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{{Short description|Ion}} |
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* Parameters work only in their own section. |
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* Parameters work only in their own section. |
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For more information, see ]. --> |
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For more information, see ]. --> |
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{{chembox |
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{{chembox |
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| verifiedrevid = 413309017 |
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| ImageFile = Tetrachloroaluminate-anion-2D-A.png |
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| ImageFile = Tetrachloroaluminate-anion-2D-A.png |
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| ImageSize = 150px |
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| ImageSize = 150px |
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| IUPACName = Tetrachloroaluminate(1–) |
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| IUPACName = Tetrachloroaluminate(1–) |
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| SystematicName = Tetrachloroaluminate(1-) |
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| OtherNames = |
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| OtherNames = |
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* Aluminate(1-), tetrachloro |
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| PubChem = |
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* tetrachloridoaluminate(1-) |
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| CASNo = |
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* tetrachloridoaluminate(1-); tetrachloroalumanuide |
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| SMILES = }} |
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* tetrachloroalumanuide |
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| Section2 = {{Chembox Properties |
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|Section1={{Chembox Identifiers |
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| Formula = AlCl<sub>4</sub><sup>–</sup> |
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| CASNo = 17611-22-2 |
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| CASNo_Ref = {{Cascite|changed|EPA}} |
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| ChEBI = 30110 |
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| ChemSpiderID = 10737456 |
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| DTXSID = DTXSID301336609 |
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| PubChem = 3728926 |
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| SMILES = Cl(Cl)(Cl)Cl |
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| StdInChI = InChI=1S/Al.4ClH/h;4*1H/q+3;;;;/p-4 |
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| StdInChIKey = BXILREUWHCQFES-UHFFFAOYSA-J |
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| InChI = InChI=1S/Al.4ClH/h;4*1H/q+3;;;;/p-4 |
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| InChIKey = BXILREUWHCQFES-UHFFFAOYSA-J |
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| Gmelin = 2297}} |
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|Section2={{Chembox Properties |
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| Formula = AlCl<sub>4</sub><sup>−</sup> |
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| Al=1 | Cl=4 |
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| Formula_Charge = -1 |
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| BoilingPt = |
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| Solubility = }} |
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| Solubility = }} |
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| Section3 = {{Chembox Hazards |
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|Section3={{Chembox Structure |
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| PointGroup = T<sub>d</sub> |
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| MainHazards = |
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| MolShape = ] |
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| FlashPt = |
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| OrbitalHybridisation = sp<sup>3</sup>}} |
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| Autoignition = }} |
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}}<!-- Text starts below--> |
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}}<!-- Text starts below--> |
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'''Tetrachloroaluminate''' <sup>−</sup> is a ] formed from ] and ]. The anion has a ] shape, similar to ] where carbon is replaced with aluminium. Some tetrachloroaluminates are soluble in organic solvents, creating an ionic non-aqueous solution, making them '''suitable''' as component of electrolytes for batteries. E.g. ] is used in some ]. |
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'''Tetrachloroaluminate''' <sup>−</sup> is an ] formed from ] and ]. The anion has a ] shape and is ] with ]. Some tetrachloroaluminates are soluble in organic solvents, creating an ionic non-aqueous solution, making them suitable as component of electrolytes for batteries. For example, ] is used in some ]. |
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== Formation == |
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] |
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Tetrachloroaluminate ions are formed as intermediates in the ] when ] is used as the catalyst. In the case of the Friedel]Crafts alkylation, the reaction can be broken into three steps as follows:<ref name="chemguide"/> |
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] |
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# The alkyl halide reacts with the strong Lewis acid to form an activated electrophile composed of the tetrachloroaluminate ion and the alkyl group. |
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#:] |
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# The aromatic ring (] in this case) reacts with the activated electrophile forming an alkylbenzenium carbocation. |
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# The alkylbenzenium carbocation reacts with a tetrachloroaluminate anion, regenerating the aromatic ring and the Lewis acid and forming ] (HCl). |
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#:] |
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A similar mechanism occurs in the Friedel-Crafts acylation.<ref>. Organic-chemistry.org. Retrieved on 2014-01-11.</ref> |
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== References == |
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{{inorganic-compound-stub}} |
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{{reflist|refs= |
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<ref name="chemguide">{{Cite web|title=electrophilic substitution - the alkylation of benzene|url=https://www.chemguide.co.uk/mechanisms/elsub/fcalkyl.html|access-date=2020-09-07|website=www.chemguide.co.uk}}</ref> |
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}} |
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] |
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] |
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] |