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Sodium Iodide

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Template:Chembox FormulaTemplate:Chembox MolarMassTemplate:Chembox StructureTemplate:Chembox EntropyTemplate:Chembox ExternalMSDSTemplate:Chembox MainHazardsTemplate:Chembox OtherAnionsTemplate:Chembox OtherCations
Sodium Iodide
Sodium iodide Sodium iodide
Identifiers
CAS number 7681-82-5 7pxY
Template:CAS (dihydrate)
PubChem 5238
ChemSpider 5048 7pxY
UNII F5WR8N145C 7pxY
ChEBI CHEBI:33167 7pxY
ChEMBL CHEMBL1644695 7pxY
RTECS number WB6475000
Jmol-3D images Image 1
Properties
Appearance white solid
deliquescent
Density 3.67 g/cm3
Melting point

661 °C, 934 K, 1222 °F

Boiling point

1304 °C, 1577 K, 2379 °F

Solubility in water 178.8 g/100 mL (20 °C)
184 g/100 mL (25 °C)
294 g/100 mL (70 °C)
Solubility soluble in ethanol and acetone (39.9 g/100 mL)
Thermochemistry
Std enthalpy of
formation
ΔfHo298
−288 kJ·mol−1[1]
Hazards
EU Index Not listed
Flash point Non-flammable
Related compounds
 Template:Cross (verify) (what is: 10pxY/Template:Cross?)
Except where noted otherwise, data are given for materials in their standard state (at 25 °C, 100 kPa)
Infobox references

Sodium iodide is a white, crystalline salt with the chemical formula NaI, and is used in radiation detection, treatment of iodine deficiency, and as a reactant in the Finkelstein reaction.

UsesEdit

Food supplementEdit

Sodium iodide, as well as potassium iodide, is commonly used to treat and prevent iodine deficiency. Iodized table salt contains one part sodium or potassium iodide to 100,000 parts of sodium chloride.[2]

Organic synthesisEdit

Sodium iodide is used in the Finkelstein reaction, for conversion of an alkyl chloride into an alkyl iodide. This method relies on the insolubility of sodium chloride in acetone to drive the reaction:

R-Cl + NaI → R-I + NaCl

Radiation physics and medicineEdit

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 and has the highest light yield of the commonly used scintillators. 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 radioactive iodide salt of sodium, Na131I, is used for the treatment of thyroid cancer and hyperthyroidism.[3]

Solubility dataEdit

Solubility of NaI in various solvents
(g NaI / 100g of solvent at 25°C)
H2O 184
Liquid ammonia 162
Liquid sulfur dioxide 15
Methanol 62.5 - 83.0
Formic acid 61.8
Acetonitrile 24.9
Acetone 28.0
Formamide 57 - 85
Acetamide 32.3
Dimethylformamide 3.7 - 6.4
[4]

See alsoEdit

ReferencesEdit

  1. 1.0 1.1 Zumdahl, Steven S. (2009). "Chemical Principles 6th Ed.".
  2. Lyday, Phyllis A. "Iodine and Iodine Compounds" in Ullmann's Encyclopedia of Industrial Chemistry, 2005, Wiley-VCH, Weinheim, ISBN 9783527306732 DOI:10.1002/14356007.a14_381 Vol. A14 pp. 382–390.
  3. The Free Dictionary: sodium iodide 131I
  4. Burgess, J. "Metal Ions in Solution" (Ellis Horwood, New York, 1978) ISBN 0-85312-027-7



External linksEdit

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The original article was at Sodium Iodide. The list of authors can be seen in the page history. As with Chemistry, the text of Wikipedia is available under the GNU Free Documentation License.


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