Inert helium may form stable compounds inside giant planets such as Jupiter, seen here by NASA's Juno spacecraft on Aug. 27, 2016.

Deep within giant planets, helium may form stable compounds with other elements, a new study finds something that was long thought never to happen in nature.

Helium is second only to hydrogen as the most common element in the universe; it exists in abundance in stars and gas giants. However, whereas hydrogen easily reacts with other elements to form compounds such as water, helium is a member of a group of elements known as the noble gases that do not bond readily with other elements.

Although helium is the most chemically inert element known, scientists have found a few instances in which it can form compounds with other elements. Still, until now, all known helium compounds either were highly unstable or were ones where the helium and the other elements barely interacted with one another. [Element Number Two: Facts About Helium]

Now lab experiments reveal that, at the kinds of high pressures that are found within gas giant planets, helium can form stable compounds with sodium.

"One more traditional assumption that helium does not form stable compounds has fallen," said study co-author Artem Oganov, director of Stony Brook University's Center for Materials by Design in New York and head of the Moscow Institute of Physics and Technology's Computational Materials Discovery laboratory.

Previous research suggested that "rules of classical chemistry break down at high pressure," Oganov said. This led study lead author Xiao Dong at Nankai University in Tianjin, China, and his colleagues to investigate whether it was possible "to break yet another rule and discover stable compounds of the most unreactive element helium," Oganov told Space.com.

The international research team searched for stable helium compounds by running calculations on two supercomputers. These machines included Tianhe II in Guangzhou, China, which is currently ranked as the world's second-most-powerful supercomputer.

Their results predicted two stable helium compounds. One is NaHe, which consists of one helium atom and two sodium atoms, while the other is NaHeO, which consists of one helium atom, two sodium atoms and one oxygen atom.

In experiments, the scientists successfully synthesized NaHe by squeezing its components between two diamonds at pressures of about 1.1 million times Earth's atmospheric pressure. The team's calculations predict that the compound will prove stable to at least up to 10 million times that pressure.

Crystal structure of NaHe, which resembles a 3D checkerboard. The purple spheres represent sodium atoms, which are inside the green cubes that represent helium atoms. The red regions inside voids of the structure show areas where localized electron pairs reside.

"This work gives a spectacular triumph of theory," Oganov said. "This very surprising compound was first predicted by theory, and only then made experimentally."

The helium atoms do not actually form any chemical bonds with the sodium atoms. Still, the presence of the helium atoms fundamentally changes the chemical interactions between the sodium atoms, forcing electrons to pair together, despite their natural tendency to repel one another.

"It is a very bizarre new kind of compound, in which helium atoms make a huge change in the way sodium atoms interact with each other," Oganov said.

To imagine what NaHe looks like, picture a 3D checkerboard of black and white cubes. In the centers of the black cubes are helium atoms, in the centers of the white cubes are pairs of electrons and at the corners of all the cubes are sodium atoms.

The calculations suggest that the other predicted helium compound, NaHeO, would be stable from 0.15 to 1.1 million times Earth's atmospheric pressure. Its structure should be similar to that of NaHe, but in place of electron pairs, it would have oxygen atoms.

These findings could "have implications for planets and perhaps also for stars," Oganov said. Although it remains uncertain what effects such helium compounds might have, researchers can no longer assume that helium is simply inert, he said.

The scientists detailed their findingsonline Feb. 6 in the journal Nature Chemistry.

Follow Charles Q. Choi on Twitter @cqchoi. Follow us @Spacedotcom, Facebookand Google+. Originally published onSpace.com.

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