Transition Metals
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Transition Metals
d- block elements that can form at least one stable ion with a incomplete d sub-level
Sc3+ and Zn2+
Do not form ions with partially filled d- shells
Complex
Central metal or ion surrounded by co-ordinately bonded ligands
Ligand
Molecule or ion that forms a co-ordinate bond with a transition metal by donating a pair of e-
Co-ordination number
Number of Co-ordinate bonds formed with the central atom or ion
Shape of Complex with 6 Co-ordinate bonds
Octahedral 90° bond angle e.g. [Fe(H2O)6]2+ [Co(NH3)6]3+ [Cu(NH3)4(H2O)2]2+
Shape of Complex with 4 Co-ordinate bonds
Tetrahedral 109.5° bond angle e.g. [CuCl4]2- yellow [CoCl4]2- blue Square Planar e.g. Cisplatin 90° bond angle
Shape of Complex with 2 Co-ordinate bonds
Linear 180° bond angle [Ag(NH3)2]+
What does the overall charge on the complex ions represent?
Total Oxidation state
Oxidation state of the Metal Ion only
Total oxidation state - Sum of Oxidation states of ligands
Oxidation state of H2O ligand
0
NH3 and H2O ligands
NH3 and H2O are similar in size and uncharged
Monodentate Ligands
Ligands that can only form one co-ordinate bond, (only donate one pair of electrons to the complex ion)
Bidentate ligands
Ligands that can form two co-ordinate bonds, ( donate two pairs of electrons)