Sodium iodide

Sodium iodide

NaI(Tl) scintillators
Identifiers
CAS Number	7681-82-5 Y 13517-06-1 (dihydrate) N
3D model (JSmol)	Interactive image
ChEBI	CHEBI:33167 Y
ChEMBL	ChEMBL1644695 N
ChemSpider	5048 Y
ECHA InfoCard	100.028.800
PubChem CID	5238
RTECS number	WB6475000
UNII	F5WR8N145C Y
CompTox Dashboard (EPA)	DTXSID2041125
InChI InChI=1S/HI.Na/h1H;/q;+1/p-1 Y Key: FVAUCKIRQBBSSJ-UHFFFAOYSA-M Y InChI=1/HI.Na/h1H;/q;+1/p-1 Key: FVAUCKIRQBBSSJ-REWHXWOFAL
SMILES [Na+].[I-]
Properties
Chemical formula	NaI
Molar mass	149.894[1]
Appearance	white solid deliquescent[1]
Odor	odorless
Density	3.67 g cm−3[1]
Melting point	661 °C (1,222 °F; 934 K)[1]
Boiling point	1,304 °C (2,379 °F; 1,577 K)[1]
Solubility in water	1587 g/L (0 °C) 1842 g/L (25 °C) 2278 g/L (50 °C) 2940 g/L (70 °C) 3020 g/L (100 °C)[2][3]
Solubility	ethanol, acetone[1]
Band gap	5.89 eV[4][5]
Magnetic susceptibility (χ)	−57×10−6 cm3 mol−1[6]
Refractive index (nD)	1.93 (300 nm) 1.774 (589 nm) 1.71 (10 μm)[7]
Structure[8]
Crystal structure	Halite, cF8
Space group	Fm3m, No. 225
Lattice constant	a = 0.6462 nm
Formula units (Z)	4
Coordination geometry	Octahedral
Thermochemistry[9]
Heat capacity (C)	52.1 J mol−1 K−1
Std molar entropy (S⦵298)	98.5 J mol−1 K−1
Std enthalpy of formation (ΔfH⦵298)	−287.8 kJ mol−1
Gibbs free energy (ΔfG⦵)	−286.1 kJ mol−1
Hazards
Occupational safety and health (OHS/OSH):
Main hazards	Irritant, can harm the unborn child
GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H315, H319, H400
Precautionary statements	P273, P305+P351+P338[10]
NFPA 704 (fire diamond)	1 0 1
Flash point	Non-flammable
Safety data sheet (SDS)	[1]
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). N verify (what is YN ?) 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.^[11] It is a chaotropic salt.

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.^[11]

Organic synthesis

Sodium iodide is used for conversion of alkyl chlorides into alkyl iodides. This method, the Finkelstein reaction,^[13] relies on the insolubility of sodium chloride in acetone to drive the reaction:^[14]

R–Cl + NaI → R–I + NaCl

Nuclear medicine

Some radioactive iodide salts of sodium, including Na¹²⁵I and Na¹³¹I, have radiopharmaceutical uses for thyroid cancer and hyperthyroidism or as radioactive tracer 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.^[15]

Radiocontrast

António Egas Moniz searched for a radiocontrast agent for cerebral angiography.^[16] After experiments on rabbits and dogs he settled upon sodium iodide as the best medium.^[16]

Solubility data

Sodium iodide exhibits high solubility in some organic solvents, unlike sodium chloride or even bromide:

Stability

Iodides (including sodium iodide) are detectably oxidized by atmospheric oxygen (O₂) to molecular iodine (I₂). I₂ and I⁻ complex to form the triiodide complex, which has a yellow color, unlike the white color of sodium iodide. Water accelerates the oxidation process, and iodide can also produce I₂ by photooxidation, therefore for maximum stability sodium iodide should be stored under dark, low temperature, low humidity conditions.

See also

• Gamma spectroscopy
• Scintillation counter
• Teratology

References

Cited sources

• Haynes, William M., ed. (2016). CRC Handbook of Chemistry and Physics (97th ed.). CRC Press. p. 4.49. ISBN 9781498754293.

External links

Wikimedia Commons has media related to Sodium iodide.

• "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. Archived from the original on June 3, 2018. Retrieved June 21, 2017.
• "Sodium iodide (Oral route, Injection route, Intravenous route)". Drugs.com. 2017. Retrieved June 21, 2017.
• "Safety Data Sheet – Sodium iodide" (PDF). Global Safety Management. January 23, 2015. Retrieved October 16, 2019.