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Postby JChen_2I » Wed Dec 04, 2019 9:35 pm

Could someone explain the placement of lone pairs necessary on ligands for the ligand to be polydentate?

Myka G 1l
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Re: Polydentate

Postby Myka G 1l » Thu Dec 05, 2019 11:03 am

For the ligand to be polydentate it needs to have more than one atom that is is highly electronegative and they need to be far enough apart that the molecule can bind in two places. For example cyanide CN- is only monodentate despite the negative charge on the carbon and lone pair on the nitrogen because the triple bond is short and cannot accommodate both the carbon and nitrogen binding to the central metal atom. However ethylenediamine is a much longer molecule and also has two areas of high electronegativity so it is able to bind at two spots on the central metal atom.

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Re: Polydentate

Postby KnarGeghamyan1B » Thu Dec 05, 2019 12:20 pm

Elaborating on what the previous comment said, CN can’t take on 2 ligands because of the electron repulsion between the ligands if the bonds are too close to each other.

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