Dinitrogen Difluoride
Get Dinitrogen Difluoride essential facts below. View Videos or join the Dinitrogen Difluoride discussion. Add Dinitrogen Difluoride to your PopFlock.com topic list for future reference or share this resource on social media.
Dinitrogen Difluoride
Dinitrogen difluoride[1]
cis-Dinitrogen difluoride (left) and trans-dinitrogen difluoride (right)
Cis-dinitrogen difluoride molecule
Trans-dinitrogen difluoride molecule
IUPAC name
cis- or trans-dinitrogen difluoride
Other names
cis- or trans-difluorodiazene
3D model (JSmol)
Molar mass 66.010 g/mol
Appearance colorless gas
Density 2.698 g/L
Melting point cis: < -195 °C (-319.0 °F; 78.1 K)
trans: -172 °C
Boiling point cis: -105.75 °C (-158.35 °F; 167.40 K)
trans: -111.45 °C
cis: 0.16 D
trans: 0 D
cis: 69.5 kJ/mol
trans: 82.0 kJ/mol
Related compounds
Other cations
azo compounds
Related Binary fluoro-azanes
nitrogen trifluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
?N verify (what is ?Y?N ?)
Infobox references

Dinitrogen difluoride is a chemical compound with the formula N2F2. It is a gas at room temperature, and was first identified in 1952 as the thermal decomposition product of the azide N3F. It has the structure F-N=N-F and exists in both a cis- and trans-form.


The cis configuration lies in a C2v symmetry and the trans-form has a symmetry of C2h. These isomers are thermally interconvertible but can be separated by low temperature fractionation. The trans-form is less thermodynamically stable but can be stored in glass vessels. The cis-form attacks glass over a time scale of about 2 weeks to form silicon tetrafluoride and nitrous oxide:[2]

2 N2F2 + SiO2 -> SiF4 + 2 N2O


Most preparations of dinitrogen difluoride give mixtures of the two isomers, but they can be prepared independently.

An aqueous method involves N,N-difluorourea with concentrated potassium hydroxide. This gives a 40% yield with three times more of the trans isomer.[3]

Difluoramine forms a solid unstable compound with potassium fluoride (or rubidium fluoride or caesium fluoride) which decomposes to dinitrogen difluoride.[3]

It can also be prepared by photolysis of tetrafluorohydrazine and bromine:[4]


The cis form of dinitrogen difluoride will react with strong fluoride ion acceptors such as antimony pentafluoride to form the N2F+ cation.

N2F2 + SbF5 -> N2F+[SbF6]-

In the solid phase, the observed N=N and N-F bond distances in the N2F+ cation are 1.089(9) and 1.257(8) Å respectively, among the shortest experimentally observed N-N and N-F bonds.


  1. ^ Lide, David R. (1998). Handbook of Chemistry and Physics (87th ed.). Boca Raton, FL: CRC Press. pp. 4-73, 5-15, 9-46. ISBN 0-8493-0594-2.
  2. ^ Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  3. ^ a b Sykes, A. G. (1989-07-17). Advances in Inorganic Chemistry. Academic Press. p. 171. ISBN 9780080578828. Retrieved 2014.
  4. ^ Leon M. Zaborowski; et al. (1973), Aaron Wold and John K. Ruff (ed.), "Chlorodifluoroamine and Difluorodiazene - B. Difluorodiazene (Dinitrogen difluoride)", Inorganic Syntheses (in German), McGraw-Hill Book Company, Inc., 14, pp. 34-39

  This article uses material from the Wikipedia page available here. It is released under the Creative Commons Attribution-Share-Alike License 3.0.



Music Scenes