Nitrogen difluoride
| Identifiers | |
|---|---|
| 3744-07-8[1] | |
| Properties | |
| NF 2 | |
| Related compounds | |
| Related nitrogen fluorides |
Nitrogen trifluoride dinitrogen tetrafluoride nitrogen monofluoride |
| Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa). | |
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| Infobox references | |
Nitrogen difluoride, also known as difluoroamino is a reactive radical molecule with formula NF2. This small molecule is in equilibrium with its dimer dinitrogen tetrafluoride.[2]
N2F4 ⇌ 2 NF2
As the temperature increases the proportion of NF2 increases.[3]
The molecule is unusual in that it has an odd number of electrons, yet is stable enough to study experimentally.[4]
Properties
The energy needed to break the N-N bond in N2F4 is 20.8 kcal/mol. This compares to 14.6 kcal/mol in N2O4 and 10.2 in N2O2 and 60 kcal/mol in hydrazine N2H4.
ΔHf = 34.421 kJ/mol.[5] The heat of dissociation of N2F4 forming NF2 is 20 kcal/mol.[6] Entropy change in this dissociation is 38.6 eu.[6]
In the molecule the N-F bond length is 1.3494 Å and the angle subtended at FNF is 103.33°.[7]
At room temperature N2F4 is mostly associated with only 0.7% in the form of NF2 at 5mm Hg pressure. When the temperature rises to 225 °C, it mostly dissociates with 99% in the form of NF2.[6]
In the infrared spectrum the N-F bond in NF2 has a symmetrical stretching frequency of 1075 cm−1. This compares to 1115 in NF, 1021 in NF3 and 998 in N2F4.[6]
The microwave spectrum shows numerous lines due to spin transitions, with or without nuclear spin transitions. The lines form set of two triplets for anti-symmetric singlet, or two triplets of triplets for symmetric triplet. Lines appear around 14-15, 24, 25, 26, 27, 28-29, 33, 60, 61, 62, 65 GHz. The rotational constants for the NF2 molecule as A=70496 MHz B=11872.2 MHz C=10136.5 MHz. Inertial defect Δ=0.1204 muÅ2. The centrifugal distortion constants are τaaaa=-7.75 τbbbb=-0.081 τaabb=0.30 τabab=-0.13.[7]
The dipole moment is 0.13 D (4.5×10−31Cm).[7]
The ground electronic state of the molecule is 2B1.[7]
The gas is often contaminated with NO or N2O.[6]
Use
Nitrogen difluoride is formed during the function of a xenon monofluoride excimer laser. Nitrogen trifluoride is the halide carrier gas, which releases fluoride ions when impacted by electrons:[1]
NF3 + e− → NF2 + F−
The free fluoride ion goes on to react with xenon cations.[1]
Nitrogen difluoride can be consumed further to yield nitrogen monofluoride.
NF2 + e− → NF + F−[1]
References
- 1 2 3 4 Trainor, Daniel W. (February 1989). "Electron dissociative attachment to nitrogen difluoride radicals". The Journal of Physical Chemistry. 93 (3): 1134–1136. doi:10.1021/j100340a022.
- ↑ F Fluorine: Compounds with Oxygen and Nitrogen. Gmelin Handbook of Inorganic Chemistry. 4. Berlin: Springer. 1986. p. 162. doi:10.1007/978-3-662-06339-2. ISBN 978-3-662-06341-5. Retrieved 29 August 2015.
- ↑ Johnson, Frederic A.; Colburn, Charles B. (July 1961). "The Tetrafluorohydrazine-Difluoroamino Radical Equilibrium". Journal of the American Chemical Society. 83 (14): 3043–3047. doi:10.1021/ja01475a018.
- ↑ Brown, R. D.; Burden, F. R.; Hart, B. T.; Williams, G. R. (1973). "The electronic structure of the NF2 radical". Theoretica Chimica Acta. 28 (4): 339–353. doi:10.1007/BF00529015.
- ↑ "Nitrogen difluoride NF2(g)".
- 1 2 3 4 5 Bohn, Robert K.; Bauer, Simon Harvey (February 1967). "An electron diffraction study of the structures of NF2 and N2F4". Inorganic Chemistry. 6 (2): 304–309. doi:10.1021/ic50048a024. molecule dimensions and angles
- 1 2 3 4 Brown, R.D.; Burden, F.R.; Godfrey, P.D.; Gillard, I.R. (August 1974). "Microwave spectrum of NF2". Journal of Molecular Spectroscopy. 52 (2): 301–321. doi:10.1016/0022-2852(74)90121-0.