Neon compounds

Neon compounds are chemical compounds containing the element neon (Ne) with other molecules or elements from the periodic table. Compounds of the noble gas neon were believed not to exist, but there are now known to be molecular ions containing neon, as well as temporary excited neon-containing molecules called excimers. Several neutral neon molecules have also been predicted to be stable, but are yet to be discovered in nature. Neon has been shown to crystallize with other substances and form clathrates or Van der Waals solids.

Neon has a high first ionization potential of 21.564 eV, which is only exceeded by that of helium (24.587 eV), requiring too much energy to make stable ionic compounds. Neon's polarisability of 0.395 Å3 is the second lowest of any element (only helium's is more extreme). Low polarisability means there will be little tendency to link to other atoms.[1] Neon has a Lewis basicity or proton affinity of 2.06 eV.[2]

Van der Waals molecules

Van der Waals molecules are those where neon is held onto other components by London dispersion forces. The forces are very weak, so the bonds will be disrupted if there is too much molecular vibration, which happens if the temperature is too high (above that of solid neon).

Neon atoms themselves can be linked together to make clusters of atoms. The dimer Ne2, trimer Ne3 and neon tetramer Ne4 have all been characterised by Coulomb explosion imaging. The molecules are made by an expanding supersonic jet of neon gas. The neon dimer has an average distance of 3.3 Å between atoms. The neon trimer is shaped approximately like an equilateral triangle with sides 3.3 Å long. However the shape is floppy and isosceles triangle shapes are also common. The first excited state of the neon trimer is 2 meV above the ground state. The neon tetramer takes the form of a tetrahedron with sides around 3.2 Å.[3]

Van der Waals molecules with metals include LiNe.[4]

More Van der Waals molecules include CF4Ne and CCl4Ne, Ne2Cl2, Ne3Cl2,[5] I2Ne, I2Ne2, I2Ne3, I2Ne4, I2NexHey (x=1-5, y=1-4).[6]

Van der Waals molecules formed with organic molecules in gas include aniline,[7] dimethyl ether,[8] 1,1-difluoroethylene,[9] pyrimidine,[10] chlorobenzene,[11] cyclopentanone,[12] cyanocyclobutane,[13] and cyclopentadienyl.[14]

Ligands

Neon can form a very weak bond to a transition metal atom as a ligand, for example Cr(CO)5Ne,[15] Mo(CO)5Ne, and W(CO)5Ne.[16]

NeNiCO is predicted to have a binding energy of 2.16 kcal/mol. The presence of neon changes the bending frequency of Ni−C−O by 36 cm−1.[17][18]

NeAuF[19] and NeBeS[20] have been isolated in noble gas matrixes.[21] NeBeCO3 has been detected by infrared spectroscopy in a solid neon matrix. It was made from beryllium gas, dioxygen and carbon monoxide.[16]

The cyclic molecule Be2O2 can be made by evaporating Be with a laser with oxygen and an excess of inert gas. It coordinates two noble gas atoms and has had spectra measured in solid neon matrices. Known neon containing molecules are the homoleptic Ne.Be2O2.Ne, and heteroleptic Ne.Be2O2.Ar and Ne.Be2O2.Kr. The neon atoms are attracted to the beryllium atoms as they have a positive charge in this molecule.[22]

Beryllium sulfite molecules BeO2S, can also coordinate neon onto the beryllium atom. The dissociation energy for neon is 0.9 kcal/mol. When neon is added to the cyclic molecule, the ∠O-Be-O decreases and the O-Be bond lengths increase.[23]

Solids

High pressure Van der Waals solids include (N2)6Ne7.[24]

Neon hydrate or neon clathrate, a clathrate, can form in ice II at 480 MPa pressure between 70 K and 260 K.[25] Other neon hydrates are also predicted resembling hydrogen clathrate, and those clathrates of helium. These include the C0, ice Ih and ice Ic forms.[25]

Neon atoms can be trapped inside fullerenes such as C60 and C70. The isotope 22Ne is strongly enriched in carbonaceous chondrite meteorites, by more than 1,000 times its occurrence on Earth. This neon is given off when a meteorite is heated.[26] An explanation for this is that originally when carbon was condensing from the aftermath of a supernova explosion, cages of carbon form that preferentially trap sodium atoms, including 22Na. Forming fullerenes trap sodium orders of magnitude more often than neon, so Na@C60 is formed. rather than the more common 20Ne@C60. The 22Na@C60 then decays radioactively to 22Ne@C60, without any other neon isotopes.[27] To make buckyballs with neon inside, buckminsterfullerene can be heated to 600 °C with neon under pressure. With three atmospheres for one hour, about 1 in 8,500,000 molecules end up with Ne@C60. The concentration inside the buckyballs is about the same as in the surrounding gas. This neon comes back out when heated to 900 °C.[28]

Dodecahedrane can trap neon from a neon ion beam to yield Ne@C20H20.[29]

Neon also forms an intercalation compound (or alloy) with fullerenes like C60. In this the Ne atom is not inside the ball, but packs into the spaces in a crystal made from the balls. It intercalates under pressure, but is unstable at standard conditions, and degases in under 24 hours.[30] However at low temperatures Ne•C60 is stable.[31]

Neon can be trapped inside some metal-organic framework compounds. In NiMOF-74 neon can be absorbed at 100 K at pressures up to 100 bars, and shows hysteresis, being retained till lower pressures. The pores easily take up six atoms per unit cell, as a hexagonal arrangement in the pores, with each neon atom close to a nickel atom. A seventh neon atom can be forced under pressure at the centre of the neon hexagons.[32]

Neon is pushed into crystals of ammonium iron formate (NH4Fe(HCOO)3) and ammonium nickel formate (NH4Ni(HCOO)3) at 1.5 GPa to yield Ne•NH4Fe(HCOO)3 and Ne•NH4Ni(HCOO)3. The neon atoms become trapped in a cage of five metal triformate units. The windows in the cages are blocked by ammonium ions. Argon does not undergo this, probably as its atoms are too big.[33]

Neon can penetrate TON zeolite under pressure. Each unit cell contains up to 12 neon atoms in the Cmc21 structure below 600 MPa. This is double the number of argon atoms that can be inserted into that zeolite. At 270 MPa occupancy is around 20% Over 600 MPa this neon penetrated phase transforms to a Pbn21 structure, which can be brought back to zero pressure. However all the neon escapes as it is depressurized.[34] Neon causes the zeolite to remain crystalline, otherwise at pressure of 20 GPa it would have collapsed and become amorphous.[34]

Silica glass also absorbs neon under pressure. At 4 GPa there are 7 atoms of neon per nm3.[34]

Ions

Ionic molecules can include neon, such as the clusters Ne
mHe+
n where m goes from 1 to 7 and n from 1 to over 20.[35] HeNe+ (helium neide) has a relatively strong covalent bond. The charge is distributed across both atoms.[36]

When metals are evaporated into a thin gas of hydrogen and neon in a strong electric field, ions are formed that are called neides. Ions observed include TiNe+, TiH2Ne+, ZnNe2+, ZrNe2+, NbNe2+, NbHNe2+, MoNe2+, RhNe2+, PdNe+, TaNe3+, WNe2+, WNe3+, ReNe3+, IrNe2+, AuNe+ (possible).[37]

SiF2Ne2+ can be made from neon and SiF2+
3 using mass spectrometer technology. SiF2Ne2+ has a bond from neon to silicon. SiF2+
3 has a very weak bond to fluorine and a high electron affinity.[38]

NeCCH+, a substituted acetylene, is predicted to be energetically stable by 5.9 kcal/mol, one of the most stable organic ions.[39]

Ionic clusters

Metal ions can attract multiple neon atoms to form clusters. The shape of the cluster molecules is determined by repulsion between neon atoms and d-orbital electrons from the metal atom. For copper, neonides are known with numbers of neon atoms up to 24, Cu+Ne1-24. Cu+Ne4 and Cu+Ne12 have much greater numbers than those with higher number of neon atoms.

Cu+Ne2 is predicted to be linear. Cu+Ne3 is predicted to be planar T shaped with an Ne-Cu-Ne angle of 91°. Cu+Ne4 is predicted to be square planar (not tetrahedral) with D4h symmetry. For alkali and alkaline earth metals the M+Ne4 cluster is tetrahedral. Cu+Ne5 is predicted to have a square pyramid shape. Cu+Ne6 has a seriously distorted octahedral shape. Cu+Ne12 has an icosahedral shape. Anything beyond that is less stable, with extra neon atoms having to make an extra shell of atoms around an icosahedral core.[40]

Neonium

The ion NeH+ formed by protonating neon, is called neonium. It is produced in an AC electric discharge through a mixture of neon and hydrogen with more produced when neon outnumbers hydrogen molecules by 36:1.[41] The dipole moment is 3.004 D.[41]

Neonium is also formed by excited dihydrogen cation reacting with neon: Ne + H2+* → NeH+ + H[42]

Far infrared spectrum of 20Ne1H+[41] 20NeD+ 22NeH+ 22NeD+
Transition observed frequency
J GHz
1←0 1 039.255
2←1 2 076.573 2 067.667
3←2 3 110.022 1 647.026 3 096.706
4←3 4 137.673 2 193.549 4 119.997 2 175.551
5←4 5 157.607 2 737.943 2 715.512
6←5 3 279.679 3 252.860
7←6 3 818.232 3 787.075
8←7 4 353.075 4 317.643
9←8 4 883.686

The infrared spectrum around 3μm has also been measured.[43]

Excimers

The Ne*
2 molecule exists in an excited state in an excimer lamp using a microhollow cathode. This emits strongly in the vacuum ultraviolet between 75 and 90 nm with a peak at 83 nm. There is a problem in that there is no window material suitable to transmit these short wavelengths, so it must be used in a vacuum. If about one part in a thousand of hydrogen gas is included, most of the Ne*
2 energy is transferred to hydrogen atoms and there is a strong monochromatic Lyman alpha emission at 121.567 nm.[44]

Cesium can form excimer molecules with neon CsNe*.[45]

A hydrogen-neon excimer is known to exist. Fluorescence was observed by Möller due to bound free transition in a Rydberg molecule of NeH*. NeH is metastable and its existence was proved by mass spectroscopy in which the NeH+ ion is neutralized and then reionized.[46] The spectrum of NeH includes lines at 1.81, 1.60 and I .46 eV, with a small band at 1.57 eV[47] The bondlength in NeH is calculated as 1.003 Å.[46]

A helium neon excimer can be found in a mixed plasma or helium and neon.[48]

Some other excimers can be found in solid neon, including Ne+
2O−
 which has a luminescence peaking around 11.65 eV, or Ne+
2F−
 luminescing around 10.16–10.37 eV and 8.55 eV.[49]

Minerals

Bokiy's crystallochemical classification of minerals included "compounds of neon" as type 82. However, no such minerals were known.[50]

Predicted compounds

Analogously to the known ArBeO and the predicted HeBeO (beryllium oxide noble gas adducts), NeBeO is expected to exist, albeit with a very weak bond dissociation energy of 9 kJ/mol. The bond is enhanced by a dipole-induced positive charge on beryllium, and a vacancy in the σ orbital on beryllium where it faces the neon.[51]

gollark: You might need to manually configure it to use "kit.osmarks.net/wiki" as the base URL, or something.
gollark: Oh, your thing keeps trying to use the internal IP.
gollark: Wikit is up.
gollark: I sure am glad I installed bee mirrors™ proactively.
gollark: ⍝"initiate bee strike" @everyone --reconnect --auth-key=d8a00fd885dd9e925d44250a5b6a0f6e

References
  1. Frenking, Gernot; Cremer, Dieter (1 March 2005). "The chemistry of the noble gas elements helium, neon, and argon — Experimental facts and theoretical predictions". Structure and Bonding. 73 (Noble Gas and High Temperature Chemistry): 17–95. doi:10.1007/3-540-52124-0_2.
  2. Grochala, Wojciech (1 November 2017). "On the position of helium and neon in the Periodic Table of Elements". Foundations of Chemistry. 20 (3): 191–207. doi:10.1007/s10698-017-9302-7.
  3. Ulrich, B.; Vredenborg, A.; Malakzadeh, A.; Schmidt, L. Ph. H.; Havermeier, T.; Meckel, M.; Cole, K.; Smolarski, M.; Chang, Z.; Jahnke, T.; Dörner, R. (30 June 2011). "Imaging of the Structure of the Argon and Neon Dimer, Trimer, and Tetramer". The Journal of Physical Chemistry A. 115 (25): 6936–6941. Bibcode:2011JPCA..115.6936U. doi:10.1021/jp1121245. PMID 21413773.
  4. Lee, Chang Jae (1 January 1991). Rotationally Resolved Laser Spectroscopy of the 3s 2Σ+ → 2p 2Π Transition in Lithium-6 Neon and Lithium Neon Van Der Waals Molecules (Ph.D.). Bibcode:1991PhDT.......128L.
  5. Hair, Sally R.; Cline, Joseph I.; Bieler, Craig R.; Janda, Kenneth C. (1989). "The structure and dissociation dynamics of the Ne2Cl2 Van der Waals complex". The Journal of Chemical Physics. 90 (6): 2935. Bibcode:1989JChPh..90.2935H. doi:10.1063/1.455893.
  6. Kenny, Jonathan E.; Johnson, Kenneth E.; Sharfin, Wayne; Levy, Donald H. (1980). "The photodissociation of van der Waals molecules: Complexes of iodine, neon, and helium". The Journal of Chemical Physics. 72 (2): 1109. Bibcode:1980JChPh..72.1109K. doi:10.1063/1.439252.
  7. Becucci, M.; Pietraperzia, G.; Castellucci, E.; Bréchignac, Ph. (May 2004). "Dynamics of vibronically excited states of the aniline–neon van der Waals complex: vibrational predissociation versus intramolecular vibrational redistribution". Chemical Physics Letters. 390 (1–3): 29–34. Bibcode:2004CPL...390...29B. doi:10.1016/j.cplett.2004.03.138.
  8. Maris, Assimo; Caminati, Walther (2003). "Rotational spectrum, dynamics, and bond energy of the floppy dimethylether⋯neon van der Waals complex". The Journal of Chemical Physics. 118 (4): 1649. Bibcode:2003JChPh.118.1649M. doi:10.1063/1.1533012.
  9. Dell’Erba, Adele; Melandri, Sonia; Millemaggi, Aldo; Caminati, Walther; Favero, Paolo G. (2000). "Rotational spectra and dynamics of the van der Waals adducts of neon and argon with 1,1-difluoroethylene". The Journal of Chemical Physics. 112 (5): 2204. Bibcode:2000JChPh.112.2204D. doi:10.1063/1.480786.
  10. Caminati, Walther; Favero, Paolo G. (1 February 1999). "Chemistry at Low Pressure and Low Temperature: Rotational Spectrum and Dynamics of Pyrimidine-Neon". Chemistry: A European Journal. 5 (2): 811–814. doi:10.1002/(SICI)1521-3765(19990201)5:2<811::AID-CHEM811>3.0.CO;2-1.
  11. Oh, Jung-Jin; Park, Inhee; Peebles, Sean A.; Kuczkowski, Robert L. (December 2001). "The rotational spectrum and structure of the chlorobenzene–neon van der Waals dimer". Journal of Molecular Structure. 599 (1–3): 15–22. Bibcode:2001JMoSt.599...15O. doi:10.1016/S0022-2860(01)00833-X.
  12. Lin, Wei. "Determination of the structure of the argon cyclopentanone and neon Van der Waals complexes". hdl:1811/49680. Cite journal requires |journal= (help)
  13. Pringle, Wallace C.; Frohman, Daniel J.; Ndugire, William; Novick, Stewart E. (1 June 2010). "The FT Microwave Spectra and Structure of the Argon and Neon Van Der Waals Complexes of Cyanocyclobutane". Archived from the original on 21 January 2018. Retrieved 4 June 2016. Cite journal requires |journal= (help)
  14. Yu, Lian; Williamson, James; Foster, Stephen C.; Miller, Terry A. (1992). "High resolution laser spectroscopy of free radical-inert gas complexes: C5H5·He, C5H5·He2, C5H5·Ne, and CH3–C5H4·He2". The Journal of Chemical Physics. 97 (8): 5273. Bibcode:1992JChPh..97.5273Y. doi:10.1063/1.463788.
  15. Perutz, Robin N.; Turner, James J. (August 1975). "Photochemistry of the Group 6 hexacarbonyls in low-temperature matrices. III. Interaction of the pentacarbonyls with noble gases and other matrices". Journal of the American Chemical Society. 97 (17): 4791–4800. doi:10.1021/ja00850a001.
  16. Zhang, Qingnan; Chen, Mohua; Zhou, Mingfei; Andrada, Diego M.; Frenking, Gernot (19 March 2015). "Experimental and Theoretical Studies of the Infrared Spectra and Bonding Properties of NgBeCO3 and a Comparison with NgBeO (Ng = He, Ne, Ar, Kr, Xe)". The Journal of Physical Chemistry A. 119 (11): 2543–2552. Bibcode:2015JPCA..119.2543Z. doi:10.1021/jp509006u. PMID 25321412.
  17. Taketsugu, Yuriko; Noro, Takeshi; Taketsugu, Tetsuya (February 2008). "Identification of the Matrix Shift: A Fingerprint for Neutral Neon Complex?". The Journal of Physical Chemistry A. 112 (5): 1018–1023. Bibcode:2008JPCA..112.1018T. doi:10.1021/jp710792c.
  18. Manceron, L; Alikhani, M.E; Joly, H.A (March 1998). "Infrared matrix isolation and DFT study of NiN2". Chemical Physics. 228 (1–3): 73–80. Bibcode:1998CP....228...73M. doi:10.1016/S0301-0104(97)00339-X.
  19. Wang, Xuefeng; Andrews, Lester; Brosi, Felix; Riedel, Sebastian (21 January 2013). "Matrix Infrared Spectroscopy and Quantum-Chemical Calculations for the Coinage-Metal Fluorides: Comparisons of Ar-AuF, Ne-AuF, and Molecules MF2 and MF3". Chemistry: A European Journal. 19 (4): 1397–1409. doi:10.1002/chem.201203306.
  20. Wang, Qiang; Wang, Xuefeng (21 February 2013). "Infrared Spectra of NgBeS (Ng = Ne, Ar, Kr, Xe) and BeS2 in Noble-Gas Matrices". The Journal of Physical Chemistry A. 117 (7): 1508–1513. Bibcode:2013JPCA..117.1508W. doi:10.1021/jp311901a. PMID 23327099.
  21. Cappelletti, David; Bartocci, Alessio; Grandinetti, Felice; Falcinelli, Stefano; Belpassi, Leonardo; Tarantelli, Francesco; Pirani, Fernando (13 April 2015). "Experimental Evidence of Chemical Components in the Bonding of Helium and Neon with Neutral Molecules". Chemistry: A European Journal. 21 (16): 6234–6240. doi:10.1002/chem.201406103. PMID 25755007.
  22. Zhang, Qingnan; Li, Wan-Lu; Zhao, Lili; Chen, Mohua; Zhou, Mingfei; Li, Jun; Frenking, Gernot (10 February 2017). "A Very Short Be-Be Distance but No Bond: Synthesis and Bonding Analysis of Ng-Be2O2-Ng′ (Ng, Ng′=Ne, Ar, Kr, Xe)". Chemistry - A European Journal. 23 (9): 2035–2039. doi:10.1002/chem.201605994. PMID 28009065.
  23. Yu, Wenjie; Liu, Xing; Xu, Bing; Xing, Xiaopeng; Wang, Xuefeng (21 October 2016). "Infrared Spectra of Novel NgBeSO2 Complexes (Ng = Ne, Ar, Kr, Xe) in Low Temperature Matrixes". The Journal of Physical Chemistry A. 120 (43): 8590–8598. Bibcode:2016JPCA..120.8590Y. doi:10.1021/acs.jpca.6b08799. PMID 27723974.
  24. Plisson, Thomas; Weck, Gunnar; Loubeyre, Paul (11 July 2014). "A High Pressure van der Waals Insertion Compound". Physical Review Letters. 113 (2): 025702. Bibcode:2014PhRvL.113b5702P. doi:10.1103/PhysRevLett.113.025702. PMID 25062210.
  25. Teeratchanan, Pattanasak; Hermann, Andreas (21 October 2015). "Computational phase diagrams of noble gas hydrates under pressure" (PDF). The Journal of Chemical Physics. 143 (15): 154507. Bibcode:2015JChPh.143o4507T. doi:10.1063/1.4933371. PMID 26493915.
  26. Jungck, M. H. A.; Eberhardt, P. (1979). "Neon-E in Orgueil Density Separates". Meteoritics. 14: 439–440. Bibcode:1979Metic..14R.439J.
  27. Dunk, P. W.; Adjizian, J.-J.; Kaiser, N. K.; Quinn, J. P.; Blakney, G. T.; Ewels, C. P.; Marshall, A. G.; Kroto, H. W. (21 October 2013). "Metallofullerene and fullerene formation from condensing carbon gas under conditions of stellar outflows and implication to stardust". Proceedings of the National Academy of Sciences. 110 (45): 18081–18086. Bibcode:2013PNAS..11018081D. doi:10.1073/pnas.1315928110. PMC 3831496. PMID 24145444.
  28. Saunders, M.; Jimenez-Vazquez, H. A.; Cross, R. J.; Poreda, R. J. (5 March 1993). "Stable Compounds of Helium and Neon: He@C60 and Ne@C60". Science. 259 (5100): 1428–1430. Bibcode:1993Sci...259.1428S. doi:10.1126/science.259.5100.1428. PMID 17801275.
  29. Jiménez-Vázquez, Hugo A.; Tamariz, Joaquín; Cross, R. James (March 2001). "Binding Energy in and Equilibrium Constant of Formation for the Dodecahedrane Compounds He@C12H12 and Ne@C12H12". The Journal of Physical Chemistry A. 105 (8): 1315–1319. doi:10.1021/jp0027243.
  30. Schirber, J. E.; Kwei, G. H.; Jorgensen, J. D.; Hitterman, R. L.; Morosin, B. (1 May 1995). "Room-temperature compressibility of C60 : Intercalation effects with He, Ne, and Ar". Physical Review B. 51 (17): 12014–12017. doi:10.1103/PhysRevB.51.12014. PMID 9977961.
  31. Aleksandrovskii, A. N.; Gavrilko, V. G.; Esel’son, V. B.; Manzhelii, V. G.; Udovidchenko, B. G.; Maletskiy, V. P.; Sundqvist, B. (December 2001). "Low-temperature thermal expansion of fullerite C60 alloyed with argon and neon". Low Temperature Physics. 27 (12): 1033–1036. doi:10.1063/1.1430848.
  32. Wood, Peter A.; Sarjeant, Amy A.; Yakovenko, Andrey A.; Ward, Suzanna C.; Groom, Colin R. (2016). "Capturing neon – the first experimental structure of neon trapped within a metal–organic environment". Chem. Commun. 52 (65): 10048–10051. doi:10.1039/C6CC04808K. PMID 27452474.
  33. Collings, Ines E.; Bykova, Elena; Bykov, Maxim; Petitgirard, Sylvain; Hanfland, Michael; Paliwoda, Damian; Dubrovinsky, Leonid; Dubrovinskaia, Natalia (4 November 2016). "Neon-Bearing Ammonium Metal Formates: Formation and Behaviour under Pressure". ChemPhysChem. 17 (21): 3369–3372. doi:10.1002/cphc.201600854. PMID 27500946.
  34. Thibaud, Jean-Marc; Rouquette, Jérôme; Dziubek, Kamil; Gorelli, Federico A.; Santoro, Mario; Garbarino, Gaston; Clément, Sébastien; Cambon, Olivier; van der Lee, Arie; Di Renzo, Francesco; Coasne, Benoît; Haines, Julien (3 April 2018). "Saturation of the Siliceous Zeolite TON with Neon at High Pressure". The Journal of Physical Chemistry C. 122 (15): 8455–8460. doi:10.1021/acs.jpcc.8b01827.
  35. Bartl, Peter; Denifl, Stephan; Scheier, Paul; Echt, Olof (2013). "On the stability of cationic complexes of neon with helium – solving an experimental discrepancy". Physical Chemistry Chemical Physics. 15 (39): 16599–604. Bibcode:2013PCCP...1516599B. doi:10.1039/C3CP52550C. PMID 23958826.
  36. Bieske, E. J.; Soliva, A. M.; Friedmann, A.; Maier, J. P. (1992). "Photoinitiated charge transfer in N2O+–Ar". The Journal of Chemical Physics. 96 (10): 7535. Bibcode:1992JChPh..96.7535B. doi:10.1063/1.462405.
  37. Kapur, Shukla; Müller, Erwin W. (February 1977). "Metal–neon compound ions in slow field evaporation". Surface Science. 62 (2): 610–620. Bibcode:1977SurSc..62..610K. doi:10.1016/0039-6028(77)90104-2.
  38. Roithová, Jana; Schröder, Detlef (2 November 2009). "Silicon Compounds of Neon and Argon". Angewandte Chemie International Edition. 48 (46): 8788–8790. doi:10.1002/anie.200903706.
  39. Frenking, Gernot; Koch, Wolfram; Reichel, Felix; Cremer, Dieter (May 1990). "Light noble gas chemistry: structures, stabilities, and bonding of helium, neon, and argon compounds". Journal of the American Chemical Society. 112 (11): 4240–4256. doi:10.1021/ja00167a020.
  40. Froudakis, George E.; Muhlhauser, Max; Farantos, Stavros C.; Sfounis, Antonis; Velegrakis, Michalis (June 2002). "Mass spectra and structures of Cu+Rgn clusters (Rg=Ne, Ar)". Chemical Physics. 280 (1–2): 43–51. Bibcode:2002CP....280...43F. doi:10.1016/S0301-0104(02)00512-8.
  41. Matsushima, Fusakazu; Ohtaki, Yuichiro; Torige, Osamu; Takagi, Kojiro (1998). "Rotational spectra of [sup 20]NeH[sup +], [sup 20]NeD[sup +], [sup 22]NeH[sup +], and [sup 22]NeD[sup +]". The Journal of Chemical Physics. 109 (6): 2242. Bibcode:1998JChPh.109.2242M. doi:10.1063/1.476791.
  42. P. J. Kuntz AND A. C. Roach (1972). "Ion-Molecule Reactions of the Rare Gases with Hydrogen Part 1.-Diatomics-in-Molecules Potential Energy Surface for ArH2+". J. Chem. Soc., Faraday Trans. 2. 68: 259–280. doi:10.1039/F29726800259.CS1 maint: uses authors parameter (link)
  43. Wong, M. (1982). "Observation of the infrared absorption spectra of 20NeH+ and 22NeH+ with a difference frequency laser". The Journal of Chemical Physics. 77 (2): 693–696. Bibcode:1982JChPh..77..693W. doi:10.1063/1.443883.
  44. Kogelschatz, Ulrich (3 May 2004). "Excimer lamps: history, discharge physics, and industrial applications". Proc. SPIE. SPIE Proceedings. 5483 (Atomic and Molecular Pulsed Lasers V): 272. Bibcode:2004SPIE.5483..272K. doi:10.1117/12.563006.
  45. Novak, R.; Bhaskar, N. D.; Happer, W. (1979). "Infrared emission bands from transitions between excited states of cesium–noble gas molecules". The Journal of Chemical Physics. 71 (10): 4052. Bibcode:1979JChPh..71.4052N. doi:10.1063/1.438174.
  46. Eric P. Parker and J.V. Ortiz (17 November 1989). "Electron Propagator Calculations on the Discrete Spectra OF ArH AND NeH". Chemical Physics Letters. 163 (4): 366–370. Bibcode:1989CPL...163..366P. doi:10.1016/0009-2614(89)85151-6.CS1 maint: uses authors parameter (link)
  47. Ketterle, W.; Walther, H. (May 1988). "A discrete spectrum of neon hydride". Chemical Physics Letters. 146 (3–4): 180–183. Bibcode:1988CPL...146..180K. doi:10.1016/0009-2614(88)87427-X.
  48. Tanaka, Y. (1972). "Absorption Spectra of Ne2 and HeNe Molecules in the Vacuum-UV Region". The Journal of Chemical Physics. 57 (7): 2964–2976. Bibcode:1972JChPh..57.2964T. doi:10.1063/1.1678691.
  49. Belov, A. G.; Fugol, I. Ya.; Yurtaeva, E. M.; Bazhan, O. V. (1 September 2000). "Luminescence of oxygen–rare gas exciplex compounds in rare gas matrices". Journal of Luminescence. 91 (1–2): 107–120. Bibcode:2000JLum...91..107B. doi:10.1016/S0022-2313(99)00623-7.
  50. Bokiy, G. B. (1994). Marfunin, Arnold S. (ed.). Advanced Mineralogy: Volume 1 Composition, Structure, and Properties of mineral Matter Concepts, Results, and Problems. Springer Science & Business Media. p. 155. ISBN 978-3-642-78525-2.
  51. Kobayashi, Takanori; Kohno, Yuji; Takayanagi, Toshiyuki; Seki, Kanekazu; Ueda, Kazuyoshi (July 2012). "Rare gas bond property of Rg–Be2O2 and Rg–Be2O2–Rg (Rg=He, Ne, Ar, Kr and Xe) as a comparison with Rg–BeO". Computational and Theoretical Chemistry. 991: 48–55. doi:10.1016/j.comptc.2012.03.020.
This article is issued from Wikipedia. The text is licensed under Creative Commons - Attribution - Sharealike. Additional terms may apply for the media files.