Zinc+chloride

Chemical Formula: ZnCl 2
 * There are nine crystalline forms known, which are colorless, white and highly soluble in water.
 * This molecule is a white crystalline, poisonous solid mostly used as a wood preservative, as well as in textile processing, metallurgical fluxes, parchment paper, and chemical synthesis. It is known for being highly water soluble.
 * Zinc chloride has a variety of uses including flux manufacture, water treatment and as an electrolyte in battery manufacture. Zinc chloride is also used in zinc plating, rubber and fiber vulcanization, textile finishing and for applications in food canning. It has a number of uses in personal care products and as an intermediate for fertilizers, antibiotics and catalysts.
 * A white, water-soluble crystalline compound, ZnCl2, used as a wood preservative, as a soldering flux, and for a variety of industrial purposes, including the manufacture of cements and paper parchment.

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 * It is a colorless crystal compound. It dissolves in water. It reacts with [|bases] to make [|zinc hydroxide].



Zinc Chloride Batteries

In the laboratory, zinc chloride finds wide use, principally as a moderate-strength [|Lewis acid]. It can [|catalyze] (A) the [|Fischer indole synthesis],[|[][|30][|]] and also (B) [|Friedel-Crafts acylation] reactions involving activated [|aromatic ring] Related to the latter is the classical preparation of the dye [|fluorescein] from [|phthalic anhydride] and [|resorcinol], which involves a [|Friedel-Crafts acylation].[|[][|33][|]] This transformation has in fact been accomplished using even the hydrated ZnCl2 sample shown in the picture above. [|Hydrochloric acid] alone reacts poorly with [|primary alcohols] and [|secondary alcohols], but a combination of HCl with ZnCl2 (known together as the "[|Lucas reagent]") is effective for the preparation of alkyl chlorides. Typical reactions are conducted at 130 °C. This reaction probably proceeds via an [|SN2 mechanism] with primary alcohols but [|SN1] pathway with secondary alcohols.
 * ~ Form ||~ Symmetry ||~ Pearson symbol ||~ Group ||~ No ||~ a (nm) ||~ b (nm) ||~ c (nm) ||~ Z ||~ ρ (g/cm3) ||
 * α || Tetragonal || tI12 || I 4 2d || 122 || 0.5398 || 0.5398 || 0.64223 || 4 || 3.00 ||
 * β || Tetragonal || tP6 || P42/nmc || 137 || 0.3696 || 0.3696 || 1.071 || 2 || 3.09 ||
 * γ || Monoclinic || mP36 || P21c || 14 || 0.654 || 1.131 || 1.23328 || 12 || 2.98 ||
 * δ || Orthorhombic || oP12 || Pna21 || 33 || 0.6125 || 0.6443 || 0.7693 || 4 || 2.98 ||

Anhydrous ZnCl2 can be prepared from zinc and [|hydrogen chloride]. Zn + 2 HCl → ZnCl2 + H2 Hydrated forms and aqueous solutions may be readily prepared similarly by treating Zn metal with hydrochloric acid. Zinc oxide and [|zinc sulfide] react with HCl: ZnS( [|s] ) + 2 [|HCl] (aq) → ZnCl2(aq) + [|H2S] ( [|g] )



[|Hydrochloric acid] alone reacts poorly with [|primary alcohols] and [|secondary alcohols], but a combination of HCl with ZnCl2 (known together as the " [|Lucas reagent] ") is effective for the preparation of alkyl chlorides. Typical reactions are conducted at 130 °C. This reaction probably proceeds via an [|SN2 mechanism] with primary alcohols but [|SN1] pathway with secondary alcohols.

It is a colorless crystal compound. It dissolves in water. It reacts with [|bases] to make [|zinc hydroxide].