chromium(III) chloride

Chromium(III) chloride (also called chromic chloride) is an inorganic chemical compound with the chemical formula . This crystalline salt forms several hydrates with the formula , among which are hydrates where ''n'' can be 5 (chromium(III) chloride pentahydrate ) or 6 (chromium(III) chloride hexahydrate ). The anhydrous compound with the formula are violet crystals, while the most common form of the chromium(III) chloride are the dark green crystals of hexahydrate, . Chromium chlorides find use as catalysts and as precursors to dyes for wool.

Structure

Anhydrous chromium(III) chloride adopts the structure, with occupying one third of the octahedral interstices in alternating layers of a pseudo- cubic close packed lattice of ions. The absence of cations in alternate layers leads to weak bonding between adjacent layers. For this reason, crystals of cleave easily along the planes between layers, which results in the flaky (micaceous) appearance of samples of chromium(III) chloride. The anhydrous is exfoliable down to the monolayer limit. If pressurized to 9.9 GPa it goes under a phase transition.

File:Chromium(III)-chloride-sheet-from-monoclinic-xtal-3D-balls-SF-overlay.png, Space-filling model of cubic close packing of chloride ions in the crystal structure of
File:Chromium(III)-chloride-sheet-from-monoclinic-xtal-3D-balls.png, Ball-and-stick model of part of a layer
File:Chromium(III)-chloride-layers-stacking-from-monoclinic-xtal-3D-balls.png, Stacking of layers

Chromium(III) chloride hydrates

The hydrated chromium(III) chlorides display the somewhat unusual property of existing in a number of distinct chemical forms (isomers), which differ in terms of the number of chloride anions that are coordinated to Cr(III) and the water of crystallization. The different forms exist both as solids and in aqueous solutions. Several members are known of the series of . The common hexahydrate can be more precisely described as . It consists of the cation ''trans''- and additional molecules of water and a chloride anion in the lattice. Two other hydrates are known, pale green and violet . Similar hydration isomerism is seen with other chromium(III) compounds.

Preparation

Anhydrous chromium(III) chloride may be prepared by chlorination of chromium metal directly, or indirectly by carbothermic chlorination of chromium(III) oxide at 650–800 °C

:

The hydrated chlorides are prepared by treatment of chromate with hydrochloric acid and aqueous methanol.

Reactions

Slow reaction rates are common with chromium(III) complexes. The low reactivity of the d³ ion can be explained using crystal field theory. One way of opening up to substitution in solution is to reduce even a trace amount to , for example using zinc in hydrochloric acid. This chromium(II) compound undergoes substitution easily, and it can exchange electrons with via a chloride bridge, allowing all of the to react quickly. With the presence of some chromium(II), solid dissolves rapidly in water. Similarly, ligand substitution reactions of solutions of are accelerated by chromium(II) catalysts.

With molten alkali metal chlorides such as potassium chloride, gives salts of the type and , which is also octahedral but where the two chromiums are linked via three chloride bridges.

The hexahydrate can also be dehydrated with thionyl chloride:
:

Complexes with organic ligands

is a Lewis acid, classified as "hard" according to the Hard-Soft Acid-Base theory. It forms a variety of adducts of the type , where L is a Lewis base. For example, it reacts with pyridine () to form the pyridine complex:
:

Treatment with trimethylsilylchloride in THF gives the anhydrous THF complex:
:

Precursor to organochromium complexes

Chromium(III) chloride is used as the precursor to many organochromium compounds, for example bis(benzene)chromium, an analogue of ferrocene:

:

Phosphine complexes derived from catalyse the trimerization of ethylene to 1-hexene.

Use in organic synthesis

One niche use of in organic synthesis is for the ''in situ'' preparation of chromium(II) chloride, a reagent for the reduction of alkyl halides and for the synthesis of (''E'')-alkenyl halides. The reaction is usually performed using two moles of per mole of lithium aluminium hydride, although if aqueous acidic conditions are appropriate zinc and hydrochloric acid may be sufficient.

:

Chromium(III) chloride has also been used as a Lewis acid in organic reactions, for example to catalyse the nitroso Diels-Alder reaction.

Dyestuffs

A number of chromium-containing dyes are used commercially for wool. Typical dyes are triarylmethanes consisting of ortho-hydroxylbenzoic acid derivatives.Thomas Gessner and Udo Mayer "Triarylmethane and Diarylmethane Dyes" in Ullmann's Encyclopedia of Industrial Chemistry 2002, Wiley-VCH, Weinheim.

Precautions

Although trivalent chromium is far less poisonous than hexavalent, chromium salts are generally considered toxic.

References

Further reading

*''Handbook of Chemistry and Physics'', 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
*''The Merck Index'', 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
*J. March, ''Advanced Organic Chemistry'', 4th ed., p. 723, Wiley, New York, 1992.
*K. Takai, in ''Handbook of Reagents for Organic Synthesis, Volume 1: Reagents, Auxiliaries and Catalysts for C-C Bond Formation'', (R. M. Coates, S. E. Denmark, eds.), pp. 206–211, Wiley, New York, 1999.

External links

International Chemical Safety Card 1316
(anhydr. CrCl₃)

(CrCl₃·6H₂O)

* ttps://www.cdc.gov/niosh/npg/npgd0140.html NIOSH Pocket Guide to Chemical Hazardsbr>IARC Monograph "Chromium and Chromium compounds"

{{Chlorides

Chromium(III) compounds
Chlorides
Metal halides
Coordination complexes