Argon

18

chlorine ← argon → potassium


Ne
↑
Ar
↓
Kr




periodic table




General


Name, Symbol, Number

argon, Ar, 18


Chemical series
noble gases


Group, Period, Block

18, 3, p


Appearance
colorless 



Atomic mass
39.948(1) g/mol


Electron configuration
[Ne] 3s2 3p6


Electrons per shell
2, 8, 8


Physical properties


Phase
gas


Density
(0 °C, 101.325 kPa)
 1.784 g/L


Melting point
83.80 K
(-189.35 °C, -308.83 °F)


Boiling point
87.30 K
(-185.85 °C, -302.53 °F)


Critical point
150.87 K, 4.898 MPa


Heat of fusion
1.18 kJ/mol


Heat of vaporization
6.43 kJ/mol


Heat capacity
(25 °C) 20.786 J/(mol·K)




Vapor pressure


P/Pa
1
10
100
1 k
10 k
100 k


at T/K
 
47
53
61
71
87



Atomic properties


Crystal structure
cubic face centered


Oxidation states
0


Electronegativity
no data (Pauling scale)


Ionization energies
(more)

1st: 1520.6 kJ/mol


2nd: 2665.8 kJ/mol


3rd: 3931 kJ/mol


Atomic radius
71 pm


Atomic radius (calc.)
71 pm


Covalent radius
97 pm


Van der Waals radius
188 pm


Miscellaneous


Magnetic ordering
nonmagnetic


Thermal conductivity
(300 K) 17.72 mW/(m·K)


Speed of sound
(gas, 27 °C) 323 m/s


CAS registry number
7440-37-1


Notable isotopes




Main article: Isotopes of argon


iso

NA

half-life

DM

DE (MeV)

DP


36Ar

0.337%

Ar is stable with 18 neutrons


37Ar

syn

35 d

ε

?

37Cl


38Ar

0.063%

Ar is stable with 20 neutrons


39Ar

syn

269 y

β-

0.565

39K


40Ar

99.600%

Ar is stable with 22 neutrons


42Ar

syn

32.9 y

β-

0.600

42K


Argon (chemical symbol Ar, atomic number 18) is a member of the noble gas family of elements. It is present in the Earth's atmosphere at slightly under one percent (by volume), making it the most common noble gas on Earth.

Contents

1 Occurrence
2 History
3 Notable Characteristics

3.1 Isotopes


4 Compounds
5 Applications
6 Footnotes
7 References
8 External links
9 Credits



The inertness of argon is a very useful property for a number of applications. For instance, it helps protect filaments in incandescent lightbulbs, it provides an inert shield for various forms of welding and during the production of reactive elements, and it offers a protective cover when growing silicon and germanium crystals. As this gas is a poor conductor of heat, it is useful for thermal insulation in energy-efficient windows and for inflating scuba diving suits. Blue argon lasers are used in surgery to weld arteries, destroy tumors, and correct eye defects. The isotope argon-39 has been used for groundwater dating and ice coring.

Occurrence
Argon constitutes 0.934 percent by volume and 1.29 percent by mass of the Earth's atmosphere, and air is the primary raw material used by industry to produce purified argon products. Argon is usually isolated by the technique of fractional distillation of liquefied air. This process also produces purified nitrogen, oxygen, neon, krypton, and xenon.
By contrast, the Martian atmosphere contains 1.6 percent of argon-40 and five ppm of argon-36. In 1973, the Mariner spaceprobe fly-by of the planet Mercury found that Mercury has a very thin atmosphere containing 70 percent argon, believed to result from releases of the gas as a decay product from radioactive materials on the planet. In 2005, the Huygens probe also discovered the presence of argon-40 on Titan, the largest moon of Saturn.[1]

History
Argon (from the Greek word αργός, meaning "inactive") was suspected to be present in air by Henry Cavendish in 1785. It was not discovered, however, until 1894, when Lord Rayleigh and Sir William Ramsay performed an experiment in which they removed all the oxygen and nitrogen from a sample of air. Argon was also encountered in 1882, by the independent research of H.F. Newall and W.N. Hartley. Each investigator observed new lines in the color spectrum of air, but they were unable to identify the element responsible for the lines. Argon became the first member of the noble gases to be discovered.

Notable Characteristics
Argon, an extremely unreactive element, is a member of the noble gas series in the periodic table. It is situated between neon and krypton in group 18 (former group 8A), and is placed after chlorine in period three.
Argon is colorless and odorless in both its liquid and gaseous forms. It is inert under most conditions and forms no confirmed stable compounds at room temperature. The creation of argon hydrofluoride (HArF)—a metastable compound of argon with fluorine and hydrogen—was first reported by researchers at the University of Helsinki in 2000 (see Compounds below).
This element can also form "clathrates" (cage-like molecules) with water, when its atoms are trapped in a lattice of water molecules. Also, argon-containing ions (such as ArH+) and excited state complexes (such as ArF) are well-known. Theoretical calculations (by computer) have shown several argon compounds that should be stable but for which no synthesis routes are currently known.
Argon and oxygen are about equally soluble in water and are 2.5 times more soluble in water than nitrogen.[2]

Isotopes
The main isotopes of argon found on Earth are 40Ar, 36Ar, and 38Ar. Naturally occurring 40K (potassium-40), with a half-life of 1.250×109 years, decays to stable 40Ar (11.2%) by electron capture and positron emission, and it also transforms to stable 40Ca (88.8%) via beta decay. These properties and ratios are used to determine the age of rocks.
In the Earth's atmosphere, 39Ar is made by cosmic ray activity, primarily with 40Ar. In the subsurface environment, argon is also produced through neutron capture by 39K or alpha emission by calcium. 37Ar is created from the decay of 40Ca as a result of subsurface nuclear explosions. It has a half-life of 35 days.

Compounds
The extreme inertness of argon and other noble gases is attributed to the electronic structure of their atoms. The atom of each of these elements has a set of eight electrons (an "octet") in its outermost shell, which gives the atom stability and makes it resistant to bonding with other elements.
Before 1962, the noble gases were considered to be entirely unable to form any compounds. Since then, however, compounds of the heavier noble gases have been synthesized. In 2000, the first argon compounds were formed by researchers at the University of Helsinki. By shining ultraviolet light onto frozen argon containing a small amount of hydrogen fluoride, argon hydrofluoride (HArF) was formed.[3] It was found to be stable up to a temperature of 40 kelvin.

Applications
 An argon-filled discharge tube glows brightly when an electric current is passed through it.
Argon is used in incandescent lighting and other applications in which diatomic nitrogen is not sufficiently inert. Argon will not react with the filament of lightbulbs even at high temperatures.
It is also used as an inert gas shield in many forms of welding, including tungsten inert gas welding.
It is a nonreactive blanket in the manufacture of titanium and other reactive elements.
It provides a protective atmosphere for growing silicon and germanium crystals.
This gas is used in plasma globes.
It is useful for thermal insulation in energy-efficient windows.
Argon-39 has been used for a number of applications, primarily ice coring. It has also been used for groundwater dating.
Cryosurgery procedures, such as cryoablation, use liquefied argon to destroy cancer cells.
Liquid argon is used in calorimetry in experimental particle physics.
Argon is used in technical scuba diving to inflate the dry suit, because the gas is inert and has low thermal conductivity.
Blue argon lasers are used in surgery to weld arteries, destroy tumors, and correct eye defects.
Given its inert qualities, it is used by museum conservators to protect old materials that are prone to gradual oxidation in air.
Footnotes

↑ Titan

↑ Properties of Argon

↑ The Noble Gases


ReferencesISBN links support NWE through referral fees
Los Alamos National Laboratory – Argon Retrieved August 31, 2007.
USGS Periodic Table - Argon Retrieved August 31, 2007.
Emsley, J. Nature’s Building Blocks. Oxford, NY: Oxford University Press, 2001.
Brown, T.L., B.E. Bursten, and H.E. LeMay. In Chemistry: The Central Science, 10th ed. Upper Saddle River, NJ: Pearson Education, Inc., 2006.
External links
All links retrieved November 5, 2021.

Argon: the essentials WebElements.com
Why Argon? by Eric Maiken
Argon Properties, Uses, Applications







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