Sodium iodide

Sodium iodide
	; NaI(Tl) scintillators
Identifiers
CAS Number	7681-82-5 ; 13517-06-1 (dihydrate) ;
3D model (JSmol)	Interactive image;
ChEBI	CHEBI:33167 ;
ChEMBL	ChEMBL1644695 ;
ChemSpider	5048 ;
ECHA InfoCard	100.028.800
PubChem CID	5238;
RTECS number	WB6475000;
UNII	F5WR8N145C ;
CompTox Dashboard (EPA)	DTXSID2041125 ;
	InChI InChI=1S/HI.Na/h1H;/q;+1/p-1 Key: FVAUCKIRQBBSSJ-UHFFFAOYSA-M ; InChI=1/HI.Na/h1H;/q;+1/p-1 Key: FVAUCKIRQBBSSJ-REWHXWOFAL;
	SMILES [Na+].[I-];
Properties
Chemical formula	NaI
Molar mass	149.894
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)
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)
Solubility	ethanol, acetone
Band gap	5.89 eV
Magnetic susceptibility (χ)	−57×10−6 cm3 mol−1
Refractive index (nD)	1.93 (300 nm); 1.774 (589 nm); 1.71 (10 μm)
Structure
Crystal structure	Halite, cF8
Space group	Fm3m, No. 225
Lattice constant	a = 0.6462 nm
Formula units (Z)	4
Coordination geometry	Octahedral
Thermochemistry
Heat capacity (C)	52.1 J mol−1 K−1
Std molar; entropy (So298)	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
Main hazards	Irritant, can harm the unborn child
Safety data sheet	[1]
	GHS labelling:
Pictograms
Signal word	Danger
Hazard statements	H315, H319, H400
Precautionary statements	P273, P305+P351+P338
NFPA 704 (fire diamond)	1 0 1
Flash point	Non-flammable
Related compounds
Other anions	Sodium fluoride; Sodium chloride; Sodium bromide;
Other cations	Lithium iodide; Potassium iodide; Rubidium iodide; Caesium iodide;
	Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
	(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.^[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[]

Monatomic NaI chains grown inside double-wall carbon nanotubes.^[12]

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, 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.^[15]

Solubility data[]

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

Solvent	Solubility of NaI (g NaI/kg of solvent at 25 °C)^[16]
H₂O	1842
Liquid ammonia	1620
Liquid sulfur dioxide	150
Methanol	625–830
Formic acid	618
Acetonitrile	249
Acetone	504
Formamide	570–850
Acetamide	323 (41.5 °C)
Dimethylformamide	37–64
Dichloromethane	0.09^[17]

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.

References[]

^ ^a ^b ^c ^d ^e ^f Haynes, p. 4.86
^ Seidell, Atherton (1919). Solubilities of inorganic and organic compounds c. 2. D. Van Nostrand Company. p. 655.
^ Haynes, p. 5.171
^ Miyata, Takeo (1969). "Exciton Structure of NaI and NaBr". Journal of the Physical Society of Japan. 27 (1): 266. Bibcode:1969JPSJ...27..266M. doi:10.1143/JPSJ.27.266.
^ Guizzetti, G.; Nosenzo, L.; Reguzzoni, E. (1977). "Optical properties and electronic structure of alkali halides by thermoreflectivity". Physical Review B. 15 (12): 5921–5926. Bibcode:1977PhRvB..15.5921G. doi:10.1103/PhysRevB.15.5921.
^ Haynes, p. 4.130
^ Haynes, p. 10.250
^ Davey, Wheeler P. (1923). "Precision Measurements of Crystals of the Alkali Halides". Physical Review. 21 (2): 143–161. Bibcode:1923PhRv...21..143D. doi:10.1103/PhysRev.21.143.
^ Haynes, p. 5.36
^ "Sodium iodide 383112". Sigma Aldrich.
^ ^a ^b Lyday, Phyllis A. (2005). "Iodine and Iodine Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 382–390. doi:10.1002/14356007.a14_381.
^ Senga, Ryosuke; Suenaga, Kazu (2015). "Single-atom electron energy loss spectroscopy of light elements". Nature Communications. 6: 7943. Bibcode:2015NatCo...6.7943S. doi:10.1038/ncomms8943. PMC 4532884. PMID 26228378.
^ 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 1. 85 (9): 2705–2712. doi:10.1039/F19898502705.

Cited sources[]

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

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" (PDF). Global Safety Management. January 23, 2015. Retrieved October 16, 2019.

[crc-1] ^ ^a ^b ^c ^d ^e ^f Haynes, p. 4.86

[2] Seidell, Atherton (1919). Solubilities of inorganic and organic compounds c. 2. D. Van Nostrand Company. p. 655.

[3] Haynes, p. 5.171

[4] Miyata, Takeo (1969). "Exciton Structure of NaI and NaBr". Journal of the Physical Society of Japan. 27 (1): 266. Bibcode:1969JPSJ...27..266M. doi:10.1143/JPSJ.27.266.

[5] Guizzetti, G.; Nosenzo, L.; Reguzzoni, E. (1977). "Optical properties and electronic structure of alkali halides by thermoreflectivity". Physical Review B. 15 (12): 5921–5926. Bibcode:1977PhRvB..15.5921G. doi:10.1103/PhysRevB.15.5921.

[6] Haynes, p. 4.130

[7] Haynes, p. 10.250

[8] Davey, Wheeler P. (1923). "Precision Measurements of Crystals of the Alkali Halides". Physical Review. 21 (2): 143–161. Bibcode:1923PhRv...21..143D. doi:10.1103/PhysRev.21.143.

[9] Haynes, p. 5.36

[10] "Sodium iodide 383112". Sigma Aldrich.

[Ullmann-11] Lyday, Phyllis A. (2005). "Iodine and Iodine Compounds". Ullmann's Encyclopedia of Industrial Chemistry. Weinheim: Wiley-VCH. pp. 382–390. doi:10.1002/14356007.a14_381.

[chains-12] Senga, Ryosuke; Suenaga, Kazu (2015). "Single-atom electron energy loss spectroscopy of light elements". Nature Communications. 6: 7943. Bibcode:2015NatCo...6.7943S. doi:10.1038/ncomms8943. PMC 4532884. PMID 26228378.

[13] 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.

[14] Streitwieser, Andrew (1956). "Solvolytic Displacement Reactions At Saturated Carbon Atoms". Chemical Reviews. 56 (4): 571–752. doi:10.1021/cr50010a001.

[15] "Scintillation Materials and Assemblies" (PDF). Saint-Gobain Crystals. 2016. Retrieved June 21, 2017.

[16] Burgess, John (1978). Metal Ions in Solution. Ellis Horwood Series in Chemical Sciences. New York: Ellis Horwood. ISBN 9780470262931.

[17] 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 1. 85 (9): 2705–2712. doi:10.1039/F19898502705.

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