Tetrasulfur tetranitride
Stereo, skeletal formula of tetrasulfur tetranitride with some measurements
Ball and stick model of tetrasulfur tetranitride
Ball and stick model of tetrasulfur tetranitride
Space-filling model of tetrasulfur tetranitride
Space-filling model of tetrasulfur tetranitride
Names
IUPAC name
Tetrasulfur tetranitride
Systematic IUPAC name
1,3,5,7-tetrathia-2,4,6,8-tetraazacyclooctan-2,4,6,8-tetrayl
Other names
  • Cyclic sulfur(III) nitride tetramer
  • Tetranitrogen tetrasulfide
  • 1λ4,3,5λ4,7,2,4,6,8-Tetrathiatetrazocine
Identifiers
3D model (JSmol)
ChemSpider
UNII
  • InChI=1S/N4S4/c1-5-2-7-4-8-3-6-1 checkY
    Key: LTPQFVPQTZSJGS-UHFFFAOYSA-N checkY
  • N1=[S]N=[S]N=[S]N=[S]1
Properties
S4N4
Molar mass 184.287 g/mol
Appearance Vivid orange, opaque crystals
Melting point 187 °C (369 °F; 460 K)
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

Tetrasulfur tetranitride is an inorganic compound with the formula S4N4. This gold-poppy coloured solid is the most important binary sulfur nitride, which are compounds that contain only the elements sulfur and nitrogen. It is a precursor to many S-N compounds and has attracted wide interest for its unusual structure and bonding.[1][2]

Nitrogen and sulfur have similar electronegativities. When the properties of atoms are so highly similar, they often form extensive families of covalently bonded structures and compounds. Indeed, a large number of S-N and S-NH compounds are known with S4N4 as their parent.

Structure

S4N4 adopts an unusual “extreme cradle” structure, with D2d point group symmetry. It can be viewed as a derivative of a (hypothetical) eight-membered ring (or more simply a 'deformed' eight-membered ring) of alternating sulfur and nitrogen atoms. The pairs of sulfur atoms across the ring are separated by 2.586 Å, resulting in a cage-like structure as determined by single crystal X-ray diffraction.[3] The nature of the transannular S–S interactions remains a matter of investigation because it is significantly shorter than the sum of the van der Waal's distances[4] but has been explained in the context of molecular orbital theory.[1] One pair of the transannular S atoms have valence 4, and the other pair of the transannular S atoms have valence 2. The bonding in S4N4 is considered to be delocalized, which is indicated by the fact that the bond distances between neighboring sulfur and nitrogen atoms are nearly identical. S4N4 has been shown to co-crystallize with benzene and the C60 molecule.[5]

Properties

S4N4 is stable to air. It is, however, unstable in the thermodynamic sense with a positive enthalpy of formation of +460 kJ/mol. This endothermic enthalpy of formation originates in the difference in energy of S4N4 compared to its highly stable decomposition products:

2 S4N4 → 4 N2 + S8

Because one of its decomposition products is a gas, S4N4 can be used as an explosive.[1] Purer samples tend to be more explosive. Small samples can be detonated by striking with a hammer. S4N4 is thermochromic, changing from pale yellow below −30 °C to orange at room temperature to deep red above 100 °C.[1]

Synthesis

S4N4 was first prepared in 1835 by M. Gregory by the reaction of disulfur dichloride with ammonia,[6] a process that has been optimized:[7]

6 S2Cl2 + 16 NH3 → S4N4 + S8 + 12 [NH4]Cl

Coproducts of this reaction include heptasulfur imide (S7NH) and elemental sulfur. A related synthesis employs [NH4]Cl instead:[1]

4 [NH4]Cl + 6 S2Cl2 → S4N4 + 16 HCl + S8

An alternative synthesis entails the use of (((CH3)3Si)2N)2S as a precursor with pre-formed S–N bonds. (((CH3)3Si)2N)2S is prepared by the reaction of lithium bis(trimethylsilyl)amide and SCl2.

2 ((CH3)3Si)2NLi + SCl2 → (((CH3)3Si)2N)2S + 2 LiCl

The (((CH3)3Si)2N)2S reacts with the combination of SCl2 and SO2Cl2 to form S4N4, trimethylsilyl chloride, and sulfur dioxide:[8]

2 (((CH3)3Si)2N)2S + 2 SCl2 + 2 SO2Cl2 → S4N4 + 8 (CH3)3SiCl + 2 SO2

Acid-base reactions

S4N4·BF3

S4N4 serves as a Lewis base by binding through nitrogen to strongly Lewis acidic compounds such as SbCl5 and SO3. The cage is distorted in these adducts.[1]

S4N4 + SbCl5 → S4N4·SbCl5
S4N4 + SO3 → S4N4·SO3

The reaction of [Pt2Cl4(P(CH3)2Ph)2] with S4N4 is reported to form a complex where a sulfur forms a dative bond to the metal. This compound upon standing is isomerised to a complex in which a nitrogen atom forms the additional bond to the metal centre.

It is protonated by H[BF4] to form a tetrafluoroborate salt:

S4N4 + H[BF4] → [S4N4H]+[BF4]−

The soft Lewis acid CuCl forms a coordination polymer:[1]

n S4N4 + n CuCl → (S4N4)n-μ-(−Cu−Cl−)n

Dilute NaOH hydrolyzes S4N4 as follows, yielding thiosulfate and trithionate:[1]

2 S4N4 + 6 OH− + 9 H2O → S2O2−3 + 2 S3O2−6 + 8 NH3

More concentrated base yields sulfite:

S4N4 + 6 OH− + 3 H2O → S2O2−3 + 2 SO2−3 + 4 NH3

Metal complexes

S4N4 reacts with metal complexes. The cage remains intact in some cases but in other cases, it is degraded.[2][9] S4N4 reacts with Vaska's complex ([Ir(Cl)(CO)(PPh3)2] in an oxidative addition reaction to form a six coordinate iridium complex where the S4N4 binds through two sulfur atoms and one nitrogen atom.

S4N4 as a precursor to other S-N compounds

Many S-N compounds are prepared from S4N4.[10] Reaction with piperidine generates [S4N5]−:

24 S4N4 + 32 C5H10NH → 8 [C5H10NH2]+[S4N5]− + 8 (C5H10N)2S + 3 S8 + 8 N2

A related cation is also known, i.e. [S4N5]+.

Treatment with tetramethylammonium azide produces the heterocycle [S3N3]−:

8 S4N4 + 8 [(CH3)4N]+[N3]− → 8 [(CH3)4N]+[S3N3]− + S8 + 16 N2

Cyclo-[S3N3]− has 10 pi-electrons.

In a related reaction, the use of the bis(triphenylphosphine)iminium azide gives a salt containing the blue [NS4]− anion:[10]

4 S4N4 + 2 [PPN]+[N3]− → 2 [PPN]+[NS4]− + S8 + 10 N2

The anion [NS4]− has a chain structure described using the resonance [S=S=N−S−S−] ↔ [−S−S−N=S=S].

S4N4 reacts with electron-poor alkynes.[11]

Chlorination of S4N4 gives thiazyl chloride.

Passing gaseous S4N4 over silver metal yields the low temperature superconductor polythiazyl or polysulfurnitride (transition temperature (0.26±0.03) K[12]), often simply called "(SN)x". In the conversion, the silver first becomes sulfided, and the resulting Ag2S catalyzes the conversion of the S4N4 into the four-membered ring S2N2, which readily polymerizes.[1]

S4N4 + 8 Ag → 4 Ag2S + 2 N2
x S4N4 → (SN)4x

Safety

S4N4 is shock-sensitive. Purer samples are more shock-sensitive than those contaminated with elemental sulfur.[7]

References

  1. 1 2 3 4 5 6 7 8 9 Greenwood, N. N.; Earnshaw, A. (1997). Chemical Elements (2nd ed.). Boston, MA: Butterworth-Heinemann. pp. 721–725.
  2. 1 2 Chivers, T. (2004). A Guide To Chalcogen-Nitrogen Chemistry. Singapore: World Scientific Publishing. ISBN 981-256-095-5.
  3. ↑ Sharma, B. D.; Donohue, J. (1963). "The Crystal and Molecular Structure of Sulfur Nitride, S4N4". Acta Crystallographica. 16 (9): 891–897. doi:10.1107/S0365110X63002401.
  4. ↑ Rzepa, H. S.; Woollins, J. D. (1990). "A PM3 SCF-MO Study of the Structure and Bonding in the Cage Systems S4N4 and S4N4X (X = N+, N−, S, N2S, P+, C, Si, B− and Al−)". Polyhedron. 9 (1): 107–111. doi:10.1016/S0277-5387(00)84253-9.
  5. ↑ Konarev, D. V.; Lyubovskaya, R. N.; Drichko, N. V.; et al. (2000). "Donor-Acceptor Complexes of Fullerene C60 with Organic and Organometallic Donors". Journal of Materials Chemistry. 10 (4): 803–818. doi:10.1039/a907106g.
  6. ↑ Jolly, W. L.; Lipp, S. A. (1971). "Reaction of Tetrasulfur Tetranitride with Sulfuric Acid". Inorganic Chemistry. 10 (1): 33–38. doi:10.1021/ic50095a008.
  7. 1 2 Villena-Blanco, M.; Jolly, W. L.; et al. (1967). S. Y. Tyree Jr (ed.). "Tetrasulfur Tetranitride, S
    4    N
    4    ". Inorganic Syntheses. 9: 98–102. doi:10.1002/9780470132401.ch26.
  8. ↑ Maaninen, A.; Shvari, J.; Laitinen, R. S.; Chivers, T (2002). Coucouvanis, Dimitri (ed.). "Compounds of General Interest". Inorganic Syntheses. 33: 196–199. doi:10.1002/0471224502.ch4. ISBN 9780471208259.
  9. ↑ Kelly, P. F.; Slawin, A. M. Z.; Williams, D. J.; Woollins, J. D. (1992). "Caged explosives: Metal-Stabilized Chalcogen Nitrides". Chemical Society Reviews. 21 (4): 245–252. doi:10.1039/CS9922100245.
  10. 1 2 Bojes, J.; Chivers, T.; Oakley, R. D.; et al. (1989). Allcock, H. R. (ed.). "Binary Cyclic Nitrogen-Sulfur Anions". Inorganic Syntheses. 25: 30–35. doi:10.1002/9780470132562.ch7. ISBN 9780470132562.
  11. ↑ Dunn, P. J.; Rzepa, H. S. (1987). "The Reaction Between Tetrasulphur Tetranitride (S4N4) and Electron-deficient Alkynes. A Molecular Orbital Study". Journal of the Chemical Society, Perkin Transactions 2. 1987 (11): 1669–1670. doi:10.1039/p29870001669.
  12. ↑ Greene, R. L.; Street, G. B.; Suter, L. J. (1975). "Superconductivity in Polysulfur Nitride (SN)x". Physical Review Letters. 34 (10): 577–579. Bibcode:1975PhRvL..34..577G. doi:10.1103/PhysRevLett.34.577.
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