This article is about the chemical element. For other uses, see Neon (disambiguation).
Chemical element, symbol Ne and atomic number 10
Neon, 10Ne
Neon
Appearance
colorless gas exhibiting an orange-red glow when placed in an electric field
Standard atomic weight Ar°(Ne)
20.1797±0.0006[1]
20.180±0.001 (abridged)[2]
Neon in the periodic table
Hydrogen
Helium
Lithium
Beryllium
Boron
Carbon
Nitrogen
Oxygen
Fluorine
Neon
Sodium
Magnesium
Aluminium
Silicon
Phosphorus
Sulfur
Chlorine
Argon
Potassium
Calcium
Scandium
Titanium
Vanadium
Chromium
Manganese
Iron
Cobalt
Nickel
Copper
Zinc
Gallium
Germanium
Arsenic
Selenium
Bromine
Krypton
Rubidium
Strontium
Yttrium
Zirconium
Niobium
Molybdenum
Technetium
Ruthenium
Rhodium
Palladium
Silver
Cadmium
Indium
Tin
Antimony
Tellurium
Iodine
Xenon
Caesium
Barium
Lanthanum
Cerium
Praseodymium
Neodymium
Promethium
Samarium
Europium
Gadolinium
Terbium
Dysprosium
Holmium
Erbium
Thulium
Ytterbium
Lutetium
Hafnium
Tantalum
Tungsten
Rhenium
Osmium
Iridium
Platinum
Gold
Mercury (element)
Thallium
Lead
Bismuth
Polonium
Astatine
Radon
Francium
Radium
Actinium
Thorium
Protactinium
Uranium
Neptunium
Plutonium
Americium
Curium
Berkelium
Californium
Einsteinium
Fermium
Mendelevium
Nobelium
Lawrencium
Rutherfordium
Dubnium
Seaborgium
Bohrium
Hassium
Meitnerium
Darmstadtium
Roentgenium
Copernicium
Nihonium
Flerovium
Moscovium
Livermorium
Tennessine
Oganesson
He ↑ Ne ↓ Ar
fluorine ← neon → sodium
Atomic number (Z)
10
Group
group 18 (noble gases)
Period
period 2
Block
p-block
Electron configuration
[He] 2s2 2p6
Electrons per shell
2, 8
Physical properties
Phase at STP
gas
Melting point
24.56 K (−248.59 °C, −415.46 °F)
Boiling point
27.104 K (−246.046 °C, −410.883 °F)
Density (at STP)
0.9002 g/L
when liquid (at b.p.)
1.207 g/cm3[3]
Triple point
24.556 K, 43.37 kPa[4][5]
Critical point
44.4918 K, 2.7686 MPa[5]
Heat of fusion
0.335 kJ/mol
Heat of vaporization
1.71 kJ/mol
Molar heat capacity
20.79[6] J/(mol·K)
Vapor pressure
P(Pa)
1
10
100
1 k
10 k
100 k
at T(K)
12
13
15
18
21
27
Atomic properties
Oxidation states
0
Ionization energies
1st: 2080.7 kJ/mol
2nd: 3952.3 kJ/mol
3rd: 6122 kJ/mol
(more)
Covalent radius
58 pm
Van der Waals radius
154 pm
Spectral lines of neon
Other properties
Natural occurrence
primordial
Crystal structure
face-centered cubic (fcc) (cF4)
Lattice constant
a = 453.77 pm (at triple point)[7]
Thermal conductivity
49.1×10−3 W/(m⋅K)
Magnetic ordering
diamagnetic[8]
Molar magnetic susceptibility
−6.74×10−6 cm3/mol (298 K)[9]
Bulk modulus
654 GPa
Speed of sound
435 m/s (gas, at 0 °C)
CAS Number
7440-01-9
History
Prediction
William Ramsay (1897)
Discovery and first isolation
William Ramsay & Morris Travers[10][11] (1898)
Isotopes of neon
v
e
Main isotopes[12]
Decay
abundance
half-life (t1/2)
mode
product
20Ne
90.5%
stable
21Ne
0.27%
stable
22Ne
9.25%
stable
Category: Neon
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Neon is a chemical element; it has symbol Ne and atomic number 10. It is the second noble gas in the periodic table.[13] Neon is a colorless, odorless, inert monatomic gas under standard conditions, with approximately two-thirds the density of air.
Neon was discovered in 1898 alongside krypton and xenon, identified as one of the three remaining rare inert elements in dry air after the removal of nitrogen, oxygen, argon, and carbon dioxide. Its discovery was marked by the distinctive bright red emission spectrum it exhibited, leading to its immediate recognition as a new element. The name neon originates from the Greek word νέον, a neuter singular form of νέος (neos), meaning 'new'. Neon is a chemically inert gas, with no known uncharged neon compounds. Existing neon compounds are primarily ionic molecules or fragile molecules held together by van der Waals forces.
The synthesis of most neon in the cosmos resulted from the nuclear fusion within stars of oxygen and helium through the alpha-capture process. Despite its abundant presence in the universe and Solar System—ranking fifth in cosmic abundance following hydrogen, helium, oxygen, and carbon—neon is comparatively scarce on Earth. It constitutes about 18.2 ppm of Earth's atmospheric volume and a lesser fraction in the Earth's crust. The high volatility of neon and its inability to form compounds that would anchor it to solids explain its limited presence on Earth and the inner terrestrial planets. Neon’s high volatility facilitated its escape from planetesimals under the early Solar System's nascent Sun's warmth.
Neon's notable applications include its use in low-voltage neon glow lamps, high-voltage discharge tubes, and neon advertising signs, where it emits a distinct reddish-orange glow.[14][15] This same red emission line is responsible for the characteristic red light of helium–neon lasers. Although neon has some applications in plasma tubes and as a refrigerant, its commercial uses are relatively limited. It is primarily obtained through the fractional distillation of liquid air, making it significantly more expensive than helium due to air being its sole source.
^"Standard Atomic Weights: Neon". CIAAW. 1985.
^Prohaska, Thomas; Irrgeher, Johanna; Benefield, Jacqueline; Böhlke, John K.; Chesson, Lesley A.; Coplen, Tyler B.; Ding, Tiping; Dunn, Philip J. H.; Gröning, Manfred; Holden, Norman E.; Meijer, Harro A. J. (4 May 2022). "Standard atomic weights of the elements 2021 (IUPAC Technical Report)". Pure and Applied Chemistry. doi:10.1515/pac-2019-0603. ISSN 1365-3075.
^Hammond, C. R. (2000). The Elements, in Handbook of Chemistry and Physics 81st edition(PDF). CRC press. p. 19. ISBN 0849304814.
^Preston-Thomas, H. (1990). "The International Temperature Scale of 1990 (ITS-90)". Metrologia. 27 (1): 3–10. Bibcode:1990Metro..27....3P. doi:10.1088/0026-1394/27/1/002.
^ abHaynes, William M., ed. (2011). CRC Handbook of Chemistry and Physics (92nd ed.). Boca Raton, FL: CRC Press. p. 4.122. ISBN 1-4398-5511-0.
^Shuen-Chen Hwang, Robert D. Lein, Daniel A. Morgan (2005). "Noble Gases". in Kirk Othmer Encyclopedia of Chemical Technology, pages 343–383. Wiley. doi:10.1002/0471238961.0701190508230114.a01.pub2
^Arblaster, John W. (2018). Selected Values of the Crystallographic Properties of Elements. Materials Park, Ohio: ASM International. ISBN 978-1-62708-155-9.
^Magnetic susceptibility of the elements and inorganic compounds, in Lide, D. R., ed. (2005). CRC Handbook of Chemistry and Physics (86th ed.). Boca Raton (FL): CRC Press. ISBN 0-8493-0486-5.
^Weast, Robert (1984). CRC, Handbook of Chemistry and Physics. Boca Raton, Florida: Chemical Rubber Company Publishing. pp. E110. ISBN 0-8493-0464-4.
^Ramsay, William; Travers, Morris W. (1898). "On the Companions of Argon". Proceedings of the Royal Society of London. 63 (1): 437–440. doi:10.1098/rspl.1898.0057.
^"Neon: History". Softciências. Retrieved 27 February 2007.
^Kondev, F. G.; Wang, M.; Huang, W. J.; Naimi, S.; Audi, G. (2021). "The NUBASE2020 evaluation of nuclear properties" (PDF). Chinese Physics C. 45 (3): 030001. doi:10.1088/1674-1137/abddae.
^Group 18 refers to the modern numbering of the periodic table. Older numberings described the rare gases as Group 0 or Group VIIIA (sometimes shortened to 8). See also Group (periodic table).
^Coyle, Harold P. (2001). Project STAR: The Universe in Your Hands. Kendall Hunt. p. 464. ISBN 978-0-7872-6763-6.
^Kohmoto, Kohtaro (1999). "Phosphors for lamps". In Shionoya, Shigeo; Yen, William M. (eds.). Phosphor Handbook. CRC Press. p. 940. ISBN 978-0-8493-7560-6.
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