text: Complexes of oxophilic metals typically are prone to hydrolysis. For example, the high valent chlorides hydrolyze rapidly to give oxides:
  :TiCl + 2 HO  →  TiO  +  4 HCl
  These reactions proceed via oxychloride intermediates.  For example, WOCl results from the partial hydrolysis of tungsten hexachloride. Hydroxide-containing intermediates are rarely observed for oxophilic metals. In contrast, the anhydrous halides of the later metals tend to hydrate, not hydrolyze, and they often form hydroxides.
  Reduced complexes of oxophilic metals tend to generate oxides by reaction with oxygen. Typically the oxide-ligand is bridging, e.g.
  :2 (CH)TiCl  +  1/2 O   →   {(CH)TiCl}O
  Only in rare cases do the products of oxygenation feature terminal oxo ligands.