Wikipedia

Triiodide

In chemistry, triiodide usually refers to the triiodide ion, I−
3. This anion, one of the polyhalogen ions, is composed of three iodine atoms. It is formed by combining aqueous solutions of iodide salts and iodine. Some salts of the anion have been isolated, including thallium(I) triiodide (Tl+[I3]−) and ammonium triiodide ([NH4]+[I3]−). Triiodide is observed to be a red colour in solution.[1]

Triiodide
Skeletal formula of triiodide
Skeletal formula of triiodide
Spacefill model of triiodide
Spacefill model of triiodide
Names
IUPAC name
Triiodide anion
Identifiers
3D model (JSmol)
ChEMBL
ChemSpider
UNII
  • InChI=1S/I3/c1-3-2/q-1 checkY
    Key: WRTMQOHKMFDUKX-UHFFFAOYSA-N checkY
  • I[I-]I
Properties
I−
3
Molar mass 380.71341 g·mol−1
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).

Nomenclature

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Other chemical compounds with "triiodide" in their name may contain three iodide centers that are not bonded to each other as the triiodide ion, but exist instead as separate iodine atoms or iodide ions. Examples include nitrogen triiodide (NI3) and phosphorus triiodide (PI3), where individual iodine atoms are covalently bonded to a central atom. As some cations have the theoretical possibility to form compounds with both triiodide and iodide ions, such as ammonium, compounds containing iodide anions in a 3:1 stoichiometric ratio should only be referred to as triiodides in cases where the triiodide anion is present. It may also be helpful to indicate the oxidation number of a metal cation, where appropriate. For example, the covalent molecule gallium triiodide (Ga2I6) is better referred to as gallium(III) iodide to emphasise that it is iodide anions that are present, and not triiodide.

Preparation

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The following exergonic equilibrium gives rise to the triiodide ion:

I2 + I− ⇌ I−
3

In this reaction, iodide is viewed as a Lewis base, and the iodine is a Lewis acid. The process is analogous to the reaction of S8 with sodium sulfide (which forms polysulfides) except that the higher polyiodides have branched structures.[2]

Structure and bonding

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The ion is linear and symmetrical. According to valence shell electron pair repulsion theory, the central iodine atom has three equatorial lone pairs, and the terminal iodine atoms are bonded axially in a linear fashion, due to the three lone pairs bonding to the central iodine-atom. In the molecular orbital model, a common explanation for the hypervalent bonding on the central iodine involves a three-center four-electron bond. The I−I bond is longer than in diatomic iodine, I2.

In ionic compounds, the bond lengths and angles of triiodide vary depending on the nature of the cation. The triiodide anion is easily polarised and in many salts, one I−I bond becomes shorter than the other. Only in combination with large cations, e.g. a quaternary ammonium such as [N(CH3)4]+, may the triiodide remain roughly symmetrical.[3]

In solution phase, the bond lengths and angles of triiodide vary depending on the nature of solvent. The protic solvents tend to localize the triiodide anion's excess charge, resulting in the triiodide anion's asymmetric structure.[4][5] For example, the triiodide anion in methanol has an asymmetric bent structure with a charge localized on the longer end of the anion.[6]

The dimensions of the triiodide [Ia−Ib−Ic]− bonds in a few sample compounds are shown below:

compound Ia−Ib (pm) Ib−Ic (pm) angle (°)
TlI3 306.3 282.6 177.9
RbI3 305.1 283.3 178.11
CsI3 303.8 284.2 178.00
NH4I3 311.4 279.7 178.55
I3− (in methanol)[6] 309.0 296.0 152.0

Properties

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The triiodide ion is the simplest polyiodide; several higher polyiodides exist. In solution, it appears yellow in low concentrations, and brown at higher concentrations. The triiodide ion is responsible for the well-known blue-black color which arises when iodine solutions interact with starch. Iodide does not react with starch; nor do solutions of iodine in nonpolar solvents.

Lugol's iodine contains potassium iodide and a stoichiometric amount of elemental iodine, so that significant amounts of triiodide ion exist in this solution. Tincture of iodine, although nominally a solution of elemental iodine in ethanol, also contains significant amounts of triiodide, due to its content of both iodide and water.

Photochemistry

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Triiodide is a model system in photochemistry. Its reaction mechanism has been studied in gas phase, solution and the solid state. In gas phase, the reaction proceeds in multiple pathways that include iodine molecule, metastable ions and iodine radicals as photoproducts, which are formed by two-body and three-body dissociation.[7][8] In condensed phases, due to confinement, geminate recombination is more common. In solution, only two-body dissociation of triiodide has been observed.[9][10] In the protic solvents, an iodine atom at the shorter end of the triiodide anion dissociates upon photoexcitation showing two-body dissociation.[6] In the solid state, the triiodide photochemistry has been studied in compounds involving quaternary ammonium cations, such as tetrabutylammonium triiodide.[11] It has been shown that the solid state photoreaction mechanism depends on the light wavelength, yielding fast recovery in a few picoseconds[12] or going through a two-stage process that involves the formation and break-up of a tetraiodide intermediate on longer timescales.[13] Besides, triiodide photochemistry is an important contributor in the environmental cycle of iodine.[14] Because of the presence of heavy iodine atoms and the well-calibrated chemical pathways, triiodide has also become a computational benchmark system for relativistic quantum chemistry.[15]

Electrochemistry

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The redox reactions of triiodide and iodide has been proposed as critical steps in dye-sensitized solar cells.[16] and rechargeable batteries.[17]

See also

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References

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  1. ^ "Halogens as oxidising agents - Chemguide".
  2. ^ Wells, A. F. (1984). Structural Inorganic Chemistry. Oxford: Clarendon Press. ISBN 0-19-855370-6.
  3. ^ Atkins; et al. (2010). Inorganic Chemistry (5th ed.). Oxford University Press. p. 431. ISBN 978-0-19-923617-6.
  4. ^ Johnson, Alan E.; Myers, Anne B. (1 January 1996). "Solvent Effects in the Raman Spectra of the Triiodide Ion: Observation of Dynamic Symmetry Breaking and Solvent Degrees of Freedom". The Journal of Physical Chemistry. 100 (19): 7778–7788. doi:10.1021/jp953052x. ISSN 0022-3654.
  5. ^ Lynden-Bell, R. M.; Kosloff, R.; Ruhman, S.; Danovich, D.; Vala, J. (8 December 1998). "Does solvation cause symmetry breaking in the I3− ion in aqueous solution?". The Journal of Chemical Physics. 109 (22): 9928–9937. doi:10.1063/1.477659. ISSN 0021-9606.
  6. ^ a b c Heo, Jun; Kim, Jong Goo; Choi, Eun Hyuk; Ki, Hosung; Ahn, Doo-Sik; Kim, Jungmin; Lee, Seonggon; Ihee, Hyotcherl (26 January 2022). "Determining the charge distribution and the direction of bond cleavage with femtosecond anisotropic x-ray liquidography". Nature Communications. 13 (1): 522. Bibcode:2022NatCo..13..522H. doi:10.1038/s41467-022-28168-0. ISSN 2041-1723. PMC 8792042. PMID 35082327.
  7. ^ Hoops, Alexandra A.; Gascooke, Jason R.; Faulhaber, Ann Elise; Kautzman, Kathryn E.; Neumark, Daniel M. (2004-04-03). "Two- and three-body photodissociation of gas phase I3−". The Journal of Chemical Physics. 120 (17): 7901–7909. Bibcode:2004JChPh.120.7901H. doi:10.1063/1.1691017. hdl:2440/34955. ISSN 0021-9606. PMID 15267705. S2CID 94632820.
  8. ^ Nakanishi, Ryuzo; Saitou, Naoya; Ohno, Tomoyo; Kowashi, Satomi; Yabushita, Satoshi; Nagata, Takashi (2007-05-28). "Photodissociation of gas-phase I3−: Comprehensive understanding of nonadiabatic dissociation dynamics". The Journal of Chemical Physics. 126 (20): 204311. Bibcode:2007JChPh.126t4311N. doi:10.1063/1.2736691. ISSN 0021-9606. PMID 17552766.
  9. ^ Banin, Uri; Ruhman, Sanford (1993-03-15). "Ultrafast photodissociation of I 3 . Coherent photochemistry in solution". The Journal of Chemical Physics. 98 (6): 4391–4403. Bibcode:1993JChPh..98.4391B. doi:10.1063/1.465066. ISSN 0021-9606.
  10. ^ Kühne, Thomas; Vöhringer, Peter (1996-12-22). "Vibrational relaxation and geminate recombination in the femtosecond-photodissociation of triiodide in solution". The Journal of Chemical Physics. 105 (24): 10788–10802. Bibcode:1996JChPh.10510788K. doi:10.1063/1.472887. ISSN 0021-9606.
  11. ^ Herbstein, F. H.; Kaftory, M.; Kapon, M.; Saenger, W. (1981-01-01). Herbstein, F. H.; Kaftory, M.; Kapon, M.; Saenger, W. (eds.). "Structures of three crystals containing approximately — linear chains of triiodide ions". Zeitschrift für Kristallographie - Crystalline Materials. 154 (1–2): 11–30. Bibcode:1981ZK....154...11H. doi:10.1524/zkri.1981.154.1-2.11. ISSN 2194-4946.
  12. ^ Poulin, Peter R.; Nelson, Keith A. (2006-09-22). "Irreversible Organic Crystalline Chemistry Monitored in Real Time". Science. 313 (5794): 1756–1760. Bibcode:2006Sci...313.1756P. doi:10.1126/science.1127826. ISSN 0036-8075. PMID 16946037. S2CID 35002522.
  13. ^ Xian, Rui; Corthey, Gastón; Rogers, David M.; Morrison, Carole A.; Prokhorenko, Valentyn I.; Hayes, Stuart A.; Miller, R. J. Dwayne (2017-03-27). "Coherent ultrafast lattice-directed reaction dynamics of triiodide anion photodissociation". Nature Chemistry. 9 (6): 516–522. Bibcode:2017NatCh...9..516X. doi:10.1038/nchem.2751. hdl:20.500.11820/52dbea74-99b4-454b-aac2-56c7be20947b. ISSN 1755-4330. PMID 28537597.
  14. ^ Raso, Angela R. W.; Custard, Kyle D.; May, Nathaniel W.; Tanner, David; Newburn, Matt K.; Walker, Lawrence; Moore, Ronald J.; Huey, L. G.; Alexander, Liz; Shepson, Paul B.; Pratt, Kerri A. (2017-09-19). "Active molecular iodine photochemistry in the Arctic". Proceedings of the National Academy of Sciences. 114 (38): 10053–10058. Bibcode:2017PNAS..11410053R. doi:10.1073/pnas.1702803114. ISSN 0027-8424. PMC 5617258. PMID 28874585.
  15. ^ Gomes, André Severo Pereira; Visscher, Lucas; Bolvin, Hélène; Saue, Trond; Knecht, Stefan; Fleig, Timo; Eliav, Ephraim (2010-08-14). "The electronic structure of the triiodide ion from relativistic correlated calculations: A comparison of different methodologies". The Journal of Chemical Physics. 133 (6): 064305. Bibcode:2010JChPh.133f4305G. doi:10.1063/1.3474571. hdl:20.500.12210/35342. ISSN 0021-9606. PMID 20707568. S2CID 8849684.
  16. ^ Gibson, Elizabeth A.; Le Pleux, Loïc; Fortage, Jérôme; Pellegrin, Yann; Blart, Errol; Odobel, Fabrice; Hagfeldt, Anders; Boschloo, Gerrit (2012-04-17). "Role of the Triiodide/Iodide Redox Couple in Dye Regeneration in p-Type Dye-Sensitized Solar Cells". Langmuir. 28 (15): 6485–6493. doi:10.1021/la300215q. ISSN 0743-7463. PMID 22432412.
  17. ^ Ma, Jizhen; Liu, Miaomiao; He, Yulong; Zhang, Jintao (2021-02-17). "Iodine Redox Chemistry in Rechargeable Batteries". Angewandte Chemie International Edition. 60 (23): 12636–12647. doi:10.1002/anie.202009871. ISSN 1433-7851. PMID 32939916. S2CID 221769817.
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