Gold(III) chloride

Gold(III) chloride
Names
IUPAC name
Gold(III) trichloride
Other names
Auric chloride
Gold trichloride
Identifiers
13453-07-1 YesY
ChEBI CHEBI:30076 YesY
ChemSpider 24244 N
Jmol interactive 3D Image
PubChem 26030
RTECS number MD5420000
UNII 15443PR153 YesY
Properties
AuCl3
(exists as Au2Cl6)
Molar mass 303.325 g/mol
Appearance Red crystals (anhydrous); golden, yellow crystals (monohydrate)[1]
Density 4.7 g/cm3
Melting point 254 °C (489 °F; 527 K) (decomposes)
68 g/100 ml (cold)
Solubility soluble in ether, slightly soluble in liquid ammonia
Structure
monoclinic
Square planar
Hazards
Main hazards Irritant
Safety data sheet See: data page
R-phrases R36/37/38
S-phrases S26 S36
Related compounds
Other anions
 Gold(III) fluoride
Gold(III) bromide
Other cations
 Gold(I) chloride
Silver(I) chloride
Platinum(II) chloride
Mercury(II) chloride
Supplementary data page
Refractive index (n),
Dielectric constant (εr), etc.
Thermodynamic
data
 Phase behaviour
solid–liquid–gas
UV, IR, NMR, MS
N verify (what is YesYN ?)
Infobox references

Gold(III) Chloride, traditionally called auric chloride, is a chemical compound of gold and chlorine. With the molecular formula AuCl3, the name gold trichloride is a simplification, referring to the empirical formula. The Roman numerals in the name indicate that the gold has an oxidation state of +3, which is common for gold compounds. There is also another related chloride of gold, gold(I) chloride (AuCl). Chloroauric acid, HAuCl4, the product formed when gold dissolves in aqua regia, is sometimes referred to as "gold chloride" or "acid gold trichloride". Gold(III) chloride is very hygroscopic and highly soluble in water as well as ethanol. It decomposes above 160 °C or in light.

Structure

AuCl3 exists as a chloride-bridged dimer both as a solid and as a vapour, at least at low temperatures.[2] Gold(III) bromide behaves analogously.[1] The structure is similar to that of iodine(III) chloride.

In gold(III) chloride, each Gold center is square planar,[1] which is typical of a metal complex with a d8 electron count. The bonding in AuCl3 is considered somewhat covalent.

Preparation

Gold(III) chloride is most often prepared by passing chlorine gas over gold powder at 180 °C:[1]

2 Au + 3 Cl2 → 2 AuCl3

Another method of preparation is by reacting Au3+ species with chloride to produce tetrachloroaurate. Its acid, chloroauric acid, is then heated to eliminate hydrogen chloride gas. Reaction with aqua regia produces gold(III) chloride:

Au(s) + 3 NO−
3(aq) + 6 H+(aq) ⇌ Au3+(aq) + 3 NO2(g) + 3 H2O(l)
Au3+(aq) + 3 NOCl(g) + 3 NO−
3(aq) → AuCl3(aq) + 6 NO2(g)
AuCl3(aq) + Cl−(aq) ⇌ AuCl−
4(aq)
2 HAuCl4(s) → Au2Cl6(s) + 2 HCl(g)

Reactions

On contact with water, AuCl
3 forms acidic hydrates and the conjugate base [AuCl
3(OH)]−
. It may be reduced by Fe2+
 causes elemental gold to be precipitated from solution.[1]

Anhydrous AuCl3 begins to decompose to AuCl at around 160 °C; however, this in turn undergoes disproportionation at higher temperatures to give gold metal and AuCl3.

AuCl3 → AuCl + Cl2 (>160 °C)
3 AuCl → AuCl3 + 2 Au (>420 °C)

AuCl3 is Lewis acidic and readily forms complexes. For example, it reacts with hydrochloric acid to form chloroauric acid (HAuCl
4):

HCl + AuCl
3 (aq) → H+
 + [AuCl
4]−

Other chloride sources, such as KCl, also convert AuCl3 into AuCl−
4. Aqueous solutions of AuCl3 react with aqueous base such as sodium hydroxide to form a precipitate of Au(OH)3, which will dissolve in excess NaOH to form sodium aurate (NaAuO2). If gently heated, Au(OH)3 decomposes to gold(III) oxide, Au2O3, and then to gold metal.[3][4][5][6][7]

Gold(III) chloride is the starting point for the synthesis of many other gold compounds. For example, reaction with potassium cyanide produces the water-soluble complex, K[Au(CN)4]:

AuCl
3 + 4 KCN → K[Au(CN)
4] + 3 KCl

Applications in organic synthesis

AuCl3 has attracted the interest of organic chemists as a mild acid catalyst for a variety reactions,[8] although no transformations have been commercialized. Gold(III) salts, especially Na[AuCl4] (prepared from AuCl3 + NaCl), provide an alternative to mercury(II) salts as catalysts for reactions involving alkynes. An illustrative reaction is the hydration of terminal alkynes to produce methylketones:[9]

Some alkynes undergo amination in the presence of gold(III) catalysts. Gold catalyses the alkylation of certain aromatic rings and a conversion of furans to phenols. For example, in acetonitrile solution, gold(III) chloride catalyses the alkylation of 2-methylfuran (sylvan) by methyl vinyl ketone at the 5-position:

The efficiency of this organogold reaction is noteworthy because both the furan and the ketone are sensitive to side-reactions such as polymerisation under acidic conditions. In some cases where alkynes are present, phenols sometimes form:[10]

This reaction involves a rearrangement that gives a new aromatic ring.[11]

References

  1. 1 2 3 4 5 Egon Wiberg; Nils Wiberg; A. F. Holleman (2001). Inorganic Chemistry (101 ed.). Academic Press. pp. 1286–1287. ISBN 0-12-352651-5.
  2. ↑ E. S. Clark; D. H. Templeton; C. H. MacGillavry (1958). "The crystal structure of gold(III) chloride". Acta Crystallogr. 11 (4): 284–288. doi:10.1107/S0365110X58000694. Retrieved 2010-05-21.
  3. ↑ N. N. Greenwood, A. Earnshaw, Chemistry of the Elements, 2nd ed., Butterworth-Heinemann, Oxford, UK, 1997
  4. ↑ Handbook of Chemistry and Physics, 71st edition, CRC Press, Ann Arbor, Michigan, 1990
  5. ↑ The Merck Index. An Encyclopaedia of Chemicals, Drugs and Biologicals. 14. Ed., 2006, p. 780, ISBN 978-0-911910-00-1.
  6. ↑ H. Nechamkin, The Chemistry of the Elements, McGraw-Hill, New York, 1968
  7. ↑ A. F. Wells, Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984
  8. ↑ G. Dyker, An Eldorado for Homogeneous Catalysis?, in Organic Synthesis Highlights V, H.-G. Schmaltz, T. Wirth (eds.), pp 48−55, Wiley-VCH, Weinheim, 2003
  9. ↑ Y. Fukuda and K. Utimoto (1991). "Effective transformation of unactivated alkynes into ketones or acetals with a gold(III) catalyst". J. Org. Chem. 56 (11): 3729. doi:10.1021/jo00011a058.
  10. ↑ A. S. K. Hashmi, T. M. Frost and J. W. Bats (2000). "Highly Selective Gold-Catalyzed Arene Synthesis". J. Am. Chem. Soc. 122 (46): 11553. doi:10.1021/ja005570d.
  11. ↑ A. Stephen, K. Hashmi, M. Rudolph, J. P. Weyrauch, M. Wölfle, W. Frey and J. W. Bats (2005). "Gold Catalysis: Proof of Arene Oxides as Intermediates in the Phenol Synthesis". Angewandte Chemie International Edition 44 (18): 2798–801. doi:10.1002/anie.200462672. PMID 15806608.
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