Carborane acid
Carborane acids H are a class of superacids, some of which are estimated to be at least one million times stronger than 100% sulfuric acid in terms of their Hammett acidity function values and possess computed pKa values well below –20, establishing them as some of the strongest known Brønsted acids. The most well studied example is the highly chlorinated derivative H. The acidity of H was found to vastly exceed that of triflic acid, CF3SO3H, and bistriflimide, 2NH, compounds previously regarded as the strongest isolable acids.
Their high acidities stem from the extensive delocalization of their conjugate bases, carboranate anions, which are usually further stabilized by electronegative groups like Cl, F, and CF3. Due to the lack of oxidizing properties and the exceptionally low nucleophilicity and high stability of their conjugate bases, they are the only superacids known to protonate C60 fullerene without decomposing it. Additionally, they form stable, isolable salts with protonated benzene, C6H7+, the parent compound of the Wheland intermediates encountered in electrophilic aromatic substitution reactions.
The fluorinated carborane acid, H, is even stronger than chlorinated carborane acid. It is able to protonate butane to form tert-butyl cation at room temperature and is the only known acid to protonate carbon dioxide to give the bridged cation, +, making it possibly the strongest known acid. In particular, CO2 does not undergo observable protonation when treated with the mixed superacids HF-SbF5 or HSO3F-SbF5.
As a class, the carborane acids form the most acidic group of well-defined, isolable substances known, far more acidic than previously known single-component strong acids like triflic acid or perchloric acid. In certain cases, like the nearly perhalogenated derivatives mentioned above, their acidities rival those of the traditional mixed Lewis-Brønsted superacids like magic acid and fluoroantimonic acid..
Acidity
A Brønsted-Lowry acid’s strength corresponds with its ability to release a hydrogen ion. One common measure of acid strength for concentrated, superacidic liquid media is the Hammett acidity function, H0. Based on its ability to quantitatively protonate benzene, the chlorinated carborane acid H was conservatively estimated to have an H0 value at or below −18, leading to the common assertion that carborane acids are at least a million times stronger than 100% sulfuric acid. However, since the H0 value measures the protonating ability of a liquid medium, the crystalline and high-melting nature of these acids precludes direct measurement of this parameter. In terms of pKa, a slightly different measure of acidity defined as the ability of a given solute to undergo ionization in a solvent, carborane acids are estimated to have pKa values below −20, even without electron-withdrawing substituents on the boron atoms, with the fully fluorinated analog H having a calculated pKa of −46. The known acid H with one fewer fluorine is expected to be only slightly weaker.In the gas phase, H has a computed acidity of 216 kcal/mol, compared to an experimentally determined acidity of 241 kcal/mol for H. In contrast, HSbF6 has a computed gas phase acidity of 255 kcal/mol, while the previous experimentally determined record holder was 2NH, a congener of bistriflimide, at 291 kcal/mol. Thus, H is likely the most acidic substance so far synthesized in bulk, in terms of its gas phase acidicity. In view of its unique reactivity, it is also a strong contender for being the most acidic substance in the condensed phase. Some even more strongly acidic derivatives have been predicted, with gas phase acidities < 200 kcal/mol.
Carborane acids differ from classical superacids in being well-defined one component substances. In contrast, classical superacids are often mixtures of a Brønsted acid and Lewis acid. Despite being the strongest acid, the boron-based carborane acids are described as being "gentle", cleanly protonating weakly basic substances without further side reactions. Whereas conventional superacids decompose fullerenes due to their strongly oxidizing Lewis acidic component, carborane acid has the ability to protonate fullerenes at room temperature to yield an isolable salt. Furthermore, the anion that forms as a result of proton transfer is nearly completely inert. This property is what makes the carborane acids the only substances that are comparable in acidity to the mixed superacids that can also be stored in a glass bottle, as various fluoride-donating species are not present or generated.
History
Carborane acid was first discovered and synthesized by Professor Christopher Reed and his colleagues in 2004 at the University of California, Riverside. Prior to carborane acid's discovery, the long-standing record of “strongest acids as single isolable compounds” was held by the two superacids, fluorosulfonic acid and trifluoromethanesulfonic acid, with pKas of −14 and −16 respectively. The parent molecule from which carborane acid is derived, an icosahedral carboranate anion,, was first synthesized at DuPont in 1967 by Walter Knoth. Research into this molecule's properties was put on hiatus until the mid 1980s when the Czech group of boron scientists, Plešek, Štíbr, and Heřmánek improved the process for halogenation of carborane molecules. These findings were instrumental in developing the current procedure for carborane acid synthesis. The process consists of treating Cs+– with, refluxing under dry argon to fully chlorinate the molecule yielding carborane acid, but this has been shown to fully chlorinate only under select conditions.In 2010, Reed published a guide giving detailed procedures for the synthesis of carborane acids and their derivatives. Nevertheless, the synthesis of carborane acids remains lengthy and difficult and requires a well-maintained glovebox and some specialized equipment. The starting material is commercially available decaborane, a highly toxic substance. The most well-studied carborane acid H is prepared in 13 steps. The last few steps are especially sensitive and require a glovebox at < 1 ppm H2O without any weakly basic solvent vapors, since bases as weak as benzene or dichloromethane will react with carborane-based electrophiles and Brønsted acids. The final step of the synthesis is the metathesis of the μ-hydridodisilylium carboranate salt with excess liquid, anhydrous hydrogen chloride, presumably driven by the formation of strong Si–Cl and H–H bonds in the volatile byproducts:
The product was isolated by evaporation of the byproducts and was characterized by its infrared and nuclear magnetic resonance, 20.4 spectra. Although the reactions used in the synthesis are analogous, obtaining a pure sample of the more acidic H turned out to be even more difficult, requiring extremely rigorous procedures to exclude traces of weakly basic impurities.
Structure
Carborane acid consists of 11 boron atoms; each boron atom is bound to a chlorine atom. The chlorine atoms serve to enhance acidity and act as shields against attacks from the outside due to the steric hindrance they form around the cluster. The cluster, consisting of the 11 borons, 11 chlorines, and a single carbon atom, is paired with a hydrogen atom, bound to the carbon atom. The boron and carbon atoms are allowed to form six bonds due to boron’s ability to form three-center, two-electron bonds.Although the structure of the carborane acid differs greatly from conventional acids, both distribute charge and stability in a similar fashion. The carboranate anion distributes its charge by delocalizing the electrons throughout the 12 cage atoms. This was shown in a single crystal X-ray diffraction study revealing shortened bond lengths in the heterocyclic portion of the ring suggesting electronic delocalization.
The chlorinated carba-closo-dodecaborate anion is an outstandingly stable anion with what has previously been described as “substitutionally inert” B–Cl vertices. The descriptor closo indicates that the molecule is formally derived from a borane of stoichiometry and charge 2–. The cagelike structure formed by the 11 boron atoms and 1 carbon atom allows the electrons to be highly delocalized through the 3D cage, and the high energy required to disrupt the boron cluster portion of the molecule is what gives the anion its remarkable stability. Because the anion is extremely stable, it will not behave as a nucleophile toward the protonated substrate, while the acid itself is completely non-oxidizing, unlike the Lewis acidic components of many superacids like antimony pentafluoride. Hence, sensitive molecules like C60 can be protonated without decomposition.