Rhodizonic acid is a chemical compound with formula H2C6O6 or (CO)4(COH)2. It can be seen as a twofold enol and fourfold ketone of cyclohexene, more precisely 5,6-dihydroxycyclohex-5-ene-1,2,3,4-tetrone.
Rhodizonic acid is usually obtained in the form of a dihydrateH2C6O6·2H2O. The latter is actually 2,3,5,5,6,6-hexahydroxycyclohex-2-ene-1,4-dione, where two of the original ketone groups are replaced by two pairs of geminal diols. The orange to deep-red and highly hygroscopic anhydrous acid can be obtained by low-pressure sublimation of the dihydrate.[1][2]
Like many other enols, rhodizonic acid can lose the hydrogen cationsH+ from the hydroxyls (pKa1 = 4.378±0.009, pKa2 = 4.652±0.014 at 25 °C),[3] yielding the hydrogen rhodizonate anion HC6O−6 and the rhodizonate anion C6O2−6. The latter is aromatic and symmetric, as the double bond and the negative charges are delocalized and evenly distributed over the six CO units. Rhodizonates tend to have various shades of red, from yellowish to purplish.
Rhodizonic acid has been used in chemical assays for barium, lead, and other metals.[4] In particular, the sodium rhodizonate test can be used to detect gunshot residue (which contains lead) in a subject's hands,[5] and to distinguish arrow wounds from gunshot wounds for hunting regulation enforcement.[6]
History
Rhodizonic acid was discovered by Austrian chemist Johann Heller in 1837, by analyzing the products of heating a mixture of potassium carbonate and charcoal.[7][8][9] The name comes from Greekῥοδίζω (rhodizō, "to tinge red"),[10] on account of the color of its salts.
Chemistry
Salts
Rhodizonates tend to have various shades of red, from yellowish to purplish, in transmitted light, with a greenish luster in reflected light.
Potassium rhodizonate can be prepared with good yield and purity by oxidizing inositol with nitric acid and reacting the result with potassium acetate in the presence of oxygen. The rhodizonate crystallizes out of the solution due to its relative insolubility in water.[11]
Sodium rhodizonate is dark brown and stable when dry,[12] but the aqueous solution decomposes in a few days, even in the refrigerator.[4]Lead rhodizonate is dark violet.[12][13]
Oxidation and decomposition
Rhodizonic acid is a member of a chain of oxidation products: benzenehexol(COH)6, tetrahydroxybenzoquinone (THBQ) (COH)4(CO)2, rhodizonic acid (COH)2(CO)4, and cyclohexanehexone(CO)6.[4] Lithium rhodizonate, together with salts of THBQ and benzenehexol, has been considered for possible use in rechargeable electrical batteries.[14] The monovalent anion C 6O− 6 has been detected in mass spectrometry experiments.[15]
Rhodizonic acid and the rhodizonate anion can lose one of the CO units to yield croconic acid(CO)3(COH)2 and the croconate anion C5O2−5, respectively, by mechanisms that are still imperfectly known. In basic solutions (pH > 10), rhodizonic acid quickly converts to the THBQ anion (CO)4−6 in the absence of oxygen, and to croconic acid in its presence. At pH 8.3 and exposure to light, solutions are stable for days in the absence of oxygen, and decompose to croconic acid and other products (possibly including cyclohexanehexone or dodecahydroxycyclohexane) in its presence.[16][17]
Structure
Acid
In solution, the acid and the hydrogen rhodizonate ion are mostly hydrated, with some of the carbonyl groups >C=O replaced by geminal hydroxyls, >C(OH)2.[3]
Salts
In anhydrous rubidium rhodizonate (Rb+)2[C6O6]2−, the rhodizonate anions are stacked in parallel columns, as are the rubidium ions. In the plane perpendicular to the columns, these are arranged as two interleaved hexagonal grids. The anions are planar.[2]
Anhydrous potassium rhodizonate (K+)2[C6O6]2− has a distinct but similar structure. The anions and cations are arranged in alternate planes. Within each plane, the anions are arranged in a hexagonal grid. Each potassium ion is arranged so that it connects symmetrically to eight oxygens of four anions, two from each adjacent plane. The anions are slightly twisted in the "boat" shape (with 0.108 Å of rms deviation from mean plane).[18] Sodium rhodizonate (Na+)2[C6O6]2− has the same structure, with slightly more distorted anions (0.113 Å rms)[19]
In solution, the rhodizonate anion is not hydrated.[3]
^Patton, E.; West, R. (1970). "New aromatic anions. VIII. Acidity constants of rhodizonic acid". Journal of Physical Chemistry. 74 (12): 2512–2518. doi:10.1021/j100706a018.
^ abBraga, D.; Cojazzi, G.; Maini, L.; Grepioni, F. (2001). "Reversible solid-state interconversion of rhodizonic acid H2C6O6 into H6C6O8 and the solid-state structure of the rhodizonate dianion C 6O2− 6 (aromatic or non-aromatic?)". New Journal of Chemistry. 25: 1221−1223. doi:10.1039/b107317f.
^ abcGelb, R. I.; Schwartz, L. M.; Laufer, D. A. (1978). "The structure of aqueous rhodizonic acid". Journal of Physical Chemistry. 82 (18): 1985–1988. doi:10.1021/j100507a006.
^ abcChalmers, R. A.; Telling, G. M. (1967). "A reassessment of rhodizonic acid as a qualitative reagent". Microchimica Acta. 55 (6): 1126–1135. doi:10.1007/BF01225955. S2CID98540174.
^Turner, E.; Gregory, W.; Parnell, E. A.; Liebig, J.; Rogers, J. B. (1846). Elements of Chemistry. Thomas, Cowperthwait & Co. Retrieved 2009-07-30. When potassium is heated in carbonic acid gas, combination takes place, and a dark olive powder is formed, composed of carbonic oxide and potassium, in the proportion C7O7+K3, or 7CO+3K. This substance is formed in large quantity in the preparation of potassium from carbonate of potash and charcoal, and is the source of great loss and inconvenience. No such compound is formed with sodium, for which reason that metal may be more cheaply prepared than potassium.
^Löwig, C. (1839). Chemie der organischen Verbindungen [Chemistry of Organic Compounds]. Zürich: F. Schultess.
^Preisler, P. W.; Berger, L. (1942). "Preparation of Tetrahydroxyquinone and Rhodizonic Acid Salts from the Product of the Oxidation of Inositol with Nitric Acid". Journal of the American Chemical Society. 64 (1): 67–69. doi:10.1021/ja01253a016.
^Chen, H.; Armand, M.; Courty, M.; Jiang, M.; Grey, C. P.; Dolhem, F.; Tarascon, J.-M.; Poizot, P. (2009). "Lithium salt of tetrahydroxybenzoquinone: toward the development of a sustainable Li-ion battery". Journal of the American Chemical Society. 131 (25): 8984–8. doi:10.1021/ja9024897. PMID19476355.
^Wyrwas, R. B.; Chick Jarrold, C. (2006). "Production of C 6O− 6 from oligomerization of CO on molybdenum anions". Journal of the American Chemical Society. 128 (42): 13688–9. doi:10.1021/ja0643927. PMID17044687.
