This week, Brian Clegg takes us back to his youth…
As a teenager, I made good use of nitromethane – which has the CH4 structure of methane with one hydrogen atom replaced by nitrogen dioxide – it was an oxidiser in the fuel for glow plug motors. But I wasn’t aware of the compound’s big brother, tetranitromethane, in which all of methane’s four hydrogen atoms are replaced with NO2. This still makes tetranitromethane a very simple organic compound – yet despite being first made in 1857, its structure has proved so elusive that it was not firmly established until 2017.
Like nitromethane, tetranitromethane is an oxidiser – but a far more powerful one. This should make it a natural for space rockets, which require an oxidiser as well as a fuel because they soon reach altitudes where there isn’t enough oxygen available. Experimental work was under way in Germany during the second world war to use tetranitromethane to extend the range of V2 rockets. Fortunately for the allies, though, tetranitromethane is – to say the least – a tricky substance to deal with. Firstly, it is extremely poisonous, causing organ and nervous system failures. And secondly, it’s a nightmare for would-be rocketeers. Not only does it freeze at around 13.9 degrees Celsius, making it an impractical liquid oxidiser outside of a temperature controlled reaction chamber, it is so good at its job that mixing in a small amount of fuel makes it a highly impact sensitive explosive – think nitroglycerine, but more sensitive.
It might seem unlikely that anyone would want to make such a touchy substance, but aside from rocket experiments, second world war Germany also used it to improve diesel fuel. As an additive in small quantities, tetranitromethane reduces the time taken for the fuel to ignite, making it more effective in high speed engines.
That apart, tetranitromethane is also used in a range of laboratory reactions, mostly to transfer nitro groups to other molecules – but its main claim to fame has to be that elusive structure. To quote a 1976 paper on its chemistry , ‘Physicochemical constants determined for tetranitromethane by different workers differ significantly, so that it is difficult to use them to describe the structure of the compound or to assess its purity.’
It would be reasonable to expect such a simple molecule to have a neat and obvious symmetrical structure, but tetranitromethane does not play ball. In their 2017 paper, Yury Vishnevskiy, Denis Tikhonov and colleagues describe it as a ‘nightmare of molecular flexibility in the gaseous and solid states.’ For decades, attempts to pin down its structure have failed, with different approaches producing a range of predictions – it’s the chemical equivalent of the old story about the blind men and the elephant, where each feels a different part of the animal and describes it as being like anything from a snake to a wall.
When tetranitromethane was first produced in 1857, ideas on the structures of molecules were still primitive. Kekulé had only just observed how frequently a carbon atom was connected to four other atoms, and the very existence of atoms as actual physical entities would be debated for several decades to come. But our modern understanding of the interactions of molecules – particularly complex organic molecules – is highly dependent on being able to determine their structures accurately.
As we have come to understand more about molecules, we have built increasingly complex models – from the balls and sticks used in schools, through the metal plates and bars in Crick and Watson’s 1953 DNA model, to the vivid computer models of protein structures we see today. However, all these models involve a major simplification – we know that, in reality, nothing at the atomic scale is motionless. Chemical bonds are not fixed sticks, but have the potential to twist and shift – and understanding tetranitromethane required taking molecular modelling to the next level.
The new analysis used a sophisticated four-dimensional model to describe the twisting and vibrating of the nitro groups around the central carbon atom when tetranitromethane is a gas, finally fitting to observed behaviour. Similarly, to explain its response to X-ray diffraction, a model of a highly disordered high temperature solid phase combined with a more structured low temperature phase has been developed.
Tetranitromethane is a dangerous substance of relatively limited practical use. But it could also transform our approach to the structures and potential interactions of molecules, moving from the limitations of a single fixed shape to realising that tetranitromethane is a morphing transformer of a compound, and taking our understanding of the detail of chemical structure to the next level.
That was Brian Clegg with tetranitromethane. Next week, Kat Arney looks at a failed angina medication that went on to become one of the world’s best known medicines…
Alas, the promising new drug was starting to look like a disappointing flop. But then the researchers noticed something a little strange in the data coming back from their trials – men taking the drug were reporting an increased number of unusual, but not entirely unwanted side effects
And if you can’t guess, you’ll have to wait to find out with Kat next week. Until then, let us know if there’s any compound you would like to hear covered – email firstname.lastname@example.org or tweet @chemistryworld. I’m Ben Valsler, thanks for joining me.