Editing Halide (section)

==Reactions==
===Redox===
Halides cannot be reduced under the usual laboratory conditions, but they all can be oxidized to the parent halogens, which are [[diatomic]].  Especially for iodide and less so for the lighter halides, intermediates can be observed and isolated.  Best characterized is [[triiodide]].  Many related species are known, including a host of [[polyiodide]]s.

===Protonation===
Halides are conjugate bases of [[hydrogen halide]]s, which are all gases.  When the protonation is conducted in aqueous solution, [[hydrohalic acid]]s are produced.

===Reaction with silver ions===
Halide salts such as [[Potassium chloride|{{chem2|KCl}}]], [[Potassium bromide|{{chem2|KBr}}]] and [[Potassium iodide|{{chem2|KI}}]] are highly soluble in water to give colorless solutions. The solutions react readily with a solution of [[silver nitrate]] {{chem2|AgNO3}}. These three halides form solid [[precipitate]]s:<ref>{{Greenwood&Earnshaw2nd| page = 1184}}</ref>
* [[Silver chloride|{{chem2|AgCl}}]]: white
* [[Silver bromide|{{chem2|AgBr}}]]: pale yellow
* [[Silver iodide|{{chem2|AgI}}]]: yellow
Similar but slower reactions occur with [[alkyl halide]]s in place of alkali metal halides, as described in the [[Beilstein test]].