Nitrous oxide

• Formula: N₂O
• Molecular weight: 44.0128
• IUPAC Standard InChI: InChI=1S/N2O/c1-2-3 Copy

  
• IUPAC Standard InChIKey: GQPLMRYTRLFLPF-UHFFFAOYSA-N Copy
• CAS Registry Number: 10024-97-2
• Chemical structure:
  This structure is also available as a 2d Mol file or as a computed 3d SD file
  The 3d structure may be viewed using Java or Javascript.
• Other names: Nitrogen oxide (N2O); Dinitrogen monoxide; Dinitrogen oxide; Laughing gas; N2O; Factitious air; Hyponitrous acid anhydride; Nitrogen oxide; UN 1070; UN 2201; Nitrogen monoxide; Nitral
• Permanent link for this species. Use this link for bookmarking this species for future reference.
• Information on this page:
  • Ion clustering data
  • References
  • Notes
• Other data available:
  • Gas phase thermochemistry data
  • Phase change data
  • Reaction thermochemistry data: reactions 1 to 50, reactions 51 to 83
  • Henry's Law data
  • Gas phase ion energetics data
  • IR Spectrum
  • Mass spectrum (electron ionization)
  • Gas Chromatography
  • Fluid Properties
• Data at other public NIST sites:
  • Microwave spectra (on physics lab web site)
  • Electron-Impact Ionization Cross Sections (on physics web site)
  • Gas Phase Kinetics Database
• Options:
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Ion clustering data

Go To: Top, References, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Data compiled as indicated in comments:
M - Michael M. Meot-Ner (Mautner) and Sharon G. Lias
B - John E. Bartmess

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. Searches may be limited to ion clustering reactions. A general reaction search form is also available.

Clustering reactions

 +  = ( • )

By formula: Br^- + N₂O = (Br^- • N₂O)

( • ) +  = ( • 2)

By formula: (Br^- • N₂O) + N₂O = (Br^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (Br^- • 2N₂O) + N₂O = (Br^- • 3N₂O)

 +  = ( • )

By formula: CH₃⁺ + N₂O = (CH₃⁺ • N₂O)

 +  = ( • )

By formula: Cl^- + N₂O = (Cl^- • N₂O)

( • ) +  = ( • 2)

By formula: (Cl^- • N₂O) + N₂O = (Cl^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (Cl^- • 2N₂O) + N₂O = (Cl^- • 3N₂O)

( • 3) +  = ( • 4)

By formula: (Cl^- • 3N₂O) + N₂O = (Cl^- • 4N₂O)

( • 4) +  = ( • 5)

By formula: (Cl^- • 4N₂O) + N₂O = (Cl^- • 5N₂O)

 +  = ( • )

By formula: F^- + N₂O = (F^- • N₂O)

( • ) +  = ( • 2)

By formula: (F^- • N₂O) + N₂O = (F^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (F^- • 2N₂O) + N₂O = (F^- • 3N₂O)

( • 3) +  = ( • 4)

By formula: (F^- • 3N₂O) + N₂O = (F^- • 4N₂O)

( • 4) +  = ( • 5)

By formula: (F^- • 4N₂O) + N₂O = (F^- • 5N₂O)

( • 5) +  = ( • 6)

By formula: (F^- • 5N₂O) + N₂O = (F^- • 6N₂O)

( • 6) +  = ( • 7)

By formula: (F^- • 6N₂O) + N₂O = (F^- • 7N₂O)

(H^- • 4294967295) +  = H^-

By formula: (H^- • 4294967295N₂O) + N₂O = H^-

HN₂O⁺ +  = (HN₂O⁺ • )

By formula: HN₂O⁺ + N₂O = (HN₂O⁺ • N₂O)

(HN₂O⁺ • ) +  = (HN₂O⁺ • 2)

By formula: (HN₂O⁺ • N₂O) + N₂O = (HN₂O⁺ • 2N₂O)

(HN₂O⁺ • 2) +  = (HN₂O⁺ • 3)

By formula: (HN₂O⁺ • 2N₂O) + N₂O = (HN₂O⁺ • 3N₂O)

(HN₂O⁺ • 3) +  = (HN₂O⁺ • 4)

By formula: (HN₂O⁺ • 3N₂O) + N₂O = (HN₂O⁺ • 4N₂O)

(HN₂O⁺ • 4) +  = (HN₂O⁺ • 5)

By formula: (HN₂O⁺ • 4N₂O) + N₂O = (HN₂O⁺ • 5N₂O)

(HN₂O⁺ • 5) +  = (HN₂O⁺ • 6)

By formula: (HN₂O⁺ • 5N₂O) + N₂O = (HN₂O⁺ • 6N₂O)

(HO^- • ) +  = (HO^- • 2)

By formula: (HO^- • N₂O) + N₂O = (HO^- • 2N₂O)

(HO^- • 2) +  = (HO^- • 3)

By formula: (HO^- • 2N₂O) + N₂O = (HO^- • 3N₂O)

(HO^- • 3) +  = (HO^- • 4)

By formula: (HO^- • 3N₂O) + N₂O = (HO^- • 4N₂O)

(HO^- • 4) +  = (HO^- • 5)

By formula: (HO^- • 4N₂O) + N₂O = (HO^- • 5N₂O)

 +  = ( • )

By formula: H₃O⁺ + N₂O = (H₃O⁺ • N₂O)

( • ) +  = ( • 2)

By formula: (H₃O⁺ • N₂O) + N₂O = (H₃O⁺ • 2N₂O)

( • 2) +  = ( • 3)

By formula: (H₃O⁺ • 2N₂O) + N₂O = (H₃O⁺ • 3N₂O)

( • 3) +  = ( • 4)

By formula: (H₃O⁺ • 3N₂O) + N₂O = (H₃O⁺ • 4N₂O)

 +  = ( • )

By formula: I^- + N₂O = (I^- • N₂O)

( • ) +  = ( • 2)

By formula: (I^- • N₂O) + N₂O = (I^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (I^- • 2N₂O) + N₂O = (I^- • 3N₂O)

( • 3) +  = ( • 4)

By formula: (I^- • 3N₂O) + N₂O = (I^- • 4N₂O)

( • 4) +  = ( • 5)

By formula: (I^- • 4N₂O) + N₂O = (I^- • 5N₂O)

( • 5) +  = ( • 6)

By formula: (I^- • 5N₂O) + N₂O = (I^- • 6N₂O)

( • 6) +  = ( • 7)

By formula: (I^- • 6N₂O) + N₂O = (I^- • 7N₂O)

( • 7) +  = ( • 8)

By formula: (I^- • 7N₂O) + N₂O = (I^- • 8N₂O)

( • 8) +  = ( • 9)

By formula: (I^- • 8N₂O) + N₂O = (I^- • 9N₂O)

( • 9) +  = ( • 10)

By formula: (I^- • 9N₂O) + N₂O = (I^- • 10N₂O)

( • 10) +  = ( • 11)

By formula: (I^- • 10N₂O) + N₂O = (I^- • 11N₂O)

( • 11) +  = ( • 12)

By formula: (I^- • 11N₂O) + N₂O = (I^- • 12N₂O)

 +  = ( • )

By formula: NO^- + N₂O = (NO^- • N₂O)

( • ) +  = ( • 2)

By formula: (NO^- • N₂O) + N₂O = (NO^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (NO^- • 2N₂O) + N₂O = (NO^- • 3N₂O)

( • 3) +  = ( • 4)

By formula: (NO^- • 3N₂O) + N₂O = (NO^- • 4N₂O)

( • 4) +  = ( • 5)

By formula: (NO^- • 4N₂O) + N₂O = (NO^- • 5N₂O)

( • 5) +  = ( • 6)

By formula: (NO^- • 5N₂O) + N₂O = (NO^- • 6N₂O)

( • 6) +  = ( • 7)

By formula: (NO^- • 6N₂O) + N₂O = (NO^- • 7N₂O)

NO₂⁺ +  = (NO₂⁺ • )

By formula: NO₂⁺ + N₂O = (NO₂⁺ • N₂O)

(NO₂⁺ • ) +  = (NO₂⁺ • 2)

By formula: (NO₂⁺ • N₂O) + N₂O = (NO₂⁺ • 2N₂O)

(NO₂⁺ • 2) +  = (NO₂⁺ • 3)

By formula: (NO₂⁺ • 2N₂O) + N₂O = (NO₂⁺ • 3N₂O)

(NO₂⁺ • 3) +  = (NO₂⁺ • 4)

By formula: (NO₂⁺ • 3N₂O) + N₂O = (NO₂⁺ • 4N₂O)

(NO₂⁺ • 4) +  = (NO₂⁺ • 5)

By formula: (NO₂⁺ • 4N₂O) + N₂O = (NO₂⁺ • 5N₂O)

(NO₂⁺ • 5) +  = (NO₂⁺ • 6)

By formula: (NO₂⁺ • 5N₂O) + N₂O = (NO₂⁺ • 6N₂O)

(N₂O₂^- • 4294967295) +  = N₂O₂^-

By formula: (N₂O₂^- • 4294967295N₂O) + N₂O = N₂O₂^-

(O^- • ) +  = (O^- • 2)

By formula: (O^- • N₂O) + N₂O = (O^- • 2N₂O)

(O^- • 2) +  = (O^- • 3)

By formula: (O^- • 2N₂O) + N₂O = (O^- • 3N₂O)

(O^- • 3) +  = (O^- • 4)

By formula: (O^- • 3N₂O) + N₂O = (O^- • 4N₂O)

(O^- • 4) +  = (O^- • 5)

By formula: (O^- • 4N₂O) + N₂O = (O^- • 5N₂O)

(O^- • 5) +  = (O^- • 6)

By formula: (O^- • 5N₂O) + N₂O = (O^- • 6N₂O)

(O^- • 6) +  = (O^- • 7)

By formula: (O^- • 6N₂O) + N₂O = (O^- • 7N₂O)

 +  = ( • )

By formula: O₂⁺ + N₂O = (O₂⁺ • N₂O)

Free energy of reaction

( • ) +  = ( • 2)

By formula: (O₂⁺ • N₂O) + N₂O = (O₂⁺ • 2N₂O)

( • 2) +  = ( • 3)

By formula: (O₂⁺ • 2N₂O) + N₂O = (O₂⁺ • 3N₂O)

( • 3) +  = ( • 4)

By formula: (O₂⁺ • 3N₂O) + N₂O = (O₂⁺ • 4N₂O)

( • 4) +  = ( • 5)

By formula: (O₂⁺ • 4N₂O) + N₂O = (O₂⁺ • 5N₂O)

( • 5) +  = ( • 6)

By formula: (O₂⁺ • 5N₂O) + N₂O = (O₂⁺ • 6N₂O)

( • 6) +  = ( • 7)

By formula: (O₂⁺ • 6N₂O) + N₂O = (O₂⁺ • 7N₂O)

 +  = ( • )

By formula: O₂^- + N₂O = (O₂^- • N₂O)

( • ) +  = ( • 2)

By formula: (O₂^- • N₂O) + N₂O = (O₂^- • 2N₂O)

( • 2) +  = ( • 3)

By formula: (O₂^- • 2N₂O) + N₂O = (O₂^- • 3N₂O)

( • 3) +  = ( • 4)

By formula: (O₂^- • 3N₂O) + N₂O = (O₂^- • 4N₂O)

( • 4) +  = ( • 5)

By formula: (O₂^- • 4N₂O) + N₂O = (O₂^- • 5N₂O)

( • 5) +  = ( • 6)

By formula: (O₂^- • 5N₂O) + N₂O = (O₂^- • 6N₂O)

References

Go To: Top, Ion clustering data, Notes

Data compilation copyright by the U.S. Secretary of Commerce on behalf of the U.S.A. All rights reserved.

Hiraoka, Aruga, et al., 1993
Hiraoka, K.; Aruga, K.; Fujimaki, S.; Yamabe, S., Comparative Study of the Gas Phase Bond Strengths of CO2 and N2O with the Halide Ions, J. Am. Soc. Mass Spectrom., 1993, 4, 1, 58, https://doi.org/10.1016/1044-0305(93)85043-W . [all data]

McMahon, Heinis, et al., 1988
McMahon, T.; Heinis, T.; Nicol, G.; Hovey, J.K.; Kebarle, P., Methyl Cation Affinities, J. Am. Chem. Soc., 1988, 110, 23, 7591, https://doi.org/10.1021/ja00231a002 . [all data]

Foster, Williamson, et al., 1974
Foster, M.S.; Williamson, A.D.; Beauchamp, J.L., Photoionization mass spectrometry of trans-azomethane, Int. J. Mass Spectrom. Ion Phys., 1974, 15, 429. [all data]

Sheldon, Ohair, et al., 1995
Sheldon, J.C.; Ohair, R.A.J.; Downard, K.M.; Gronert, S.; Krempp, M.; Depuy, C.H.; Bowie, J.H., A potential surface map of the H-/N2O system. The gas phase ion chemistry of HN2O-, Aust. J. Chem., 1995, 48, 155. [all data]

Hiraoka, Fujimaki, et al., 1994
Hiraoka, K.; Fujimaki, S.; Aruga, K.; Sato, T.; Yamabe, S., Gas-Phase Solavtion of NO+, O2+, N2O+, and H3O+ with N2O, J. Chem. Phys., 1994, 101, 5, 4073, https://doi.org/10.1063/1.467524 . [all data]

Szulejko and McMahon, 1992
Szulejko, J.; McMahon, T.B., personal communication, 1992. [all data]

Kim, Wenthold, et al., 1998
Kim, J.B.; Wenthold, P.G.; Lineberger, W.C., Photoelectron spectroscopy of OH-(N2O)(n=1-5), J. Chem. Phys., 1998, 108, 3, 830-837, https://doi.org/10.1063/1.475447 . [all data]

Arnold, Bradforth, et al., 1995
Arnold, D.W.; Bradforth, S.E.; Kim, E.H.; Neumark, D.M., Study of I-(CO2)n, Br-(CO2)n, and I-(N2O)n clusters by anion photoelectron spectroscopy, J. Chem. Phys., 1995, 102, 9, 3510, https://doi.org/10.1063/1.468576 . [all data]

Illies, 1988
Illies, A.J., Thermochemistry of the Gas - Phase Ion - Molecule Clustering of CO2+CO2, SO2+CO2, N2O+N2O, O2+CO2, NO+CO2 and NO+N2O: Description of a New Hybrid Drift Tube/Ion Source with Coaxial Electron Beam and Ion Exit Apertures, J. Phys. Chem., 1988, 92, 10, 2889, https://doi.org/10.1021/j100321a037 . [all data]

Hendricks, de Clercq, et al., 2002
Hendricks, J.H.; de Clercq, H.L.; Freidhoff, C.B.; Arnold, S.T.; Eaton, J.G.; Fancher, C.; Lyapustina, S.A.; S., Anion solvation at the microscopic level: Photoelectron spectroscopy of the solvated anion clusters, NO-(Y)(n), where Y=Ar, Kr, Xe, N2O, H2S, NH3, H2O, and C2H4(OH)(2), J. Chem. Phys., 2002, 116, 18, 7926-7938, https://doi.org/10.1063/1.1457444 . [all data]

Coe, Snodgrass, et al., 1987
Coe, J.V.; Snodgrass, J.T.; Freidhoff, C.B.; McHugh, K.M.; Bowen, K.H., Photoelectron spectroscopy of the negative cluster ions, NO-(N₂O)n=1,2, J. Chem. Phys., 1987, 87, 4302. [all data]

Hiraoka, Fujimaki, et al., 1994, 2
Hiraoka, K.; Fujimaki, S.; Aruga, K.; Yamabe, S., Gas-phase clustering reactions of O2(-), NO-, and O- with N2O: Isomeric structures for (NO-N2O)(-), J. Phys. Chem., 1994, 98, 34, 8295, https://doi.org/10.1021/j100085a006 . [all data]

Coe, Snodgrass, et al., 1986
Coe, J.V.; Snodgrass, J.T.; Freidhoff, C.B.; McHugh, K.M.; Bowen, K.H., Negative ion photoelectron spectroscopy of N₂O^- and (N₂O)₂^-, Chem. Phys. Lett., 1986, 124, 274. [all data]

Cameron, Aitken, et al., 1994
Cameron, B.R.; Aitken, C.G.; Harland, P.W., Appearence Energies of Small Cluster Ions and their Fragments, J. Chem. Soc. Faraday Trans., 1994, 90, 7, 935, https://doi.org/10.1039/ft9949000935 . [all data]

Linn and Ng, 1981
Linn, S.H.; Ng, C.Y., Photoionization Study of CO2, N2O Dimers and Clusters, J. Chem. Phys., 1981, 75, 10, 4921, https://doi.org/10.1063/1.441931 . [all data]

Li and Continetti, 2002
Li, R.J.; Continetti, R.E., Studies of the excited state dynamics of N2O2 by dissociative photodetachment of N2O2-, J. Phys. Chem. A, 2002, 106, 7, 1183-1189, https://doi.org/10.1021/jp013330u . [all data]

Osboen, Leahy, et al., 1996
Osboen, D.L.; Leahy, D.J.; Cyr, D.R.; Neumark, D.M., Photodissociation Spectroscopy and Dynamics of the N2O2- Anion, J. Chem. Phys., 1996, 104, 13, 5026, https://doi.org/10.1063/1.471132 . [all data]

Adams and Bohme, 1970
Adams, N.G.; Bohme, D., Flowing Afterglow Studies of Formation and Reactions of Cluster Ions of O₂⁺, O₂^-, and O^-, J. Chem. Phys., 1970, 52, 6, 3133, https://doi.org/10.1063/1.1673449 . [all data]

Notes

Go To: Top, Ion clustering data, References

• Symbols used in this document:
  

  T	Temperature
  ΔrG°	Free energy of reaction at standard conditions
  ΔrH°	Enthalpy of reaction at standard conditions
  ΔrS°	Entropy of reaction at standard conditions

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