Structure & Reactivity
TM4. Chelation in Transition Metal Complexes
Each ligand that binds to a transition metal donates a pair of its electrons to the metal, sharing those electrons in a metal-ligand bond. Counting the total number of electrons in the metal's valence shell is fairly easy when you know that each ligand contributes two electrons.
But what if a ligand could contribute more than two electrons? Take a look at the following table. Each of the ligands shown here can bind to a metal twice. The ligand forms two bonds to the metal, donating two pairs of electrons. It might seem obvious, but forming two bonds to the metal means the ligand binds more tightly to the metal. Remember the lego-like nature of transition metal complexes: ligands can come and go, but these ligands are less likely to go; they hold on.
These ligands are called bidentate ligands. That means, literally, that they have two teeth. That doesn't sound like much, but the ligands we have seen previously are described as monodentate; they have only one tooth. Bidentate ligands can bite into the metal, and hold onto it, more strongly than monodentate ones.
Another term used for these kinds of ligands is derived from the Greek chele, for claw. These ligands grab onto the metal like the claw of a lobster or crab; they chelate. The "chelate effect" is the tendency of these ligands to bind firmly to a metal, whereas monodentate ligands might come off more easily.
Determine the charges (or oxidation states) on the metals in the following complexes:
a) K[Cr(ox)2(OH2)2] b) K[Mn(acac)3] c) [Cr(en)2Cl2]PF6 d) [Co(en)2(OH)Cl]ClO4
e) Na3[Mn(ox)3] f) K3[Cr(ox)3] g) Na[Au(bpy)(CN)2]
Determine the electron count on the metal in each of the complexes from the previous problem.
See a more in-depth discussion of coordination complexes in a later course.
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