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How do you make lithium melt in the cold?

Date:
January 11, 2011
Source:
Carnegie Institution
Summary:
Sophisticated tools allow scientists to subject the basic elements of matter to conditions drastic enough to modify their behavior. By doing this, they can expand our understanding of matter. A research team was able to demonstrate surprising properties of the element lithium under intense pressure and low temperatures.

Sophisticated tools allow scientists to subject the basic elements of matter to conditions drastic enough to modify their behavior. By doing this, they can expand our understanding of matter. A research team including three Carnegie scientists was able to demonstrate surprising properties of the element lithium under intense pressure and low temperatures.

Their results were published Jan. 9 on the Nature Physics website.

Lithium is the first metal in the periodic table and is the least dense solid element at room temperature. It is most commonly known for its use in batteries for consumer electronics, such as cell phones and laptop computers. And, with only three electrons per atom, lithium should behave like a model, simple metal.

However, this research has shown that under pressure ranging between about 395,000 atmospheres (40 GPa) and about 592,000 atmospheres (60 GPa), lithium behaves in a manner that's anything but simple. Not only does it become a liquid at room temperature, but it then refuses to freeze until the temperature reaches a chilly -115o F. At pressures above about 592,000 atmospheres (60 GPa), when lithium does eventually solidify, it is into a range of highly complex, crystalline states. The highest pressure reached in the study was about 1.3 million atmospheres (130 GPa).

The research team, including Malcolm Guthrie, Stanislav Sinogeikin and Ho-kwang (Dave) Mao, of Carnegie's Geophysical Laboratory, believe that this exotic behavior is directly due to the exceptionally low mass of the lithium atom. An elementary result of quantum physics is that atoms continue to move, even when cooled to the lowest possible temperature. As the mass of an atom decreases, the importance of this residual, so called 'zero-point,' energy increases. The researchers speculate that, in the case of lithium, the zero-point energy increases with pressure to the point that melting occurs. This work raises the possibility of uncovering a material which never freezes. The prospect of a metallic liquid at even the lowest temperatures raises the intriguing possibility of an entirely novel material, a superconducting liquid, as proposed previously by theorists for hydrogen at very high pressure.

This work is supported by a research grant from the UK Engineering and Physical Sciences Research Council and facilities made available by the European Synchrotron Radiation Facility. It is also based on work supported as part of the EFree initiative, funded by the US Department of Energy, Office of Science. HPCAT, where some of the research was conducted, is supported by DOE-BES, DOE-NNSA, and NSF. APS, where some data were collected is supported by DOE-BES, One of the researchers received support from the Royal Society.


Story Source:

The above story is based on materials provided by Carnegie Institution. Note: Materials may be edited for content and length.


Journal Reference:

  1. Christophe L. Guillaume, Eugene Gregoryanz, Olga Degtyareva, Malcolm I. McMahon, Michael Hanfland, Shaun Evans, Malcolm Guthrie, Stanislav V. Sinogeikin, H-K. Mao. Cold melting and solid structures of dense lithium. Nature Physics, 2011; DOI: 10.1038/nphys1864

Cite This Page:

Carnegie Institution. "How do you make lithium melt in the cold?." ScienceDaily. ScienceDaily, 11 January 2011. <www.sciencedaily.com/releases/2011/01/110110121715.htm>.
Carnegie Institution. (2011, January 11). How do you make lithium melt in the cold?. ScienceDaily. Retrieved September 22, 2014 from www.sciencedaily.com/releases/2011/01/110110121715.htm
Carnegie Institution. "How do you make lithium melt in the cold?." ScienceDaily. www.sciencedaily.com/releases/2011/01/110110121715.htm (accessed September 22, 2014).

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