Sodium iodide
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| Identifiers | |||
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| 3D model (JSmol) |
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| ChEBI | |||
| ChemSpider | |||
| ECHA InfoCard | 100.028.800 | ||
| PubChem CID |
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| RTECS number | WB6475000 | ||
| UNII | |||
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| Properties | |||
| NaI | |||
| Molar mass | 149.89 g mol−1 | ||
| Appearance | white solid deliquescent | ||
| Odor | odorless | ||
| Density | 3.67 g cm−3 | ||
| Melting point | 661 °C (1,222 °F; 934 K) | ||
| Boiling point | 1,304 °C (2,379 °F; 1,577 K) | ||
| 158.7 g/100 mL (0 °C) 184.2 g/100 mL (25 °C) 227.8 g/100 mL (50 °C) 294 g/100 mL (70 °C) 302 g/100 mL (100 °C)[1] | |||
| Acidity (pKa) | 8–9.5 | ||
| −57.0 × 10−6 cm3 mol−1 | |||
| Refractive index (nD) |
1.7745 | ||
| Structure | |||
| Halite | |||
| Octahedral | |||
| Thermochemistry | |||
| Std molar entropy (S |
91 J mol−1 K−1[2] | ||
| Std enthalpy of formation (ΔfH |
−288 kJ mol−1[2] | ||
| Hazards | |||
| Main hazards | Irritant, can harm the unborn child | ||
| Safety data sheet | |||
| Flash point | Non-flammable | ||
| Related compounds | |||
| Other anions |
Sodium fluoride Sodium chloride Sodium bromide Sodium astatide | ||
| Other cations |
Lithium iodide Potassium iodide Rubidium 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). | |||
 verify (what is  ?) | |||
| Infobox references | |||
Sodium iodide (chemical formula NaI) is an ionic compound formed from the chemical reaction of sodium metal and iodine. Under standard conditions, it is a white, water-soluble solid comprising a 1:1 mix of sodium cations (Na+) and iodide anions (I−) in a crystal lattice. It is used mainly as a nutritional supplement and in organic chemistry. It is produced industrially as the salt formed when acidic iodides react with sodium hydroxide.[3]
Uses
Food supplement
Sodium iodide, as well as potassium iodide, is commonly used to treat and prevent iodine deficiency. Iodized table salt contains 10 ppm iodide.[3]
Organic synthesis
Sodium iodide is used for conversion of an alkyl chlorides into an alkyl iodides. This method, the Finkelstein reaction,[5] relies on the insolubility of sodium chloride in acetone to drive the reaction:[6]
Nuclear medicine
Some radioactive iodide salts of sodium, including Na125I and Na131I, have radiopharmaceutical uses, such as in the treatment of thyroid cancer and hyperthyroidism or as radiolabeling tracers in imaging (see Isotopes of iodine > Radioiodines I-123, I-124, I-125, and I-131 in medicine and biology).
Thallium-doped NaI(Tl) scintillators
Sodium iodide activated with thallium, NaI(Tl), when subjected to ionizing radiation, emits photons (i.e., scintillate) and is used in scintillation detectors, traditionally in nuclear medicine, geophysics, nuclear physics, and environmental measurements. NaI(Tl) is the most widely used scintillation material. The crystals are usually coupled with a photomultiplier tube, in a hermetically sealed assembly, as sodium iodide is hygroscopic. Fine-tuning of some parameters (i.e., radiation hardness, afterglow, transparency) can be achieved by varying the conditions of the crystal growth. Crystals with a higher level of doping are used in X-ray detectors with high spectrometric quality. Sodium iodide can be used both as single crystals and as polycrystals for this purpose. The wavelength of maximum emission is 415 nm.[7]
Solubility data
Sodium iodide exhibits high solubility in some organic solvents, unlike sodium chloride or even bromide:
| Solvent | Solubility of NaI (g NaI/100 g of solvent at 25 °C)[8] |
|---|---|
| H2O | 184.2 |
| Liquid ammonia | 162 |
| Liquid sulfur dioxide | 15 |
| Methanol | 62.5–83.0 |
| Formic acid | 61.8 |
| Acetonitrile | 24.9 |
| Acetone | 50.4425 |
| Formamide | 57–85 |
| Acetamide | 32.3 (41.5 °C) |
| Dimethylformamide | 3.7–6.4 |
| Dichloromethane | 0.009[9] |
See also
References
- ↑ Seidell, Atherton (1919). Solubilities of inorganic and organic compounds c. 2. D. Van Nostrand Company. p. 655.
- 1 2 Zumdahl, Steven S. (2009). Chemical Principles (6th ed.). Houghton Mifflin. p. A23. ISBN 0-618-94690-X.
- 1 2 Lyday, Phyllis A. (2005). "Iodine and Iodine Compounds". Ullmann's Encyclopedia of Industrial Chemistry. A14. Weinheim: Wiley-VCH. pp. 382–390. ISBN 978-3-527-30673-2. doi:10.1002/14356007.a14_381.
- ↑ Senga, Ryosuke; Suenaga, Kazu (2015). "Single-atom electron energy loss spectroscopy of light elements". Nature Communications. 6: 7943. PMC 4532884
. PMID 26228378. doi:10.1038/ncomms8943. - ↑ Finkelstein, Hank (1910). "Darstellung organischer Jodide aus den entsprechenden Bromiden und Chloriden". Ber. Dtsch. Chem. Ges. (in German). 43 (2): 1528–1532. doi:10.1002/cber.19100430257.
- ↑ Streitwieser, Andrew (1956). "Solvolytic Displacement Reactions At Saturated Carbon Atoms". Chemical Reviews. 56 (4): 571–752. doi:10.1021/cr50010a001.
- ↑ "Scintillation Materials and Assemblies" (PDF). Saint-Gobain Crystals. 2016. Retrieved June 21, 2017.
- ↑ Burgess, John (1978). Metal Ions in Solution. Ellis Horwood Series in Chemical Sciences. New York: Ellis Horwood. ISBN 9780470262931.
- ↑ De Namor, Angela F. Danil; Traboulssi, Rafic; Salazar, Franz Fernández; De Acosta, Vilma Dianderas; De Vizcardo, Yboni Fernández; Portugal, Jaime Munoz (1989). "Transfer and partition free energies of 1:1 electrolytes in the water–dichloromethane solvent system at 298.15 K". Journal of the Chemical Society, Faraday Transactions I. 85 (9): 2705–2712. doi:10.1039/F19898502705.
External links
- "ICSC 1009 – Sodium Iodide (Anhydrous)". International Chemical Safety Card. April 20, 2005. Retrieved June 21, 2017.
- "Material Safety Data Sheet (MSDS) – Safety data for sodium iodide". ScienceLab.com. May 21, 2013. Retrieved June 21, 2017.
- "Sodium iodide (Oral route, Injection route, Intravenous route)". Drugs.com. 2017. Retrieved June 21, 2017.
- "Safety Data Sheet – Sodium iodide / Thallium Crystal" (PDF). Saint Gobain. February 27, 2014. Retrieved June 21, 2017.
