S₄N₄ is stable to air. It is, however, unstable in the thermodynamic sense with a positive enthalpy of formation of +460 kJ mol⁻¹. This endothermic enthalpy of formation anticipates its inherent instability, and originates in the difference in energy of S₄N₄ compared to its highly stable decomposition products:

S₄N₄ → 2 N₂ + ½ S₈

 Although many complex molecules are unstable in a thermodynamic sense yet stable kinetically, this is uncommon for very simple compositions, such as sulfur nitride.
 Because one of its decomposition products is a gas, S₄N₄ is an explosive. 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.
IUPAC Name: 2$l^{4},4,6$l^{4},8-Tetrathia-1,3,5,7-tetrazacycloocta-1,2,5,6-tetraene
The MF of Tetranitrogen tetrasulfide (CAS NO.28950-34-7) is N₄S₄.

                                 
The MW of Tetranitrogen tetrasulfide (CAS NO.28950-34-7) is 184.29.
Synonyms of Tetranitrogen tetrasulfide (CAS NO.28950-34-7): Tetranitrogen tetrasulfide ; Tetrasulfur tetranitride
Solubility in other solvents: CS₂, benzene
Solubility in water: Insoluble
Appearance Orange solid  
Index of Refraction: 1.123 
Density: 2.28 g/ml 
Melting Point: 187 °C

 Many important S-N compounds are prepared from S₄N₄.

 S₄N₄ was first prepared in 1835 by W. Gregory, by the reaction of sulfur monochloride with ammonia.Until recently, S₄N₄ was prepared by the reaction of ammonia with SCl₂ in carbon tetrachloride followed by extraction into dioxane, producing sulfur and ammonium chloride as side-products:

24 SCl₂ + 64 NH₃ → 4 S₄N₄ + S₈ + 48 NH₄Cl

A related synthesis employs sulfur monochloride and NH₄Cl instead:
         4 NH₄Cl + 6 S₂Cl₂ → S₄N₄ + 16 HCl + S₈

 S₄N₄ is shock-sensitive, thus grinding solid samples should be avoided. Purer samples are reportedly more sensitive than those contaminated with elemental sulfur.

 It 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.
 Nitrogen and sulfur have similar electronegativities. When atoms are so evenly matched, they often form extensive families of covalently bonded structures. Indeed, a large number of S-N and S-NH compounds are known with S₄N₄ as their parent.
 S₄N₄ adopts an unusual “extreme cradle” structure, with D_2d point group symmetry. It can be viewed as a derivative of a hypothetical 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. 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 but has been explained in the context of molecular orbital theory. 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 almost the same.