Dichloramine: Difference between revisions
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| verifiedrevid = 437036929 |
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| ImageFileL1 = Dichloramine-2D.png |
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| ImageSizeL1 = 130 |
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| ImageFileR1 = Dichloramine-3D-spacefill.png |
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| ImageSizeR1 = 110 |
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| IUPACName = |
| IUPACName = |
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| OtherNames = |
| OtherNames = Chlorimide |
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|Section1={{Chembox Identifiers |
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| InChI = 1/Cl2HN/c1-3-2/h3H |
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| InChIKey = JSYGRUBHOCKMGQ-UHFFFAOYAB |
| InChIKey = JSYGRUBHOCKMGQ-UHFFFAOYAB |
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| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
| StdInChI_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
| StdInChIKey_Ref = {{stdinchicite|correct|chemspider}} |
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| StdInChIKey = JSYGRUBHOCKMGQ-UHFFFAOYSA-N |
| StdInChIKey = JSYGRUBHOCKMGQ-UHFFFAOYSA-N |
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| CASNo_Ref = {{cascite|correct|PubChem}} |
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| CASNo = |
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| CASNo = 3400-09-7 |
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| DTXSID = DTXSID4074936 |
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| UNII_Ref = {{fdacite|changed|FDA}} |
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| UNII = KGU33GRT44 |
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| PubChem = 76939 |
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| ChemSpiderID = 69389 |
| ChemSpiderID = 69389 |
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| SMILES = ClNCl |
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|Section2={{Chembox Properties |
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| Formula = {{chem2|NHCl2}} |
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| N=1 | Cl=2 | H=1 |
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| Appearance = yellow gas<ref name="HoWi">Holleman-Wiberg: Lehrbuch der Anorganischen Chemie, 102. Auflage, Berlin 2007, {{ISBN|978-3-11-017770-1}}.</ref> |
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|Section7={{Chembox Hazards |
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|Section8={{Chembox Related |
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| OtherCompounds = {{ubl|[[Ammonia]]|[[Monochloramine]]|[[Nitrogen trichloride]]}} |
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'''Dichloramine''' is a reactive inorganic compound |
'''Dichloramine''' is a reactive [[inorganic compound]] with the [[chemical formula]] {{chem2|auto=1|NHCl2}}. It is one of the three [[chloramines]] of [[ammonia]], the others being [[monochloramine]] ({{chem2|NH2Cl}}) and [[nitrogen trichloride]] ({{chem2|NCl3}}). This yellow gas is unstable and reacts with many materials.<ref name="HoWi"/> It is formed by a reaction between [[ammonia]] and [[chlorine]] or [[sodium hypochlorite]]. It is a byproduct formed during the synthesis of monochloramine and nitrogen trichloride. |
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== Synthesis == |
== Synthesis == |
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Dichloramine can be prepared by a reaction between [[ |
Dichloramine can be prepared by a reaction between [[monochloramine]] and [[chlorine]] or [[sodium hypochlorite]]:<ref name="HoWi"/> |
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:{{chem2|NH2Cl + Cl2 → NHCl2 + [[Hydrogen chloride|HCl]]}} |
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:<math>\mathrm{NH_2Cl + Cl_2 \longrightarrow NHCl_2 + HCl}</math> |
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== Reactions == |
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Dichloramine reacts with the [[hydroxide ion]], which can be present in [[water]] or comes from water molecules, to yield [[nitroxyl]] and the [[chloride ion]].<ref name="White Chlorine">{{cite book|last1=White|first1=George Clifford|title=The handbook of chlorination|date=1986|publisher=Van Nostrand Reinhold|location=New York|isbn=0-442-29285-6|pages=169|edition=2nd}}</ref> |
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== References == |
== References == |
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<references/> |
<references/> |
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{{Nitrogen compounds}} |
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[[Category:Inorganic amines]] |
[[Category:Inorganic amines]] |
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[[Category:Chlorides]] |
[[Category:Chlorides]] |
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[[Category:Nitrogen halides]] |
[[Category:Nitrogen halides]] |
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[[Category:Gases with color]] |
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[[de:Dichloramin]] |