title: Gallium(III) bromide
text: # Gallium(III) bromide
  
  Gallium(III) bromide $(GaBr_3)$ is a chemical compound, and one of four gallium trihalides.
  
  ## Introduction
  
  Gallium(III) bromide is, at room temperature and atmospheric pressure, a white, crystalline powder which reacts favorably and exothermically with water. Solid gallium tribromide is stable at room temperature and can be found primarily in its dimeric form. $GaBr_3$ can form an intermediate halide, $Ga_2Br_{7;}$ however, this is not as common as with $GaCl_3.$ It is a member of the gallium trihalide group and is similar to $GaCl_3,$ and $GaI_3,$ but not $GaF_3,$ in its preparation and uses. $GaBr_3$ is a milder Lewis acid than $AlBr_3,$ and has more versatile chemistry due to the comparative ease of reducing gallium, but is more reactive than $GaCl_3.$
  
  $GaBr_3$ is similar spectroscopically to aluminum, indium, and thallium trihalides excluding trifluorides.
  
  ## Preparation
  
  One method of preparing $GaBr_3$ is to heat elemental gallium in the presence of bromine liquid under vacuum. Following the highly exothermic reaction, the mixture is allowed to rest and then subjected to various purifying steps. This method from the turn of the twentieth century remains a useful way of preparing $GaBr_{3.}$ Historically, gallium was obtained by electrolysis of its hydroxide in solution of potassium hydroxide, however today it is obtained as a byproduct of aluminium and zinc production.
  
  $GaBr_3$ can be synthesized by exposing gallium to bromine in an environment free of water, oxygen and grease. The result is a gas which must be crystallized in order to form bromide purchased by laboratories. Below is the equation:
  
      2 Ga(s) + 3 $Br_2(l)$ ⟶ 2 $GaBr_3(g)$
  
  ## Structure
  
  The $GaBr_3$ monomer has trigonal planar geometry, but when it forms the dimer $Ga_2Br_6$ the geometry around the gallium center distorts to become roughly tetrahedral. As a solid, $GaBr_3$ forms a monoclinic crystalline structure with a unit cell volume of 524.16 $Å^3.$ Additional specifications for this unit cell are as follows: a = 8.87 Å, b = 5.64 Å, c =11.01 Å, α = 90˚, β = 107.81˚, γ = 90˚.
  
  ## Complexes
  
  Gallium is the lightest group 13 metal with a filled d-shell, and has an electronic configuration of ([Ar] $3d^{10}$ $4s^2$ $4p^1)$ below the valence electrons that could take part in d-π bonding with ligands. The somewhat high oxidation state of Ga in $Ga(III)Br_3,$ low electronegativity, and high polarizability allow $GaBr_3$ to behave as a "soft acid" in terms of the Hard-Soft-Acid-Base (HSAB) theory. The Lewis acidity of all the gallium trihalides, $GaBr_3$ included, has been extensively studied thermodynamically, and the basicity of $GaBr_3$ has been established with a number of donors.
  
  $GaBr_3$ is capable of accepting an additional $Br^−$ ion or unevenly splitting its dimer to form $[GaBr_4]^−,$ a tetrahedral ion of which crystalline salts can be obtained. This ionic complex is further capable of binding to . The $Br^−$ ion can be just as easily substituted with a neutral ligand. Typically these neutral ligands, with form $GaBr_3$ L and sometimes $GaBr_3L_2,$ will form a tetrahedral bipyramidal geometric structure with the Br in an equatorial position due to their large effective nuclear charge. Additionally, $GaBr_3$ can be used as a catalyst in certain oxidative addition reactions.
  
  ## Uses
  
  $GaBr_3$ is used as a catalyst in organic synthesis, with similar mechanism to $GaCl_{3.}$ However, due to its greater reactivity, it is sometimes disfavored because of the greater versatility of $GaCl_3.$ $GaBr_3$ as well as other gallium trihalides and group 13 metal trihalides can be used as catalysts in the oxidative addition of organic compounds. It has been verified that the $GaBr_3$ dimer cleaves unevenly into $[GaBr_4]^−$ and $[GaBr_2]^+.$ The entire mechanism is uncertain partly because intermediate states are not always stable enough for study, and partially because $GaBr_3$ is studied less frequently than $GaCl_3.$ Ga(III) itself is a useful Lewis acid for organic reactions because its full d-electron shell makes it able to accept variable numbers of ligands, but will readily give up ligands if conditions prove favorable.
  
  