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Antimony tribromide has two crystalline forms, both having orthorhombic symmetries. When a warm carbon disulfide solution of SbBr 3 is rapidly cooled, it crystallizes into the needle-like α-SbBr 3, which then slowly converts to the more stable β form. [2] Antimony tribromide hydrolyzes in water to form hydrobromic acid and antimony trioxide:
The flame retarding effect of antimony trioxide is produced by the formation of halogenated antimony compounds, [76] which react with hydrogen atoms, and probably also with oxygen atoms and OH radicals, thus inhibiting fire. [77] Markets for these flame-retardants include children's clothing, toys, aircraft, and automobile seat covers.
Tribromide is the anion with the chemical formula Br 3 −, or salts containing it: . Tetrabutylammonium tribromide; Tetrabromophosphonium tribromide; Pyridinium perbromide; Sodium and potassium tribromides can be prepared by reacting NaBr or KBr with aqueous bromine.
Antimony has fewer tendencies to anionic behaviour than ordinary nonmetals. [293] Its solution chemistry is characterised by the formation of oxyanions. [294] Like arsenic, antimony generally forms compounds in which it has an oxidation state of +3 or +5. [349] The halides, and the oxides and their derivatives are illustrative examples. [296]
Also, Lewis-acidic antimony compounds have recently been investigated to extend the chemistry of boron because of the isolobal analogy between the vacant p orbital of borane and σ*(Sb–X) orbitals of stiborane, and the similar electronegativities of antimony (2.05) and boron (2.04).
Nitrogen tribromide reacts instantly with ammonia in dichloromethane solution at −87 °C to yield NBrH 2. [7] NBr 3 + 2 NH 3 → 3 NH 2 Br. It also reacts with iodine in dichloromethane solution at −87 °C to produce NBr 2 I, which is a red-brown solid that stable up to -20 °C. [7] NBr 3 + I 2 → NBr 2 I + IBr
Arsenic trioxide powder.. Compounds of arsenic resemble in some respects those of phosphorus which occupies the same group (column) of the periodic table.The most common oxidation states for arsenic are: −3 in the arsenides, which are alloy-like intermetallic compounds, +3 in the arsenites, and +5 in the arsenates and most organoarsenic compounds.
It is far less reactive than the other nitrogen trihalides nitrogen trichloride, nitrogen tribromide, and nitrogen triiodide, all of which are explosive. Alone among the nitrogen trihalides it has a negative enthalpy of formation. It is prepared in modern times both by direct reaction of ammonia and fluorine and by a variation of Ruff's method. [6]