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Fullerene C 60. Fullerene chemistry is a field of organic chemistry devoted to the chemical properties of fullerenes. [1] [2] [3] Research in this field is driven by the need to functionalize fullerenes and tune their properties. For example, fullerene is notoriously insoluble and adding a suitable group can enhance solubility. [1]
For instance, there are 1812 non-isomorphic fullerenes C 60. Note that only one form of C 60, buckminsterfullerene, has no pair of adjacent pentagons (the smallest such fullerene). To further illustrate the growth, there are 214,127,713 non-isomorphic fullerenes C 200, 15,655,672 of which have no adjacent pentagons. Optimized structures of many ...
A transition metal fullerene complex is a coordination complex wherein fullerene serves as a ligand. Fullerenes are typically spheroidal carbon compounds, the most prevalent being buckminsterfullerene, C 60. [2] One year after it was prepared in milligram quantities in 1990, [3] C 60 was shown to function as a ligand in the complex [Ph 3 P] 2 ...
Alternatively, endohedral hydrogen fullerenes can be produced by opening and closing a fullerene by organic chemistry methods. A recent example of endohedral fullerenes includes single molecules of water encapsulated in C 60. [10] Noble gas endofullerenes are predicted to exhibit unusual polarizability.
Heterofullerenes are classes of fullerenes, at least one carbon atom is replaced by another element. [1] [2] Based on spectroscopy, substitutions have been reported with boron (borafullerenes), [3] [4] nitrogen (azafullerenes), [5] [6] oxygen, [7] arsenic, germanium, [8] phosphorus, [9] silicon, [10] [11] iron, copper, nickel, rhodium [11] [12] and iridium. [11]
The method was simple and efficient to prepare the material in gram amounts per day (1990) which has boosted the fullerene research and is even today applied for the commercial production of fullerenes. The discovery of practical routes to C 60 led to the exploration of a new field of chemistry involving the study of fullerenes.
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However the group 12 metals have much lower melting and boiling points since their full d subshells prevent d–d bonding, which again tends to differentiate them from the accepted transition metals. Mercury has a melting point of −38.83 °C (−37.89 °F) and is a liquid at room temperature.