Oxohalide


Molecular oxohalides are a group of chemical compounds in which both oxygen and halogen atoms are attached to another chemical element A in a single molecule. They have the general formula AOmXn, X = F, Cl, Br, I. The element A may be a main group element, a transition element or an actinide. The term oxohalide, or oxyhalide, may also refer to minerals and other crystalline substances with the same overall chemical formula, but having an ionic structure.

Synthesis

Oxohalides can be seen as compounds intermediate between oxides and halides. There are three general methods of synthesis:
In addition, various oxohalides can be made by halogen exchange reactions and this reaction can also lead to the formation of mixed oxohalides such as POFCl2 and CrO2FCl.

Properties

In relation to the oxide or halide, for a given oxidation state of an element A, if two halogen atoms replace one oxygen atom, or vice versa, the overall charge on the molecule is unchanged and the coordination number of the central atom decreases by one. For example, both phosphorus oxychloride, POCl3 and phosphorus pentachloride, PCl5 are neutral covalent compounds of phosphorus in the +5 oxidation state. If an oxygen atom is simply replaced by a halogen atom the charge increases by +1, but the coordination number is unchanged. This is illustrated by the reaction of a mixture of a chromate or dichromate salt and potassium chloride with concentrated sulfuric acid.
The chromyl chloride produced has no electrical charge and is a volatile covalent molecule that can be distilled out of the reaction mixture.
Oxohalides of elements in high oxidation states are strong oxidizing agents, with oxidizing power similar to the corresponding oxide or halide. Most oxohalides are easily hydrolyzed. For example, chromyl chloride is hydrolyzed to chromate in the reverse of the synthetic reaction, above. The driving force for this reaction is the formation of A-O bonds which are stronger than A-Cl bonds. This gives a favourable enthalpy contribution to the Gibbs free energy change for the reaction
Many oxohalides can act as Lewis acids. This is particularly so with oxohalides of coordination number 3 or 4 which, in accepting one or more electron pairs from a Lewis base, become 5- or 6- coordinate. Oxohalide anions such as 2− can be seen as acid-base complexes of the oxohalide with more halide ions acting as Lewis bases. Another example is VOCl2 which forms the trigonal bipyramidal complex VOCl22 with the base trimethylamine.
The vibrational spectra of many oxohalides have been assigned in detail. They give useful information on relative bond strengths. For example, in CrO2F2, the Cr–O stretching vibrations are at 1006 cm−1 and 1016 cm−1 and the Cr–F stretching vibrations are at 727 cm−1 and 789 cm−1. The difference is much too large to be due to the different masses of O and F atoms. Rather, it shows that the Cr–O bond is much stronger than the Cr–F bond. M–O bonds are generally considered to be double bonds and this is backed up by measurements of M–O bond lengths. It implies that the elements A and O are chemically bound together by a σ bond and a π bond.
Oxohalides of elements in high oxidation states are intensely coloured owing to ligand to metal charge transfer transitions.

Main group elements

Selenium and tellurium form similar compounds and also the oxo-bridged species F5AOAF5. They are non-linear with the A-O-A angle of 142.5, 142.4 and 145.5° for S, Se and Te, respectively. The tellurium anion −, known as teflate, is a large and rather stable anion, useful for forming stable salts with large cations.
A selection of known oxohalides of transition metals is shown below, and more detailed lists are available in the literature. X indicates various halides, most often F and Cl.
Oxidation stateoxohalides
3VOCl, VOBr, FeOCl
42−, Cl3TiOTiCl3, VOCl2, 2−
5VOX3,VO2X, −, 2−, MnOCl3, TcOCl3, VOF3, VOCl3, NbOCl3
6CrO2Cl2, −, ReOX4, ReO2F2, OsOF4, CrO2F2, MoOCl4 MoO2Cl2, WO2Cl2, WOCl4
7MnO3Cl, ReOF5, ReO2F3, ReO3Cl, OsOF5
8OsO2F4, OsO3F2

File:O bridged oxohalide.png|thumb|left|Structure of the 2− and 4− ions
File:Agteflate.png|thumb|2 molecule. Colours: black – C, green – F, red – O, brown – Te, grey – Ag. Hydrogen atoms are not shown in this picture.
High oxidation states of the metal are dictated by the fact that oxygen is a strong oxidizing agent, as is fluorine. Bromine and iodine are relatively weak oxidizing agents, so fewer oxobromides and oxoiodides are known. Structures for compounds with d0 configuration are predicted by VSEPR theory. Thus, CrO2Cl2 is tetrahedral, OsO3F2 is trigonal bipyramidal, XeOF4 is square pyramidal and OsOF5 is octahedral. The d1 complex ReOCl4 is square pyramidal.
The compounds 2− and 4− have two MX5 groups joined by a bridging oxygen atom. Each metal has an octahedral environment. The unusual linear M—O—M structure can be rationalized in terms of molecular orbital theory, indicating the presence of dπ — pπ bonding between the metal and oxygen atoms. Oxygen bridges are present in more complex configurations like M22 or 2.
In the actinide series, uranyl compounds such as UO2Cl2 and 2− are well known and contain the linear UO2 moiety. Similar species exist for neptunium and plutonium.

Minerals and ionic compounds

is a rare example of a mineral oxohalide. The crystal structure has a tetragonal symmetry and can be thought of as consisting of layers of Cl−, Bi3+ and O2− ions, in the order Cl-Bi-O-Bi-Cl-Cl-Bi-O-Bi-Cl. This layered, graphite-like structure results in a relatively low hardness of bismoclite and most other oxohalide minerals. Those other minerals include terlinguaite Hg2OCl, formed by the weathering of mercury-containing minerals. Mendipite, Pb3O2Cl2, formed from an original deposit of lead sulfide in a number of stages is another example of a secondary oxohalide mineral.
The elements iron, antimony, bismuth and lanthanum form oxochlorides of general formula MOCl. MOBr and MOI are also known for Sb and Bi. Many of their crystal structures have been determined.