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Neon

10
20.18
Ne
Neon

Element Stats

Select a temperature unit to update boiling and melting point values.

Physical

Physical Properties
PropertyValuePropertyValue
Appearancecolorless gas exhibiting an orange-red glow when placed in a high voltage electric field
ClassificationNoble GasesDensity0.9002 g/cm³ at STP
Boiling Point27.104 KMelting Point24.56 K

Atomic

Atomic Properties
PropertyValuePropertyValue
Atomic Number10Atomic Mass20.17976
Van Der Waals Radius154Atomic Radius (empirical)--

Electronic & Chemical

Electronic and Chemical Properties
PropertyValuePropertyValue
Electronegativity--Electron Affinity-116 kJ/mol
Electron Configuration1s2 2s2 2p6
Oxidation States0
Ionization Energies

Showing 5 of 10 ionization energies.

  1. 2080.7 kJ/mol
  2. 3952.3 kJ/mol
  3. 6122 kJ/mol
  4. 9371 kJ/mol
  5. 12177 kJ/mol

History

In 1898, during a six-week period, British chemists William Ramsay and Morris Travers discovered three noble gases by evaporating liquid air and extracting the gases one-by-one (a process called fractional distillation). Krypton was the first gas to be identified, then Ramsay and Travers repeated the same experiment, this time changing the pressure to evaporate solid Argon. Because of the tweaked distillation process, the gas that evaporated first was neon which, when collected in an atomic spectrometer, glowed a brilliant red-orange light. The bright color shocked the scientists as Travers noted, "the blaze of crimson light from the tube told its own story and was a sight to dwell upon and never forget."

Neon as we know it, bright and descriptive on storefront signs and motel vacancy notices, did not come to be until the 1900s. In 1902, George Claude collected neon as a by-product of his air-liquefication business and in 1910, he sealed the neon in a tube (similar to the modern use) and tried to sell the tubes as an indoor lighting source. This business attempt was not successful because homeowners weren’t fond of the intense colors, but in 1912, Claude found success in using neon tubes for advertising.

Properties

Colorless and odorless, neon is the second-lightest noble gas. The notable reddish glow occurs when it is collected in a vacuum discharge tube.

Uses

The most common use of neon is in brightly lit signs used for advertising. Neon is also used to make high-voltage indicators and switching gear, lightning arresters, diving equipment, and lasers. These signs and buttons typically use electricity to get the gas to emit its bright red color. Liquid neon is also used for cryogenic freezing, a process that preserves items in extremely low temperatures.

In combination with other elements, neon has even more applications. For example, neon is used in the helium-neon lasers used for supermarket checkout scanners, printers, and more.

Compounds

Neon is an inert gas, which means it does not react with other chemical elements and doesn't form compounds.

Forms

Neon also has six unstable isotopes in addition to its three stable ones. Neon's main isotope neon-20 is created by the nuclear fusion that happens in the core of stars.

Sources

Neon is rare on Earth, though common in the universe and solar system (stable isotopes of neon are found in stars). The atmosphere is the primary source of neon. It is collected by evaporating liquified air (fractional distillation).

Fun Facts

Always on that Orange Vibe

Real neon lights are reddish-orange. Neon signs in other colors use other methods such as a combination of neon and other gases, like argon, or colored glass tubes.

Neon signs are lit

An Orange Crush neon sign recently sold for $189,750, making it the most expensive sign ever sold at auction. It was found in its original packaging in an abandoned storage unit in New Mexico.

Isotope GOAT

In an experiment with neon, the early 20th century physicist J.J Thompson was the first to observe isotopes of a stable (non-radioactive) element. Before his experiment, scientists thought that there were only isotopes of radioactive elements. His experiment with neon was also the first example of mass-spectrometry, an analytical technique still widely used today.

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