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Sodium's explosive secrets revealed

The spectacular reaction of alkali metals with water was poorly understood —
despite being a staple of chemistry classes.

Philip Ball

26
January 2015

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Coulomb explosion

The researchers explain how they discovered that the electrostatic, or
Coulomb, force is behind the dramatic but erratic behaviour of bulk sodium and
potassium.

Philip Mason/Czech Academy of Sciences

It’s the classic piece of chemical tomfoolery: take a lump of sodium or
potassium metal, toss it into water and watch the explosion. Although this piece
of pyrotechnics has amazed generations of chemistry students, until now it has
been misunderstood, a paper in Nature Chemistry reveals1.

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The explosion, say Pavel Jungwirth and his collaborators at the Czech Academy
of Sciences in Prague, is not merely a consequence of the ignition of the
hydrogen gas that the alkali metals release from water. That may happen
eventually, but it begins as something far stranger: a rapid exodus of electrons
followed by explosion of the metal driven by electrical repulsion.

The neurologist and celebrated author Oliver Sacks, who is also a chemistry
enthusiast, described the phenomenon as “chemistry with a vengeance” in his book
Uncle Tungsten2.
He wrote of how, as a boy, he and his friends bought a lump of sodium from the
local chemicals supplier and dumped it into the Highgate Ponds in North London:
“It took fire instantly and sped around and around on the surface like a
demented meteor, with a huge sheet of yellow flame above it.”

In bulk, sodium is a silvery metal, a soft solid at room temperature. If it
comes in contact with water, it produces sodium hydroxide and hydrogen.
Potassium reacts even more vigorously. These reactions unleash a lot of heat, so
it seemed straightforward to think that the explosions resulted from the
hydrogen igniting.

Phil Mason

But for a chemical reaction to have a runaway explosive outcome,
the reactants need to mix quickly and efficiently, Jungwirth points out. In
the case of the alkali metals, however, the hydrogen gas and steam released at
the surface of the metal should prevent more water from reaching it. Without a
constant supply of water to fuel it, the reaction should peter out.

Jungwirth’s colleague Philip Mason was determined to find out what was really
going on — despite the hazards. In one run, he removed his face shield to blow
out a small fire, only to have a piece of metal go off in his face, scratching
his cheek. To get a reliable reaction — sodium sometimes oxidizes on the surface
and will not explode — Mason used an alloy of sodium and potassium that is
liquid at room temperature.

High-speed cameras revealed a vital clue to what was fuelling the violent
reaction in the early stages. The reaction starts less than a millisecond after
the metal droplet, released from a syringe, enters the water. After just 0.4 ms,
‘spikes’ of metal shoot out from the droplet, too fast to be expelled by
heating. What’s more, between 0.3 and 0.5 ms, this spiking droplet becomes
surrounded by a dark blue/purple colour in the solution.

The reason for these two observations became clear when Jungwirth’s colleague
Frank Uhlig carried out quantum-mechanical computer simulations of the process
with clusters of just 19 sodium atoms. He found that each of the atoms at the
surface of the cluster loses an electron within just several picoseconds
(10–12 s), and that these electrons shoot into the surrounding water,
where they are solvated (surrounded by water molecules)3.

Solvated electrons in water are known to have the deep blue colour briefly
observed in the videos. Their departure leaves the metal cluster full of
positively charged ions, which repel each other. The result is a so-called
Coulomb explosion, in which the cluster bursts apart owing to its ions’ mutual
electrostatic (Coulombic) repulsion.

“The paper gives a complete and interesting account of the early stages of
the reaction”, says inorganic chemist James Dye of Michigan State University in
East Lansing, an expert in solvated electrons. “I have done the demonstration
dozens of times and wondered why sodium globules often danced on the surface,
while potassium leads to explosive behaviour.”

Journal name:

Nature

DOI:

doi:10.1038/nature.2015.16771

References

Mason, P. E.
et al. Nature Chem. http://dx.doi.org/10.1038/nchem.2161
(2015).

Sacks, O. Uncle Tungsten 123 (Picador, London, 2001).

Young, R. M.
& Neumark, D. M.
Chem. Rev. 112,
5553–5577 (2012).

Article

PubMed

ISI

ChemPort

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Philip Ball

Philip is a freelance science writer and a consultant editor
for Nature. He can often be heard on radio and television, and is the
author of several scientific books for the lay reader, including H2O: A
Biography of Water (shortlisted for a National Book Critics Circle Award); and
Critical Mass (win…

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