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Acetylacetone is an organic compound with the chemical formula . It is classified as a 1,3-diketone. It exists in equilibrium with a tautomer . The mixture is a colorless liquid. These tautomers interconvert so rapidly under most conditions that they are treated as a single compound in most applications. Acetylacetone is a building block for the synthesis of many coordination complexes as well as heterocyclic compounds.
| 11.7 |
| 42 |
| 10 |
| 7.2 |
| 5.7 |
| 2 |
| 0.23 |
The keto and enol tautomers of acetylacetone coexist in solution. The enol form has C2v symmetry, meaning the hydrogen atom is shared equally between the two oxygen atoms. In the gas phase, the equilibrium constant, Kketo→enol, is 11.7, favoring the enol form. The two tautomeric forms can be distinguished by NMR spectroscopy, IR spectroscopy and other methods.
The equilibrium constant tends to be high in nonpolar solvents; when Kketo→enol is equal or greater than 1, the enol form is favoured. The keto form becomes more favourable in polar, hydrogen-bonding solvents, such as water. The enol form is a vinylogous analogue of a carboxylic acid.
| 9.8 |
| 12.5 |
| 10.16 |
| 13.41 |
Acetylacetone is a weak acid. It forms the acetylacetonate anion (commonly abbreviated ):
In the acetylacetonate anion, both bonds are equivalent. Both central bonds are equivalent as well, with one hydrogen atom bonded to the central carbon atom (the atom numbered C3 according to the IUPAC nomenclature of organic chemistry). These equivalencies are because there is a resonance between the four bonds in the O−C2−C3−C4−O linkage in the acetylacetonate anion. Each of the four bonds in the linkage has a bond order of about 1.5, and the two oxygen atoms equally share the negative charge. The acetylacetonate anion is a bidentate ligand. IUPAC recommended p Ka values for this equilibrium in aqueous solution at 25 °C are 8.99 ± 0.04 ( I = 0), 8.83 ± 0.02 ( I = 0.1 M ) and 9.00 ± 0.03 ( I = 1.0 M ; I = Ionic strength). Values for mixed solvents are available. Very strong bases, such as organolithium compounds, will deprotonate acetylacetone twice. The resulting dilithium species can then be alkylated at the carbon atom at the position 1.
Laboratory routes to acetylacetone also begin with acetone. Acetone and acetic anhydride () upon the addition of boron trifluoride () catalyst:
A second synthesis involves the base-catalyzed condensation (e.g., by sodium ethoxide ) of acetone and ethyl acetate, followed by acidification of the sodium acetylacetonate (e.g., by hydrogen chloride HCl):
Because of the ease of these syntheses, many analogues of acetylacetonates are known. Some examples are benzoylacetone, dibenzoylmethane and Butyl group analogue 2,2,6,6-tetramethyl-3,5-heptanedione. Trifluoroacetylacetone and hexafluoroacetylacetonate are also used to generate volatile .
Both oxygen atoms bind to the metal to form a six-membered chelate ring. In some cases the chelate effect is so strong that no added base is needed to form the complex.
Reactions
Condensations
Acetylacetone is a versatile bifunctional precursor to heterocycles because both keto groups may undergo condensation. For example, condensation with hydrazine produces while condensation with urea provides . Condensation with two aryl- or alkylamines gives , wherein the oxygen atoms in acetylacetone are replaced by NR (R = aryl, alkyl).
Coordination chemistry
Sodium acetylacetonate, Na(acac), is the precursor to many acetylacetonate complexes. A general method of synthesis is to treat a metal salt with acetylacetone in the presence of a base:
Biodegradation
The enzyme acetylacetone dioxygenase cleaves a central carbon-carbon bond of acetylacetone, producing acetate and Methylglyoxal. The enzyme is iron(II)-dependent, but it has been proven to bind to zinc as well. Acetylacetone degradation has been characterized in the bacterium Acinetobacter johnsonii.
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