<P> The halogens form many binary, diamagnetic interhalogen compounds with stoichiometries XY, XY, XY, and XY (where X is heavier than Y), and bromine is no exception . Bromine forms a monofluoride and monochloride, as well as a trifluoride and pentafluoride . Some cationic and anionic derivatives are also characterised, such as BrF − 2, BrCl − 2, BrF + 2, BrF + 4, and BrF + 6 . Apart from these, some pseudohalides are also known, such as cyanogen bromide (BrCN), bromine thiocyanate (BrSCN), and bromine azide (BrN). </P> <P> The pale - brown bromine monofluoride (BrF) is unstable at room temperature, disproportionating quickly and irreversibly into bromine, bromine trifluoride, and bromine pentafluoride . It thus cannot be obtained pure . It may be synthesised by the direct reaction of the elements, or by the comproportionation of bromine and bromine trifluoride at high temperatures . Bromine monochloride (BrCl), a red - brown gas, quite readily dissociates reversibly into bromine and chlorine at room temperature and thus also cannot be obtained pure, though it can be made by the reversible direct reaction of its elements in the gas phase or in carbon tetrachloride . Bromine monofluoride in ethanol readily leads to the monobromination of the aromatic compounds PhX (para-bromination occurs for X = Me, Bu, OMe, Br; meta - bromination occurs for the deactivating X =--CO Et,--CHO,--NO); this is due to heterolytic fission of the Br--F bond, leading to rapid electrophilic bromination by Br . </P> <P> At room temperature, bromine trifluoride (BrF) is a straw - coloured liquid . It may be formed by directly fluorinating bromine at room temperature and is purified through distillation . It reacts explosively with water and hydrocarbons, but is a less violent fluorinating reagent than chlorine trifluoride . It reacts vigorously with boron, carbon, silicon, arsenic, antimony, iodine, and sulfur to give fluorides, and also reacts with most metals and their oxides: as such, it is used to oxidise uranium to uranium hexafluoride in the nuclear industry . Refractory oxides tend to be only partially fluorinated, but here the derivatives KBrF and BrF SbF remain reactive . Bromine trifluoride is a useful nonaqueous ionising solvent, since it readily dissociates to form BrF + 2 and BrF − 4 and thus conducts electricity . </P> <P> Bromine pentafluoride (BrF) was first synthesised in 1930 . It is produced on a large scale by direct reaction of bromine with excess fluorine at temperatures higher than 150 ° C, and on a small scale by the fluorination of potassium bromide at 25 ° C. It is a very vigorous fluorinating agent, although chlorine trifluoride is still more violent . Bromine pentafluoride explodes on reaction with water and fluorinates silicates at 450 ° C . </P>

An element x forms two compounds with bromine