Difference between revisions of "Neon" - New World Encyclopedia

Vapor pressure
10	fluorine ← neon → sodium
	periodic table
General
Name, Symbol, Number	neon, Ne, 10
Chemical series	noble gases
Group, Period, Block	18, 2, p
Appearance	colorless ;
Atomic mass	20.1797(6) g/mol
Electron configuration	1s2 2s2 2p6
Electrons per shell	2, 8
Physical properties
Phase	gas
Density	(0 °C, 101.325 kPa); 0.9002 g/L
Melting point	24.56 K; (-248.59 °C, -415.46 °F)
Boiling point	27.07 K; (-246.08 °C, -410.94 °F)
Critical point	44.4 K, 2.76 MPa
Heat of fusion	0.335 kJ/mol
Heat of vaporization	1.71 kJ/mol
Heat capacity	(25 °C) 20.786 J/(mol·K)
Atomic properties
Crystal structure	cubic face centered
Oxidation states	no data
Ionization energies; (more)	1st: 2080.7 kJ/mol
	2nd: 3952.3 kJ/mol
	3rd: 6122 kJ/mol
Atomic radius (calc.)	38 pm
Covalent radius	69 pm
Van der Waals radius	154 pm
Miscellaneous
Magnetic ordering	nonmagnetic
Thermal conductivity	(300 K) 49.1 mW/(m·K)
Speed of sound	(gas, 0 °C) 435 m/s
CAS registry number	7440-01-9
Notable isotopes

Latest revision as of 16:18, 11 November 2022

Neon (chemical symbol Ne, atomic number 10) is the fourth most abundant chemical element in the universe, but it is just a trace element in the air. As a member of the noble gas series, it is nearly inert. Under ordinary conditions, it is colorless, but in a vacuum discharge tube, it gives a reddish-orange glow. Consequently, the main use of neon is to make flashy signs for advertising. In addition, a mixture of helium and neon gases is used to make a gas laser, and liquid neon is a low-temperature refrigerant.

Discovery and occurrence

Neon (from the Greek word νέος, meaning "new") was discovered by Scottish chemist William Ramsay and English chemist Morris Travers in 1898, during their studies of liquefied air.

Neon is the fourth most abundant element in the universe.[1] In the Earth's atmosphere, however, it occurs in only trace amounts—at 1 part in 65,000. It is industrially produced by cryogenic fractional distillation of liquefied air.

Notable characteristics

Neon is part of the noble gas series in the periodic table. As such, it is an extremely unreactive element. It follows helium in group 18 (former group 8A) and is placed after fluorine in period 2. The gas is composed of single atoms and is therefore described as "monatomic."

Neon is less dense than air and is the second-lightest noble gas, after helium. Its low density suggests that it may slowly leak out of the Earth's atmosphere and escape into space, thus providing an explanation for its scarcity on Earth. By contrast, argon (another noble gas) is denser than air and remains within the Earth's atmosphere.

Neon has over 40 times the refrigerating capacity of liquid helium and three times that of liquid hydrogen (on a per unit volume basis). For most applications, it is a less expensive refrigerant than helium.

Of all the rare gases, neon has the most intense discharge at normal voltages and currents. As noted above, it glows reddish-orange in a vacuum discharge tube.

Isotopes

Neon has three stable isotopes:

²⁰Ne (90.48%), with 10 neutrons in the nucleus of each atom;
²¹Ne (0.27%), with 11 neutrons in the nucleus of each atom; and
²²Ne (9.25%), with 12 neutrons in the nucleus of each atom.

Compounds

Given the extreme inertness of neon, its compounds are hard to find. It does, however, appear to form an unstable hydrate. In addition, research involving specialized techniques (including mass spectrometry) has shown that neon can form various ions, either by itself or in combination with other elements. These ions include Ne⁺, (NeAr)⁺, (NeH)⁺, and (HeNe⁺).

Applications

Neon is often used in signs

The reddish-orange color that neon emits in neon lamps is widely used for advertising signs. The word "neon" has become a generic term for these types of lights, although many other gases are used to produce different colors of light.

Neon and helium may be used together to make a type of gas laser called a helium-neon laser. In addition, liquefied neon is commercially used as a cryogenic refrigerant in applications not requiring the lower temperature range attainable with liquid helium, which is more expensive.

Neon is also used in the following devices:

vacuum tubes
high-voltage indicators
lightning arrestors
wave meter tubes
television tubes

External links

All links retrieved November 11, 2022.

Credits

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Neon ^history

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History of "Neon"

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-{{otheruses}}
+{{Copyedited}}{{Paid}}{{Images OK}}{{Submitted}}{{Approved}}
+[[Category:Public]]
 {{Elementbox_header | number=10 | symbol=Ne | name=neon | left=[[fluorine]] | right=[[sodium]] | above=[[helium|He]] | below=[[argon|Ar]] | color1=#c0ffff | color2=green }}
 {{Elementbox_series | [[noble gas]]es }}
@@ Line 36: / Line 37: @@
 {{Elementbox_footer | color1=#c0ffff | color2=green }}
-'''Neon''' is the [[chemical element]] in the periodic table that has the symbol '''Ne''' and [[atomic number]] 10. A colorless, nearly [[inert]] [[noble gas]], neon gives a distinct reddish glow when used in vacuum discharge tubes and [[neon lamp]]s and is found in air in trace amounts.
+'''Neon''' (chemical symbol '''Ne''', [[atomic number]] 10) is the fourth most abundant [[chemical element]] in the universe, but it is just a trace element in the air. As a member of the [[noble gas]] series, it is nearly inert. Under ordinary conditions, it is colorless, but in a vacuum discharge tube, it gives a reddish-orange glow. Consequently, the main use of neon is to make flashy signs for advertising. In addition, a mixture of helium and neon gases is used to make a gas laser, and liquid neon is a low-temperature refrigerant.
+{{toc}}
+== Discovery and occurrence ==
+Neon (from the [[Greek language|Greek]] word ''νέος'', meaning "new") was discovered by Scottish chemist [[William Ramsay]] and English chemist [[Morris Travers]] in 1898, during their studies of liquefied air.
+Neon is the fourth most abundant element in the [[universe]].[http://education.jlab.org/itselemental/ele010.html] In the [[Earth's atmosphere]], however, it occurs in only trace amounts&mdash;at 1 part in 65,000. It is industrially produced by cryogenic fractional distillation of liquefied air.
 == Notable characteristics ==
-Neon is the second-lightest [[noble gas]], glows [[red]]dish-[[Orange (colour)|orange]] in a [[vacuum discharge tube]] and has over 40 times the [[refrigerating capacity]] of liquid [[helium]] and three times that of liquid [[hydrogen]] (on a per unit volume basis). In most applications it is a less expensive [[refrigerant]] than helium. Neon has the most intense discharge at normal voltages and currents of all the rare gases.
+Neon is part of the noble gas series in the [[periodic table]]. As such, it is an extremely unreactive element. It follows [[helium]] in group 18 (former group 8A) and is placed after fluorine in period 2. The gas is composed of single atoms and is therefore described as "monatomic."
+Neon is less dense than air and is the second-lightest noble gas, after helium. Its low density suggests that it may slowly leak out of the Earth's atmosphere and escape into space, thus providing an explanation for its scarcity on Earth. By contrast, [[argon]] (another noble gas) is denser than air and remains within the Earth's atmosphere.
+Neon has over 40 times the refrigerating capacity of liquid helium and three times that of liquid [[hydrogen]] (on a per unit volume basis). For most applications, it is a less expensive [[refrigerant]] than helium.
+Of all the rare gases, neon has the most intense discharge at normal voltages and currents. As noted above, it glows reddish-orange in a [[vacuum discharge tube]].
+=== Isotopes ===
+Neon has three stable [[isotope]]s:
+*<sup>20</sup>Ne (90.48%), with 10 neutrons in the nucleus of each atom;
+*<sup>21</sup>Ne (0.27%), with 11 neutrons in the nucleus of each atom; and
+*<sup>22</sup>Ne (9.25%), with 12 neutrons in the nucleus of each atom.
+== Compounds ==
+Given the extreme inertness of neon, its compounds are hard to find. It does, however, appear to form an unstable [[hydrate]]. In addition, research involving specialized techniques (including ''mass spectrometry'') has shown that neon can form various ions, either by itself or in combination with other elements. These ions include Ne<sup>+</sup>, (Ne[[argon|Ar]])<sup>+</sup>, (Ne[[hydrogen|H]])<sup>+</sup>, and ([[helium|He]]Ne<sup>+</sup>).
 == Applications ==
 [[Image:Neon_signage_Club.jpg|thumb|left|210px| Neon is often used in [[neon sign|signs]]]]
-The reddish-orange color that neon emits in [[Neon lamp|neon light]]s is widely used to make advertising [[neon sign|signs]]. The word "neon" is also used generically for these types of lights even though many other gases are used to produce different colors of light. Other uses:
+The reddish-orange color that neon emits in neon lamps is widely used for advertising signs. The word "neon" has become a generic term for these types of lights, although many other gases are used to produce different colors of light.
+Neon and helium may be used together to make a type of gas laser called a ''helium-neon laser''. In addition, liquefied neon is commercially used as a cryogenic [[refrigerant]] in applications not requiring the lower temperature range attainable with liquid helium, which is more expensive.
+Neon is also used in the following devices:
 * vacuum tubes
 * high-voltage indicators
@@ Line 50: / Line 79: @@
 * wave meter tubes
 * [[television]] tubes
-* Neon and helium are used to make a type of gas [[helium-neon laser|laser]]
-* Liquefied neon is commercially used as a [[cryogenic]] [[refrigerant]] in applications not requiring the lower temperature range attainable with more expensive liquid helium refrigeration.
-== History ==
-Neon ([[Greek language|Greek]] ''νέος'' meaning "new") was discovered by Scottish chemist [[William Ramsay]] and English chemist [[Morris Travers]] in [[1898]].
-== Occurrence ==
-Neon is a [[monatomic]] [[gas]] at [[standard conditions]]. Neon is rare, found in the [[Earth's atmosphere]] at 1 part in 65,000 and industrially produced by cryogenic [[fractional distillation]] of liquified air. Neon, like [[water vapor]], is less dense than air; unlike water vapor, which condenses into a liquid below the stratosphere and is thus trapped in Earth's atmosphere, neon may slowly leak out into space, which could explain its scarcity on Earth.{{Citation needed}} [[Argon]], in contrast, is denser than air and so remains within Earth's atmosphere.
-== Compounds ==
-The [[ion]]s, Ne<sup>+</sup>, (Ne[[argon|Ar]])<sup>+</sup>, (Ne[[hydrogen|H]])<sup>+</sup>, and ([[helium|He]]Ne<sup>+</sup>), have been observed from optical and [[mass spectrometry|mass spectrometric]] research. In addition, neon forms an unstable [[hydrate]].
-== Isotopes ==
-Neon has three [[stable isotope]]s: <sup>20</sup>Ne (90.48%), <sup>21</sup>Ne (0.27%) and <sup>22</sup>Ne (9.25%). <sup>21</sup>Ne and <sup>22</sup>Ne are [[nucleogenic]] and their variations are well understood. In contrast, <sup>20</sup>Ne is not known to be nucleogenic and the causes of its variation in the [[Earth]] have been hotly debated. The principal [[nuclear reaction]]s which generate neon [[isotope]]s are [[neutron emission]], [[alpha decay]] reactions on <sup>24</sup>Mg and <sup>25</sup>Mg, which produce <sup>21</sup>Ne and <sup>22</sup>Ne, respectively. The [[alpha particle]]s are derived from [[uranium]]-series [[decay chain]]s, while the [[neutron]]s are mostly produced by secondary reactions from alpha particles. The net result yields a trend towards lower <sup>20</sup>Ne/<sup>22</sup>Ne and higher <sup>21</sup>Ne/<sup>22</sup>Ne ratios observed in uranium-rich rocks such as [[granite]]s. Isotopic analysis of exposed terrestrial [[rock (geology)|rocks]] has demonstrated the [[cosmogenic]] production of <sup>21</sup>Ne. This isotope is generated by [[spallation]] reactions on [[magnesium]], [[sodium]], [[silicon]], and [[aluminium]]. By analyzing all three isotopes, the cosmogenic component can be resolved from [[magma]]tic neon and nucleogenic neon. This suggests that neon will be a useful tool in determining cosmic [[exposure age]]s of surficial rocks and [[meteorite]]s.[http://www.onafarawayday.com/Radiogenic/Ch11/Ch11-2.htm]
-Similar to [[xenon]], neon content observed in samples of [[volcano|volcanic]] [[gas]]es are enriched in <sup>20</sup>Ne, as well as nucleogenic <sup>21</sup>Ne, relative to <sup>22</sup>Ne content. The neon isotopic content of these mantle-derived samples represent a non-atmospheric source of neon. The <sup>20</sup>Ne-enriched components are attributed to exotic primordial rare gas components in the Earth, possibly representing [[solar neon]]. Elevated <sup>20</sup>Ne abundances are also found in [[diamond]]s, further suggesting a solar neon reservoir in the Earth.[http://www.mantleplumes.org/Ne.html]
-==References==
-*[http://periodic.lanl.gov/elements/10.html Los Alamos National Laboratory &ndash; Neon]
-* [http://wwwrcamnl.wr.usgs.gov/isoig/period/ne_iig.html USGS Periodic Table - Neon]
 == External links ==
-{{Commons|Neon}}
+All links retrieved November 11, 2022.
-{{wiktionary|neon}}
 * [http://www.webelements.com/webelements/elements/text/Ne/index.html WebElements.com &ndash; Neon]
 * [http://education.jlab.org/itselemental/ele010.html It's Elemental &ndash; Neon]
-* [http://www.compchemwiki.org/index.php?title=Neon Computational Chemistry Wiki]
+*[http://wwwrcamnl.wr.usgs.gov/isoig/period/ne_iig.html USGS Periodic Table - Neon]
-[[Category:Neon| ]]
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