Ammonium iodide
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| ECHA InfoCard | 100.031.548 | ||
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| 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 | |||
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| 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).
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Ammonium iodide is the inorganic compound with the formula NH4I. It is an ionic compound. It takes the form of a white solid, though 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.[2]
Structure
[edit]Ammonium iodide is a salt that crystallizes in a motif akin those for the alkali metal iodides and most other ammonium halides. Several phases have been characterized, which are similar but not identical to those of ammonium chloride.[3]
Under pressure, the compound melts congruently.
Preparation
[edit]Ammonium iodide can be made in lab by treating ammonia with iodine and the reductant hydrogen peroxide:[4]
- 2 NH3 + I2 + H2O2 → 2 NHI + O2
Uses
[edit]Ammonium iodide is used as a dietary supplement to treat iodine deficiency.[5]
Properties and reactions
[edit]Vinyl sulfones have been prepared using ammonium iodide.[6]
In green chemistry, ammonium iodide and an oxidant (e.g., H2O2) iodinate ketones and aromatic compounds.[7]
References
[edit]- ↑ Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. ISBN 0-12-352651-5.
- ↑ 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.
- ↑ Pistorius, Carl W.F.T. (1976). "Phase relations and structures of solids at high pressures". Progress in Solid State Chemistry. 11: 1–151. doi:10.1016/0079-6786(76)90012-1.
- ↑ M. Schmeisser (1963). "Chlorine, Bromine, Iodine". In G. Brauer (ed.). Handbook of Preparative Inorganic Chemistry, 2nd Ed. Vol. 1pages=289. NY,NY: Academic Press.
- ↑ "Ammonium Iodide: Benefits, Risks, and Safety in Dietary Supplements". www.digicomply.com. Retrieved 2023-11-21.
- ↑ 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.
- ↑ 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.
