J.M. Van den Berg Acta Crystallogr 20 (1966) 905
  13. ↑ C. P. J. M. van der Vorst, G. C. Verschoor, W. J. A. Maaskant, Acta Crystallogr. 1978, B34, 3333.
  14. ↑ Organic Syntheses, Coll. Vol. 10, p.170 (2004); Vol. 79, p.59 (2002)
  15. ↑ Jennifer A. J. Pardo J.A.J., Cowley A.R. , Downs A.J. , Greene T.M. Acta Crystallogr. (2005). C61, 200
  16. ↑ Gravereau P, Chaminade J.P, Gaewdang., T., Grannec J., Pouchard M., Hagenmuller P. Acta Crystallogr. (1992). C48, 769
  17. ↑ Spiro Inorg Chem 4 1290 (1965)
  18. ↑ Bubenheim W., Frenzen G., Muller U. Acta Crystallogr. C, 51, 6, (1995), 1120.
  19. ↑ Ishihara H., Dou S., Gesing T.M., Paulus H., Fuess H., Weiss A. Journal of Molecular Structure 471, 1 (1998)175
  20. ↑ Dubenskyy V., Ruck M., Z Anorg. Allgem. Chemie , 629, (2003), 3, 375
  21. ↑ Taylor M. J. Kloo L. A. Journal of Raman Spectroscopy 31, 6, (2000), 465
  22. ↑ . Meyer Z. Anorg. allgem. Chem. 1978, 445, 140
  23. ↑ Sinclair I., Worrall I.J. Can. J. Chem./Rev. can. chim. 60(6): 695-698 (1982)
  24. ↑ Xiao-Wang Li , Robinson G, Pennington W.T Main Group Chemistry 1, (1996) 301
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