Sodium hyponitrite

Sodium hyponitrite is a solid ionic compound with formula Na
2N
2O
2 or (Na+
)2[ON=NO]2−.[1]

Sodium hyponitrite
Identifiers
3D model (JSmol)
ChemSpider
  • InChI=1S/H2N2O2.2Na/c3-1-2-4;;/h(H,1,4)(H,2,3);;/q;2*+1/p-2
    Key: HLJWMCUZPYEUDI-UHFFFAOYSA-L
  • N(=N[O-])[O-].[Na+].[Na+]
  • trans-form: [Na+].[O-]/N=N/[O-].[Na+]
  • cis-form: [Na+].[O-]\N=N/[O-].[Na+]
Properties
Na2N2O2
Molar mass 105.99 g/mol
Appearance colorless crystals
Density 2.466 g/cm3
Melting point 100 °C (212 °F; 373 K)
Boiling point 335 °C (635 °F; 608 K) decomposes
soluble
Solubility insoluble in ethanol
Except where otherwise noted, data are given for materials in their standard state (at 25 °C [77 °F], 100 kPa).
Infobox references

There are cis and trans forms of the hyponitrite ion N
2O2−
2. The trans form is more common, but the cis form can be obtained too, and it is more reactive than the trans form.[1][2]

Trans isomer

The trans isomer is colorless and soluble in water and insoluble in ethanol and ether.[3][4]

Preparation

Sodium hyponitrite (trans) is conventionally prepared by reduction of sodium nitrite with sodium amalgam.[5][6][7]

2 NaNO2 + 4 Na(Hg) + 2 H2O → Na2N2O2 + 4 NaOH + 4 Hg

Sodium hyponitrite (trans) was prepared in 1927 by A. W. Scott by reacting alkyl nitrites, hydroxylammonium chloride, and sodium ethoxide[4][8]

RONO + NH2OH + 2 EtONa → Na2N2O2 + ROH + 2 EtOH

An earlier method, published by D. Mendenhall in 1974, reacted gaseous nitric oxide (NO) with sodium metal in 1,2-dimethoxyethane, toluene, and benzophenone. The salt was then extracted with water.[9] The method was later modified to use pyridine.

Other methods included oxidation of a concentrated solution of hydroxylamine with sodium nitrite in an alkaline medium; or electrolysis of sodium nitrite.[10]

Hydrates

A variety of hydrates Na
2N
2O
2(H
2O)x of the trans isomer have been reported, with x including 2, 3.5, 4, 5, 6, 7, 8, and 9;[11][3][12] but there is some dispute.[13]

The hydration water seems to be just trapped in the crystal lattice rather than coordinated to the ions.[13] The anhydrous substance can be obtained by drying the hydrates over phosphorus pentoxide and then heating them to 120 °C.[13]

Reactions

Sodium hyponitrite (trans) in solution is decomposed by carbon dioxide CO
2 from air to form sodium carbonate.[14]

Liquid N2O4 oxidises sodium hyponitrite (trans) to give sodium peroxohyponitrite Na2+
2[ON=NOO]2−).[15][1]

Cis isomer

The cis isomer of sodium hyponitrite is a white crystalline solid, insoluble in aprotic solvents, and (unlike the trans isomer) decomposed by water and other protic solvents.[2]

Preparation

The cis isomer of can be prepared by passing nitric oxide (NO) through a solution of sodium metal in liquid ammonia at −50 °C.[1]

The cis isomer was also obtained in 1996 by C. Feldmann and M. Jansen by heating sodium oxide Na
2O with 77 kPa of nitrous oxide N
2O (laughing gas) in a sealed tube at 360 °C for 2 hours. The two reagents combined to yield the cis hyponitrite quantitatively as white microcrystals.[8][2]

Properties and reactions

The anhydrous cis salt is stable up to 325 °C, when it disproportionates to nitrogen and sodium orthonitrite:[2]

3 Na
2N
2O
2 → 2 Na
3O(NO
2) + 2 N
2

It is generally more reactive than the trans isomer.[1]

See also

References
  1. Egon Wiberg, Arnold Frederick Holleman (2001) Inorganic Chemistry, Elsevier ISBN 0-12-352651-5
  2. Claus Feldmann, Martin Jansen (1996), "cis-Sodium Hyponitrite - A New Preparative Route and a Crystal Structure Analysis". Angewandte Chemie International Edition in English, volume 35, issue 15, pages 1728–1730. doi:10.1002/anie.199617281
  3. Trambaklal Mohanlal Oza, Rajnikant Hariprasad Thaker (1955), "The Thermal Decomposition of Silver Hyponitrite". Journal of the American Chemical society, volume 77, issue 19, pages 4976–4980. doi:10.1021/ja01624a007
  4. A. W. Scott (1927), "Sodium Hyponitrite". J. Am. Chem. Soc., volume = 49, issue 4, pages = 986–987. doi:10.1021/ja01403a502
  5. Addison, C. C.; Gamlen G. A.; Thompson, R. (1952). "70. The ultra-violet absorption spectra of sodium hyponitrite and sodium α-oxyhyponitrite : the analysis of mixtures with sodium nitrite and nitrate". J. Chem. Soc.: 338–345. doi:10.1039/jr9520000338.
  6. Neumann, R. C., Jr. Bussey, R. J. (1970). "High pressure studies. V. Activation volumes for combination and diffusion of geminate tert-butoxy radicals". J. Am. Chem. Soc. 92 (8): 2440–2445. doi:10.1021/ja00711a039.{{cite journal}}: CS1 maint: multiple names: authors list (link)
  7. Greenwood, Norman N.; Earnshaw, Alan (1997). Chemistry of the Elements (2nd ed.). Butterworth-Heinemann. ISBN 978-0-08-037941-8.
  8. Catherine E. Housecroft; Alan G. Sharpe (2008). "Chapter 15: The group 15 elements". Inorganic Chemistry (3rd ed.). Pearson. p. 468. ISBN 978-0-13-175553-6.
  9. G. David Mendenhall (1974), "Convenient synthesis of silver hyponitrite". Journal of the American Chemical society, volume 96, issue 15, page 5000. doi:10.1021/ja00822a054
  10. Polydoropoulos, C. N. Chem. Ind. (London) 1963, 1686 and references therein.
  11. James Riddick Partington and Chandulal Chhotalal Shah (1931), "Investigations on hyponitrites. Part I. Sodium hyponitrite: preparation and properties". Journal of the Chemical Society (Resumed), paper CCLXXXII, pages 2071-2080. doi:10.1039/JR9310002071
  12. C.N. Polydoropoulos, S.D. Voliotis (1967), "Sodium hyponitrite hexahydrate". Journal of Inorganic and Nuclear Chemistry, volume 29, issue 12, pages 2899–2901. doi:10.1016/0022-1902(67)80121-0
  13. Gary L. Stucky, Jack L. Lambert, R. Dean Dragsdorf (1969), "The hydrates of sodium hyponitrite". Journal of Inorganic and Nuclear Chemistry, volume 31, issue 1, pages 29–32 doi:10.1016/0022-1902(69)80050-3
  14. Charlotte N. Conner, Caroline E. Donald, Martin N. Hughes, Christina Sami (1989), "The molar absorptivity of sodium hyponitrite". Polyhedron, volume 8, issue 21, pages 2621-2622. doi:10.1016/S0277-5387(00)81166-3
  15. M. N. Hughes and H. G. Nicklin (1969), "The action of dinitrogen tetroxide on sodium hyponitrite". Journal of the Chemical Society D: Chemical Communications, volume 1969, issue 2, page 80a. doi:10.1039/C2969000080A
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