BROMINE, 



mine, but it is not decomposed by iodine. Its action with me- 

 tals is precisely similar to that of hydrochloric acid. Hydro- 

 bromic acid is not decomposed when heated with oxygen, and 

 water is not decomposed by bromine, so that the affinity of 

 bromine and oxygen for hydrogen may be inferred to be nearly 

 equal. This acid, or a soluble bromide, produces white preci- 

 pitates with the nitrates of silver, lead and suboxide of mercury, 

 which are very similar to the chlorides of these metals. The 

 other metallic bromides correspond in solubility with the chlo- 

 rides. The bromide of silver, like the chloride, is soluble in 

 ammonia. 



Bromic acid, Br O 5 . Bromine is dissolved by the strong 

 alkaline bases, and occasions a decomposition exactly similar 

 to that produced by chlorine, in which a bromide of the metal 

 and bromate of the metallic oxide are formed. The bromic 

 acid may be separated from bromate of barytes by sulphuric 

 acid, and its solution may be concentrated to a certain point, 

 like chloric acid, beyond which it undergoes decomposition. It 

 has not been isolated. The chief points of difference between 

 chloric and bromic acid are, that the latter alone is decomposed 

 by sulphurous and phosphorous acids, and by sulphuretted 

 hydrogen ; and while all the chlorates are soluble, it is said, that 

 the bromates of silver and suboxide of mercury are insoluble, 

 the former being a white and the latter a yellowish white preci- 

 pitate. Bromic acid is the only known oxide of bromine. 



Chloride of bromine, Br C1 5 . Chlorine gas is absorbed by 

 bromine, and a volatile fluid of a reddish yellow colour pro- 

 duced. This chloride appears to dissolve in water without 

 decomposition, but in an alkaline solution, it is converted into 

 chloride and bromate. 



Bromide of sulphur. Bromine combines when mixed with 

 flowers of sulphur, forming a fluid of an oily appearance and 

 reddish tint, much resembling chloride of sulphur in appear- 

 ance and properties. This bromide dissolves both sulphur and 

 bromine, and has not been obtained in a state of sufficient 

 purity for analysis. 



Bromides of phosphorus, P Br 3 and P Br 5 . If bromine and 

 phosphorus are brought into contact in a flask filled with car- 

 bonic acid gas, a violent action with ignition takes place, of 

 which the products are a volatile crystalline solid, and a yel- 

 lowish liquid. The former, when decomposed by water, affords 



