Ammonium iodide

Ammonium iodide
The ammonium cation
The ammonium cation
The iodide anion
The iodide anion
ball-and-stick model of an ammonium cation (left) and an iodide anion (right)
Identifiers
3D model (JSmol)
ChemSpider
ECHA InfoCard 100.031.548 Edit this at Wikidata
UNII
  • InChI=1S/HI.H3N/h1H;1H3 checkY
    Key: UKFWSNCTAHXBQN-UHFFFAOYSA-N checkY
  • InChI=1/HI.H3N/h1H;1H3
    Key: UKFWSNCTAHXBQN-UHFFFAOYAU
  • [I-].[NH4+]
Properties
NH4I
Molar mass 144.94 g/mol
Appearance White crystalline powder
Density 2.51 g/cm3
Melting point 551 °C (1,024 °F; 824 K) (sublimes)
Boiling point 235 °C (455 °F; 508 K) (in vacuum)
155 g/100 mL (0 °C)
172 g/100 mL (20 °C)
250 g/100 mL (100 °C)
−66.0×10−6 cm3/mol
Hazards
NFPA 704 (fire diamond)
NFPA 704 four-colored diamondHealth 2: Intense or continued but not chronic exposure could cause temporary incapacitation or possible residual injury. E.g. chloroformFlammability 0: Will not burn. E.g. waterInstability 0: Normally stable, even under fire exposure conditions, and is not reactive with water. E.g. liquid nitrogenSpecial hazards (white): no code
2
0
0
Flash point Non-flammable
Related compounds
Other anions
 Ammonium fluoride
Ammonium chloride
Ammonium bromide
Other cations
 Sodium iodide
Potassium iodide
Phosphonium 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 checkY☒N ?)

Ammonium iodide is the inorganic compound with the formula NH4I. A white solid. It is an ionic compound, although impure samples appear yellow. This salt consists of ammonium cation and an iodide anion.[1] It can be prepared by the action of hydroiodic acid on ammonia. It is easily soluble in water, from which it crystallizes in cubes. It is also soluble in ethanol. Ammonium iodide in aqueous solutions are observed as acidic and display elevated vapor pressures at high temperatures[2]

Preparation

Ammonium iodide can be made in lab by treating ammonia with hydroiodic acid:

NH3 + HI → NH4I

Uses

Ammonium iodide is used as dietary supplement to treat iodine deficiency.[3]

Properties and Reactions

Ammonium iodide has recently been used in many research studies and experiments.

Vinyl sulfones have been prepared using ammonium iodide,.[4]

Organic reactions are not synthesized with organic solvents due to their increasing detrimental effects on the human body and ecosystem.[5] Many chemists have altered organic reactions to exclude solvents in order to have successful sustainable syntheses. A report was presented on an organic synthesis for the iodination of ketones and aromatic compounds using ammonium iodide and H2O2 (hydrogen peroxide).[5] This resulted in the products' high yields, which were gathered more efficiently, in a shorter duration compared to the use of the abrasive compound: molecular iodine[5]

References

  1. ^ Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
  2. ^ Kirk-Othmer, ed. (2001-01-26). Kirk-Othmer Encyclopedia of Chemical Technology (1 ed.). Wiley. doi:10.1002/0471238961.0113131523051920.a01.pub2. ISBN 978-0-471-48494-3.
  3. ^ "Ammonium Iodide: Benefits, Risks, and Safety in Dietary Supplements". www.digicomply.com. Retrieved 2023-11-21.
  4. ^ Gao, Xiaofang; Pan, Xiaojun; Gao, Jian; Huang, Huawen; Yuan, Gaoqing; Li, Yingwei (2015). "Ammonium iodide-induced sulfonylation of alkenes with DMSO and water toward the synthesis of vinyl methyl sulfones". Chemical Communications. 51 (1): 210–212. doi:10.1039/C4CC07606K. PMID 25406694.
  5. ^ a b c Kulkarni, Pramod; Kondhare, Dasharath; Varala, Ravi; Zubaidha, Pudukulathan (2013). "Cyclization of 2′-hydroxychalcones to flavones using ammonium iodide as an iodine source: An eco-friendly approach". Journal of the Serbian Chemical Society. 78 (7): 909–916. doi:10.2298/jsc120901119k. ISSN 0352-5139.