Editing Antimony (section)

===Halides===
Antimony forms two series of [[halide]]s: {{chem2|SbX3}} and {{chem2|SbX5}}. The trihalides {{chem2|SbF3|link=antimony trifluoride}}, {{chem2|SbCl3|link=antimony trichloride}}, {{chem2|SbBr3|link=antimony tribromide}}, and {{chem2|SbI3|link=antimony triiodide}} are all molecular compounds having [[trigonal pyramidal molecular geometry]]. The trifluoride is prepared by the reaction of [[antimony trioxide]] with [[hydrofluoric acid]]:<ref>[[#Wiberg|Wiberg and Holleman]], pp. 761–762</ref>
:{{chem2|Sb2O3 + 6 HF -> 2 SbF3 + 3 H2O}}
It is [[Lewis acid]]ic and readily accepts fluoride ions to form the complex anions {{chem2|SbF4-}} and {{chem2|SbF5(2-)}}. Molten antimony trifluoride is a weak [[electrical conductor]]. The trichloride is prepared by dissolving [[stibnite]] in [[hydrochloric acid]]:<ref name="Ullmann" />
:{{chem2|Sb2S3 + 6 HCl -> 2 SbCl3 + 3 H2S}}
Arsenic sulfides are not readily attacked by the hydrochloric acid, so this method offers a route to As-free Sb.

[[File:Antimony-pentafluoride-monomer-3D-balls.png|thumb|upright|left|Structure of gaseous {{chem2|SbF5}}]]
The pentahalides {{chem2|SbF5|link=antimony pentafluoride}} and {{chem2|SbCl5|link=antimony pentachloride}} have [[trigonal bipyramidal molecular geometry]] in the gas phase, but in the liquid phase, {{chem2|SbF5}} is [[polymer]]ic, whereas {{chem2|SbCl5}} is monomeric.<ref>[[#Wiberg|Wiberg and Holleman]], p. 761</ref> Antimony pentafluoride is a powerful Lewis acid used to make the [[superacid]] [[fluoroantimonic acid]] ({{chem2|H2F+*SbF6-}}).

[[Oxohalide|Oxyhalides]] are more common for antimony than for arsenic and phosphorus. [[Antimony trioxide]] dissolves in concentrated acid to form oxoantimonyl compounds such as [[antimony oxychloride|SbOCl]] and {{chem2|(SbO)2SO4}}.<ref>[[#Wiberg|Wiberg and Holleman]], p. 764</ref>