ব্যবহারকারী:Shuvo Mazumder/খেলাঘর
টেমপ্লেট:ভালো নিবন্ধ কেবল উইকিপিডিয়া:ভালো নিবন্ধ-এর জন্য।
নামসমূহ | |
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ইউপ্যাক নাম
aluminium chloride
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অন্যান্য নাম
aluminium(III) chloride
aluminum trichloride | |
শনাক্তকারী | |
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ত্রিমাত্রিক মডেল (জেমল)
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সিএইচইবিআই | |
কেমস্পাইডার | |
ইসি-নম্বর | |
পাবকেম CID
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আরটিইসিএস নম্বর |
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ইউএনআইআই | |
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বৈশিষ্ট্য | |
AlCl3 | |
আণবিক ভর | 133.34 g/mol (anhydrous) 241.43 g/mol (hexahydrate) |
বর্ণ | white or pale yellow solid, hygroscopic |
ঘনত্ব | 2.48 g/cm3 (anhydrous) 1.3 g/cm3 (hexahydrate) |
গলনাঙ্ক | ১৯২.৪ °সে (৩৭৮.৩ °ফা; ৪৬৫.৫ K) (anhydrous) ১০০ °সে (২১২ °ফা; ৩৭৩ K) (hexahydrate) ১৮০ °সে (৩৫৬ °ফা; ৪৫৩ K) (sublimes) |
স্ফুটনাঙ্ক | ১২০ °সে (২৪৮ °ফা; ৩৯৩ K) (hexahydrate) |
43.9 g/100 ml (0 °C) 44.9 g/100 ml (10 °C) 45.8 g/100 ml (20 °C) 46.6 g/100 ml (30 °C) 47.3 g/100 ml (40 °C) 48.1 g/100 ml (60 °C) 48.6 g/100 ml (80 °C) 49 g/100 ml (100 °C) | |
দ্রাব্যতা | soluble in hydrogen chloride, ethanol, chloroform, carbon tetrachloride slightly soluble in benzene |
বাষ্প চাপ | 133.3 Pa (99 °C) 13.3 kPa (151 °C)[১] |
সান্দ্রতা | 0.35 cP (197 °C) 0.26 cP (237 °C)[১] |
গঠন | |
স্ফটিক গঠন | Monoclinic, mS16 |
Space group | C12/m1, No. 12 |
Coordination geometry |
Octahedral (solid) Tetrahedral (liquid) |
আণবিক আকৃতি | Trigonal planar (monomeric vapour) |
তাপ রসায়নবিদ্যা | |
তাপ ধারকত্ব, C | 91 J/mol·K[১] |
স্ট্যন্ডার্ড মোলার এন্ট্রোফি এস |
111 J/mol·K[২] |
গঠনে প্রমান এনথ্যাল্পির পরিবর্তন ΔfH |
−704.2 kJ/mol[১][২] |
গিবসের মুক্ত শক্তি (ΔfG˚)
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-628.6 kJ/mol[১] |
ঔষধসংক্রান্ত | |
ATC code | |
ঝুঁকি প্রবণতা | |
জিএইচএস চিত্রলিপি | [৩] |
জিএইচএস সাংকেতিক শব্দ | বিপদজনক |
জিএইচএস বিপত্তি বিবৃতি | H314[৩] |
জিএইচএস সতর্কতামূলক বিবৃতি | P280, P310, P305+351+338[৩] |
এনএফপিএ ৭০৪ | |
প্রাণঘাতী ডোজ বা একাগ্রতা (LD, LC): | |
LD৫০ (মধ্যমা ডোজ)
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anhydrous: 380 mg/kg, rat (oral) hexahydrate: 3311 mg/kg, rat (oral) |
যুক্তরাষ্ট্রের স্বাস্থ্য অনাবৃতকরণ সীমা (NIOSH): | |
PEL (অনুমোদনযোগ্য)
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none[৪] |
REL (সুপারিশকৃত)
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2 mg/m3[৪] |
IDLH (তাৎক্ষণিক বিপদ
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N.D.[৪] |
সম্পর্কিত যৌগ | |
অন্যান্য অ্যানায়নসমূহ
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Aluminium fluoride Aluminium bromide Aluminium iodide |
অন্যান্য ক্যাটায়নসমূহ
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Boron trichloride Gallium trichloride Indium(III) chloride Magnesium chloride |
সম্পর্কিত Lewis acids
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Iron(III) chloride Boron trifluoride |
সুনির্দিষ্টভাবে উল্লেখ করা ছাড়া, পদার্থসমূহের সকল তথ্য-উপাত্তসমূহ তাদের প্রমাণ অবস্থা (২৫ °সে (৭৭ °ফা), ১০০ kPa) অনুসারে দেওয়া হয়েছে। | |
যাচাই করুন (এটি কি ?) | |
তথ্যছক তথ্যসূত্র | |
Aluminium chloride (AlCl3) is the main compound of aluminium and chlorine. It is white, but samples are often contaminated with iron trichloride, giving it a yellow colour. The solid has a low melting and boiling point. It is mainly produced and consumed in the production of aluminium metal, but large amounts are also used in other areas of chemical industry. The compound is often cited as a Lewis acid. It is an example of an inorganic compound that "cracks" at mild temperature, reversibly changing from a polymer to a monomer.
Structure[সম্পাদনা]
AlCl3 adopts three different structures, depending on the temperature and the state (solid, liquid, gas). Solid AlCl3 is a sheet-like layered cubic close packed layers. In this framework, the Al centres exhibit octahedral coordination geometry.[৫] In the melt, aluminium trichloride exists as the dimer Al2Cl6, with tetracoordinate aluminium. This change in structure is related to the lower density of the liquid phase (1.78 g/cm3) vs solid aluminium trichloride (2.48 g/cm3). Al2Cl6 dimers are also found in the vapour phase. At higher temperatures, the Al2Cl6 dimers dissociate into trigonal planar AlCl3, which is structurally analogous to BF3. The melt conducts electricity poorly,[৬] unlike more ionic halides such as sodium chloride.
Reactions[সম্পাদনা]
Anhydrous aluminium chloride is a powerful Lewis acid, capable of forming Lewis acid-base adducts with even weak Lewis bases such as benzophenone and mesitylene.[৭] It forms tetrachloroaluminate AlCl4− in the presence of chloride ions.
Aluminium chloride reacts with calcium and magnesium hydrides in tetrahydrofuran forming tetrahydroaluminates.
Reactions with water[সম্পাদনা]
Aluminium chloride is hygroscopic, having a very pronounced affinity for water. It fumes in moist air and hisses when mixed with liquid water as the Cl− ions are displaced with H2O molecules in the lattice to form the hexahydrate AlCl3·6H2O (also white to yellowish in color). The anhydrous phase cannot be regained on heating as HCl is lost leaving aluminium hydroxide or alumina (aluminium oxide):
- Al(H2O)6Cl3 → Al(OH)3 + 3 HCl + 3 H2O
On strong heating (~400°C), the aluminium oxide is formed from the aluminium hydroxide via:
- 2 Al(OH)3 → Al2O3 + 3 H2O
Aqueous solutions of AlCl3 are ionic and thus conduct electricity well. Such solutions are found to be acidic, indicative of partial hydrolysis of the Al3+ ion. The reactions can be described (simplified) as:
- [Al(H2O)6]3+ ⇌ [Al(OH)(H2O)5]2+ + H+
Aqueous solutions behave similarly to other aluminium salts containing hydrated Al3+ ions, giving a gelatinous precipitate of aluminium hydroxide upon reaction with dilute sodium hydroxide:
- AlCl3 + 3 NaOH → Al(OH)3 + 3 NaCl
Synthesis[সম্পাদনা]
Aluminium chloride is manufactured on a large scale by the exothermic reaction of aluminium metal with chlorine or hydrogen chloride at temperatures between ৬৫০ থেকে ৭৫০ °সে (১,২০২ থেকে ১,৩৮২ °ফা).[৬]
- 2 Al + 3 Cl2 → 2 AlCl3
- 2 Al + 6 HCl → 2 AlCl3 + 3 H2
Aluminum chloride may be formed via a single displacement reaction between copper chloride and aluminum metal.
- 2Al +3 CuCl2 →2AlCl3 + 3Cu
In the US in 1993, approximately 21,000 tons were produced, not counting the amounts consumed in the production of aluminium.[৮]
Hydrated aluminium trichloride is prepared by dissolving aluminium oxides in hydrochloric acid. Metallic aluminum also readily dissolves in Hydrochloric acid ─ releasing hydrogen gas and generating considerable heat. Heating this solid does not produce anhydrous aluminium trichloride, the hexahydrate decomposes to aluminium oxide when heated to ৩০০ °সে (৫৭২ °ফা):[৮]
- 2 AlCl3 + 3 H2O → Al2O3 + 6 HCl
Aluminium also forms a lower chloride, aluminium(I) chloride (AlCl), but this is very unstable and only known in the vapour phase.[৬]
Uses[সম্পাদনা]
Anhydrous aluminium trichloride[সম্পাদনা]
AlCl3 is probably the most commonly used Lewis acid and also one of the most powerful. It finds application in the chemical industry as a catalyst for Friedel–Crafts reactions, both acylations and alkylations. Important products are detergents and ethylbenzene. It also finds use in polymerization and isomerization reactions of hydrocarbons.
The Friedel–Crafts reaction[৭] is the major use for aluminium chloride, for example in the preparation of anthraquinone (for the dyestuffs industry) from benzene and phosgene.[৬] In the general Friedel–Crafts reaction, an acyl chloride or alkyl halide reacts with an aromatic system as shown:[৭]
The alkylation reaction is more widely used than the acylation reaction, although its practice is more technically demanding because the reaction is more sluggish. For both reactions, the aluminium chloride, as well as other materials and the equipment, should be dry, although a trace of moisture is necessary for the reaction to proceed.[তথ্যসূত্র প্রয়োজন] A general problem with the Friedel–Crafts reaction is that the aluminium chloride catalyst sometimes is required in full stoichiometric quantities, because it complexes strongly with the products. This complication sometimes generates a large amount of corrosive waste. For these and similar reasons, more recyclable or environmentally benign catalysts have been sought. Thus, the use of aluminium trichloride in some applications is being displaced by zeolites.
Aluminium chloride can also be used to introduce aldehyde groups onto aromatic rings, for example via the Gattermann-Koch reaction which uses carbon monoxide, hydrogen chloride and a copper(I) chloride co-catalyst.[৯]
Aluminium chloride finds a wide variety of other applications in organic chemistry.[১০] For example, it can catalyse the "ene reaction", such as the addition of 3-buten-2-one (methyl vinyl ketone) to carvone:[১১]
AlCl3 is also widely used for polymerization and isomerization reactions of hydrocarbons. Important examples include the manufacture of ethylbenzene, which used to make styrene and thus polystyrene, and also production of dodecylbenzene, which is used for making detergents.[৬]
Aluminium chloride combined with aluminium in the presence of an arene can be used to synthesize bis(arene) metal complexes, e.g. bis(benzene)chromium, from certain metal halides via the so-called Fischer-Hafner synthesis.
Hydrated aluminium chlorides[সম্পাদনা]
The hexahydrate has few applications, but aluminium chlorohydrate is a common component in antiperspirants at low concentrations.[৮] Hyperhidrosis sufferers need a much higher concentration (12% or higher), sold under such brand names as Xeransis, Drysol, DryDerm, sunsola, Maxim, Odaban, CertainDri, B+Drier, Chlorhydrol, Anhydrol Forte and Driclor.
Symmetry and Dipole moment[সম্পাদনা]
Aluminium chloride belongs to the point group D3h in its monomeric form and D2h in its dimeric form. Both forms of aluminium chloride, however, do not possess a dipole moment because the bond dipole moments cancel each other out.
Safety[সম্পাদনা]
Anhydrous AlCl3 reacts vigorously with bases, so suitable precautions are required. It can cause irritation to the eyes, skin, and the respiratory system if inhaled or on contact.[১২]
Aluminum chloride has been established as a neurotoxin.[১৩][১৪][১৫][১৬]
References[সম্পাদনা]
- ↑ ক খ গ ঘ ঙ http://chemister.ru/Database/properties-en.php?dbid=1&id=353
- ↑ ক খ Zumdahl, Steven S. (২০০৯)। Chemical Principles 6th Ed.। Houghton Mifflin Company। আইএসবিএন 0-618-94690-X।
- ↑ ক খ গ Sigma-Aldrich Co. Retrieved on 2014-05-05.
- ↑ ক খ গ "NIOSH Pocket Guide to Chemical Hazards #0024" (ইংরেজি ভাষায়)। ন্যাশনাল ইনস্টিটিউট ফর অকুপেশনাল সেফটি অ্যান্ড হেলথ (NIOSH)।
- ↑ In contrast, AlBr3 has a more molecular structure, with the Al3+ centers occupying adjacent tetrahedral holes of the close-packed framework of Br− ions.A. F. Wells, Structural Inorganic Chemistry, Oxford Press, Oxford, United Kingdom, 1984.
- ↑ ক খ গ ঘ ঙ N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, Pergamon Press, Oxford, United Kingdom, 1984.
- ↑ ক খ গ G. A. Olah (ed.), Friedel-Crafts and Related Reactions, Vol. 1, Interscience, New York, 1963.
- ↑ ক খ গ Otto Helmboldt, L. Keith Hudson, Chanakya Misra, Karl Wefers, Wolfgang Heck, Hans Stark, Max Danner, Norbert Rösch "Aluminum Compounds, Inorganic" in Ullmann's Encyclopedia of Industrial Chemistry 2007, Wiley-VCH, Weinheim.ডিওআই:10.1002/14356007.a01_527.pub2
- ↑ L. G. Wade, Organic Chemistry, 5th edition, Prentice Hall, Upper Saddle River, New Jersey, United States, 2003.
- ↑ P. Galatsis, in: Handbook of Reagents for Organic Synthesis: Acidic and Basic Reagents, (H. J. Reich, J. H. Rigby, eds.), pp. 12–15, Wiley, New York, 1999.
- ↑ B. B. Snider (১৯৮০)। "Lewis-acid catalyzed ene reactions"। Acc. Chem. Res.। 13 (11): 426। ডিওআই:10.1021/ar50155a007।
- ↑ http://www.solvaychemicals.us/static/wma/pdf/5/1/1/8/ALCL.pdf
- ↑ He BP, Strong MJ (জানুয়ারি ২০০০)। "A morphological analysis of the motor neuron degeneration and microglial reaction in acute and chronic in vivo aluminum chloride neurotoxicity"। J. Chem. Neuroanat.। 17 (4): 207–15। ডিওআই:10.1016/S0891-0618(99)00038-1। পিএমআইডি 10697247।
- ↑ Zubenko GS, Hanin I (অক্টোবর ১৯৮৯)। "Cholinergic and noradrenergic toxicity of intraventricular aluminum chloride in the rat hippocampus"। Brain Res.। 498 (2): 381–4। ডিওআই:10.1016/0006-8993(89)91121-9। পিএমআইডি 2790490।
- ↑ Peng JH, Xu ZC, Xu ZX; ও অন্যান্য (আগস্ট ১৯৯২)। "Aluminum-induced acute cholinergic neurotoxicity in rat"। Mol. Chem. Neuropathol.। 17 (1): 79–89। ডিওআই:10.1007/BF03159983। পিএমআইডি 1388451।
- ↑ Banks, W.A.; Kastin, A.J. (১৯৮৯)। "Aluminum-induced neurotoxicity: alterations in membrane function at the blood–brain barrier"। Neurosci Biobehav Rev। 13 (1): 47–53। ডিওআই:10.1016/S0149-7634(89)80051-X। পিএমআইডি 2671833।
External links[সম্পাদনা]
- International Chemical Safety Card 1125
- Index of Organic Synthesis procedures that utilize AlCl3
- The period 3 chlorides
- MSDS
- Government of Canada Fact Sheets and Frequently Asked Questions: Aluminum Salts
Aw
এটি Shuvo Mazumder-এর ব্যবহারকারী খেলাঘর। ব্যবহারকারী খেলাঘর হচ্ছে ব্যবহারকারী'র ব্যবহারকারী পাতার একটি উপপাতা। এটি ব্যবহারকারীর জন্য একটি তৎক্ষণাৎ পরীক্ষা এবং পাতা উন্নয়নের স্থান হিসেবে কাজ করে এবং এটি বিশ্বকোষীয় নিবন্ধ নয়। আপনি এখানে নিজস্ব খেলাঘর তৈরি করতে বা সম্পাদনা করতে পারেন। অন্যান্য খেলাঘরগুলি: প্রধান খেলাঘর | খেলাঘর ২, খেলাঘর ৩ | টেমপ্লেট খেলাঘর একটি নিবন্ধ লিখেছেন এবং তা সৃষ্টির অনুরোধ করতে প্রস্তুত? |