Allotropes - Main Group Elements, Inorganic Chemistry, CSIR-NET, Chemical Sciences - Government Jobs PDF Download

New Allotropes of Main Group Elements​

 Boron​

Boron is positioned on the left side of carbon in the periodic table and known to take some unique cluster structures because of its electron deficiency and the property to form three-center two-electron bonds. A number of boron clusters of the B_nH_n²⁻ type that take deltahedral structures (polyhedral structures consisting of equilateral triangular sides), are known. Dodecahydrododecaborate ion (B₁₂H₁₂²⁻), for example, has a beautiful icosahedral structure.

Many of the allotropes of boron form larger network assemblies consisting of this B₁₂ icosahedral cluster. For example, α-rhombohedral boron has a nanostructure in which the icosahedral clusters are packed in a similar way to the arrangement called “cubic close packing.” In addition, other structural variations are known such as amorphous boron and “face-centered cubic” metal form of boron (which exists only under high pressure conditions).

Then, is it possible for boron to form spherical caged structures like fullerene? Although the exact boron analogue of C₆₀ may be too difficult, B₈₀, which has boron atoms added to the center of each hexagonal side, was considered stable enough to exist and computational studies have been done.

More recently, however, the B₄₀ cluster was discovered (Nat. Chem. 2014, 6, 727.). The formation of this all-boron fullerene was confirmed by Lai-Sheng Wang's group at Brown University, who treated boron with laser irradiation and cooled with helium gas.

Named “borospherene”, this molecule consists of 48 triangles, 2 six-membered rings, and 4 seven-membered rings, all based on boron atoms. As shown in the figure below, it belongs to the D_2d point group. It is somewhat hard to picture and really makes you wonder why this shape is so stable. It is possible that other borospherenes with different number of boron atoms and structure will be discovered in near future.

Separately from borospherene, the Wang group has considered a boron-based sheet-like structure and named it “borophene” from its relation to graphene. The structure of borophene contains a planar six-membered ring surrounded by a network of triangles. The Wang group has shown evidence for the formation of this B₃₆cluster, which is considered as a basic unit (Nat. Commun. 2013, 5, 3113.). The science of boron, like carbon did, could develop further to expand the fascinating world of “nano-borons.”

Nitrogen

Let us move on to nitrogen, the other neighbor of carbon. Neutral allotropes of nitrogen had long been unknown other than normal N₂ gas, but the existence of tetranitrogen (N4) was confirmed in 2002 . However, its lifetime was only microseconds long and it was too unstable to be isolated. The fragmentation pattern suggested that the structure of tetranitrogen was linear and formed by the weak interaction of two N₂ molecules.
Besides that, the nitrogen analogues of benzene (hexazine, N₆), cubane (N₈), and fullerene (N₆₀) have been investigated theoretically even though they have not been synthesized actually. These compounds, if they can be prepared, are expected to release high energies upon decomposition and thus have a potential application as explosive materials.

Theoretically considered nitrogen allotropes

In 2004, Max Planck Institute for Chemistry in Germany reported the synthesis of “polynitrogen”. In this work, it was found that nitrogen atoms form a single-bonded polymeric network when compressed under the conditions of 110 GPa and 2000 K.

This polynitrogen is thought to possess five times or even higher energy capacity than the most powerful nonnuclear explosives known today. Explosives of this kind have appeared in science fictions in the past, but they are becoming a reality. Of course, this polymeric allotrope of nitrogen can be neither prepared practically nor stored, so it has no prospect of being used as a weapon.

As for solely nitrogen-based ions, azide ion (N₃⁻) is known for a long time. Its handling requires caution because of its explosive property, but it has a wide application including preservative and detonating agent. In organic synthesis, it is a useful regent used traditionally as a source of nitrogen.

There is also an ion called pentazolyl anion (N₅⁻), which is an all-nitrogen pentagonal ion isoelectric to cyclopentadienyl anion. It was obtained by [3+2] cycloaddition of p-methoxybenzenediazonium cation and azide that formed the pentazole skeleton, followed by oxidative deprotection using cerium ammonium nitrate.  Even though the anion is stabilized to an extent by the aromaticity, the repulsions between the nitrogen atoms cause it to decompose with the half-life of 2.2 days.

As another example, there is a species called pentazenium cation (N₅⁺) . This substance was discovered by the High Energy Density Matter program run by the U.S. Air Force.

Pentazenium was prepared by reacting fluorodiazonium (N₂F⁺) and azide. The SbF₆⁻ salt of pentazenium was stable enough for isolation and X-ray crystallographic analysis, and the cation was found to have a V-shaped bent structure.

In theory, this pentazenium cation and azide or pentazolyl anion would form a salt composed of only nitrogen atoms. But who would dare to try to synthesize it, considering its easily predictable explosive nature? Well, it turns out that similar experiments have been done and salts like N₅⁺[B(N₃)₄]⁻ and N₅⁺[P(N₃)₆]⁻ have been actually synthesized. This paper has a picture of an exploded Teflon tube and the experimental section is filled with cautionary remarks, describing an extreme case of chemical research.

Oxygen​

A well-known allotrope of oxygen is ozone (O₃). It is a pale blue toxic gas and its strong oxidizing property is second only to fluorine. Ozone is produced by ultraviolet irradiation or silent discharge of oxygen, and in synthetic laboratories, it is used to oxidatively cleave carbon-carbon double bonds in the reaction known as ozonolysis. In some areas, it is used for disinfection of tap water.

The presence of tetraoxygen, the quartet of oxygen atoms, was predicted in 1924 by Gilbert Lewis, who is famous for formulating the definition of acids and bases. The experimental demonstration, however, proved difficult and had been elusive until 2001, when the group at University of Rome finally detected it by mass spectrometry. The structure of tetraoxygen was neither four-membered ring nor Y-shaped as anticipated, but turned out to be a complex of two oxygen molecules, one in ground state and the other in excited state.

There is one more allotrope of oxygen. When oxygen is compressed with gradually increased pressure at room temperature, the volume decreases steeply after 10 GPa and the color changes from blue to red. The identity of this so-called “red oxygen” had long been a mystery, but it was elucidated in 2006 to be the O₈ cluster composed of four oxygen molecules based on the powder X-ray diffraction patterns . The discovery came as a major surprise as this “octaoxygen” structure had not been predicted even theoretically.