Chemistry:Hafnium(IV) iodide
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| File:HfI4.tif | |
| Names | |
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| IUPAC name
Hafnium(IV) iodide
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| Other names
hafnium tetraiodide, tetraiodohafnium
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| Identifiers | |
3D model (JSmol)
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| ChemSpider | |
| EC Number |
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PubChem CID
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| Properties | |
| HfI4 | |
| Molar mass | 686.11[1] |
| Appearance | red-orange[1] |
| Density | 5.60 g/cm3[1] |
| Melting point | 449 °C (840 °F; 722 K)[1] |
| Boiling point | 394 °C (741 °F; 667 K)[1] (sublimes) |
| Structure | |
| Monoclinic, mS40 | |
| C2/c, No. 15[2] | |
a = 1.1787 nm, b = 1.1801 nm, c = 1.2905 nm
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| Related compounds | |
Other anions
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Hafnium(IV) fluoride Hafnium(IV) chloride Hafnium(IV) bromide |
Other cations
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Titanium(IV) iodide Zirconium(IV) iodide |
Related compounds
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Hafnium(III) iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Tracking categories (test):
Hafnium(IV) iodide is the inorganic compound with the formula HfI4. It is a red-orange, moisture sensitive, sublimable solid that is produced by heating a mixture of hafnium with excess iodine.[2] It is an intermediate in the crystal bar process for producing hafnium metal.
In this compound, the hafnium centers adopt octahedral coordination geometry. Like most binary metal halides, the compound is a polymeric. It is one-dimensional polymer consisting of chains of edge-shared bioctahedral Hf2I8 subunits, similar to the motif adopted by HfCl4. The nonbridging iodide ligands have shorter bonds to Hf than the bridging iodide ligands.[2]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 Haynes, William M., ed (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.66. ISBN 1439855110.
- ↑ 2.0 2.1 2.2 Krebs, B.; Sinram, D. (1980). "Hafniumtetrajodid HfI4: Struktur und eigenschaften. Ein neuer AB4-strukturtyp". Journal of the Less Common Metals 76 (1–2): 7–16. doi:10.1016/0022-5088(80)90005-3.
| HI | He | ||||||||||||||||
| LiI | BeI2 | BI3 | CI4 | NI3 | I2O4, I2O5, I4O9 |
IF, IF3, IF5, IF7 |
Ne | ||||||||||
| NaI | MgI2 | AlI3 | SiI4 | PI3, P2I4 |
S | ICl, ICl3 |
Ar | ||||||||||
| KI | CaI2 | Sc | TiI4 | VI3 | CrI3 | MnI2 | FeI2 | CoI2 | NiI2 | CuI | ZnI2 | Ga2I6 | GeI2, GeI4 |
AsI3 | Se | IBr | Kr |
| RbI | SrI2 | YI3 | ZrI4 | NbI5 | Mo | Tc | Ru | Rh | Pd | AgI | CdI2 | InI3 | SnI4, SnI2 |
SbI3 | TeI4 | I | Xe |
| CsI | BaI2 | HfI4 | TaI5 | W | Re | Os | Ir | Pt | AuI | Hg2I2, HgI2 |
TlI | PbI2 | BiI3 | Po | AtI | Rn | |
| Fr | RaI2 | Rf | Db | Sg | Bh | Hs | Mt | Ds | Rg | Cn | Nh | Fl | Mc | Lv | Ts | Og | |
| ↓ | |||||||||||||||||
| La | Ce | Pr | Nd | Pm | SmI2 | Eu | Gd | TbI3 | Dy | Ho | Er | Tm | Yb | Lu | |||
| Ac | ThI4 | Pa | UI3, UI4 |
Np | Pu | Am | Cm | Bk | Cf | EsI3 | Fm | Md | No | Lr | |||
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