Rubidium iodide is a salt of rubidium and iodine, with the chemical formula RbI. It is a white solid with a melting point of 642 °C.
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Rubidium iodide
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3D model (JSmol)
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| ECHA InfoCard | 100.029.271 |
PubChem CID
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CompTox Dashboard (EPA)
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| Properties | |
| RbI | |
| Molar mass | 212.3723 g/mol |
| Appearance | solid |
| Density | 3.110 g/cm 3 |
| Melting point | 646.85 °C (1,196.33 °F; 920.00 K) |
| Boiling point | 1,304 °C (2,379 °F; 1,577 K) |
| 152 g/100 mL | |
| −72.2·10−6 cm3/mol | |
| Hazards | |
| Lethal dose or concentration (LD, LC): | |
LD50 (median dose)
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4708 mg/kg (oral, rat) |
| Safety data sheet (SDS) | External MSDS |
| Related compounds | |
Other anions
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Rubidium fluoride Rubidium chloride Rubidium bromide Rubidium astatide |
Other cations
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Lithium iodide Sodium iodide Potassium iodide Caesium iodide Francium iodide |
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
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Preparation
editRubidium iodide can be synthesized in several ways. One is to use a mixed reaction of rubidium hydroxide and hydriodic acid/hydrogen iodide:[1]
- RbOH + HI → RbI + H2O
Another method is to neutralize rubidium carbonate with hydriodic acid:[1]
- Rb2CO3 + 2HI → 2RbI + H2O + CO2
Another method is to use rubidium metal to react directly with iodine, but because rubidium metal is very expensive, it is the least commonly used method. In addition, rubidium reacts violently with halogens and burns:[1]
- 2Rb + I2 → 2RbI
Properties
editRubidium iodide forms colorless crystals, and has a red-violet flame color. The refractive index of the crystals is nD = 1.6474.[2] It reacts with halogens to form polyhalides: RbI3, RbICl2, RbICl4.[3] It is easily soluble in water, liquid ammonia, sulfuric acid, RbI·6NH3 and RbI·3SO2. Rubidium iodide is soluble only in the following solvents:
| Solvent | 0 °C | 25 °C |
|---|---|---|
| Acetonitrile | 1.478 | 1.350 |
| Propionitrile | 0.274 | 0.305 |
| Nitromethane | 0.567 | 0.518 |
| Acetone | 0.960 | 0.674 |
| Furfural | 4,930 |
The standard enthalpy of formation of rubidium iodide is ΔfH0298 = −328.7 kJ mol−1,[5] the standard free enthalpy of formation ΔG0298 = −325.7 kJ mol−1,[5] and the standard molar entropy S0298 = 118.11 J K−1·mol−1.[5]
Rubidium iodide has a sodium chloride structure; its lattice constant is a = 7.326 Å, and the Rb–I bond length is 3.66 Å.[3]
Applications
editRubidium iodide is used as a component of eye drops, in which it is sold in Romania under the name Rubjovit® (containing 8 mg/ml RbI).[6] Another product is Polijodurato®. However, there are studies that show that rubidium iodide has allergy-triggering[7] and inflammation-causing[8] side effects. Homeopathic products containing rubidium iodide are available under the name 'Rubidium iodatum'. In the past, towards the end of the 19th century, it was used to treat syphilis.[9]
It found isolated use in organic synthesis, for example for the targeted saponification of a polymethylated phosphate.[10]
References
edit- ^ a b c "WebElements". Archived from the original on 2008-04-18. Retrieved 23 February 2006.
- ^ Ans, Jan d'; Ans, Jan d' (1998). Elemente, anorganische Verbindungen und Materialien. Taschenbuch für Chemiker und Physiker / D'Ans (4., neubearb. u. rev. Aufl ed.). Location not known: Publisher not known. ISBN 978-3-540-60035-0.
- ^ a b 『化学大辞典』 共立出版、1993年
- ^ Aterton Seidell (1940). Solubilities Of Organic Compounds Vol - I. Carnegie-Mellon University Hunt Library, N.Sathyanarayanan. D.Van Nostrand Co.
- ^ a b c Dickerson, Richard E.; Sichting, Hans-Werner, eds. (1988). Prinzipien der Chemie (2., bearb. und erw. Aufl ed.). Berlin: de Gruyter. ISBN 978-3-11-009969-0.
- ^ Jurja, Sanda, et al. "Correlation between effectiveness and antioxidant activity of some anti cataract eye drops." Rev Chim (Bucharest) 67 (2016): 1004-1007.
- ^ "Allergen Rubidium Allergie enthalten Allergologie". www.alles-zur-allergologie.de. Retrieved 2023-09-16.
- ^ Cameli, N.; Bardazzi, F.; Morelli, R.; Tosti, A. (Nov 1990). "Contact dermatitis from rubidium iodide in eyedrops". Contact Dermatitis. 23 (5): 377–378. doi:10.1111/j.1600-0536.1990.tb05182.x.
- ^ Paschalis, C.; Jenner, F. A.; Lee, C. R. (May 1978). "Effects of rubidium chloride on the course of manic-depressive illness". Journal of the Royal Society of Medicine. 71 (5): 343–352. doi:10.1177/014107687807100507. ISSN 0141-0768. PMC 1436619. PMID 349155.
- ^ Turhanen, Petri A. (2014-07-03). "Synthesis of Triple-Bond-Containing 1-Hydroxy-1,1-bisphosphonic Acid Derivatives To Be Used as Precursors in "Click" Chemistry: Two Examples". The Journal of Organic Chemistry. 79 (13): 6330–6335. doi:10.1021/jo500831r. ISSN 0022-3263.
Bibliography
edit- CRC Handbook of Chemistry and Physics, 77th edition