Chromium(III) chloride

Chromium(III) chloride (also called chromic chloride) is a violet coloured solid with the formula CrCl₃.

Although it is ionic, the solid state structure is kinetically inert so that anhydrous CrCl₃ is surprisingly reluctant to dissolve in water. However, in the presence of a trace of a reducing agent capable of reducing Cr³⁺ to Cr²⁺, the CrCl₃ dissolves rapidly to form soluble complexes containing hydrated Cr³⁺ ions. The common commercial form of the hydrate is the dark green complex shown in the picture, [CrCl₂(H₂O)₄]Cl.2H₂O, but two other forms are known, viz., pale green [CrCl(H₂O)₅]Cl₂.H₂O and violet [Cr(H₂O)₆]Cl₃.

This inertness means that CrCl₃ is generally sluggish to react without the presence of a reducing agent. When it does react it undergoes ligand substitution reactions to form other complexes of chromium(III). It reacts as a Lewis acid, forming stable chloro complexes such as [CrCl₆]^3-.

Additional recommended knowledge

Recognize and detect the effects of electrostatic charges on your balance

Weighing the right way

Guide to balance cleaning: 8 simple steps

Chemical properties

Chromium(III) chloride is a Lewis acid, classified as "hard" according to the Hard-Soft Acid-Base theory. However it is also a chloro complex which is quite inert to substitution, so in fact it is ordinarily quite unreactive. The low reactivity of the d³ Cr³⁺ ion can be explained using crystal field theory. One way of opening CrCl₃ up to substitution in solution is to reduce even a trace amount to CrCl₂, for example using zinc in hydrochloric acid. This chromium(II) compound undergoes substitution easily, and it can exchange electrons with CrCl₃ via a chloride bridge, allowing all of the CrCl₃ to react quickly.

The most common form of CrCl₃ sold commercially is a dark green hexahydrate with the structure [CrCl₂(H₂O)₄]Cl.2H₂O, and like the anhydrous form it is also very inert towards substitution.

If substitution reactions are performed in the presence of a trace of Cr²⁺, then CrCl₃ can undergo substitution with ligands such as water (giving violet [Cr(H₂O)₆]³⁺) or pyridine:

CrCl₃ + 3 C₅H₅N → [CrCl₃(C₅H₅N)₃]

Such complexes are usually octahedral.

With molten alkali metal chlorides such as potassium chloride, CrCl₃ gives octahedral complexes of the type K₃CrCl₆, as well as K₃Cr₂Cl₉ which is also octahedral but where the two chromiums are linked via three chloride bridges.

Preparation

Anhydrous chromium(III) chloride may be prepared from chromium metal and chlorine directly, or indirectly using chromium(III) oxide with carbon and chlorine at 800 °C^[4]:

Cr₂O₃(s) + 3 C(s) + 3 Cl₂(g) → 2 CrCl₃(s) + 3 CO(g)

It may also be prepared from the hexahydrate, by heating with thionyl chloride which reacts with the water of hydration.

The hydrated chloride may be made by dissolving the metal in hydrochloric acid.

Uses

Chromium(III) chloride is used as the source of chromium for many inorganic compounds of chromium, for example dibenzenechromium(0), an analogue of ferrocene:

A significant use of CrCl₃ in organic synthesis is for the in situ preparation of chromium(II) chloride, a popular reagent for (A) reduction of alkyl halides and for (B) the synthesis of (E)-alkenyl halides. The reaction is usually performed using two moles of CrCl₃ 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.⁸ it has a tae

Precautions

Although trivalent chromium is far less poisonous than hexavalent, chromium salts are generally considered highly toxic. Avoid ingestion and inhalation of dust. Wear gloves and goggles.

References

1. N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997.
2. Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990.
3. The Merck Index, 7th edition, Merck & Co, Rahway, New Jersey, USA, 1960.
4. D. Nicholls, Complexes and First-Row Transition Elements, Macmillan Press, London, 1973.
5. A. F. Wells, 'Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984.
6. J. March, Advanced Organic Chemistry, 4th ed., p. 723, Wiley, New York, 1992.
7. 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.
8. Calvet, G.; Dussaussois, M.; Blanchard, N.; Kouklovsky, C. Organic Letters 2004, 6, 2449-2451.