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Nitrogen trifluoride

Names
IUPAC name Nitrogen trifluoride
Other names Nitrogen fluoride Trifluoramine Trifluorammonia
Identifiers
CAS Number	7783-54-2
3D model (JSmol)	Interactive image
ChEBI	CHEBI:30231
ChemSpider	22959
ECHA InfoCard	100.029.097
EC Number	232-007-1
Gmelin Reference	1551
PubChem CID	24553
RTECS number	QX1925000
UNII	4402F4X0RH
UN number	2451
CompTox Dashboard (EPA)	DTXSID4040181
InChI InChI=1S/F3N/c1-4(2)3Key: GVGCUCJTUSOZKP-UHFFFAOYSA-N InChI=1/F3N/c1-4(2)3Key: GVGCUCJTUSOZKP-UHFFFAOYAA
SMILES FN(F)F
Properties
Chemical formula	NF3
Molar mass	71.00 g/mol
Appearance	colorless gas
Odor	moldy
Density	3.003 kg/m (1 atm, 15 °C) 1.885 g/cm (liquid at b.p.)
Melting point	−207.15 °C (−340.87 °F; 66.00 K)
Boiling point	−129.06 °C (−200.31 °F; 144.09 K)
Solubility in water	0.021 g/100 mL
Vapor pressure	44.0 atm(−38.5 °F or −39.2 °C or 234.0 K)
Refractive index (nD)	1.0004
Structure
Molecular shape	trigonal pyramidal
Dipole moment	0.234 D
Thermochemistry
Heat capacity (C)	53.26 J/(mol·K)
Std molar entropy (S298)	260.3 J/(mol·K)
Std enthalpy of formation (ΔfH298)	−31.4 kcal/mol −109 kJ/mol
Gibbs free energy (ΔfG)	−84.4 kJ/mol
Hazards
GHS labelling:
Hazard statements	H270, H280, H332, H373
Precautionary statements	P220, P244, P260, P304+P340, P315, P370+P376, P403
NFPA 704 (fire diamond)	1 0 0OX
Flash point	Non-flammable
Lethal dose or concentration (LD, LC):
LC50 (median concentration)	2000 ppm (mouse, 4 h) 9600 ppm (dog, 1 h) 7500 ppm (monkey, 1 h) 6700 ppm (rat, 1 h) 7500 ppm (mouse, 1 h)
NIOSH (US health exposure limits):
PEL (Permissible)	TWA 10 ppm (29 mg/m)
REL (Recommended)	TWA 10 ppm (29 mg/m)
IDLH (Immediate danger)	1000 ppm
Safety data sheet (SDS)	AirLiquide
Related compounds
Other anions	nitrogen trichloride nitrogen tribromide nitrogen triiodide ammonia
Other cations	phosphorus trifluoride arsenic trifluoride antimony trifluoride bismuth trifluoride
Related binary fluoro-azanes	tetrafluorohydrazine
Related compounds	dinitrogen difluoride
Except where otherwise noted, data are given for materials in their standard state (at 25 °C , 100 kPa). Y verify (what is  ?) Infobox references

Nitrogen trifluoride is the inorganic compound with the formula (NF
₃). It is a colorless, non-flammable, toxic gas with a slightly musty odor. In contrast with ammonia, it is nonbasic. It finds increasing use within the manufacturing of flat-panel displays, photovoltaics, LEDs and other microelectronics. NF
₃ is a greenhouse gas, with a global warming potential (GWP) 17,200 times greater than that of CO
₂ when compared over a 100-year period.

Synthesis and reactivity

Nitrogen trifluoride can be prepared from the elements in the presence of an electric discharge. In 1903, Otto Ruff prepared nitrogen trifluoride by the electrolysis of a molten mixture of ammonium fluoride and hydrogen fluoride. It is far less reactive than the other nitrogen trihalides nitrogen trichloride, nitrogen tribromide, and nitrogen triiodide, all of which are explosive. Alone among the nitrogen trihalides it has a negative enthalpy of formation. It is prepared in modern times both by direct reaction of ammonia and fluorine and by a variation of Ruff's method. It is supplied in pressurized cylinders.

NF
₃ is slightly soluble in water without undergoing chemical reaction. It is nonbasic with a low dipole moment of 0.2340 D. By contrast, ammonia is basic and highly polar (1.47 D). This contrast reflects the differing electronegativities of H vs F.

Similar to dioxygen, NF₃ is a potent yet sluggish oxidizer. It oxidizes hydrogen chloride to chlorine:

2 NF₃ + 6 HCl → 6 HF + N₂ + 3 Cl₂

However, it only attacks (explosively) organic compounds at high temperatures. Consequently it is compatible under standard conditions with several plastics, as well as steel and Monel.

Above 200-300 °C, NF₃ reacts with metals, carbon, and other reagents to give tetrafluorohydrazine:

2NF₃ + Cu → N₂F₄ + CuF₂

NF₃ reacts with fluorine and antimony pentafluoride to give the tetrafluoroammonium salt:

NF₃ + F₂ + SbF₅ → NF
₄SbF
₆

NF₃ and B₂H₆ react vigorously even at cryogenic temperatures to give nitrogen gas, boron trifluoride, and hydrofluoric acid.

Applications

High-volume applications such as DRAM computer memory production, the manufacturing of flat panel displays and the large-scale production of thin-film solar cells use NF
₃.

Etching

Nitrogen trifluoride is primarily used to remove silicon and silicon-compounds during the manufacturing of semiconductor devices such as LCD displays, some thin-film solar cells, and other microelectronics. In these applications NF
₃ is initially broken down within a plasma. The resulting fluorine radicals are the active agents that attack polysilicon, silicon nitride and silicon oxide. They can be used as well to remove tungsten silicide, tungsten, and certain other metals. In addition to serving as an etchant in device fabrication, NF
₃ is also widely used to clean PECVD chambers.

NF
₃ dissociates more readily within a low-pressure discharge in comparison to perfluorinated compounds (PFCs) and sulfur hexafluoride (SF
₆). The greater abundance of negatively-charged free radicals thus generated can yield higher silicon removal rates, and provide other process benefits such as less residual contamination and a lower net charge stress on the device being fabricated. As a somewhat more thoroughly consumed etching and cleaning agent, NF₃ has also been promoted as an environmentally preferable substitute for SF
₆ or PFCs such as hexafluoroethane.

The utilization efficiency of the chemicals applied in plasma processes varies widely between equipment and applications. A sizeable fraction of the reactants are wasted into the exhaust stream and can ultimately be emitted into Earth's atmosphere. Modern abatement systems can substantially decrease atmospheric emissions. NF
₃ has not been subject to significant use restrictions. The annual reporting of NF
₃ production, consumption, and waste emissions by large manufacturers has been required in many industrialized countries as a response to the observed atmospheric growth and the international Kyoto Protocol.

Highly toxic fluorine gas (F₂, diatomic fluorine) is a climate neutral replacement for nitrogen trifluoride in some manufacturing applications. It requires more stringent handling and safety precautions, especially to protect manufacturing personnel.

Nitrogen trifluoride is also used in hydrogen fluoride and deuterium fluoride lasers, which are types of chemical lasers. There it is also preferred to fluorine gas due to its more convenient handling properties

Greenhouse gas

The GWP of NF
₃ is second only to SF
₆ in the group of Kyoto-recognised greenhouse gases, and NF
₃ was included in that grouping with effect from 2013 and the commencement of the second commitment period of the Kyoto Protocol. It has an estimated atmospheric lifetime of 740 years, although other work suggests a slightly shorter lifetime of 550 years (and a corresponding GWP of 16,800).

Since 1992, when less than 100 tons were produced, production grew to an estimated 4000 tons in 2007 and is projected to increase significantly. World production of NF₃ is expected to reach 8000 tons a year by 2010. By far the world's largest producer of NF
₃ is the US industrial gas and chemical company Air Products & Chemicals. An estimated 2% of produced NF
₃ is released into the atmosphere. Robson projected that the maximum atmospheric concentration is less than 0.16 parts per trillion (ppt) by volume, which will provide less than 0.001 Wm of IR forcing. The mean global tropospheric concentration of NF₃ has risen from about 0.02 ppt (parts per trillion, dry air mole fraction) in 1980, to 0.86 ppt in 2011, with a rate of increase of 0.095 ppt yr, or about 11% per year, and an interhemispheric gradient that is consistent with emissions occurring overwhelmingly in the Northern Hemisphere, as expected. This rise rate in 2011 corresponds to about 1200 metric tons/y NF₃ emissions globally, or about 10% of the NF₃ global production estimates. This is a significantly higher percentage than has been estimated by industry, and thus strengthens the case for inventorying NF₃ production and for regulating its emissions. One study co-authored by industry representatives suggests that the contribution of the NF₃ emissions to the overall greenhouse gas budget of thin-film Si-solar cell manufacturing is clear.

The UNFCCC, within the context of the Kyoto Protocol, decided to include nitrogen trifluoride in the second Kyoto Protocol compliance period, which begins in 2012 and ends in either 2017 or 2020. Following suit, the WBCSD/WRI GHG Protocol is amending all of its standards (corporate, product and Scope 3) to also cover NF₃.

Safety

Skin contact with NF
₃ is not hazardous, and it is a relatively minor irritant to mucous membranes and eyes. It is a pulmonary irritant with a toxicity considerably lower than nitrogen oxides, and overexposure via inhalation causes the conversion of hemoglobin in blood to methemoglobin, which can lead to the condition methemoglobinemia. The National Institute for Occupational Safety and Health (NIOSH) specifies that the concentration that is immediately dangerous to life or health (IDLH value) is 1,000 ppm.

See also

• IPCC list of greenhouse gases
• Nitrogen pentafluoride
• Tetrafluorohydrazine

Notes

1. This vapour pressure is the pressure at its critical temperature – below ordinary room temperature.

References

1. Air Products; Physical Properties for Nitrogen Trifluoride
2. Sinke, G. C. (1967). "The enthalpy of dissociation of nitrogen trifluoride". J. Phys. Chem. 71 (2): 359–360. doi:10.1021/j100861a022.
3. Inorganic Chemistry, p. 462, at Google Books
4. ^ NIOSH Pocket Guide to Chemical Hazards. "#0455". National Institute for Occupational Safety and Health (NIOSH).
5. "Nitrogen trifluoride". Immediately Dangerous to Life or Health Concentrations (IDLH). National Institute for Occupational Safety and Health (NIOSH).
6. ^ Philip B. Henderson, Andrew J. Woytek "Fluorine Compounds, Inorganic, Nitrogen" in Kirk‑Othmer Encyclopedia of Chemical Technology, 1994, John Wiley & Sons, NY. doi:10.1002/0471238961.1409201808051404.a01 Article Online Posting Date: December 4, 2000
7. ^ "Climate Change 2007: The Physical Sciences Basis" (PDF). IPCC. Retrieved 2008-07-03. {{cite journal}}: Cite journal requires |journal= (help)
8. Robson, J. I.; Gohar, L. K.; Hurley, M. D.; Shine, K. P.; Wallington, T. (2006). "Revised IR spectrum, radiative efficiency and global warming potential of nitrogen trifluoride". Geophys. Res. Lett. 33 (10): L10817. Bibcode:2006GeoRL..3310817R. doi:10.1029/2006GL026210.
9. Richard Morgan (2008-09-01). "Beyond Carbon: Scientists Worry About Nitrogen's Effects". The New York Times. Archived from the original on 2018-01-23. Retrieved 2008-09-07.
10. Lidin, P. A.; Molochko, V. A.; Andreeva, L. L. (1995). Химические свойства неорганических веществ (in Russian). pp. 442–455. ISBN 978-1-56700-041-2.
11. Otto Ruff, Joseph Fischer, Fritz Luft (1928). "Das Stickstoff-3-fluorid". Zeitschrift für Anorganische und Allgemeine Chemie. 172 (1): 417–425. doi:10.1002/zaac.19281720132.{{cite journal}}: CS1 maint: multiple names: authors list (link)
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13. Ruff, John K. (1967). "Derivatives of Nitrogen Fluorides". Chemical Reviews. 67 (6): 665–680. doi:10.1021/cr60250a004.
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    ₃, the greenhouse gas missing from Kyoto". Geophys. Res. Lett. 35 (12): L12810. Bibcode:2008GeoRL..3512810P. doi:10.1029/2008GL034542.
16. Tsai, W.-T. (2008). "Environmental and health risk analysis of nitrogen trifluoride (NF
    ₃), a toxic and potent greenhouse gas". J. Hazard. Mater. 159 (2–3): 257–63. doi:10.1016/j.jhazmat.2008.02.023. PMID 18378075.
17. H. Reichardt, A. Frenzel and K. Schober (2001). "Environmentally friendly wafer production: NF
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21. "Climate Change Indicators: Atmospheric Concentrations of Greenhouse Gases - Figure 4". U.S. Environmental Protection Agency. 27 June 2016. Retrieved 2021-03-05.
22. "Atmospheric Flask NF3". National Oceanic and Atmospheric Administration. 2020-06-30.
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25. Robson, Jon. "Nitrogen trifluoride (NF₃)". Royal Meteorological Society. Archived from the original on May 16, 2008. Retrieved 2008-10-27. {{cite journal}}: Cite journal requires |journal= (help)
26. Arnold, Tim; Harth, C. M.; Mühle, J.; Manning, A. J.; Salameh, P. K.; Kim, J.; Ivy, D. J.; Steele, L. P.; Petrenko, V. V.; Severinghaus, J. P.; Baggenstos, D.; Weiss, R. F. (2013-02-05). "Nitrogen trifluoride global emissions estimated from updated atmospheric measurements". Proc. Natl. Acad. Sci. USA. 110 (6): 2029–2034. Bibcode:2013PNAS..110.2029A. doi:10.1073/pnas.1212346110. PMC 3568375. PMID 23341630.
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External links

• National Pollutant Inventory – Fluoride and compounds fact sheet at the Wayback Machine (archived December 22, 2003)
• NF₃ Code of Practice (European Industrial Gas Association)]
• WebBook page for NF₃
• CDC - NIOSH Pocket Guide to Chemical Hazards

• Inorganic amines
• Nitrogen fluorides
• Greenhouse gases
• Industrial gases
• Nitrogen(III) compounds