Argon compounds

Source: Wikipedia, the free encyclopedia.

Argon compounds, the chemical compounds that contain the element

molecular ions containing argon have been made and also detected in space. One solid interstitial compound of argon, Ar1C60 is stable at room temperature. Ar1C60 was discovered by the CSIRO
.

Argon ionises at 15.76 eV, which is higher than hydrogen, but lower than helium, neon or fluorine.

effective core potentials are used to model the inner electrons, so that their contributions do not have to be individually computed. More powerful computers since the 1990s have made this kind of in silico study much more popular, being much less risky and simpler than an actual experiment.[5]
This article is mostly based on experimental or observational results.

The argon fluoride laser is important in photolithography of silicon chips. These lasers make a strong ultraviolet emission at 192 nm.[6]

Argonium

Main article: Argonium

molecular hydrogen H2 is in the range of 0.0001 to 0.001.[1]

Argonium is formed when H2+ reacts with Ar atoms:[1]

Ar + H+
2 → ArH+ + H[1]

and it is also produced from Ar+ ions produced by cosmic rays and X-rays from neutral argon:

Ar+ + H2 → *ArH+ + H[1] 1.49 eV.[7]

When ArH+ encounters an electron, dissociative recombination can occur, but it is extremely slow for lower energy electrons, allowing ArH+ to survive for a much longer time than many other similar protonated cations.

ArH+ + e− → ArH* → Ar + H[1]

Artificial ArH+ made from earthly Ar contains mostly the isotope 40Ar rather than the cosmically abundant 36Ar. Artificially it is made by an electric discharge through an argon-hydrogen mixture.[8]

Natural occurrence

In the

column density of ArH+ in the Crab Nebula is between 1012 and 1013 atoms per square centimeter.[7] Possibly the energy required to excite the ions so that then can emit, comes from collisions with electrons or hydrogen molecules.[7] Towards the Milky Way centre the column density of ArH+ is around 2×1013 cm−2.[1]

Cluster argon cations

The diargon cation, Ar+
2 has a binding energy of 1.29 eV.[9]

The triargon cation Ar+
3 is linear, but has one Ar−Ar bond shorter than the other. Bond lengths are 2.47 and 2.73

ångströms. The dissociation energy to Ar and Ar2+ is 0.2 eV. In line with the molecule's asymmetry, the charge is calculated as +0.10, +0.58 and +0.32 on each argon atom, so that it greatly resembles Ar+
2 bound to a neutral Ar atom.[10]

Larger charged argon clusters are also detectable in mass spectroscopy. The tetraargon cation is also linear. Ar+
13

evaporating from the cluster one at a time. The process of destroying a cluster by light is called photofragmentation.[11]

Negatively-charged argon clusters are thermodynamically unstable, and therefore cannot exist. Argon has a negative electron affinity.[11]

Argon monohydride

Neutral argon hydride, also known as argon monohydride (ArH), was the first discovered noble gas hydride. J. W. C. Johns discovered an emission line of ArH at 767 nm and announced the find in 1970. The molecule was synthesized using X-ray irradiation of mixtures of argon with hydrogen-rich molecules such as H2, H2O, CH4 and CH3OH.[12] The X-ray excited argon atoms are in the 4p state.[13]

Argon monohydride is unstable in its ground state, 4s, as a neutral inert gas atom and a hydrogen atom repel each other at normal intermolecular distances. When a higher-energy-level ArH* emits a photon and reaches the ground state, the atoms are too close to each other, and they repel and break up. However a

Rydberg molecules, also known as excimers. These Rydberg molecules can be considered as a protonated argon core, surrounded by an electron in one of many possible higher energy states.[15]

Formation: Ar + ν → Ar*;  Ar* + H2 → ArH* + H[12]

Instead of dihydrogen, other hydrogen containing molecules can also have a hydrogen atom abstracted by excited argon, but note that some molecules bind hydrogen too strongly for the reaction to proceed. For example, acetylene will not form ArH this way.[12]

In the van der Waals molecule of ArH, the bond length is calculated to be about 3.6 Å and the

dissociation energy calculated to be 0.404 kJ/mol (33.8 cm−1).[16] The bond length in ArH* is calculated as 1.302 Å.[17]

The spectrum of argon monohydride, both ArH* and Ar

predissociated, blurring out the lines.[19] In the UV spectrum a continuous band exists from 200 to 400 nm. This band is due to two different higher states: B2Π → A2Σ+ radiates over 210–450 nm, and E2Π → A2Σ+ is between 180 and 320 nm.[20] A band in the near infrared from 760 to 780 nm.[21]

Other ways to make ArH include a Penning-type discharge tube, or other electric discharges. Yet another way is to create a beam of ArH+ (argonium) ions and then neutralize them in laser-energized caesium vapour. By using a beam, the lifetimes of the different energy states can be observed, by measuring the profile of electromagnetic energy emitted at different wavelengths.[22] The E2π state of ArH has a radiative lifetime of 40 ns. For ArD the lifetime is 61 ns. The B2Π state has a lifetime of 16.6 ns in ArH and 17 ns in ArD.[20]

Argon polyhydrides

The argon dihydrogen cation ArH+
2 has been predicted to exist and to be detectable in the interstellar medium. However it has not been detected as of 2021.[23] ArH+
2 is predicted to be linear in the form Ar−H−H. The H−H distance is 0.94 Å. The dissociation barrier is only 2 kcal/mol (8 kJ/mol), and ArH+
2 readily loses a hydrogen atom to yield ArH+.[24] The force constant of the ArH bond in this is 1.895 mdyne/Å2 (1.895×1012 Pa).[25]

The argon trihydrogen cation ArH+
3 has been observed in the laboratory.[23][26] ArH2D+, ArHD+
2 and ArD+
3 have also been observed.[27] The argon trihydrogen cation is planar in shape, with an argon atom off the vertex of a triangle of hydrogen atoms.[28]

Argoxonium

The argoxonium ion ArOH+ is predicted to be bent molecular geometry in the 11A′ state. 3Σ− is a triplet state 0.12 eV higher in energy, and 3A″ is a triplet state 0.18 eV higher. The Ar−O bond is predicted to be 1.684 Å long[23] and to have a force constant of 2.988 mdyne/Å2 (2.988×1012 Pa).[25]

ArNH+

ArNH+ is a possible ionic molecule to detect in the lab, and in space, as the atoms that compose it are common. ArNH+ is predicted to be more weakly bound than ArOH+, with a force constant in the Ar−N bond of 1.866 mdyne/Å2 (1.866×1012 

angle at the nitrogen atom is predicted to be 97.116°. The Ar−N lengths should be 1.836 Å and the N−H bond length would be 1.046 Å[25][29]

Argon dinitrogen cation

The argon dinitrogen linear cationic complex has also been detected in the lab:

Ar + N+
2 → ArN+
2 photodissociation→ Ar+ + N2.[23]

The dissociation yields Ar+, as this is a higher-energy state.[9] The binding energy is 1.19 eV.[9] The molecule is linear. The distance between two nitrogen atoms is 1.1 Å. This distance is similar to that of neutral N2 rather than that of N+
2 ion. The distance between one nitrogen and the argon atom is 2.2 Å.[9] The vibrational band origin for the nitrogen bond in ArN+
2 (V = 0 → 1) is at 2272.2564 cm−1 compared with N2+ at 2175 and N2 at 2330 cm−1.[9]

In the process of photodissociation, it is three times more likely to yield Ar+ + N2 compared to Ar + N+
2.[30]

ArHN+
2

ArHN+
2 has been produced in a supersonic jet expansion of gas and detected by Fourier transform microwave spectroscopy.[26] The molecule is linear, with the atoms in the order Ar−H−N−N. The Ar−H distance is 1.864 Å. There is a stronger bond between hydrogen and argon than in ArHCO+.[31]

The molecule is made by the following reaction:

ArH+ + N2 → ArHN+
2.[31]

Bis(dinitrogen) argon cation

The argon ion can bond two molecules of dinitrogen (N2) to yield an ionic complex with a linear shape and structure N=N−+Ar−N=N. The N=N bond length is 1.1014 Å, and the nitrogen to argon bond length is 2.3602 Å. 1.7 eV of energy is required to break this apart to N2 and ArN+
2. The band origin of an infrared band due to antisymmetric vibration of the N=N bonds is at 2288.7272 cm−1. Compared to N2 it is redshifted 41.99 cm−1. The ground state rotational constant of the molecule is 0.034296 cm−1.[30]

Ar(N
2)+
2 is produced by a supersonic expansion of a 10:1 mixture of argon with nitrogen through a nozzle, which is impacted by an

electron beam.[30]

ArN2O+

ArN2O+ absorbs photons in four violet–ultraviolet wavelength bands leading to breakup of the molecule. The bands are 445–420, 415–390, 390–370, and 342 nm.[32][33]

ArHCO+

ArHCO+ has been produced in a supersonic-jet expansion of gas and detected by Fabry–Perot-type Fourier transform microwave spectroscopy.[26][34]

The molecule is made by this reaction

ArH+ + CO → ArHCO+.[31]

Carbon dioxide–argon ion

ArCO+
2 can be excited to form ArCO+
2* where the positive charge is moved from the carbon dioxide part to the argon. This molecule may occur in the upper atmosphere. Experimentally the molecule is made from a low-pressure argon gas with 0.1%

electron beam. Argon is ionized, and can transfer the charge to a carbon dioxide molecule.[35] The dissociation energy of ArCO+
2 is 0.26 eV.[35]

ArCO+
2 + CO2 → Ar + CO
2·CO+
2 (yields 0.435 eV.)[35]

van der Waals molecules

Neutral argon atoms bind very weakly to other neutral atoms or molecules to form

London dispersion forces. The atoms that are to combine with argon can be produced by evaporation with a laser or alternatively by an electric discharge. The known molecules include AgAr, Ag2Ar, NaAr, KAr, MgAr, CaAr, SrAr, ZnAr, CdAr, HgAr, SiAr,[36] InAr, CAr,[37] GeAr,[38] SnAr,[39] and BAr.[40] SiAr was made from silicon atoms derived from Si(CH3)4.[41]

In addition to the very weakly bound van der Waals molecules, electronically excited molecules with the same formula exist. As a formula these can be written ArX*, with the "*" indicating an excited state. The atoms are much more strongly bound with a covalent bond. They can be modeled as an ArX+ surrounded by a higher energy shell with one electron. This outer electron can change energy by exchanging photons and so can fluoresce. The widely used argon fluoride laser makes use of the ArF* excimer to produce strong ultraviolet radiation at 192 nm. The argon chloride laser using ArCl* produces even shorter ultraviolet at 175 nm, but is too feeble for application.[42] The argon chloride in this laser comes from argon and chlorine molecules.[43]

Argon clusters

Cooled argon gas can form clusters of atoms.

face-centered cubic (fcc) structure, as in solid argon. It is the surface energy that maintains an icosahedral shape, but for larger clusters internal pressure will attract the atoms into an fcc arrangement.[11] Neutral argon clusters are transparent to visible light.[11]

Diatomic van der Waals molecules

Molecule Binding energy
ground Σ state
(cm−1) 		Binding energy
excited Π state
(cm−1) 		Ground state
bond length
(Å) 		Excited state
bond length
(Å) 		CAS number[44]
ArH 30736-04-0
ArHe 12254-69-2
LiAr 42.5 925 4.89 2.48[45]
BAr 149358-32-7
ArNe 12301-65-4
NaAr 40 560 56633-38-6
MgAr
 44 246 72052-59-6
AlAr 143752-09-4
SiAr[46]
ArCl 54635-29-9
Ar2 12595-59-4
KAr 42 373 12446-47-8
CaAr 62 134 72052-60-9
SrAr 68 136
NiAr 401838-48-0
ZnAr 96 706 72052-61-0
GaAr 149690-22-2
GeAr[38]
KrAr 51184-77-1
AgAr 90 1200
CdAr[47] 106 544 72052-62-1
InAr[48] 146021-90-1
SnAr[39]
ArXe 58206-67-0
AuAr 195245-92-2
HgAr 131 446 87193-95-1

ArO* is also formed when

vacuum ultraviolet
. It can be detected by its luminescence:

O2 + hv → O+
2 + e−;  O+
2 + e− → 2O*;  O* + Ar → ArO*.[49]

Light emitted by ArO* has two main bands, one at 2.215 eV, and a weaker one at 2.195 eV.[50]

Argon sulfide, ArS* luminesces in the

near infrared at 1.62 eV. ArS is made from UV irradiated OCS in an argon matrix. The excited states lasts for 7.4 and 3.5 μs for spectrum peak and band respectively.[51]

Triatomic van der Waals molecules

Cluster molecules containing

dichlorine and more than one argon atom can be made by forcing a 95:5 mixture of helium and argon and a trace of chlorine though a nozzle. ArCl2 exists in a T shape. Ar2Cl2 has a distorted tetrahedron shape, with the two argon atoms 4.1 Å from each other, and their axis 3.9 Å from the Cl2. The van der Waals bond energy is 447 cm−1. Ar3Cl2 also exists with a van der Waals bond energy of 776 cm−1.[52]

The linear Ar·Br2 molecule has a continuous spectrum for bromine molecule X → B transitions. The spectrum of bromine is blue-shifted and spread out when it binds an argon atom.[53]

ArI2 shows a spectrum that adds satellite bands to the higher vibrational bands of I2.[54] The ArI2 molecule has two different isomers, one shape is linear, and the other is T-shaped. The dynamics of ArI2 is complex. Breakup occurs through different routes in the two isomers. The T shape undergoes intramolecular vibrational relaxation, whereas the linear one directly breaks apart.[55] Diiodine clusters, I2Arn have been made.[56]

The ArClF cluster has a linear shape.[57] The argon atom is closest to the chlorine atom.[53]

Linear ArBrCl can also rearrange to ArClBr, or a T-shaped isomer.[58]

Multiple argon atoms can "

icosahedral shape. Molecules from Ar·H2O to Ar14·H2O have been studied.[59]

ArBH was produced from boron monohydride (BH) which in turn was created from diborane by way of an ultraviolet 193 nm laser. The BH-argon mixture was expanded through a 0.2 mm diameter nozzle into a vacuum. The gas mixture cools and Ar and BH combine to yield ArBH. A band spectrum that combines the A1Π←X1Σ+ electronic transition, with vibration and rotation can be observed. The BH has singlet spin, and this is the first known van der Waals complex with a singlet spin pair of atoms. For this molecule the rotational constant is 0.133 cm−1, The dissociation energy is 92 cm−1 and distance from argon to boron atom is 3.70 Å.[60] ArAlH is also known to exist.[61]

MgAr2 is also known.[47]

Polyatomic van der Waals molecules

Some linear polyatomic molecules can form T-shaped van der Waals complexes with argon. These include

carbon oxysulfide, and ClCN. Others attach the argon atom at one end to continue to be linear, including HCN.[62]

Other polyatomic van der Waals compounds of argon, include those of fluorobenzene,[63] formyl radical (ArHCO),[64] 7-azaindole,[65] glyoxal,[66] sodium chloride (ArNaCl),[67] ArHCl,[68] and cyclopentanone.[69]

Molecule Name Ground state
binding energy
(cm−1) 		Closest position or atom
to argon 		Ground state
bond length of Ar
(Å) 		Bond angle
from atom
(degrees) 		Bond stretch force
or frequency 		dipole moment D CAS number references
(CH3)2F2Si·Ar Difluorodimethylsilane – argon
CH2F2·Ar Difluoromethane – argon F 3.485 58.6 [70]
CF3CN
trifluoromethylcyanide
argon 		C1 3.73 77 947504-98-5 [71]
CF2HCH3·Ar
1,1-difluoroethane
argon 		F – [72]
CH2FCH2F·Ar
1,2-difluoroethane
argon 		181 F 3.576 61 264131-14-8 [73]
CH3CHO·Ar Acetaldehyde argon 161 C-1 3.567 76.34 158885-13-3 [74]
C2H4O·Ar
oxirane
argon 		200 O 3.606 (CM) 72.34 [75]
ArBF3 Boron trifluoride argon B 3.325 on axis ArBF ≈90.5° 0.030 mdyn/Å 0.176 [76]
ArC6H6 benzene-argon on sixfold axis 3.53 from plane 0.12 [77]
ArPF3 argon phosphorus trifluoride complex P 3.953 from centre of mass 70.3° on PF2 face [78]
Ar-NCCN argon–cyanogen van der Waals complex centre of molecule 3.58 90° T shape 30 cm−1 0.0979 [62]
DCCDAr argon-deuterated acetylene centre of molecule 3.25 90° T shape 0.0008 mdyn/Å / 8.7 cm−1 [62]
SO3Ar sulfur trioxide argon S 3.350 on axis 90° from SO bond 0.059 mdyn/Å / 61 cm−1 [79]
Ar•HCCH acetylene argon T shape [80]
OCS•Ar [80]
CH3OH•Ar [80]
CH3Cl•Ar [80]
Pyridine argon [80]
Pyrrole argon [80]

Aqueous argon

Argon dissolved in water causes the pH to rise to 8.0,[81] apparently by reducing the number of oxygen atoms available to bind protons.[82]

With ice, argon forms a clathrate hydrate. Up to 0.6 GPa, the clathrate has a cubic structure. Between 0.7 and 1.1 GPa the clathrate has a tetragonal structure. Between 1.1 and 6.0 GPa the structure is body centered orthorhombic. Over 6.1 GPa, the clathrate converts into solid argon and ice VII.[83] At atmospheric pressure the clathrate is stable below 147 K.[84] At 295 K the argon pressure from the clathrate is 108 MPa.[85]

Argon fluorohydride

Argon fluorohydride was an important discovery in the rejuvenation of the study of noble gas chemistry. HArF is stable in solid form at temperatures below 17 K.[86] It is prepared by photolysis of hydrogen fluoride in a solid argon matrix.[87] HArArF would have such a low barrier to decomposition that it will likely never be observed.[88] However HBeArF is predicted to be more stable than HArF.[89]

Uranium compounds

CUO in a solid argon matrix can bind one, or a few argon atoms to yield CUO·Ar, CUO·Ar3 or CUO·Ar4. CUO itself is made by evaporating

octahedral, with a uranium centre and with the noble gas atoms around the equator.[92]

UO+
2 can bind up to five noble gas atoms in a ring around a linear O=+U=O core.[93] These molecules are produced when uranium metal is laser ablated into dioxygen. This produces UO, UO2, UO3, U+, and importantly UO+
2. UO+
2 is then condensed into a noble gas matrix, either a pure element or a mixture. Heavier noble gas atoms will tend to displace the lighter atoms. Ionic molecules produced this way include UO
2Ne
4Ar+
, UO
2Ne
3Ar+
2, UO
2Ne
2Ar+
3, UO
2NeAr+
4, UO
2Ar+
5, UO
2Ar
4Kr+
, UO
2Ar
3Kr+
2, UO
2Ar
2Kr+
3, UO
2ArKr+
4, UO
2Ar
4Xe+
, UO
2Ar
3Xe+
2, UO
2Ar
2Xe+
3, and UO
2ArXe+
4, which are identified by a shift in the U=O antisymmetric stretching frequency.[93]

Neutral UO2 condensed in solid argon is converted from one electronic state to another by the argon atom ligands. In argon the electron configuration is 5f2(δφ) whereas in neon it is 5f17s1 (the state 3H4g compared to 3Φ2u). This is because the argon atoms have a larger antibonding interaction with the 7s1 electron, forcing it into a different subshell. The argonated compound has a stretching frequency of 776 cm−1 compared to 914.8 cm−1 in neon.[94] The argon uranium dioxide molecule is likely UO2Ar5.[95]

Beryllium oxide

When

beryllia is evaporated into the matrix) ArBeO will be formed, and is observable by its infrared spectrum. The beryllia molecule is strongly polarised, and the argon atom is attracted to the beryllium atom.[92][96] The bond strength of Ar−Be is calculated to be 6.7 kcal/mol (28 kJ/mol). The Ar−Be bond length is predicted to be 2.042 Å.[97]

The cyclic Be2O2 molecule can bind two argon atoms, or one argon along with another noble gas atom.[98]

Analogously, beryllium reacting with hydrogen sulfide and trapped in an argon matrix at 4 K forms ArBeS. It has a binding energy calculated to be 12.8 kcal/mol (54 kJ/mol).[99]

ArBeO2CO (beryllium carbonate) has been prepared (along with Ne, Kr and Xe adducts).[100]

The cyclic beryllium sulfite molecule can also coordinate an argon atom onto the beryllium atom in solid neon or argon matrix.[101]

Carbonyl compounds

carbonyls that can react with argon. These were actually argon compounds discovered in 1975, and were known before the discovery of HArF, but are usually overlooked.[102] Tungsten normally forms a hexacarbonyl, but when subject to ultraviolet radiation it breaks into a reactive pentacarbonyl. When this is condensed into a noble gas matrix the infrared and UV spectrum varies considerably depending on the noble gas used. This is because the noble gas present binds to the vacant position on the tungsten atom. Similar results also occur with molybdenum and chromium.[103] Argon is only very weakly bound to tungsten in ArW(CO)5.[92][104] The Ar−W bondlength is predicted to be 2.852 Å.[103] The same substance is produced for a brief time in supercritical argon at 21 °C.[105] For ArCr(CO)5 the band maximum is at 533 nm (compared to 624 nm in neon, and 518 nm in krypton). Forming 18-electron complexes, the shift in spectrum due to different matrices was much smaller, only around 5 nm. This clearly indicates the formation of a molecule using atoms from the matrix.[5]

Other carbonyls and complexed carbonyls also have reports of bonding to argon. These include Ru(CO)2(PMe3)2Ar, Ru(CO)2(dmpe)2Ar, η6-C6H6Cr(CO)2Ar.[106] Evidence also exists for ArHMn(CO)4, ArCH3Mn(CO)4, and fac-(η2-dfepe)Cr(CO)3Ar.[5]

Other noble gas complexes have been studied by photolysis of carbonyls dissolved in liquid rare gas, possibly under pressure. These Kr or Xe complexes decay on the time scale of seconds, but argon does not seem to have been studied this way. The advantage of liquid noble gases is that the medium is completely transparent to infrared radiation, which is needed to study the bond vibration in the solute.[5]

Attempts have been made to study carbonyl–argon adducts in the gas phase, but the interaction appears to be too weak to observe a spectrum. In the gas form, the absorption lines are broadened into bands because of rotation that happens freely in a gas.

dimerize, eliminating argon.[5]

Coinage metal monohalides

The argon

coinage metal monohalides were the first noble gas metal halides discovered, when the metal monohalide molecules were put through an argon jet. There were first found in Vancouver in 2000.[107]
ArMX with M = Cu, Ag or Au and X = F,[108] Cl or Br have been prepared. The molecules are linear. In ArAuCl the Ar−Au bond is 2.47 Å, the stretching frequency is 198 cm−1 and the dissociation energy is 47 kJ/mol.[109] ArAgBr also has been made.[109] ArAgF has a dissociation energy of 21 kJ/mol.[109] The Ar−Ag bond-length in these molecules is 2.6 Å.[109] ArAgCl is isoelectronic with AgCl−
2 which is better known.[109] The Ar−Cu bond length in these molecules is 2.25 Å.[109]

Transition metal oxides

In a solid argon matrix

VO2 forms VO2Ar2, and VO4 forms VO4·Ar with binding energy calculated to be 12.8 and 5.0 kcal/mol (53 and 21 kJ/mol).[110] Scandium in the form of ScO+ coordinates five argon atoms to yield ScOAr+
5.[111] these argon atoms can be substituted by numbers of krypton or xenon atoms to yield even more mixed noble gas molecules. With yttrium, YO+ bonds six argon atoms, and these too can be substituted by varying numbers of krypton or xenon atoms.[112]

In the case of transition metal monoxides, ScO, TiO and VO do not form a molecule with one argon atom. However CrO, MnO, FeO, CoO and NiO can each coordinate one argon atom in a solid argon matrix.[113] The metal monoxide molecules can be produced by laser ablation of the metal trioxide, followed by condensation on solid argon. ArCrO absorbs at 846.3 cm−1, ArMnO at 833.1, ArFeO at 872.8, ArCoO at 846.2, Ar58NiO at 825.7 and Ar60NiO at 822.8 cm−1. All these molecules are linear.[113]

There are also claims of argon forming coordination molecules in NbO2Ar2, NbO4Ar, TaO4Ar,[114] VO2Ar2, VO4Ar,[110] Rh(η2-O2)Ar2, Rh(η2-O2)2Ar2, Rh(η2-O2)2(η1-OO)Ar.[115][116][117]

Tungsten trioxide, WO3, and tungsten dioxide mono-superoxide (η2-O2)WO2 can both coordinate argon in an argon matrix. The argon can be replaced by xenon or molecular oxygen to make xenon coordinated compounds or superoxides. For WO3Ar the binding energy is 9.4 kcal/mol and for (η2-O2)WO2 it is 8.1 kcal/mol.[118]

Other transition metal compounds

ArNiN2 binds argon with 11.52 kcal/mol. The bending frequency of ArN2 is changed from 310.7 to 358.7 cm−1 when argon attaches to the nickel atom.[119]

Other ions

Some other binary ions observed that contain argon include BaAr2+ and BaAr2+
2,[120] VAr+, CrAr+, FeAr+, CoAr+, and NiAr+.[5]

Gold and silver cluster ions can bind argon. Known ions are Au
3Ar+
, Au
3Ar+
2, Au
3Ar+
3, Au
2AgAr+
3 and AuAg
2Ar+
3. These have a triangular shaped metallic core with argon bound at the vertexes.[2]

ArF+ is also known[5] to be formed in the reaction

F+
2 + Ar → ArF+ + F

and also

Ar+ + F2 → ArF+ + F.

and also

SF2+
4 + Ar → ArF+ + SF+
3.[121]

The ions can be produced by ultraviolet light at 79.1 nm or less.[122] The ionisation energy of fluorine is higher than that of argon, so breakup occurs thus:

ArF+ → Ar+ + F.[123]

The millimeter wave spectrum of ArF+ between 119.0232 and 505.3155 GHz has been measured to calculate molecular constants B0 = 14.8788204 GHz, D0 = 28.718 kHz.

SbF−
6 or AuF−
6 anions.[123][125]

Excited or ionized argon atoms can react with molecular iodine gas to yield ArI+[126] Argon plasma is used as an ionisation source and carrier gas in

electrothermal vaporization or using helium gas can avoid these interference problems.[127] Argon can also form an anion with chlorine, ArCl−,[131]
though this is not a problem for mass spectrometry applications as only cations are detected.

The argon borynium ion, BAr+ is produced when BBr+ at energies between 9 and 11 eV reacts with argon atoms. 90% of the positive charge is on the argon atom.[132]

ArC+ ions can be formed when argon ions impact carbon monoxide with energies between 21 and 60 eV. However more C+ ions are formed, and when the energy is on the high side, O+ is higher.[133]

ArN+ can form when argon ions impact

dinitrogen with energies between 8.2 and 41.2 eV and peaking around 35 eV. However far more N+
2 and N+ are produced.[134]

ArXe+ is held together with a strength of 1445 cm−1 when it is in the X electronic state, but 1013 cm−1 when it is in the B excited state.[33]

Metal–argon cations are called "argides". The argide ions produced during

mass spectroscopy
have higher intensity when the binding energy of the ion is higher. Transition elements have higher binding and ion flux intensity compared to main group elements. Argides can be formed in the plasma by excited argon atoms reacting with another element atom, or by an argon atom binding with another ion:

Ar+ + M → ArM+ + e−; M+ + Ar → ArM+.[135]

Doubly charged cations, called

superelectrophiles, are capable of reacting with argon. Ions produced include ArCF2+
2 ArCH+
2, ArBF+
2 and ArBF2+
 containing bonds between argon and carbon or boron.[136]

Doubly ionised acetylene HCCH2+ reacts inefficiently with argon to yield HCCAr2+. This product competes with the formation of Ar+ and argonium.[137]

The SiF2+
3 ion reacts with argon to yield ArSiF2+
2.[138]

Ion Bond length
(Å) 		Dissociation energy
(kJ/mol)[5] 		Excited state
bond length (Å) 		Excited state
dissociation energy
ArH+ 3.4 eV
LiAr+[135] 2.343 0.30 eV
BeAr+[135] 4100 cm−1[139]
BAr+[132] 2.590 210
ArC+[140]
ArN+[135] 3.5 2.16 eV[141]
ArO+[135]
ArF+[123] 1.637 194
NaAr+[135] 19.3
MgAr+[135] 2.88[142] 1200 cm−1[139]
AlAr+[135] 982 cm−1[143]
SiAr+[135]
ArP+[135]
ArS+[135]
ArCl+[135]
Ar+
2[135]
CaAr+ 700 cm−1[139]
ScAr+[135]
TiAr+ 0.31eV[144]
VAr+ 2.65[145] 37,D0=2974 cm−1[142]
CrAr+ 28,D0=2340[142]
MnAr+[135] 0.149 eV[144]
FeAr+ 0.11 eV[144]
CoAr+[145] 2.385[146] 49,D0=4111 cm−1[146]
NiAr+ 53,D0=4572[142]
CuAr+[135] 0.53 eV[144]
ZnAr+ 2.72[147] 0.25 eV,[144] D0=2706 cm−1[147]
GaAr+[135]
AsAr+[135]
RbAr+[148]
SrAr+ 800[139]
ZrAr+ 2.72 D0 = 2706 cm−1[147] 3.050 1179 cm−1
NbAr+ 2.677[142] 37,D0=3106 cm−1[142]
AgAr+[135]
InAr+[149]
ArI+[126]
BaAr+ 600 cm−1[139]

Polyatomic cations

Metal ions can also form with more than one argon atom, in a kind of argon metal cluster. Different sized metal ions at the centre of a cluster can fit different geometries of argons atoms around the ion.

time of flight mass spectrometer analysis and by the photodissociation spectrum. Other study methods include Coulomb explosion analysis.[151] Argon-tagging is a technique whereby argon atoms are weakly bound to a molecule under study. It results in a much lower temperature of the tagged molecules, with sharper infra-red absorption lines. The argon-tagged molecules can be disrupted by photons of a particular wavelength.[152]

Lithium ions add argon atoms to form clusters with more than a hundred argon atoms. The clusters Li+Ar4, and Li+Ar4 are particularly stable and common. Calculations show that the small clusters are all quite symmetrical. Li+Ar2 is linear, Li+Ar3 is flat and triangular shaped with D3h symmetry, Li+Ar4 is tetrahedral, Li+Ar5 could be a square pyramid or trigonal bipyramid shape. Li+Ar6 is an octahedron shape with Li at the centre. Li+Ar7 or slightly larger clusters have a core octahedron of argon atoms with one or more triangular faces capped by other argon atoms. The bonding is much weaker, which explains their greater scarcity.[153]

Sodium forms clusters with argon atoms with peaks at numbers of 8, 10, 16, 20, 23, 25 and 29, and also at the icosahedral numbers of 47, 50, 57, 60, 63, 77, 80, 116 and 147 argon atoms. This includes the square antiprism (8) and the capped square antiprism (10 atoms).[149] In Ti+Ar1−n the argon atoms induce a mixing of the ground electronic state of 3d24s1 with 3d34s0. When a plasma of titanium in expanding argon gas is made via a laser, clusters from Ti+Ar up to Ti+Ar50 are formed. But Ti+Ar6 is much more common than all the others. In this the six argon atoms are arranged in an octahedron shape around the central titanium ion. For Ti+Ar2 DFT calculations predict it is linear, Ti+Ar3 is not even flat, and has one short and two longer Ti-Ar bonds. Ti+Ar4 is a distorted tetrahedron, with one longer Ti-Ar bond. Ti+Ar5 is an asymmetrical trigonal bipyramid shape with one bond shorter. For clusters with seven or more argon atoms, the structure contains a Ti+Ar6 octahedton with triangular faces caped by more argon atoms.[154]

Cu+Ar2 is predicted to be linear. Cu+Ar3 is predicted to be planar T-shaped with an Ar-Cu-Ar angle of 93°. Cu+Ar4 is predicted to be rhombic planar (not square or tetrahedral). For alkali and alkaline earth metals the M+Ar4 cluster is tetrahedral. Cu+Ar5 is predicted to have a rhombic pyramid shape. Cu+Ar6 has a flattened octahedral shape. Cu+Ar7 is much less stable, and the seventh argon atom is outside an inner shell of six argon atoms. This is called capped octahedral. A complete second shell of argon atoms yields Cu+Ar34. Above this number a structural change takes place with an icosahedral arrangement with Cu+Ar55 and Cu+Ar146 having more stability.[155]

With a strontium ion Sr+ from two to eight argon atoms can form clusters. Sr+Ar2 has a triangle shape with C2v symmetry. Sr+Ar3 has a trigonal pyramid shape with C3v symmetry. Sr+Ar4 has two trigonal pyramids sharing a face and strontium at the common apex. It has a C2v symmetry. Sr+Ar6 has a pentagonal pyramid of argon atoms with the strontium atom below the base.[156]

Niobium tetraargide, Nb+Ar4 probably has the argon atoms arranged in a square around the niobium. Similarly for vanadium tetraargide, V+Ar4. The hexaargides, Co+Ar6 and Rh+Ar6 likely have octahedral argon arrangement.[150] Indium monocation forms clusters with multiple argon, with magic numbers at 12, 18, 22, 25, 28, 45 and 54, and 70 argon atoms, which are numbers for icosahedral shapes.[149]

By zapping copper metal with a UV laser in an argon-carbon monoxide mixture, argon tagged copper carbonyl cations are formed. These ions can be studied by observing which wavelengths of infrared radiation cause the molecules to break up. These molecular ions include CuCO+Ar, Cu(CO)2+Ar, Cu(CO)3+Ar, Cu(CO)4+Ar which are respectively disrupted to lose argon, by infrared wavenumbers 2216, 2221, 2205 and 2194 cm−1 respectively. The argon binding energy is respectively 16.3, 1.01, 0.97 and 0.23 kcal/mol. The infrared absorption peak for Cu(CO)3+Ar is 2205 cm−1 compared to 2199 cm−1 for Cu(CO)3+. For Cu(CO)4+Ar the peak is at 2198 cm−1 compared to 2193 for Cu(CO)4+. For Cu(CO)2+Ar the peak is at 2221 cm−1 compared to 2218.3 for argon free, and for CuCO+Ar the peak is at 2216 cm−1 considerably different to 2240.6 cm−1 for CuCO+. Computationally predicted shapes for these molecular ions are linear for CuCO+Ar, slightly bent T-shaped for Cu(CO)2+Ar and a trigonal pyramid with argon at the top and a flat star like copper tricarbonyl forming the base.[157]

Ions studied by argon tagging include the hydrated proton H+(H2O)nAr with n=2 to 5,[158] hydrated 18-crown-6 ether alkali metal ions,[159] hydrated alkali metal ions,[160] transition metal acetylene complexes,[161] protonated ethylene,[162] and IrO4+.[163]

Argon methyl cations, (or methyliumargon) ArxCH3+ are known for n=1 to 8. CH3+ is a Y shape, and when argon atoms are added they go above and below the plane of the Y. If more argon atoms are added they line up with the hydrogen atoms. ΔH0 for ArCH3+ is 11 kcal/mol, and for Ar2CH3+ it is 13.5 kcal/mol (for 2Ar + CH3+).[164]

Boroxyl ring cationic complexes with argon [ArB3O4]+, [ArB3O5]+, [ArB4O6]+ and [ArB5O7]+ were prepared via a laser vaporization at cryogenic temperatures and investigated by infrared gas phase spectroscopy.[3] They were the first large stable gas phase complexes that feature strong dative bonding between argon and boron.

Dications

Dications with argon are known for the coinage metals. Known dications include CuArn2+ and AgArn2+ for n=1-8, with a peak occurrence of CuAr42+, or AgAr42+, and AuArn2+ n=3–7. In addition to the four argon atoms, the six argon atoms clusters have enhanced concentration. The stability of the ions with two positive charges is unexpected as the ionization energy of argon is lower than the second ionization energy of the metal atom. So the positive second charge on the metal atom should move to the argon, ionizing it, and then forming a highly repulsive molecule that undergoes a Coulomb explosion. However these molecules appear to be kinetically stable, and to transfer the charge to an argon atom, they have to pass through a higher energy state.[165] The clusters with four argon atoms are expected to be square planar, and those with six, to be octahedral distorted by the Jahn–Teller effect.

Ion Metal first ionization energy
eV 		Metal second ionization
eV 		binding energy
eV[165] 		Dissociation energy
(kJ/mol) 		Bond length
(Å)
Cu2+Ar 7.73 20.29 0.439 2.4
Ag2+Ar 7.58 21.5 0.199 2.6
Au2+Ar 9.22 20.5 0.670 2.6

Polyatomic anions

icosahedral
symmetry. B – pink, C – grey, N – dark blue, Ar – blue.

Examples of anions containing strong bonds with noble gases are extremely rare: generally nucleophilic nature of anions results in their inability to bind to noble gases with their negative electron affinity. However, the 2017 discovery of "superelectrophilic anions",[166] gas phase fragmentation products of closo-dodecaborates, led to the observation of stable anionic compounds containing a boron-noble gas bond with significant degree of covalent interaction. The most reactive superelectrophilic anion [B12(CN)11]−, fragmentation product of cyanated cluster [B12(CN)12]2-, was reported to bind argon spontaneously at room temperature.[4]

Solid compounds

Armand Gautier noticed that rock contained argon (and also nitrogen) that was liberated when the rock was dissolved in acid[167] however how the argon was combined in rock was ignored by the scientific community.[168]

Fullerene solvates

Solid buckminsterfullerene has small spaces between the C60 balls. Under 200 MPa pressure and 200 °C heat for 12 hours, argon can be intercalated into the solid to form crystalline Ar1C60. Once this cools down it is stable at standard conditions for months. Argon atoms occupy octahedral interstitial sites. The crystalline lattice size is almost unchanged at room temperature, but is slightly larger than pure C60 below 265 K. However argon does stop the buckyballs spinning below 250 K, a lower temperature than in pure C60.[169]

Solid C70 fullerene will also absorb argon under pressure of 200 MPa and at a temperature of 200 °C. C70·Ar has argon in octahedral sites and has the rock salt structure, with cubic crystals in which the lattice parameter is 15.001 Å. This compares to the pure C70 lattice parameter of 14.964 Å, so the argon forces the crystals to expand slightly. The C70 ellipsoidal balls rotate freely in the solid, they are not locked into position by extra argon atoms filling the holes. Argon gradually escapes over a couple of days when the solid is stored at standard conditions, so that C70·Ar is less stable than C60·Ar. This is likely to be due to the shape and internal rotation allowing channels through which Ar atoms can move.[170]

When fullerenes are dissolved and crystallized from toluene, solids may form with toluene included as part of the crystal. However, if this crystallization is performed under a high pressure argon atmosphere, toluene is not included, being replaced by argon. The argon is then removed from the resultant crystal by heating to produce unsolvated solid fullerene.[171]

Clathrate

Argon forms a clathrate with hydroquinone (HOC6H4OH)3•Ar.[172] When crystallised from benzene under a pressure of 20 atmospheres of argon, a well defined structure containing argon results.[173] An argon-phenol clathrate 4C6H5OH•Ar is also known. It has a binding energy of 40 kJ/mol.[168] Other substituted phenols can also crystallise with argon.[172] The argon water clathrate is described in the Aqueous argon section.

Argon difluoride

Argon difluoride, ArF2, is predicted to be stable at pressures over 57 GPa. It should be an electrical insulator.[174]

Ne2Ar and Ar2Ne

At around 4 K there are two phases where neon and argon are mixed as a solid: Ne2Ar and Ar2Ne.[175] With Kr, solid argon forms a disorganized mixture.[176]

ArH4

Under high pressure stoichiometric solids are formed with hydrogen and oxygen: Ar(H2)2 and Ar(O2)3.[177]

Ar(H2)2 crystallises in the hexagonal C14 MgZn2 Laves phase. It is stable to at least 200 GPa, but is predicted to change at 250 GPa to an AlB2 structure. At even higher pressures the hydrogen molecules should break up followed by metallization.[177]

ArO and ArO6

Oxygen and argon under pressure at room temperature form several different alloys with different crystal structures. Argon atoms and oxygen molecules are similar in size, so that a greater range of miscibility occurs compared to other gas mixtures. Solid argon can dissolve up to 5% oxygen without changing structure. Below 50% oxygen a

hexagonal close packed phase exists. This is stable from about 3GPa to 8.5 GPa. Typical formula is ArO. With more oxygen between 5.5 and 7 GPa, a cubic Pm3n structure exists, but under higher pressure it changes to a I42d space group form. With more than 8.5 GPa these alloys separate to solid argon and ε-oxygen. The cubic structure has a unit cell edge of 5.7828 Å at 6.9 GPa. The representative formula is Ar(O2)3.[178]

ArHe2

Using

density-functional theory ArHe2 is predicted to exist with the MgCu2 Laves phase structure at high pressures below 13.8 GPa. Above 13.8 GPa it transforms to AlB2 structure.[179]

Ar-TON

Under pressure argon inserts into zeolite. Argon has an atomic radius of 1.8 Å, so it can insert into pores if they are big enough. Each unit cell of the TON zeolite can contain up to 5 atoms of argon, compared to 12 of neon. Argon infused TON zeolite (Ar-TON) is more compressible than Ne-TON as the unoccupied pores become elliptical under increased pressure. When Ar-TON is brought to atmospheric pressure, the argon only desorbs slowly, so that some remains in the solid without external pressure for a day.[180]

Nickel argide

At 140 GPa and 1500K nickel and argon form an alloy, NiAr.

argon-40 that should be produced during the radioactive decay that produces geothermal heating seems to exist on the Earth.[182]

Organoargon chemistry

Organoargon chemistry describes the synthesis and properties of chemical compounds containing a carbon to argon chemical bond.

Very few such compounds are known. The reaction of acetylene dications with argon produced HCCAr2+ in 2008.[183] Reaction of the CF2+3 dication with argon produced ArCF2+2: this reaction is unique to argon among the noble gases.[184]

The compound FArCCH has been theoretically studied and is predicted to be stable.[185] FArCCF might also be stable enough to synthesise and detect, but probably not FArCCArF.[186] Calculations in 2015 suggest that FArCCH and FArCH3 are stable, but not FArCN.[187] FArCC− should be kinetically stable, as is also expected of the krypton and xenon (but not helium) analogues.[188] HArC4H (for which the krypton analogue is known) and HArC6H have also been predicted as stable.[189] FArCO+ and ClArCO+ should be metastable and might be possible to characterise under cryogenic conditions.[190] Calculations suggest that HArCCF and HCCArF should be stable, and that HNgCCF molecules should be more stable than HNgCCH (Ng = Ar, Kr, Xe); the corresponding krypton species have been experimentally produced, but not the argon species despite an experimental attempt. HCCNgCN and HCCNgNC (Ng = Ar, Kr, Xe) are likewise computed to be stable, but experimental searches for them have failed.[191]

References

  1. ^
    S2CID 44021593
    .
  2. ^
    S2CID 41139746
    .
  3. ^
    PMID 28989687
    .
  4. ^
    PMID 30952786
    .
  5. ^
    ISBN 9780120236527
    .
  6. ^ La Fontaine, B. (October 2010). "Lasers and Moore's Law". SPIE Professional: 20.
  7. ^
    S2CID 37578581
    .
  8. doi:10.1016/0022-2852(88)90173-7
    .
  9. ^
    S2CID 45850131
    .
  10. doi:10.1016/0009-2614(91)87146-3
    .
  11. ^
    ISBN 978-0-7484-0930-3
    .
  12. ^
    doi:10.1016/0301-0104(81)80318-7
    .
  13. doi:10.1016/0009-2614(80)80523-9
    .
  14. ^
    PMID 9571129
    .
  15. S2CID 101818571
    .
  16. doi:10.1080/00268979909483006
    .
  17. doi:10.1016/0009-2614(89)85151-6
    .
  18. ^
    doi:10.1063/1.471578
    .
  19. ^
    PMID 9571128
    .
  20. ^
    doi:10.1063/1.464416
    .
  21. doi:10.1016/0301-0104(86)85144-8
    .
  22. doi:10.1139/p94-159
    .
  23. ^
    doi:10.1016/j.molap.2015.12.001
    .
  24. doi:10.1039/F29726800259
    .
  25. ^
    doi:10.1002/qua.25180
    .
  26. ^
    PMID 9645933
    .
  27. S2CID 121592414
    .
  28. S2CID 122050884
    .
  29. doi:10.1016/j.jms.2016.03.003
    .
  30. ^
    doi:10.1063/1.481868
    .
  31. ^
    doi:10.1063/1.1518025
    .
  32. doi:10.1063/1.469286
    .
  33. ^
    doi:10.1063/1.462405
    .
  34. doi:10.1063/1.473416
    .
  35. ^
    doi:10.1021/ja00296a003
    .
  36. doi:10.1063/1.459949
    .
  37. doi:10.1063/1.481835
    .
  38. ^
    doi:10.1063/1.1529662
    .
  39. ^
    PMID 15267664
    .
  40. doi:10.1063/1.473649
    .
  41. doi:10.1063/1.457929
    .
  42. ISBN 978-0-12-637450-6
    .
  43. S2CID 120130546
    .
  44. ISBN 978-3-540-69953-8
    .
  45. doi:10.1016/0009-2614(94)01476-C
    .
  46. doi:10.1063/1.1473814
    .
  47. ^
    doi:10.1063/1.462108
    .
  48. S2CID 95444756
    .
  49. PMID 18190199
    .
  50. doi:10.1063/1.437161
    .
  51. doi:10.1063/1.91149
    .
  52. doi:10.1021/j100382a027
    .
  53. ^
    S2CID 21324093
    .
  54. doi:10.1063/1.435530
    .
  55. PMID 11031288
    .
  56. doi:10.1063/1.463716
    .
  57. doi:10.1063/1.1681622
    .
  58. doi:10.1016/j.chemphys.2015.07.013
    .
  59. doi:10.1063/1.468097
    .
  60. doi:10.1063/1.467603
    .
  61. ISSN 0021-9606
    .
  62. ^
    doi:10.1063/1.446877
    .
  63. PMID 22482554
    .
  64. doi:10.1063/1.474469
    .
  65. PMID 16164344
    .
  66. doi:10.1063/1.462018
    .
  67. doi:10.1063/1.477754
    .
  68. doi:10.1063/1.463470
    .
  69. PMID 24428820
    .
  70. ISBN 978-3-642-10370-4
    , retrieved 2024-01-08
  71. ISBN 978-3-642-10370-4
  72. ISBN 978-3-642-10370-4
    .
  73. doi:10.1016/S0009-2614(00)00326-2
    .
  74. doi:10.1016/S0022-2852(03)00197-8
    .
  75. doi:10.1016/S0022-2860(01)00846-8
    .
  76. doi:10.1021/ja00494a008
    .
  77. doi:10.1016/0009-2614(90)87230-O
    .
  78. hdl:2027.42/26836
    .
  79. doi:10.1063/1.439908
    .
  80. ^
    ISBN 9781847555076
    .
  81. doi:10.1021/j100868a060
    .
  82. doi:10.1016/0013-4686(69)80014-9
    .
  83. doi:10.1021/jp021458l
    .
  84. S2CID 93956695
    .
  85. doi:10.2174/1874396X00802010095
    .
  86. S2CID 4382128
    .
  87. ^
    doi:10.2174/138527206776818964
    .
  88. PMID 19053096
    .
  89. PMID 17887844
    .
  90. ^
    PMID 12148982
    .
  91. ^
    S2CID 45390086
    .
  92. ^
    PMID 12617681
    .
  93. ^
    PMID 15127451
    .
  94. PMID 17461564
    .
  95. PMID 15025460
    .
  96. doi:10.1021/ja00080a069
    .
  97. doi:10.1016/0009-2614(94)00697-0
    .
  98. ISBN 9783527803545
    .
  99. PMID 23327099
    .
  100. PMID 25321412
    .
  101. PMID 27723974
    .
  102. doi:10.1016/j.ccr.2012.10.013
    .
  103. ^
    doi:10.1021/om9704962
    .
  104. doi:10.1021/ja00034a003
    .
  105. doi:10.1021/ja960485k
    .
  106. doi:10.1016/j.ccr.2012.07.017
    .
  107. S2CID 13525010
    .
  108. PMID 23001952
    .
  109. ^
    doi:10.1021/ja000874l
    .
  110. ^
    PMID 16451016
    .
  111. PMID 16834012
    .
  112. PMID 16366626
    .
  113. ^
    PMID 16970371
    .
  114. doi:10.1016/j.chemphys.2008.03.026
    .
  115. PMID 17201389
    .
  116. doi:10.1016/B978-0-08-097774-4.00128-5
    .
  117. S2CID 98517909
    .
  118. S2CID 58603219
    .
  119. PMID 15267486
    .
  120. doi:10.1021/jz900009q
    .
  121. doi:10.1002/ange.201006486
    .
  122. doi:10.1016/0009-2614(70)80331-1
    .
  123. ^
    doi:10.1021/ja00183a005
    .
  124. doi:10.1016/0022-2852(92)90562-3
    .
  125. S2CID 91636049
    .
  126. ^
    S2CID 98595129
    .
  127. ^
    ISSN 0003-2700
    .
  128. S2CID 46457224
    .
  129. doi:10.1039/JA9900500431
    .
  130. PMID 19955552
    .
  131. S2CID 29240758
    .
  132. ^
    doi:10.1021/jp993091z
    .
  133. doi:10.1063/1.455708
    .
  134. doi:10.1063/1.457934
    .
  135. ^
    doi:10.1039/JA9961100643
    .
  136. doi:10.1016/j.ijms.2012.05.006
    .
  137. PMID 19039346
    .
  138. doi:10.1002/ange.200903706
    .
  139. ^
    doi:10.1063/1.472090
    .
  140. doi:10.1063/1.437518
    .
  141. doi:10.1063/1.459850
    .
  142. ^
    doi:10.1016/0009-2614(96)01095-0
    .
  143. doi:10.1063/1.466840
    .
  144. ^
    doi:10.1016/j.sab.2012.02.008
    .
  145. ^
    doi:10.1088/1742-6596/774/1/012023
    .
  146. ^
    doi:10.1016/0009-2614(94)00828-0
    .
  147. ^
    doi:10.1016/0009-2614(95)00006-P
    .
  148. S2CID 4246089
    .
  149. ^
    doi:10.1155/1997/49504
    .
  150. ^
    doi:10.1016/S0009-2614(97)01203-7
    .
  151. doi:10.1103/PhysRevLett.80.261
    .
  152. ISBN 9780549671015
    .
  153. doi:10.1016/S0301-0104(00)00175-0
    .
  154. doi:10.1016/S0009-2614(99)00162-1
    .
  155. doi:10.1016/S0301-0104(02)00512-8
    .
  156. S2CID 10006288
    .
  157. PMID 21861528
    .
  158. PMID 20232806
    .
  159. PMID 21675737
    .
  160. doi:10.1021/jz200530v
    .
  161. PMID 15669839
    .
  162. doi:10.1016/j.cplett.2009.08.063
    .
  163. S2CID 4463905
    .
  164. doi:10.1016/0009-2614(91)85060-A
    .
  165. ^
    doi:10.1063/1.1352036
    .
  166. PMID 28560843
    .
  167. ^ Gautier, Armand (January 1901). "Chimie Geologique – Surl'existence d'azotures, argonures, arseniures, et iodures sans les roches crystalliniennes". Comptes Rendus Hebdomadaires des Séances de l'Académie des Sciences (in French). 132: 934.
  168. ^
    ISBN 9780841232518
    .
  169. doi:10.1016/S0022-3697(97)00096-6
    .
  170. doi:10.1016/S0022-3697(98)00017-1
    .
  171. doi:10.2320/jinstmet.75.671
    .
  172. ^
    ISBN 978-3-540-52124-2
    .
  173. S2CID 4134617
    .
  174. S2CID 119249355
    .
  175. S2CID 250894931
    .
  176. doi:10.1103/PhysRevB.73.184116
    .
  177. ^
    doi:10.2138/rmg.2000.41.12
    .
  178. doi:10.1103/PhysRevB.82.014112
    .
  179. S2CID 49570874
    .
  180. doi:10.1021/acs.jpcc.8b01827
    .
  181. ^ Dalton, Louisa (30 October 2019). "Argon reacts with nickel under pressure-cooker conditions". Chemical & Engineering News. Retrieved 6 November 2019.
  182. S2CID 210511220
    .
  183. PMID 19039346
    .
  184. doi:10.1021/jz900274p
    .
  185. doi:10.1063/1.1613631
    .
  186. PMID 17880047
    .
  187. doi:10.1002/qua.24804
    .
  188. PMID 23181302
    .
  189. PMID 16734457
    .
  190. PMID 24295279
    .
  191. PMID 20205379
    .

External links
Retrieved from "https://en.wikipedia.org/w/index.php?title=Argon_compounds&oldid=1204265449"