n-Butyl lithium is hexameric in the solid state[1] and in cyclohexane solutions. Why? Here I try to find out some of its secrets.
The crystal structure reveals the following points of interest:
The lithium cluster has twelve electrons available for bonding; if the Li is considered as Li+, balanced by six C– carbanions, the twelve electrons come from the six carbon lone pairs pointing towards each of six triangular faces. An ELF analysis can help identify how these twelve electrons are arranged. Shown below is the environment of a single Li-face, with the ELF basin ringed. It integrates to 2.08 electrons. So each tetrahedral cluster of three lithiums and one carbanion could be considered as a two-electron-four-centre bond, perhaps a natural progression from the two-electron-three-centre bonding found in a slightly less electron deficient system such as diborane.
NBOs (natural bond orbitals) reflect this character. An NBO represents a localised two-electron orbital, and analysis indeed reveals six such orbitals, each having the form shown below.
This picture in turn leads us to identify this system as spherically aromatic[2]. The three-dimensional equivalent of the Hückel rule is that any system with 2(N+1)2 σ or π electrons (or both) in a cluster can be considered aromatic/diatropic. In this case, N=0 and hence the magic count is 2 for each of the six CLi3 tetrahedra. The diatropic ring current might be manifested in the computed 1H NMR chemical shifts of the CH2– protons (-0.8ppm). Aromaticity does not immediately spring to mind with the name n-butyl lithium, but this unprepossessing molecule has six aromatic regions!
Each lithium atom is in turn hemispherically surrounded by three of these 2.08 electron basins (below, although the ELF centroid is very much biased towards the carbon, indicating considerable ionicity). What wonderful electronic economy! Despite there being only twelve electrons to be shared amongst six lithium atoms, each lithium manages nevertheless to surround itself with 6.24 electrons. All crammed into one half sphere, leaving a nice coordination hole; n-butyl lithium is after all a highly reactive species (even as a hexamer).
I want to finish by exploring the observation that two of the six n-butyl groups adopt a gauche conformation. In free n-butane itself, around 31% of the population adopts this shape, which curiously is around the same proportion as is found in the hexameric structure of n-butyl lithium. More generally, a search of the Cambridge database for compounds containing such groups reveals the following distribution; about 1 in 7.
Well, when you deprive a molecule of electrons, as any species with lithium must invariably suffer from, it is wonderful how the system responds. In this sense, a hexameric structure seems a very natural outcome. And it has brought us the two-electron-four-centre bond and the associated spherical aromaticity, both of which are a nice bonus.
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I computed a coarse grid of NICS to see what happens around the vicinity of the (CH3Li)6 hexamer. Truly aromatic systems should display negative NICS values inside but positive NICS values outside of the cage/(or ring). But this does not happen for (CH3Li)6! See two views below (the largest isotropic NICS value around the C atom is –48.5 ppm, cage center: –1.05 ppm, Li3 three membered ring center: –4.58 ppm). It seems like any "diatropicity" inherent to (CH3Li)6 arises predominately from local circulations around the highly shielded carbanion C centers. On this basis, it is probably difficult to justify (CH3Li)6 as being aromatic, despite its negative NICS values at certain positions in the molecule.
I also checked the 1H chemical shifts of the CH3 protons in (CH3Li)6 vs. the methyl anion, CH3(–). The protons in (CH3Li)6 are indeed downfield relative to CH3(–) (supportive of possible aromaticity), but only by 0.22 to 0.50 ppm!
The currents look like those of an aggregate of alternating anions and cations. Overall currents are close to zero but all in all diamagnetic.
Thanks all for the various great insights.
They have helped make for a fascinating analysis of what might have appeared to be an insignificant molecule. I will point this discussion out to our students; I am sure they will love it!
PS: The currents in particular do not resemble cluster/3D aromatic currents, which are diatropic vortices passing through the hole cluster, without central paratropic vortices.
Can you please provide me the coordinate file for the Butyl lithium hexamer. I was trying to optimize it.
Coordinates can be obtained from any of the 3D models visualised by clicking on the image as per instruction and using the JSmol menu, or by clicking on any of the three hyperlinks in the text which lead to data on a data repository.