Nitrogen difluoride

Nitrogen difluoride
Identifiers
CAS Number	3744-07-8[1];
3D model (JSmol)	Interactive image;
ChemSpider	121681;
PubChem CID	138039;
CompTox Dashboard (EPA)	DTXSID90190888 ;
	InChI InChI=1S/F2N/c1-3-2 Key: BBZREMAMWBDNHH-UHFFFAOYSA-N;
	SMILES [N](F)F;
Properties
Chemical formula	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).
	(what is ?)
	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 m^uÅ². The centrifugal distortion constants are τ_aaaa=-7.75 τ_bbbb=-0.081 τ_aabb=0.30 τ_abab=-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]

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References

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)".
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
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. Bibcode:1974JMoSp..52..301B. doi:10.1016/0022-2852(74)90121-0.

Extra reading

Goodfriend, P.L.; Woods, H.P. (January 1964). "The absorption spectrum of NF2". Journal of Molecular Spectroscopy. 13 (1–4): 63–66. Bibcode:1964JMoSp..13...63G. doi:10.1016/0022-2852(64)90055-4.
Jacox, Marilyn E.; Milligan, Dolphus E.; Guillory, William A.; Smith, Jerry J. (August 1974). "Matrix-isolation study of the vacuum-ultraviolet photolysis of NF3". Journal of Molecular Spectroscopy. 52 (2): 322–327. Bibcode:1974JMoSp..52..322J. doi:10.1016/0022-2852(74)90122-2.
Heidner, R. F.; Helvajian, Henry; Koffend, J. Brooke (August 1987). "Tunable UV laser photolysis of NF2: Quantum yield for NF(a1Δ) production". The Journal of Chemical Physics. 87 (3): 1520–1524. Bibcode:1987JChPh..87.1520H. doi:10.1063/1.453262.
Papakondylis, Aristotle; Mavridis, Aristides (December 1993). "Electronic and geometrical structure of the NF2 radical" (PDF). Chemical Physics Letters. 216 (1–2): 167–172. Bibcode:1993CPL...216..167P. doi:10.1016/0009-2614(93)E1254-E.
Cai, Z.-L.; Sha, G.-H.; Zhang, C.-H.; Huang, M.-B. (March 1991). "Ab initio study of low-lying electronic states of the NF2 radical". Chemical Physics Letters. 178 (2–3): 273–278. Bibcode:1991CPL...178..273C. doi:10.1016/0009-2614(91)87068-M.

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[trainor89-1] 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.

[2] 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.

[Johnson61-3] 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.

[brown73-4] 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.

[5] "Nitrogen difluoride NF₂(g)".

[bohn67-6] 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

[brown74-7] 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. Bibcode:1974JMoSp..52..301B. doi:10.1016/0022-2852(74)90121-0.