Thallium halides

The thallium halides include monohalides, where thallium has oxidation state +1, trihalides where thallium generally has oxidation state +3 and some intermediate halides with mixed +1 and +3 oxidation states. These materials find use in specialized optical settings, such as focusing elements in research spectrophotometers. Compared to the more common zinc selenide-based optics, materials such as thallium bromoiodide enable transmission at longer wavelengths. In the infrared, this allows for measurements as low as 350 cm⁻¹ (28 µm), whereas zinc selenide is opaque by 21.5 µm and ZnSe optics are generally only usable to 650 cm⁻¹ (15 µm).

Monohalides

Thallium(I) iodide has the CsCl crystal structure

The monohalides all contain thallium with oxidation state +1. Parallels can be drawn between the thallium(I) halides and their corresponding silver salts, for example thallium(I) chloride and bromide are light sensitive and thallium(I) fluoride is more soluble in water than the chloride and bromide.

Thallium(I) fluoride: TlF is a white crystalline solid, with a mp of 322 °C. It is readily soluble in water unlike the other $Tl(I)$ halides. The normal room temperature form has a similar structure to $α -PbO$ which has a distorted rock salt structure with essentially five coordinate thallium, the sixth fluoride ion is at 370 pm. At 62 °C it transforms to a tetragonal structure. This structure is unchanged up to pressure of 40 GPa.^[1]; The room temperature structure has been explained in terms of interaction between Tl 6s and the F 2p states producing strongly antibonding Tl-F states. The structure distorts to minimise these unfavourable covalent interactions.^[2]

Thallium(I) chloride: TlCl is a light sensitive, white crystalline solid, mp 430 °C. The crystal structure is the same as CsCl.

Thallium(I) bromide: TlBr is a light sensitive, pale yellow crystalline solid, mp 460 °C. The crystal structure is the same as CsCl.

Thallium(I) iodide: At room temperature $TlI$ is a yellow crystalline solid, mp 442 °C. The crystal structure is a distorted rock salt structure known as the $β -TlI$ structure. At higher temperatures the colour changes to red with a structure the same as CsCl.

Thallium(I) mixed halides

Thallium bromoiodide and thallium bromochloride are mixed salts of thallium(I) that are used in spectroscopy as an optical material for transmission, refraction and focusing of infrared radiation. The materials were first grown by R. Koops in the laboratory of Olexander Smakula at the Carl Zeiss Optical Works, Jena in 1941.^[3]^[4] The red bromoiodide was coded KRS-5 ^[5] and the colourless bromochloride, KRS-6 ^[6] and this is how they are commonly known. The KRS prefix is an abbreviation of “Kristalle aus dem Schmelz-fluss”, (crystals from the melt). The compositions of KRS-5 and KRS-6 approximate to $TlBr 0.4 I 0.6$ and $TlBr 0.3 Cl 0.7$ . KRS-5 is the most commonly used, its properties of being relatively insoluble in water and non-hygroscopic, make it an alternative to KBr, CsI and AgCl.^[7]

Trihalides

The thallium trihalides are less stable than their corresponding aluminium, gallium and indium counterparts and chemically quite distinct. The triiodide does not contain thallium with oxidation state +3 but is a thallium(I) compound and contains the linear triiodide (I₃⁻) ion.

Thallium(III) fluoride: TlF₃ is a white crystalline solid , mp 550 °C. The crystal structure is the same as YF₃ and $β -BiF 3$ . In this the thallium atom is 9 coordinate,(tricapped trigonal prismatic). It can be synthesised by fluoridation of the oxide, Tl₂O₃, with F₂, BrF₃ or SF₄ at 300 °C.

Thallium(III) chloride: TlCl₃ has a distorted Cr(III) chloride structure like AlCl₃ and InCl₃. Solid TlCl₃ is unstable and disproportionates at 40 °C, losing chlorine to give TlCl. It can be prepared in CH₃CN by treating a solution of TlCl with Cl₂ gas.

Thallium(III) bromide: This unstable compound disproportionates at less than 40 °C to TlBr₂. It can be prepared in CH₃CN by treating a solution of TlBr with Br₂ gas. In water the tetrahydrate complex can be prepared by adding bromine to a stirred suspension of TlBr.^[8]

Thallium(I) triiodide: $TlI 3$ is a black crystalline solid prepared from $TlI$ and $I 2$ in aqueous HI. It does not contain thallium(III), but has the same structure as CsI₃ containing the linear I₃⁻ ion.

Mixed valence halides

As a group these are not well characterised. They contain both Tl(I) and Tl(III), where the thallium(III) atom is present as complex anions e.g. TlCl₄⁻.

$TlCl 2$: This is formulated as $Tl I Tl III Cl 4$ .

$Tl 2 Cl 3$: This yellow compound is formulated $Tl I 3 Tl III Cl 6$ .^[9]

$Tl 2 Br 3$: This compound is similar to $Tl 2 Cl 3$ and is formulated $Tl I 3 Tl III Br 6$ ^[10]

$TlBr 2$: This pale brown solid is formulated $Tl I Tl III Br 4$

$Tl 3 I 4$: This compound has been reported as an intermediate in the synthesis of $TlI 3$ from $TlI$ and $I 2$ . The structure is not known.

Halide complexes

Thallium(I) complexes: Thallium(I) can form complexes of the type (TlX₃)²⁻ and (TlX₄)³⁻ both in solution and when thallium(I) halides are incorporated into alkali metal halides. These doped alkali metal halides have new absorption and emission nbands and are used as phosphors in scintillation radiation detectors.

Thallium(III) fluoride complexes: The salts NaTlF₄ and Na₃TlF₆ do not contain discrete tetrahedral and octahedral anions. The structure of NaTlF₄ is the same as fluorite (CaF₂) with Na^I and Tl^III atoms occupying the 8 coordinate Ca^II sites. Na₃TlF₆ has the same structure as cryolite, Na₃AlF₆. In this the thallium atoms are octahedrally coordinated. Both compounds are usually considered to be mixed salts of Na⁺ and Tl³⁺.

Thallium(III) chloride complexes: Salts of tetrahedral TlCl₄⁻ and octahedral TlCl₆³⁻are known with various cations.

Salts containing TlCl₅²⁻ with a square pyramidal structure are known. Interestingly some salts, that nominally contain TlCl₅²⁻ actually contain the dimeric anion Tl₂Cl₁₀⁴⁻, long chain anions where Tl^III is 6 coordinate and the octahedral units are linked by bridging chlorine atoms, or mixed salts of Tl^IIICl₄ and Tl^IIICl₆.^[11]

The ion Tl₂Cl₉³⁻ where thallium atoms are octahedrally coordinated with three bridging chlorine atoms has been identified in the Caesium salt, Cs₃Tl₂Cl₉.

Thallium(III) bromide complexes: Salts of Tl^IIIBr₄⁻ and Tl^IIIBr₆³⁻ are known with various cations.

The TlBr₅²⁻ anion has been characterised in a number of salts and is trigonal bipyramidal. Some other salts that nominally contain TlBr₅²⁻ are mixed salts containing TlBr₄⁻ and Br⁻.^[12]

Thallium(III) iodide complexes: Salts of $Tl III I 4 -$ are known. The $Tl III$ anion is stable even though the triiodide is a thallium(I) compound.

General references

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

Footnotes

↑ U.Haussermann, P.Berastegui, S.Carlson, J.Haines, and J.Leger Angewandte Chemie, 31, pp. 4760 (2001)
↑ A-V Mudring Eur. J. Inorg. Chem. 2007, 882
↑ Koops, R. (1948). "Optical structural subjects from binary mixed crystals". Optik (3): 298–304.
↑ Smakula A., J. Kalnajs and V. Sils (March 1953). "Inhomogeneity of Thallium Halide Mixed Crystals and Its Elimination". Laboratory for Insulation Research Technical Report 67. Massachusetts Institute of Technology. Retrieved October 17, 2012.
↑ Crystran Data for KRS5 http://www.crystran.co.uk/krs5-thallium-bromoiodide-tlbrtli.htm
↑ Crystran Data for KRS6 http://www.crystran.co.uk/krs6-thallium-bromochloride-tlbrtlcl.htm
↑ Frank Twyman (1988) Prism and Lens Making: A Textbook for Optical Glassworkers CRC Press ISBN 0-85274-150-2, page 170
↑ Glaser J. (1979) Acta Chem. Scand. A33, 789. T605.
↑ Bohme R., Rath J.,Grunwald B., Thiele G., Z. Naturforsch. B 36, 1366 (1980).
↑ Ackermann R., Hirschle C., Rotter H.W., Thiele G. Z. fur Anorg. Allgem. Chemie 2002, 628(12), 2675-2682.
↑ James M. A., Clyburne J. A. C., Linden A., James B. D, Liesegang J., Zuzich V. Can. J. Chem., 1996, 74, 1490
↑ Linden A. , Nugent K.W., Petridis A., James B. D., Inorg. Chim. Acta, 1999, 285, 122.

Thallium compounds

TBCCO Tl(C₂H₃O₂)₃ TlN₃ TlH TlOH Tl(OH)₃ TlI TlI₃ TlBr Tl₂CO₃ TlCl TlF Tl₂O Tl₂O₃ Tl₂SO₄ Tl₂S Tl₂Te Tl(NO₃)₃

Fluorine compounds

AgF AgF₂ Ag₂F AlF₃ AmF₃ AmF₄ AsF₃ AsF₅ AuF₃ BF₃ B₂F₄ BaF₂ BeF₂ BiF₃ BiF₅ BrF₃ BrF₅ CF₄ C₂F₆ CaF₂ CdF₂ CeF₃ ClF₃ ClF₅ CoF₂ CoF₃ CrF₂ CrF₃ CrF₄ CrF₅ CrF₆ CsF CuF DyF₃ ErF₃ EuF₂ EuF₃ DF HF FI KF LiF NaF RbF TlF FeF₂ HgF₂ Hg₂F₂ KrF₂ MgF₂ MnF₂ NiF₂ F₂O F₂O₄ PbF₂ PdF₂ SnF₂ SrF₂ XeF₂ ZnF₂ ZrF₂ FeF₃ GaF₃ GdF₃ HoF₃ InF₃ LaF₃ LuF₃ MnF₃ F₃N NdF₃ F₃P PrF₃ PuF₃ SbF₃ ScF₃ SmF₃ TbF₃ TiF₃ TlF₃ TmF₃ UF₃ VF₃ YF₃ YbF₃ GeF₄ HfF₄ MoF₄ F₄N₂ PbF₄ PuF₄ SF₄ SeF₄ SiF₄ SnF₄ TeF₄ ThF₄ UF₄ VF₄ WF₄ XeF₄ ZrF₄ IF₅ NbF₅ PF₅ SbF₅ TaF₅ UF₅ VF₅ WF₅ MoF₆ OsF₆ PtF₆ ReF₆ SF₆ SeF₆ TeF₆ UF₆ WF₆ XeF₆ IF₇ ReF₇ IrF₃ IrF₆ OsF₄ OsF₅ PmF₃ PrF₄ PuF₆ ReF₄ ReF₅ RhF₆ RuF₃ RuF₄ RuF₅ RuF₆ TcF₅ TcF₆ VF₂ YbF₂ AgBF₄ AgPF₆ Cs₂AlF₅ K₃AlF₆ Na₃AlF₆ KAsF₆ LiAsF₆ NaAsF₆ HBF₄ KBF₄ LiBF₄ NaBF₄ RbBF₄ Ba(BF₄)₂ Ni(BF₄)₂ Pb(BF₄)₂ Sn(BF₄)₂ BaClF BaSiF₆ BaGeF₆ BrOF₃ BrO₂F CBrF₃ CBr₂F₂ CBr₃F CClF₃ CCl₂F₂ CCl₃F CFN CF₂O CF₃I CHF₃ CH₂F₂ CH₃F C₂Cl₃F₃ C₂H₃F C₆H₅F C₇H₅F₃ C₁₅F₃₃N ClFO₂ CrFO₄ CrF₂O₂ CsBF₄ NH₄F FNO FNO₂ FNO₃ KHF₂ NaHF₂ ThOF₂ NH₅F₂ F₂OS F₃OP F₃PS HPF₆ HSbF₆ KPF₆ KSbF₆ LiPF₆ NaPF₆ NaSbF₆ Na₂SiF₆ Na₂TiF₆ Na₂ZrF₆ TlPF₆ IOF₃ K₂NbF₇ K₂TaF₇ IO₃F

Chemical formulas

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