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Which stability order is correct?

  1. $\ce{[Ni(en)2]^2+} > \ce{[Ni(dmg)2]}$
  2. $\ce{[Fe(edta)]^2-} > \ce{[Fe(en)3]^3+}$

In the first case I think the stability depends upon the strength of the ligand so is $\ce{en}$ stronger than $\ce{dmg}$ to form a more stable compound? As the oxidation state of nickel is same for both the cases.

In the second case the oxidation state of iron is +2 and +3, respectively. But I am confused if the metal with higher oxidation state is more stable or the metal with lower oxidation state is more stable?

Does stability depends upon the number of chelating groups?

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  • $\begingroup$ In general, metal with higher oxidation state forms more stable complex. $\endgroup$ – Zenix Nov 18 '19 at 16:00
  • $\begingroup$ But that does not appear to be the case in the second example where +2 is more stable than +3 of fe $\endgroup$ – studious Nov 19 '19 at 1:47

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