|Jmol interactive 3D||Image
|Molar mass||136.24 g·mol−1|
|Appearance||White to off-white powder|
|Density||1.08 g/cm3 (20 °C), solid|
|Melting point||270 °C (518 °F; 543 K)|
|Solubility in other solvents||Soluble in hydrocarbons|
Refractive index (nD)
|cubic, space group Fm3m|
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
|what is ?)(|
Adamantane is a colorless, crystalline chemical compound with a camphor-like odor. With a formula C10H16, it is a cycloalkane and also the simplest diamondoid. Adamantane molecules consist of four connected cyclohexane rings arranged in the "armchair" configuration. It is unique in that it is both rigid and virtually stress-free. A boat-shaped configuration can also exist. Adamantane is the most stable among all the isomers with formula C10H16, which include the somewhat similar twistane. The spatial arrangement of carbon atoms in adamantane molecule is the same as in the diamond crystal. This motivates the name adamantane, which is derived from the Greek adamantinos (relating to steel or diamond).
The discovery of adamantane in petroleum in 1933 launched a new field of chemistry dedicated to studying the synthesis and properties of polyhedral organic compounds. Adamantane derivatives have found practical application as drugs, polymeric materials and thermally stable lubricants.
- 1 History and synthesis
- 2 Natural occurrence
- 3 Physical properties
- 4 Nomenclature
- 5 Chemical properties
- 6 Uses
- 7 Adamantane analogues
- 8 References
History and synthesis
The possibility of the existence of a hydrocarbon with the C10H16 formula and diamond-like structure of the molecule was suggested by H. Decker at a conference in 1924. Decker called this molecule decaterpene and was surprised that it had not been synthesized yet.
The first attempt of laboratory synthesis was made by German chemist Hans Meerwein in 1924 using reaction of formaldehyde with diethyl malonate in the presence of piperidine. Instead of adamantane, Meerwein obtained 1,3,5,7-tetracarbomethoxybicyclo[3.3.1]nonane-2,6-dione. This compound was later named Meerwein's ester and used in the syntheses of adamantane and its derivatives. Later, another German chemist D. Bottger tried to obtain adamantane using Meerwein's ester as precursor. However, the product, tricyclo-[184.108.40.206,7] decane ring system, was again an adamantane derivative.
Adamantane was first synthesized by Vladimir Prelog in 1941 from Meerwein's ester. The process was impractical as it contained five stages (simplified in the image below) and had a yield of about 0.16%. However, it was sometimes used to synthesize certain derivatives of adamantane.
Prelog's method was refined in 1956. The decarboxylation yield was increased by the addition of the Heinsdecker pathway (11%), and the Hoffman reaction (24%) that raised the total yield to 6.5%. The process was still too complex, and a more convenient method was found by Paul von Ragué Schleyer in 1957: dicyclopentadiene was first hydrogenated in the presence of a catalyst (e.g. platinum dioxide) and then transformed into adamantane using a Lewis acid (e.g. aluminium chloride) as another catalyst. This method increased the yield to 30–40% and provided an affordable source of adamantane; it therefore stimulated characterization of adamantane and is still used in the laboratory practice. The adamantane synthesis yield was later increased to 60% and nowadays, adamantane is an affordable chemical compound with a cost of the order $1/gram.
All the above methods yield adamantane in the form of polycrystalline powder. Using this powder, single crystals can be grown from the melt, solution or vapor phase (e.g. with the Bridgman–Stockbarger technique). Melt growth result in the worst crystalline quality with a mosaic spread in the X-ray reflection of about 1°. Best crystals are obtained from the liquid phase, but the growth is inpracticably slow – several months for a 5–10 mm crystal. Growth from the vapor phase is a reasonable compromise in terms of speed and quality. Adamantane is sublimated in a quartz tube placed in a furnace, which is equipped with several heaters maintaining a certain temperature gradient (about 10 °C/cm for adamantane) along the tube. Crystallization starts at one end of the tube which is kept near the freezing point of adamantane. Slow cooling of the tube, while maintaining the temperature gradient, gradually shifts the melting zone (rate ~2 mm/hour) producing a single-crystal boule.
Before adamantane was synthesized, it was isolated from petroleum by the Czech chemists S. Landa, V. Machacek and M. Mzourek in 1932 . They used fractional distillation, which separates the organic molecule components of petroleum based on their boiling points. Landa et al. could produce only a few milligrams of adamantane, but noticed its high boiling and melting points. Because of the (assumed) similarity of its structure to that of diamond, the new compound was named adamantane.
Beside adamantane, petroleum contains more than thirty of its derivatives. Their isolation from a complex mixture of hydrocarbons is possible due to their high melting point and the ability to distill with water vapor and form stable adducts with thiourea.
Pure adamantane is a colorless crystalline solid with a characteristic camphor smell. It is practically insoluble in water, but readily soluble in nonpolar organic solvents. Adamantane has an unusually high melting point for a hydrocarbon. At 270 °C, its melting point is much higher than other hydrocarbons with the same molecular weight, such as camphene (45 °C), limonene (−74 °C), ocimene (50 °C), terpinene (60 °C) or twistane (164 °C), or than a linear C10H22 hydrocarbon decane (−28 °C). However, adamantane slowly sublimates even at room temperature. Adamantane can distill with water vapor.
Adamantane molecule consists of three condensed cyclohexane rings fused in the chair conformation. The molecular parameters were deduced by electron diffraction and X-ray crystallography. The carbon–carbon bond length is 1.54 Å and is almost identical to that of diamond, and the carbon–hydrogen distance is 1.112 Å.
At ambient conditions, adamantane crystallizes in a face-centered cubic structure (space group Fm3m, a = 9.426 ± 0.008 Å, four molecules in the unit cell) containing orientationally disordered adamantane molecules. This structure transforms into an ordered body-centered tetragonal phase (a = 6.641 Å, c = 8.875 Å) with two molecules per cell either upon cooling to 208 K or pressurizing to above 0.5 GPa.
This phase transition is of the first order; it is accompanied by an anomaly in the heat capacity, elastic and other properties. In particular, whereas adamantane molecules freely rotate in the cubic phase, they are frozen in the tetragonal one; the density increases stepwise from 1.08 to 1.18 g/cm3 and the entropy changes by a significant amount of 1594 J/(mol·K).
Elastic constants of adamantane were measured using large (centimeter-sized) single crystals and the ultrasonic echo technique. The principal value of the elasticity tensor, C11, was deduced as 7.52, 8.20 and 6.17 GPa for the <110>, <111> and <100> crystalline directions. For comparison, the corresponding values for crystalline diamond are 1161, 1174 and 1123 GPa. The arrangement of carbon atoms is the same in adamantane and diamond. However, in the adamantane solid, molecules do not form a covalent lattice as in diamond, but interact through weak Van der Waals forces. As a result, adamantane crystals are very soft and plastic.
The nuclear magnetic resonance (NMR) spectrum of adamantane consists of two poorly resolved signals, which correspond to the inequivalent sites 1 and 2 (see picture below). Their positions are 1.873 ppm and 1.756 ppm for adamantane in CDCl3 and 1H NMR, and are 28.46 ppm and 37.85 ppm for 13C NMR. The simplicity of the NMR spectrum is a good monitor of the purity of adamantane – most derivatives have lower molecular symmetry and therefore more complex spectra.
Mass spectra of adamantane and its derivatives are rather characteristic. The main peak at m/z = 136 corresponds to the C
16 ion. Its fragmentation results in weaker signals as m/z = 93, 80, 79, 67, 41 and 39.
|Frequency of vibrations, cm−1||Assignment*|
|970||ρ(CH2), ν(C−C), δ(HCC)|
|2850||ν(C−H) in CH2 groups|
|2910||ν(C−H) in CH2 groups|
|2930||ν(C−H) in CH2 groups|
* Legends correspond to different types of oscillations: δ – deformation, ν – stretching, ρ and ω – out of plane deformation vibrations of CH2 groups.
If adamantane molecules have four different substituents at every nodal carbon site, then they are chiral and optically active. As in biphenyls, the center of chirality does not belong to any particular carbon atom. Such optical activity was described in adamantane in 1969 with the four different substituents being hydrogen, bromine and methyl and carboxyl group. The values of specific rotation are small and are usually within 1°.
The adamantane molecule is composed of only carbon and hydrogen and has high Td symmetry. Therefore, its 16 hydrogen and 10 carbon atoms can be described by only two sites, which are labeled in the figure as 1 (4 equivalent sites) and 2 (6 equivalent sites).
Usually, hydrocarbons which contain only σ-bonds are relatively inert chemically. However, adamantane and its derivatives are highly reactive. This property is particularly evident in the ionic reactions where carbocations are formed as intermediates.
The dication of adamantane was obtained in solutions of superacids. It also has elevated stability due to the phenomenon called "three-dimensional aromaticity" or homoaromaticity, This four-center two-electron bond involves one pair of electrons delocalized among the four bridgehead atoms.
Most reactions of adamantane occur via the 3-coordinated carbon sites and are described in the subsections below. The 2-coordinated, bridging carbon sites are much less reactive. They are involved in the reaction of adamantane with concentrated sulfuric acid which produces adamantanone.
The carbonyl group of adamantanone allows further reactions via the bridging site. For example, adamantanone is the starting compound for obtaining such derivatives of adamantane as 2-adamantanecarbonitrile and 2-methyl-adamantane.
Adamantane readily reacts with various brominating agents, including molecular bromine. The composition and the ratio of the reaction products depend on the reaction conditions and especially the presence and type of catalysts.
The rate of bromination is accelerated upon addition of Lewis acids and is unchanged by irradiation or addition of free radicals. This indicates that the reaction occurs via an ionic mechanism.
The first fluorinations of adamantane were conducted using 1-hydroxyadamantane and 1-aminoadamantane as initial compounds. Later, fluorination was achieved starting from adamantane itself. In all these cases, reaction proceeded via formation of adamantane cation which then interacted with fluorinated nucleophiles. Fluorination of adamantane with gaseous fluorine has also been reported.
tert-butanol (t-BuOH) and sulfuric acid were added to generate adamantane cation; the cation was then carboxylated by carbon monoxide generated in situ in the interaction between the formic and sulfuric acids. The fraction of carboxylated adamantane was 55-60%.
Adamantane interacts with benzene in the presence of Lewis acids, resulting in a Friedel–Crafts reaction. Aromatically substituted adamantane derivatives can be easily obtained starting from 1-hydroxyadamantane. In particular, the reaction with anisole proceeds under normal conditions and does not require a catalyst.
Nitration of adamantane is a difficult reaction characterized by moderate yields. An important nitrogen-substituted drug amantadine can be prepared by reacting adamantane with bromine or nitric acid to give the bromide or nitroester at the 1- position. Reaction of either compound with acetonitrile affords the acetamide, which is hydrolyzed to give 1-adamantylamine:
In dye lasers, adamantane may be used to extend the life of the gain medium; it cannot be photoionized under atmosphere because its absorption bands lie in the vacuum-ultraviolet region of the spectrum. Photoionization energies have been determined for adamantane as well as for several bigger diamondoids.
All medical applications known so far involve not pure adamantane, but its derivatives. The first adamantane derivative used as a drug was amantadine – first (1967) as an antiviral drug against various strains of flu and then to treat Parkinson's disease. Other drugs among adamantane derivatives include adapalene, adapromine, amantadine, bromantane, carmantadine, chlodantane, dopamantine, memantine, rimantadine, saxagliptin, tromantadine, and vildagliptin. Polymers of adamantane have been patented as antiviral agents against HIV.
In designer drugs
Potential technological applications
Some alkyl derivatives of adamantane have been used as a working fluid in hydraulic systems. Adamantane-based polymers might find application for coatings of touchscreens, and there are prospects for using adamantane and its homologues in nanotechnology. For example, the soft cage-like structure of adamantane solid allow incorporation of guest molecules, which can be released inside the human body upon breaking the matrix. Adamantane could be used as molecular building blocks for self-assembly of molecular crystals.
Many molecules adopt adamantane-like cage structures. Those include phosphorus trioxide P4O6, arsenic trioxide As4O6, phosphorus pentoxide P4O10 = (PO)4O6, phosphorus pentasulfide P4S10 = (PS)4S6, and hexamethylenetetramine C6N4H12 = N4(CH2)6. Particularly notorious is tetramethylenedisulfotetramine, often shortened to "tetramine", a rodenticide banned in most countries for extreme toxicity to humans. The silicon analogue of adamantane, sila-adamantane, was synthesized in 2005.
Adamantane cages can be stacked together to produce higher diamondoids, such as diamantane (C14H20 – two fused adamantane cages), triamantane (C18H24), tetramantane (C22H28), pentamantane (C26H32), hexamantane (C26H30), etc. Their synthesis is similar to that of adamantane and like adamantane, they can also be extracted from petroleum, though at even much smaller yields.
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