هيدروكبريتيد الأمونيوم

Ammonium hydrosulfide
الأسماء
	اسم أيوپاك ammonium hydrosulfide
	أسماء أخرى ammonium bisulfide; ammonium hydrogen sulfide
Identifiers
رقم CAS
3D model (JSmol)	Interactive image;
ChemSpider	23805 ;
ECHA InfoCard	100.031.974
رقم EC	235-184-3;
PubChem CID	25515;
رقم RTECS	BS4900000;
UNII	A824D6LXMB;
UN number	2683
CompTox Dashboard (EPA)	DTXSID20894064 ;
InChI	InChI={{{value}}}
SMILES
الخصائص
الصيغة الجزيئية	(NH4)HS
كتلة مولية	51.111 g/mol
المظهر	Yellow-orange fuming liquid (in solution). White rhombic crystals (anhydrous).
الكثافة	1.17 g/cm3
نقطة الغليان
قابلية الذوبان في الماء	Miscible
قابلية الذوبان	soluble in alcohol, liquid ammonia, liquid hydrogen sulfide; insoluble in benzene, hexane and ether
معامل الانكسار (nD)	1.74
المخاطر
خطر رئيسي	Toxic
ن.م.ع. مخطط تصويري
ن.م.ع. كلمة الاشارة	Danger
ن.م.ع. عبارات المخاطر	H314, H400.
ن.م.ع. العبارات الاحتياطية	P260, P264, P273, P280, P301+P330+P331, P303+P361+P353, P304+P340, P305+P351+P338, P310, P321, P363, P391, P405, P501
NFPA 704 (معيـَّن النار)	3 3
	الجرعة أو التركيز القاتل (LD, LC):
LD50 (الجرعة الوسطى)	168 mg/kg (rat, oral)
مركبات ذا علاقة
أنيونات أخرى	محلول الأمونيا
كاتيونات أخرى	هيدروكبريتيد الصوديوم
	ما لم يُذكر غير ذلك، البيانات المعطاة للمواد في حالاتهم العيارية (عند 25 °س [77 °ف]، 100 kPa).
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	مراجع الجدول

هيدروكبريتيد الأمونيوم Ammonium hydrosulfide هو مركب كيميائي صيغته (NH₄)HS.

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التكوين

It is the salt derived from the ammonium cation and the hydrosulfide anion. The salt exists as colourless, water-soluble, micaceous crystals. On Earth the compound is encountered mainly as a solution, not as the solid, but NH₄SH ice is believed to be a substantial component of the cloud decks of the gas-giant planets Jupiter and Saturn, with sulfur produced by its photolysis responsible for the color of some of those planets' clouds. ويمكن توليده من خلط كبريتيد الهيدروجين والأمونيا.

التحضير

Solutions of ammonium hydrosulfide can be prepared by passing hydrogen sulfide gas through concentrated ammonia solution.^[4] According to a detailed 1895 report, hydrogen sulfide reacts with concentrated aqueous ammonia solution at room temperature to give (NH₄)₂S·2NH₄HS. When this species is cooled to 0 °C and treated with additional hydrogen sulfide, one obtains (NH₄)₂S·12NH₄HS.^[5] An ice-cold solution of this substance kept at 0 °C and having hydrogen sulfide continually passed through it gives the hydrosulfide.

The common "stink bomb" consists of an aqueous solution of ammonium sulfide. The mixture easily converts to ammonia and hydrogen sulfide gases. This conversion illustrates the ease of the following equilibrium:

(NH₄)SH

NH₃ + H₂S

Ammonia and hydrogen sulfide each have a powerful and unpleasant smell.

"كبريتيد الأمونيوم"

Aqueous solutions of ammonium sulfide (CAS registry number 12135-76-1), also known as diammonium sulfide are commercially available, although the composition of these solutions is uncertain as they could consist of a mixture of ammonia and (NH₄)SH. Ammonium sulfide solutions are used occasionally in photographic developing, to apply patina to bronze, and in textile manufacturing. Also, due to its offensive smell, it is the active ingredient in a variety of pranks including the common stink bomb. It can be used as a selective reducing agent (cf 2,4-Dinitrochlorobenzene), where there are two nitro groups only one of them is selectively reduced.

The 1990-1991 CRC Handbook of Physics and Chemistry gives information for anhydrous ammonium monosulfide ((NH₄)₂S) and ammonium pentasulfide ((NH₄)₂S₅) as separate from anhydrous ammonium hydrosulfide (NH₄HS), describing the former two both as yellow crystalline substances that are soluble in cold water and alcohol, and which both decompose in hot water or at high temperature in general (115°C for the pentasulfide), but the latter as a white crystalline solid (which also decomposes in hot water).^[1]

الهامش

^ ^أ ^ب ^ت Lide, David R., ed. (1990). "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (71st ed.). CRC Press, inc. p. 4-45 (That's 1 page.).
^ Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8
^ قالب:GESTIS
^ Goodman, J. T.; Rauchfuss, T. B. (2002). "Tetraethylammonium-tetrathioperrhenate [Et₄N][ReS₄]". Inorganic Syntheses. 33: 107–110. doi:10.1002/0471224502.ch2.
^ W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277.

[CRC-1] أ ^ب ^ت Lide, David R., ed. (1990). "Physical Constants of Inorganic Compounds". CRC Handbook of Chemistry and Physics (71st ed.). CRC Press, inc. p. 4-45 (That's 1 page.).

[2] Pradyot Patnaik. Handbook of Inorganic Chemicals. McGraw-Hill, 2002, ISBN 0-07-049439-8

[GESTIS-3] قالب:GESTIS

[4] Goodman, J. T.; Rauchfuss, T. B. (2002). "Tetraethylammonium-tetrathioperrhenate [Et₄N][ReS₄]". Inorganic Syntheses. 33: 107–110. doi:10.1002/0471224502.ch2.

[5] W. P. Bloxam (1895). "The Sulphides and Polysulphides of Ammonium". J. Chem. Soc., Trans. 67: 283. doi:10.1039/CT8956700277.

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