Tetrasulfur tetranitride is an inorganic compound with the formula . This vivid orange, opaque, crystalline explosive 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 as their parent.
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 Waals radii[4] but has been explained in the context of molecular orbital theory. 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 is considered to be delocalized, which is indicated by the fact that the bond distances between neighboring sulfur and nitrogen atoms are nearly identical. has been shown to co-crystallize with benzene and the molecule.[5]
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 compared to its highly stable decomposition products:
is shock and friction sensitive and because one of its decomposition products is a gas, it is considered a primary explosive.[6] Purer samples tend to be more sensitive. Small samples can be detonated by striking with a hammer. is thermochromic, changing from pale yellow below −30 °C to orange at room temperature to deep red above 100 °C.
was first prepared in 1835 by M. Gregory by the reaction of disulfur dichloride with ammonia,[7] a process that has been optimized:[8]
Coproducts of this reaction include heptasulfur imide and elemental sulfur, and the latter equilibrates with more and ammonium sulfide:[9]
A related synthesis employs instead:
An alternative synthesis entails the use of as a precursor with pre-formed S–N bonds. is prepared by the reaction of lithium bis(trimethylsilyl)amide and .
The reacts with the combination of and to form, trimethylsilyl chloride, and sulfur dioxide:[10]
is a Lewis base at nitrogen. It binds to strong Lewis acids, such as and , or :
The cage is distorted in these adducts.
reacts with metal complexes, but the bonding situation may be quite complex. The cage remains intact in some cases but in other cases, it is degraded.[2] [11] For example, the soft Lewis acid CuCl forms a coordination polymer:
Reportedly, initially forms a complex with at sulfur. This compound, upon standing, isomerizes to additionally bond through a nitrogen atom. oxidatively adds to Vaska's complex (to form a hexacoordinate iridium complex where the binds through two sulfur atoms and one nitrogen atom.[2]
Dilute NaOH hydrolyzes as follows, yielding thiosulfate and trithionate:
More concentrated base yields sulfite:
Many S-N compounds are prepared from .[12]
In electrophilic substitution or 1,3-dipolar cycloaddition reactions, S4N4 behaves as a combination of the dithionitronium synthon and the sulfide synthon. Thus it adds to arenes and electron-rich alkynes to give 1,2,5thiadiazoles.[13] Electron-poor alkynes attack to give a different cycloadduct of stoichiometry RC(NS)2SC.[14] [13] With electron-rich alkenes, S4N4 behaves as a Diels-Alder diene.[13]
Passing gaseous over silver metal yields the low temperature superconductor polythiazyl or polysulfurnitride (transition temperature (0.26±0.03) K[15]), often simply called "(SN)x". In the conversion, the silver first becomes sulfided, and the resulting catalyzes the conversion of the into the four-membered ring, which readily polymerizes.
Oxidation of with elemental chlorine gives thiazyl chloride, but milder reagents give S4N:
3 S4N4 + 2 S2Cl2 → 4 [S<sub>4</sub>N<sub>3</sub>]+Cl-
S4N4 + RC(=O)Cl → [S<sub>4</sub>N<sub>3</sub>]+Cl- + RNCOThat cation is relatively non-electrophilic and planar, with a delocalized π system. However, it adds triphenylphosphine to give [S(NPPh<sub>3</sub>)<sub>3</sub>]3+[Cl<sup>−</sup>]3, a triimide analogue to sulfur trioxide. Conversely, S4N salts react with aluminum azide to recover S4N4.[13]
Treatment with tetramethylammonium azide produces the similar 10-π heterocycle :
In a related reaction, the use of the bis(triphenylphosphine)iminium azide gives a salt containing the blue anion:
has a chain structure approximated by the resonance .
Reaction with piperidine generates :
A related cation is also known, i.e. .
Triphenylphosphine abstracts a sulfur atom, replacing it with another triphenylphosphine moiety:[13]
S4N4 + 2 PPh3 → S3(PPh3)N4 + SPPh3
is a categorized as a primary explosive that is shock and friction sensitive. While comparable to pentaerythritol tetranitrate (PETN) in terms of impact sensitivity, its friction sensitivity is equal to or even lower than lead azide.[16] Purer samples are more shock-sensitive than those contaminated with elemental sulfur.[8]