Inorganic Compound Reactions Flashcards
are 2+ ions or 3+ ions more acidic in solution and why
3+ ions are much more acidic
3+ ions are smaller and more highly charged, so have a higher charge density. they attract the electrons from the oxygen of the ligands much more strongly. this weakens the O-H bonds, so the complex readily releases a H+ ion into the solution, making it acidic
what kind of acid is the complex ion acting as? why?
[Fe(H2O)6]3+ <–> [Fe(H2O)5(OH)]2+ + H+
bronsted-lowry - donates a proton
define a Lewis acid
electron pair acceptor
define a Lewis base
electron pair donor
what is acting as the Lewis acid and what is acting as the Lewis base during the formation of complex ions
the metal ion is acting as the Lewis acid and the ligands as Lewis bases
complex ion and colour of Fe 2+ in aqueous solution
[Fe(H2O)^]2+ (aq)
green
complex ion and colour of Fe 2+ when adding NaOH (dropwise and excess)
[Fe(H2O)4(OH)2] (s)
green ppt, goes brown on standing in air
complex ion and colour of Fe 2+ when adding NH3 (dropwise and excess)
[Fe(H2O)4(OH)2] (s)
green ppt, goes brown on standing in air
complex ion and colour of Fe 2+ when adding Na2CO3
FeCO3
green ppt
why does the green ppt go brown on standing in air in the reaction of Fe 2+ with NH3
oxygen in the air oxidises Fe 2+ to Fe 3+, and [Fe(OH)3(H2O)3] is brown, so colour changes
complex ion and colour of Cu 2+ in aqueous solution
[Cu(H2O)6] 2+
blue
complex ion and colour of Cu 2+ when adding NaOH (dropwise and excess)
[Cu(H2O)4(OH)2] (s)
blue ppt
complex ion and colour of Cu 2+ when adding NH3 dropwise
[Cu(H2O)4(OH)2] (s)
blue ppt
complex ion and colour of Cu 2+ when adding NH3 excess
[Cu(H2O)2(NH3)4] 2+ (aq)
deep blue solution
complex ion and colour of Cu 2+ add Na2CO3
CuCO3
blue-green ppt