Neon is one of the noble gases and makes up only a tiny fraction of Earth’s atmosphere. It’s not just used to light up the iconic neon signs in your favorite bars, but also plays an important role in fundamental chemical research.
The chemical element is a colorless, odorless, tasteless gas at room temperature and pressure. It is on the right side of the periodic table and sits next to argon, krypton, and xenon. It is highly inert and does not react with other elements, except by forming molecular ions or excimers (short-lived dimeric molecules).
It was discovered in 1898 by British chemists William Ramsay and Morris Travers. They found it in a sample of liquid air, along with nitrogen, oxygen, and argon. They froze the sample, then evaporated it to separate the gases. The resulting neon was reddish-orange, and Ramsay’s son suggested the name “neon,” based on the Greek word neos, meaning new.
When exposed to an electric current in a discharge tube, neon can be “ionized.” An electron is accelerated up to its maximum kinetic energy, so it’s no longer bound to the atom it’s associated with. This allows other electrons to move freely around the atom, and this is what gives the gas its characteristic glow. Using high voltage AC, it’s possible to get neon to ionize continuously, creating a plasma of charged particles that carries an electric current. This is what happens inside the tubes that are used to make those familiar neon signs.
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