Gold(III) chloride



Structure
IUPAC name Gold(III) chloride
Other names Auric chloride
Gold trichloride
Identifiers
CAS number 13453-07-1
RTECS number MD5420000 (anhydrous)
Properties
Molecular formula AuCl3
(exists as Au2Cl6)
Molar mass 303.325 g/mol (anhydrous)
Appearance Red crystalline solid
Density 3.9 g/cm3 (solid)
Melting point

254 °C (527 K)
(decomposes)

Solubility in water 68 g/100 ml (cold)
Structure
Crystal structure monoclinic
Coordination
geometry
Square planar
Hazards
MSDS External MSDS
Main hazards Irritant
R-phrases R36/37/38
S-phrases Template:S26-36
Related Compounds
Other anions Gold(III) fluoride
Gold(III) bromide
Other cations Mercury(II) chloride
Supplementary data page
Structure and
properties
εr, etc.
Thermodynamic
data
Phase behaviour
Solid, liquid, gas
Spectral data MS
Except where noted otherwise, data are given for
materials in their standard state
(at 25 °C, 100 kPa)

Infobox disclaimer and references

Gold(III) chloride, traditionally called auric chloride, is one of the most common aqua regia, is sometimes referred to rather loosely as "gold chloride", "acid gold trichloride" or even "gold(III) chloride trihydrate".

Gold(III) chloride is very ligands.

Structure


AuCl3 exists as a dimer both as a solid and as a vapour; the bromide AuBr3 follows the same pattern. Each Au center is square planar. This structure is reminiscent of the bitetrahedral structures adopted by electronegativity (for a metal) of gold.

Chemical properties

disproportionation at higher temperatures to give gold metal and AuCl3.

AuCl3 → AuCl + Cl2 (>160 °C)

3 AuCl → AuCl3 + 2 Au (>420 °C)

AuCl3 is a hydrochloric acid, chloroauric acid (HAuCl4) is formed:

HCl(aq) + AuCl3(aq) → H+AuCl4(aq)

Ionic chlorides such as KCl will also form the AuCl4 ion with AuCl3.

Aqueous solutions of AuCl3 react with alkalis such as precipitate of impure 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.[1][2][3][4][5][6]

Preparation

Gold(III) chloride is most often prepared by direct chlorination of the metal at high temperatures:

2 Cl2 → 2 AuCl3

Uses

Gold(III) chloride is one of the most common gold compounds and it is therefore used as the starting point for the synthesis of many other gold compounds, for example the water-soluble complex KAu(CN)4:

AuCl3 + 4 KCl

Gold(III) ketones, for example:[7]


Ketones are generally formed in over 90% yield under these conditions. Also useful is the related amination of alkynes which can use gold(III) catalysis.

In recent years AuCl3 has begun to attract the interest of organic chemists as a mild acid catalyst for other reactions such as methyl vinyl ketone at the 5-position:


The reaction gives a 91% yield in only 40 minutes at room temperature, using only 1 mole% of AuCl3 in alkynes are present, a phenol may be formed:[8]


The reaction undergoes a complex rearrangement that leads to formation of the new aromatic ring[9]

Precautions

Gold(III) chloride should be handled wearing gloves and goggles; direct contact with the material should be avoided.

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. ^ H. Nechamkin, The Chemistry of the Elements, McGraw-Hill, New York, 1968
  5. ^ A. F. Wells, Structural Inorganic Chemistry, 5th ed., Oxford University Press, Oxford, UK, 1984
  6. ^ 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
  7. ^ Y. Fukuda, K. Utimoto, J. Org. Chem. 56, 3729-3731 (1991)
  8. ^ A. S. K. Hashmi, T. M. Frost, J. W. Bats, J. Am. Chem. Soc. 122, 11553-11554 (2000)
  9. ^ Hashmi, A. S. K.; Rudolph, M.; Weyrauch, J. P.; Wölfle, M.; Frey, W.; Bats, J. W. Angew. Chem. Int. Ed. 2005, 44, 2798-2801
 
This article is licensed under the GNU Free Documentation License. It uses material from the Wikipedia article "Gold(III)_chloride". A list of authors is available in Wikipedia.