Chemistry:Ruthenium(III) iodide
| Names | |
|---|---|
| Other names
Ruthenium triiodide
| |
| Identifiers | |
3D model (JSmol)
|
|
| |
| |
| Properties | |
| RuI3 | |
| Density | 5.25 g cm−3 |
| sparingly soluble[1] | |
| Structure | |
| hexagonal[1] | |
| Thermochemistry | |
Std molar
entropy (S |
−247 J mol−1 K−1[1] |
Std enthalpy of
formation (ΔfH⦵298) |
−159 kJ mol−1[1] |
| Related compounds | |
Other anions
|
Ruthenium(III) fluoride Ruthenium(III) chloride Ruthenium(III) bromide |
Other cations
|
Iron(III) iodide Osmium(III) iodide Technetium(III) iodide Rhodium(III) iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
| Infobox references | |
Ruthenium(III) iodide is a chemical compound containing ruthenium and iodine with the formula RuI
3. It is a black solid.[2]
Preparation
Ruthenium(III) iodide can be prepared in several ways.[1][3]
The reaction of ruthenium tetroxide with aqueous hydroiodic acid:[4]
- RuO
4 + excess HI → RuI
3
The thermal decomposition of pentaammineruthenium(III) iodide:[3]
- Ru(NH
3)
5I
3 → RuI
3 + 5 NH
3
The salt metathesis reaction of hydrated ruthenium(III) chloride with potassium iodide in aqueous solution:[1]
- RuCl
3 · xH
2O + 3 KI → RuI
3 + 3 KCl + xH
2O
Direct combination of the elements has been reported to succeed under some conditions (350 °C) but not others (500 °C and 20 atm):[1]
- 2 Ru + 3 I
2 → 2 RuI
3
Structure
Ruthenium(III) iodide adopts an extended structure with octahedral coordination geometry at ruthenium.[4] There is some doubt about the characterisation of ruthenium(III) iodide and it may be an oxohalide or a hydroxyhalide.[1]
References
- ↑ 1.0 1.1 1.2 1.3 1.4 1.5 1.6 1.7 Seddon, Elaine A.; Seddon, Kenneth R. (1984). The Chemistry of Ruthenium. Elsevier. p. 161. ISBN 0-444-42375-3.
- ↑ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. p. 1083. ISBN 978-0-08-037941-8.
- ↑ 3.0 3.1 Cotton, Simon A. (1997). Chemistry of Precious Metals. Springer Netherlands. p. 3. ISBN 9780751404135.
- ↑ 4.0 4.1 Housecroft, C. E.; Sharpe, A. G. (2008). Inorganic Chemistry (3rd ed.). Prentice Hall. p. 779. ISBN 978-0-13-175553-6.
| 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 | |||
 |  |
