# Disulfur diiodide

Disulfur diiodide is an unstable inorganic chemical compound with the chemical formula S$_2$I$_2$. It is a red-brown solid that decomposes above −30 °C to elemental sulfur and iodine.

## Production
### Reaction of sulfur and iodine

The first attempt and claim to produce a sulfur iodide were made in 1813 by Bernard Courtois when exploring the properties of his newly discovered element, iodine. He reacted to sulfur and iodine, claiming they had made a compound. However, this production was doubted by Gay-Lussac. Between 1827 and 1896, more attempts were made to make sulfur iodide by combining the elements; however, all were inconclusive on the existence of the compound or failed. Later, when thermal analysis was developed, it was shown that when the elements were combined, it only resulted in a mixture, not a compound.

### Production by double replacement

When attempts to produce sulfur iodide by the direct combination of the elements failed to overcome the low thermodynamic stability of the compound, production by double replacement was attempted between 1833 and 1886. Some reactions that were attempted was the reaction of disulfur dichloride and hydroiodic acid:
    S$_2$Cl$_2$ + 2 HI → S$_2$I$_2$ + 2 HCl
The reaction of hydrogen sulfide and iodine trichloride:
    3 H$_2$S + 2 ICl$_3$ → S$_3$I$_2$ + 6 HCl
The reaction of hydroiodic acid and sulfur:
    2 HI + 3 S → H$_2$S + S$_2$I$_2$
The reaction of disulfur dichloride and potassium iodide:
    S$_2$Cl$_2$ + 2 KI → S$_2$I$_2$ + 2 KCl
and more, all assumed to have failed to produce sulfur iodide. However, the reaction between S$_2$Cl$_2$ and HI attempted in 1835 was later proven to have produced disulfur diiodide.
In 1940, another production was attempted with the fourth reaction and was reported to have detected various sulfur iodides, such as disulfur diiodide and sulfur diiodide (SI$_2$). When observing the reaction of very dilute disulfur dichloride in carbon tetrachloride and potassium iodide:
    S$_2$Cl$_2$ + 2 KI → 2 S + I$_2$ + 2 KCl
they observed a color change from yellow to reddish-brown to finally violet, which was assumed to be evidence for the formation of sulfur iodides. The compound was found to decompose at room temperature slowly in a solution, with the decomposition rate increasing with increasing temperature.

### Isolation

Disulfur diiodide was first isolated by the reaction of disulfur dichloride and potassium iodide, sodium iodide, or hydrogen iodide in pentane at −90 °C, and verified by infrared spectroscopy.

## Properties

Disulfur diiodide is light-sensitive and is soluble in various haloalkanes, such as carbon tetrachloride.

## Other sulfur iodides

Sulfur diiodide (SI$_2$) has finally been reported in an argon matrix at 9 K by the reaction of sulfur dichloride and iodine; however, this has been disputed.
Sulfur and iodine react in antimony pentafluoride or arsenic pentafluoride to form the S$_7$I$^+$ ion, which is stable at room temperature, unlike other sulfur-iodine compounds.
The empirical formula of disulfur diiodide is SI. It is therefore sometimes called sulfur monoiodide, but S$_2$I$_2$ is a covalently bound molecule and is not the same as a SI molecule or an ionic salt having 1:1 stoichiometry. The true sulfur monoiodide molecule is a radical.