Neon is a monatomic atom that is considered relatively inert. It does not even combine with itself to form a diatomic molecule, as do some other gases. Know the Uses of Neon, Chemical Properties of Neon and more. Neon is the tenth element with a total of 10 electrons. In writing the electron configuration for neon the first two electrons will go in the 1s orbital. Since 1s can only hold two electrons the next 2 electrons for Ne go in the 2s orbital. The remaining six electrons will go in the 2p orbital. Each neon atom has 10 protons. There are three stable isotopes of the element, with atoms having 10 neutrons (neon-20), 11 neutrons (neon-21), and 12 neutrons (neon-22). Because it has a stable octet for its outer electron shell, neon atoms have 10 electrons and no net electrical charge. Oct 29, 2019 - Explore Paula Smith's board 'Neon atom' on Pinterest. See more ideas about neon atom, atom, atom model. Below is a 3D model of a Neon atom. As it is the 10th element, Neon has 10 protons (purple) in its nucleus, and in the most common isotope, 10 neutrons (green) as well. It has this same number of electrons (blue) that orbit the nucleus - 2 in the first energy level and 8 in the second.
GAS DISCHARGE TUBES emit different colors depending on the element contained inside. Neon signs are orange, like the word physics above.
It's much easier to explain why neon isn't inert in a discharge tube than it is to explain why it is inert to chemical reactions. The voltage across a discharge tube will accelerate a free electron up to some maximum kinetic energy. The voltage must be large enough so that this energy is more than that required to 'ionize' the atom. An ionized atom has had an electron plucked out of an orbital to make it a 'free' particle, and the atom it leaves behind has become a positively charged ion. The resulting plasma of charged ions and electrons carries the electric current between the tube's electrodes.
The photo (above) shows a gas discharge sign designed by Sam Sampere of Syracuse University. This sign incorporates a neon discharge tube (the orange word 'Physics') and mercury discharge tubes (the blue word 'Experience' and the outer frame). The sculpture at the bottom of the sign represents the electric and magnetic fields of light. The white and yellow sine waves in the sculpture are actually fluorescent lights. These fluorescent lights are mercury discharge tubes with special coatings on their inner walls. The ultraviolet light emitted by the mercury discharge inside a tube is absorbed by the coating, which subsequently emits light of a different color (and with a lower photon energy). Depending on the exact material of the coating, a whole range of colors can be obtained.
So why do these gas discharges emit light? As an alternative to being removed by an energetic collision, an electron on an atom can be excited. One speaks of the electron as having been promoted to an orbital of higher energy. When the electron eases back down to its original orbital, a particle of light (a photon) carries away the energy of excitationand the discharge tube glows! A photon's energy (its wavelength or color) depends on the energy difference between orbitals. A given atom can emit photons at many energies corresponding to its different pairs of orbitals. This series of photon energiesthe emission lines to a spectroscopistis unique to a particular atom. As can be seen in the sign, the mercury discharge tubes have a very different hue than the neon discharge tube does. The inert gas helium was actually discovered this way, and observations of sunlight revealed a series of photon energies that had never before been seen in discharges on the earth.
The chemical inertness of certain gases is subtler to explain. Generally speaking, when two atoms come into proximity, the highest energy, or valence, orbitals of the atoms change substantially and the electrons on the two atoms reorganize. If this reorganization lowers the total energy of the electrons involved, a chemical bond can form. For ordinary, non-inert atoms, the electrons are relatively pliable and bonds often form. The electrons in inert gases, however, are relatively resistant to this proximity effect, so these gases very rarely bond to form molecules.
The apparent contradiction between the inertness of a gas (with respect to chemical bonding) and its liveliness (in a glow discharge) is an example of a broader phenomenon that we might call the unbearable inertness of matter. An atom may be considered as an inert, unreactive particle as long as the energy of its interaction with other particles (including photons) is small enough so that the atom's electrons don't get excited. Atoms of inert gases like neon are the most tenaciously laid back. Still, as interaction energies increase, even they lose their inertness, and we ultimately get a soup of inert nuclei and electronsa highly excited plasma. Increase the energy more (actually, a lot more), and the nuclei are no longer so inert either. We get instead a brew of nucleonsas in a neutron star. Step up the energy some more, and we enter the realm of quarks. Here even nucleons are no longer inertand we have returned to the incredibly energetic, primordial conditions that prevailed shortly after the big bang.
Answer originally posted December 4, 2001.
Neon Atomic Number
Neon is a noble gas, and perhaps surprisingly, the fifth most plentiful element in the cosmos (after hydrogen, helium, oxygen and carbon); however, its abundance in Earth’s atmosphere is rather rare (about 18 ppm). No known neutral compounds exist with this chemically unreactive element, and therefore neon cannot affix itself to any solids. It is theorized that neon’s volatile nature with high vapor pressure and relative lightness caused the element to escape in large quantities during the formation of Earth as a planet, under the sun’s blanket of heat. Neon was discovered, as with many noble gases, through fractional distillation of liquefied air in 1898 by British chemists Sir William Ramsay and Morris Travers. In fact, this rare atmospheric element was discovered a mere two weeks after another noble gas, krypton. This method of isolating atmospheric elements was clearly fruitful as Ramsay won the Nobel Prize for Chemistry in 1904 for these numerous discoveries.
Neon is an iconic element and can only be produced through fractional distillation of liquefied air. Because of these two factors, neon can be a relatively expensive element to produce and purchase. Its attractive characteristics in lighting applications are enabled by its activation (atom separation and recombination in a vacuum tube) at nominal voltages and currents in modern electrical systems. Neon itself is reddish-orange when activated, but lighting apparatuses can replicate a number of colors in the visible spectrum when neon is mixed with other gases. For this reason, neon was the precursor of today’s modern plasma displays and TV screens. Lesser known applications include neon as a refrigerant in its liquid form. It has 40 times the refrigerant capacity of liquid helium and three times the refrigerant capacity of liquid hydrogen.
Neon has three stable isotopes: 20Ne, 21Ne, and 22Ne. 21Ne and 22Ne are both primordial (have existed since the formation of the earth) and nucleogenic (produced through naturally-occurring nuclear reactions). The nucleogenic instances of neon isotopes are known to be a result of nuclear reactions, primarily with 24Mg and 25Mg. 20Ne, on the other hand, is known to be primordial but not nucleogenic. The relative sources of 20Ne, while the most abundant of the three isotopes on earth, is debated to this day. Due to the enriched amounts of 20Ne in volcanic gas and its presence in diamonds, some theorize that there may exist a “solar neon reservoir” in the Earth. Throughout this scientific discovery and analysis process of all three naturally-occurring neon isotopes, it is now being theorized that neon can be useful in determining cosmic exposure ages of meteorites and rocks located on a planetary body’s surface.
Neon is a Block P, Group 18, Period 10 element. The number of electrons in each of Neon's shells is 2, 8 and its electronic configuration is 1s2 2s2 2p6. In its elemental form neon's CAS number is 7440-01-9. The neon atom has a covalent radius of 58.pm and it's Van der Waals radius is 154.pm. Neon is found in small amounts in the Earth's atmosphere and is commercially produced by cryogenic fractional distillation of liquefied air. Neon was discovered and first isolated by Sir William Ramsay and Morris W. Travers in 1898. The origin of the name comes from the Greek word neon meaning new.
Neon information, including technical data, properties, and other useful facts are specified below. Scientific facts such as the atomic structure, ionization energy, abundance on Earth, conductivity, and thermal properties are included.
|Element Category:||noble gases|
|Group, Period, Block:||18, 2, p|
|Melting Point:||-248.59°C, -415.462°F, 24.56 K|
|Boiling Point:||-246.053°C, -410.895°F, 27.097 K|
|Density:||1442 (5 K) kg·m3|
|Liquid Density @ Melting Point:||1.207 g·cm3|
|Density @ 20°C:||0.0009 g/cm3|
|Density of Solid:||1444 kg·m3|
|Triple Point:||24.556 K, 43.37 kPa|
|Critical Point:||44.4918 K, 2.7686 MPa|
|Heat of Fusion (kJ·mol-1):||0.324|
|Heat of Vaporization (kJ·mol-1):||1.736|
|Heat of Atomization (kJ·mol-1):||0|
|Thermal Conductivity:||49.1x10-3 W·m-1·K-1|
|Molar Heat Capacity:||5R/2 = 20.786 J·mol-1·K-1|
|Bulk Modulus:||654 GPa|
|Speed of Sound:||(gas, 0 °C) 435 m·s-1|
|Allred Rochow Electronegativity:||4.84|
|Mulliken-Jaffe Electronegativity:||3.98 (12.5% s orbital)|
Neon Atom Structure
|Covalent Radius:||58 pm|
|Covalent Radius (Å):||0.62|
|Van der Waals Radius:||154 pm|
|Oxidation States:||1, 0|
|Crystal Structure:||face-centered cubic|
|Electron Affinity (kJ·mol-1)||Not stable|
|1st Ionization Energy:||2080.7 kJ·mol-1|
|2nd Ionization Energy:||3952.3 kJ·mol-1|
|3rd Ionization Energy:||6122 kJ·mol-1|
|Earth - Total:||0.50E-8 cm^3/g|
|Mercury - Total:||N/A|
|Venus - Total:||49E-8 cm^3/g|
|Earth - Seawater (Oceans), ppb by weight:||0.12|
|Earth - Seawater (Oceans), ppb by atoms:||0.037|
|Earth - Crust (Crustal Rocks), ppb by weight:||3|
|Earth - Crust (Crustal Rocks), ppb by atoms:||3|
|Sun - Total, ppb by weight:||1000000|
|Sun - Total, ppb by atoms:||70000|
|Stream, ppb by weight:||N/A|
|Stream, ppb by atoms:||N/A|
|Meterorite (Carbonaceous), ppb by weight:||N/A|
|Meterorite (Carbonaceous), ppb by atoms:||N/A|
|Typical Human Body, ppb by weight:||N/A|
|Typical Human Body, ppb by atom:||N/A|
|Universe, ppb by weight:||1300000|
|Universe, ppb by atom:||80000|
|Discovered By:||William Ramsay & Morris Travers|
|First Isolation:||William Ramsay & Morris Travers (1898)|
Health, Safety & Transportation Information for Neon
Neon is not toxic and is chemically inert, and thus poses minimal environmental or health threats. At room temperature, neon is typically only harmful when its presence leads to displacement of oxygen in the air, creating potential for asphyxiation. Liquid neon is extremely cold; therefore skin contact with the liquid can cause frostbite, and should be avoided.
Neon Atomic Mass
|Material Safety Data Sheet||MSDS|
|Globally Harmonized System of |
Classification and Labelling (GHS)
Neon has three stable isotopes: 20Ne, 21Ne, and 22Ne
Neon Atom Drawing
|Nuclide||Isotopic Mass||Half-Life||Mode of Decay||Nuclear Spin||Magnetic Moment||Binding Energy (MeV)||Natural Abundance|
(% by atom)
|16Ne||16.025761(22)||9E-21 s [122(37) keV]||2p to 14O||0+||N/A||94.75||-|
|17Ne||17.017672(29)||109.2(6) ms||ß+ + p to 16O; ß+ + a to 13N; ß+ to 17F||1/2-||N/A||110.28||-|
|18Ne||18.0057082(3)||1.672(8) s||EC to 18F||0+||N/A||129.54||-|
|19Ne||19.0018802(3)||17.296(5) s||EC to 19F||1/2+||-1.885||141.34||-|
|23Ne||22.99446690(11)||37.24(12) s||ß- to 23Na||5/2+||-1.08||180.18||-|
|24Ne||23.9936108(4)||3.38(2) min||ß- to 24Na||0+||N/A||189.19||-|
|25Ne||24.997737(28)||602(8) ms||ß- to 25Na||(3/2)+||N/A||193.54||-|
|26Ne||26.000461(29)||197(1) ms||ß- to 26Na; ß- + n to 25Na||0+||N/A||198.83||-|
|27Ne||27.00759(12)||32(2) ms||ß- to 27Na; ß- + n to 26Na||(3/2+)#||N/A||200.38||-|
|28Ne||28.01207(16)||18.3(22) ms||ß- to 28Na; ß- + n to 27Na||0+||N/A||203.8||-|
|29Ne||29.01939(29)||15.6(5) ms||ß- to 29Na||(3/2+)#||N/A||205.36||-|
|30Ne||30.02480(61)||5.8(2) ms||ß- to 30Na||0+||N/A||208.78||-|
|31Ne||31.03311(97)#||3.4(8) ms||ß- to 31Na; ß- + n to 30Na||7/2-#||N/A||208.48||-|
|32Ne||32.04002(86)#||3.5(9) ms||ß- + n to 31Na; ß- to 32Na||0+||N/A||210.03||-|
|34Ne||34.05703(87)#||1# ms [>1.5 µs]||Unknown||0+||N/A||210.35||-|