Editing Interhalogen (section)

==Properties==
Typically, interhalogen bonds are more reactive than diatomic halogen bonds, because interhalogen bonds are weaker than diatomic halogen bonds, except for F<sub>2</sub>. If interhalogens are exposed to water, they convert to [[halide]] and [[oxyhalide]] ions. With BrF<sub>5</sub>, this reaction can be [[explosion|explosive]]. If interhalogens are exposed to [[silicon dioxide]], or [[metal]] oxides, then silicon or metal respectively bond with one of the types of halogen, leaving free diatomic halogens and diatomic oxygen. Most interhalogens are halogen fluorides, and all but three (IBr, AtBr, and AtI) of the remainder are halogen chlorides. Chlorine and bromine can each bond to five fluorine atoms, and iodine can bond to seven. AX and AX<sub>3</sub> interhalogens can form between two halogens whose [[electronegativity|electronegativities]] are relatively close to one another. When interhalogens are exposed to metals, they react to form metal halides of the constituent halogens. The oxidation power of an interhalogen increases with the number of halogens attached to the central atom of the interhalogen, as well as with the decreasing size of the central atom of the compound. Interhalogens containing fluorine are more likely to be [[volatility (chemistry)|volatile]] than interhalogens containing heavier halogens.<ref name = "Chemistry of Interhalogens"/>

Interhalogens with one or three halogens bonded to a central atom are formed by two elements whose electronegativities are not far apart. Interhalogens with five or seven halogens bonded to a central atom are formed by two elements whose sizes are very different. The number of smaller halogens that can bond to a large central halogen is guided by the ratio of the [[atomic radius]] of the larger halogen over the atomic radius of the smaller halogen. A number of interhalogens, such as IF<sub>7</sub>, react with all metals except for those in the [[platinum group]]. IF<sub>7</sub>, unlike interhalogens in the XY<sub>5</sub> series, does not react with the fluorides of the [[alkali metals]].<ref name = "Chemistry of Interhalogens"/>

ClF<sub>3</sub> is the most reactive of the XY<sub>3</sub> interhalogens. ICl<sub>3</sub> is the least reactive. BrF<sub>3</sub> has the highest thermal stability of the interhalogens with four atoms. ICl<sub>3</sub> has the lowest. Chlorine trifluoride has a boiling point of −12&nbsp;°C. Bromine trifluoride has a boiling point of 127&nbsp;°C and is a liquid at [[room temperature]]. Iodine trichloride melts at 101&nbsp;°C.<ref name = "Chemistry of Interhalogens"/>

Most interhalogens are [[covalent]] gases. Some interhalogens, especially those containing bromine, are [[liquid]]s, and most iodine-containing interhalogens are solids. Most of the interhalogens composed of lighter halogens are fairly colorless, but the interhalogens containing heavier halogens are deeper in color due to their higher [[molecular weight]]. In this respect, the interhalogens are similar to the halogens. The greater the difference between the electronegativities of the two halogens in an interhalogen, the higher the boiling point of the interhalogen. All interhalogens are [[diamagnetic]]. The [[bond length]] of interhalogens in the XY series increases with the size of the constituent halogens. For instance, ClF has a bond length of 1.628&nbsp;[[angstrom|Å]], and IBr has a bond length of 2.47&nbsp;Å.<ref name = "Chemistry of Interhalogens"/>