| 词条 | Ammonium iodide |
| 释义 |
| Verifiedfields = changed | Watchedfields = changed | verifiedrevid = 470456251 | Name = Ammonium iodide | ImageFileL1 = Ammonium.svg | ImageSizeL1 = 90px | ImageNameL1 = The ammonium cation | ImageFileR1 = I-.svg | ImageSizeR1 = 20px | ImageNameR1 = The iodide anion | ImageFile2 = Ammonium-iodide-3D-balls.png | ImageSize2 = 180px | ImageName2 = ball-and-stick model of an ammonium cation (left) and an iodide anion (right) | ImageName = Ammonium iodide |Section1={{Chembox Identifiers | UNII_Ref = {{fdacite|correct|FDA}} | UNII = OZ8F027LDH | InChI = 1/HI.H3N/h1H;1H3 | SMILES = [I-].[NH4+] | InChIKey = UKFWSNCTAHXBQN-UHFFFAOYAU | StdInChI_Ref = {{stdinchicite|correct|chemspider}} | StdInChI = 1S/HI.H3N/h1H;1H3 | StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} | StdInChIKey = UKFWSNCTAHXBQN-UHFFFAOYSA-N | CASNo = 12027-06-4 | CASNo_Ref = {{cascite|correct|CAS}} | ChemSpiderID_Ref = {{chemspidercite|correct|chemspider}} | ChemSpiderID =23785 | PubChem = 25487 |Section2={{Chembox Properties | Formula = NH4I | MolarMass = 144.94 g/mol | Appearance = White crystalline powder | Density = 2.51 g/cm3 | Solubility = 155 g/100 mL (0 °C) 172 g/100 mL (20 °C) 250 g/100 mL (100 °C) | MeltingPtC = 551 | MeltingPt_notes = (sublimes) | BoilingPtC = 235 | BoilingPt_notes = (in vacuum) | MagSus = -66.0·10−6 cm3/mol |Section7={{Chembox Hazards | ExternalSDS = | MainHazards = | NFPA-H = 2 | NFPA-F = 0 | NFPA-R = 0 | FlashPt = Non-flammable |Section8={{Chembox Related | OtherAnions = Ammonium fluoride Ammonium chloride Ammonium bromide | OtherCations = Sodium iodide Potassium iodide | OtherCompounds = }}Ammonium iodide is the chemical compound NH4I. It is used in photographic chemicals and some medications.[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. It gradually turns yellow on standing in moist air, owing to decomposition with liberation of iodine.[1] PreparationAmmonium iodide can be made in lab by reacting ammonia or ammonium hydroxide with hydroiodic acid or hydrogen iodide gas: NH3 + HI → NH4I NH4OH + HI → NH4I + H2O It is also formed by the decomposition of ammoniated triiodoamine (an explosive). References1. ^1 Holleman, A. F.; Wiberg, E. Inorganic Chemistry Academic Press: San Diego, 2001. {{ISBN|0-12-352651-5}}. {{inorganic-compound-stub}} 3 : Iodides|Nonmetal halides|Ammonium compounds |
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