Nitrogen

• Formula: N₂
• Molecular weight: 28.0134
• IUPAC Standard InChI: InChI=1S/N2/c1-2 Copy

  
• IUPAC Standard InChIKey: IJGRMHOSHXDMSA-UHFFFAOYSA-N Copy
• CAS Registry Number: 7727-37-9
• 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 gas; N2; UN 1066; UN 1977; Dinitrogen; Molecular nitrogen; Diatomic nitrogen; Nitrogen-14
• Permanent link for this species. Use this link for bookmarking this species for future reference.
• Information on this page:
  • Reaction thermochemistry data (reactions 51 to 100)
  • References
  • Notes
• Other data available:
  • Gas phase thermochemistry data
  • Phase change data
  • Reaction thermochemistry data: reactions 1 to 50, reactions 101 to 150, reactions 151 to 156
  • Henry's Law data
  • Gas phase ion energetics data
  • Ion clustering data
  • Mass spectrum (electron ionization)
  • Constants of diatomic molecules
  • Fluid Properties
• Data at other public NIST sites:
  • Electron-Impact Ionization Cross Sections (on physics web site)
  • Computational Chemistry Comparison and Benchmark Database
  • Gas Phase Kinetics Database
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Reaction thermochemistry 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 by: Michael M. Meot-Ner (Mautner) and Sharon G. Lias

Note: Please consider using the reaction search for this species. This page allows searching of all reactions involving this species. A general reaction search form is also available. Future versions of this site may rely on reaction search pages in place of the enumerated reaction displays seen below.

Reactions 51 to 100

( •  • ) +  = ( • 2 • )

By formula: (H₃O⁺ • N₂ • H₂O) + N₂ = (H₃O⁺ • 2N₂ • H₂O)

(NO₂⁺ • 10) +  = (NO₂⁺ • 11)

By formula: (NO₂⁺ • 10N₂) + N₂ = (NO₂⁺ • 11N₂)

(NO₂⁺ • 11) +  = (NO₂⁺ • 12)

By formula: (NO₂⁺ • 11N₂) + N₂ = (NO₂⁺ • 12N₂)

( • 9) +  = ( • 10)

By formula: (O₂⁺ • 9N₂) + N₂ = (O₂⁺ • 10N₂)

( • 9) +  = ( • 10)

By formula: (N₂⁺ • 9N₂) + N₂ = (N₂⁺ • 10N₂)

(NO₂⁺ • 9) +  = (NO₂⁺ • 10)

By formula: (NO₂⁺ • 9N₂) + N₂ = (NO₂⁺ • 10N₂)

(N₃⁺ • 10) +  = (N₃⁺ • 11)

By formula: (N₃⁺ • 10N₂) + N₂ = (N₃⁺ • 11N₂)

( • 5) +  = ( • 6)

By formula: (O₂⁺ • 5N₂) + N₂ = (O₂⁺ • 6N₂)

( • 6) +  = ( • 7)

By formula: (O₂⁺ • 6N₂) + N₂ = (O₂⁺ • 7N₂)

( • 7) +  = ( • 8)

By formula: (O₂⁺ • 7N₂) + N₂ = (O₂⁺ • 8N₂)

( • 8) +  = ( • 9)

By formula: (O₂⁺ • 8N₂) + N₂ = (O₂⁺ • 9N₂)

( • 2) +  = ( • 3)

By formula: (N₂⁺ • 2N₂) + N₂ = (N₂⁺ • 3N₂)

( • 3) +  = ( • 4)

By formula: (N₂⁺ • 3N₂) + N₂ = (N₂⁺ • 4N₂)

( • 4) +  = ( • 5)

By formula: (N₂⁺ • 4N₂) + N₂ = (N₂⁺ • 5N₂)

( • 5) +  = ( • 6)

By formula: (N₂⁺ • 5N₂) + N₂ = (N₂⁺ • 6N₂)

( • 6) +  = ( • 7)

By formula: (N₂⁺ • 6N₂) + N₂ = (N₂⁺ • 7N₂)

( • 7) +  = ( • 8)

By formula: (N₂⁺ • 7N₂) + N₂ = (N₂⁺ • 8N₂)

( • 8) +  = ( • 9)

By formula: (N₂⁺ • 8N₂) + N₂ = (N₂⁺ • 9N₂)

(NO₂⁺ • 2) +  = (NO₂⁺ • 3)

By formula: (NO₂⁺ • 2N₂) + N₂ = (NO₂⁺ • 3N₂)

(NO₂⁺ • 3) +  = (NO₂⁺ • 4)

By formula: (NO₂⁺ • 3N₂) + N₂ = (NO₂⁺ • 4N₂)

(NO₂⁺ • 4) +  = (NO₂⁺ • 5)

By formula: (NO₂⁺ • 4N₂) + N₂ = (NO₂⁺ • 5N₂)

(NO₂⁺ • 5) +  = (NO₂⁺ • 6)

By formula: (NO₂⁺ • 5N₂) + N₂ = (NO₂⁺ • 6N₂)

(NO₂⁺ • 6) +  = (NO₂⁺ • 7)

By formula: (NO₂⁺ • 6N₂) + N₂ = (NO₂⁺ • 7N₂)

(NO₂⁺ • 7) +  = (NO₂⁺ • 8)

By formula: (NO₂⁺ • 7N₂) + N₂ = (NO₂⁺ • 8N₂)

(NO₂⁺ • 8) +  = (NO₂⁺ • 9)

By formula: (NO₂⁺ • 8N₂) + N₂ = (NO₂⁺ • 9N₂)

( • 4) +  = ( • 5)

By formula: (NO^- • 4N₂) + N₂ = (NO^- • 5N₂)

( • 5) +  = ( • 6)

By formula: (NO^- • 5N₂) + N₂ = (NO^- • 6N₂)

( • 6) +  = ( • 7)

By formula: (NO^- • 6N₂) + N₂ = (NO^- • 7N₂)

( • 7) +  = ( • 8)

By formula: (NO^- • 7N₂) + N₂ = (NO^- • 8N₂)

( • 8) +  = ( • 9)

By formula: (NO^- • 8N₂) + N₂ = (NO^- • 9N₂)

(N₃⁺ • 9) +  = (N₃⁺ • 10)

By formula: (N₃⁺ • 9N₂) + N₂ = (N₃⁺ • 10N₂)

(HN₂⁺ • 9) +  = (HN₂⁺ • 10)

By formula: (HN₂⁺ • 9N₂) + N₂ = (HN₂⁺ • 10N₂)

(NO₂⁺ • ) +  = (NO₂⁺ • 2)

By formula: (NO₂⁺ • N₂) + N₂ = (NO₂⁺ • 2N₂)

(N₃⁺ • 3) +  = (N₃⁺ • 4)

By formula: (N₃⁺ • 3N₂) + N₂ = (N₃⁺ • 4N₂)

(N₃⁺ • 4) +  = (N₃⁺ • 5)

By formula: (N₃⁺ • 4N₂) + N₂ = (N₃⁺ • 5N₂)

(N₃⁺ • 5) +  = (N₃⁺ • 6)

By formula: (N₃⁺ • 5N₂) + N₂ = (N₃⁺ • 6N₂)

(N₃⁺ • 6) +  = (N₃⁺ • 7)

By formula: (N₃⁺ • 6N₂) + N₂ = (N₃⁺ • 7N₂)

(N₃⁺ • 7) +  = (N₃⁺ • 8)

By formula: (N₃⁺ • 7N₂) + N₂ = (N₃⁺ • 8N₂)

(N₃⁺ • 8) +  = (N₃⁺ • 9)

By formula: (N₃⁺ • 8N₂) + N₂ = (N₃⁺ • 9N₂)

(HN₂⁺ • 5) +  = (HN₂⁺ • 6)

By formula: (HN₂⁺ • 5N₂) + N₂ = (HN₂⁺ • 6N₂)

(HN₂⁺ • 6) +  = (HN₂⁺ • 7)

By formula: (HN₂⁺ • 6N₂) + N₂ = (HN₂⁺ • 7N₂)

(HN₂⁺ • 7) +  = (HN₂⁺ • 8)

By formula: (HN₂⁺ • 7N₂) + N₂ = (HN₂⁺ • 8N₂)

(HN₂⁺ • 8) +  = (HN₂⁺ • 9)

By formula: (HN₂⁺ • 8N₂) + N₂ = (HN₂⁺ • 9N₂)

( • ) +  = ( •  • )

By formula: (O₂^- • O₂) + N₂ = (O₂^- • N₂ • O₂)

(N₃⁺ • 2) +  = (N₃⁺ • 3)

By formula: (N₃⁺ • 2N₂) + N₂ = (N₃⁺ • 3N₂)

(N₃⁺ • ) +  = (N₃⁺ • 2)

By formula: (N₃⁺ • N₂) + N₂ = (N₃⁺ • 2N₂)

( • 2) +  = ( •  • 2)

By formula: (H₃O⁺ • 2H₂O) + N₂ = (H₃O⁺ • N₂ • 2H₂O)

( • ) +  = ( •  • )

By formula: (H₃O⁺ • H₂O) + N₂ = (H₃O⁺ • N₂ • H₂O)

( • 2) +  = ( • 3)

By formula: (CF₃⁺ • 2N₂) + N₂ = (CF₃⁺ • 3N₂)

( • 3) +  = ( • 4)

By formula: (CF₃⁺ • 3N₂) + N₂ = (CF₃⁺ • 4N₂)

References

Go To: Top, Reaction thermochemistry data, Notes

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

Gheno and Fitaire, 1987
Gheno, F.; Fitaire, M., Association of N2 with NH4+ and H3O+(H2O)n, n = 1,2,3, J. Chem. Phys., 1987, 87, 2, 953, https://doi.org/10.1063/1.453250 . [all data]

Hiraoka and Yamabe, 1989
Hiraoka, K.; Yamabe, S., How are Nitrogen Molecules Bound to NO2+ and NO+?, J. Chem. Phys., 1989, 90, 6, 3268, https://doi.org/10.1063/1.455880 . [all data]

Hiraoka and Nakajima, 1988
Hiraoka, K.; Nakajima, G., A Determination of the Stabilities of N2+(N2)n and O2+(N2)n with n = 1 - 11 from Measurements of the Gas - Phase Ion Equilibria, J. Chem. Phys., 1988, 88, 12, 7709, https://doi.org/10.1063/1.454285 . [all data]

Hiraoka and Yamabe, 1989, 2
Hiraoka, K.; Yamabe, S., Stabilities of the N3+(N2)n Cluster Ions with n = 1 - 11, Chem. Phys. Lett., 1989, 154, 2, 139, https://doi.org/10.1016/S0009-2614(89)87275-6 . [all data]

Hiraoka and Mori, 1989
Hiraoka, K.; Mori, T., Gas Phase Stabilities of the Cluster Ions H+(CO)2(CO)n, H+(N2)2(N2)n and H+(O2)2(O2)n with n = 1 - 14, Chem. Phys., 1989, 137, 1-3, 345, https://doi.org/10.1016/0301-0104(89)87119-8 . [all data]

Hiraoka, 1988
Hiraoka, K., Determination of the Stabilities of O₃^-(N₂)n, O₃^-(O₂)n, and O₄^-(N₂)n from Measurements of the Gas Phase Equilibria, Chem. Phys., 1988, 125, 2-3, 439, https://doi.org/10.1016/0301-0104(88)87096-4 . [all data]

Hiraoka, Nasu, et al., 1996
Hiraoka, K.; Nasu, M.; Fujimaki, S.; Ignacio, E.W.; Yamabe, S., Gas-Phase Stability and Structure of the Cluster Ions CF3+(CO)n, CF3+(N2)n, CF3+((CF4)n, and CF4H+(CF4)n, J. Phys. Chem., 1996, 100, 13, 5245, https://doi.org/10.1021/jp9530010 . [all data]

Notes

Go To: Top, Reaction thermochemistry data, References

• Symbols used in this document:
  

  ΔrH°	Enthalpy of reaction at standard conditions
  ΔrS°	Entropy of reaction at standard conditions

• Data from NIST Standard Reference Database 69: NIST Chemistry WebBook
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