Editing Chalcogen (section)

===With halogens=== <!-- Chalcohalide redirects here -->
Chalcogens also form compounds with [[halogen]]s known as '''chalcohalides''', or '''chalcogen halides'''. The majority of simple chalcogen halides are well-known and widely used as chemical [[reagent]]s. However, more complicated chalcogen halides, such as sulfenyl, sulfonyl, and sulfuryl halides, are less well known to science. Out of the compounds consisting purely of chalcogens and halogens, there are a total of 13 chalcogen fluorides, nine chalcogen chlorides, eight chalcogen bromides, and six chalcogen iodides that are known.{{dubious|date=September 2014}} The heavier chalcogen halides often have significant molecular interactions. Sulfur fluorides with low valences are fairly unstable and little is known about their properties.{{dubious|date=September 2014}} However, sulfur fluorides with high valences, such as [[sulfur hexafluoride]], are stable and well-known. [[Sulfur tetrafluoride]] is also a well-known sulfur fluoride. Certain selenium fluorides, such as [[selenium difluoride]], have been produced in small amounts. The crystal structures of both [[selenium tetrafluoride]] and [[tellurium tetrafluoride]] are known. Chalcogen chlorides and bromides have also been explored. In particular, selenium dichloride and sulfur dichloride can react to form [[Organoselenium chemistry|organic selenium compounds]]. Dichalcogen dihalides, such as Se<sub>2</sub>Cl<sub>2</sub> also are known to exist. There are also mixed chalcogen-halogen compounds. These include SeSX, with X being chlorine or bromine.{{dubious|date=September 2014}} Such compounds can form in mixtures of [[sulfur dichloride]] and selenium halides. These compounds have been fairly recently structurally characterized, as of 2008. In general, diselenium and disulfur chlorides and bromides are useful chemical reagents. Chalcogen halides with attached metal atoms are soluble in organic solutions.{{dubious|date=September 2014}} One example of such a compound is {{chem2|[[Mo]]S2Cl3}}. Unlike selenium chlorides and bromides, selenium [[iodide]]s have not been isolated, as of 2008, although it is likely that they occur in solution. Diselenium diiodide, however, does occur in equilibrium with selenium atoms and iodine molecules. Some tellurium halides with low valences, such as {{chem2|Te2Cl2}} and {{chem2|Te2Br2}}, form [[polymer]]s when in the [[Solid-state chemistry|solid state]]. These tellurium halides can be synthesized by the reduction of pure tellurium with [[superhydride]] and reacting the resulting product with tellurium tetrahalides. Ditellurium dihalides tend to get less stable as the halides become lower in atomic number and atomic mass. Tellurium also forms iodides with even fewer iodine atoms than diiodides. These include TeI and Te<sub>2</sub>I. These compounds have extended structures in the solid state. Halogens and chalcogens can also form halochalcogenate [[anion]]s.<ref name="handbook"/>