Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the \(+3\) rather than in the \(+2\) oxidation state (for metals that form stable \(+3\) ions in the first place). Suggest an explanation, keeping in mind the Lewis acid-base nature of the metal-ligand bond.

Short Answer

Expert verified
A possible explanation for the greater stability of coordination compounds for the metal in the +3 oxidation state rather than in the +2 oxidation state is that the increased charge of the metal ion leads to stronger metal-ligand bonds due to its stronger ability to accept electron pairs from the ligands. This stronger bond results in a higher overall stability for the coordination compound, considering the Lewis acid-base nature of the metal-ligand bond.

Step by step solution

01

Recall the Lewis acid-base concept

To better understand the question, we need to recall the Lewis acid-base concept. According to the Lewis theory, a Lewis acid is a substance that can accept an electron pair, and a Lewis base is a substance that can donate an electron pair. In a coordination compound, the metal ion acts as a Lewis acid by accepting electron pairs from the ligands, which are the Lewis bases.
02

Consider the charge of the metal ion

In our given scenario, we are comparing the stability of coordination compounds formed with a metal ion in the +2 oxidation state and another in the +3 oxidation state. In general, a higher charge on the metal ion indicates a stronger ability to attract electron pairs from the ligands.
03

Evaluate the strength of the metal-ligand bond

The strength of the metal-ligand bond is determined by the ability of the metal ion to accept electron pairs from the ligands and the ability of the ligands to donate electron pairs to the metal ion. A stronger bond between the metal ion and the ligand should result in higher stability for the coordination compound.
04

Compare the Lewis acid strength of +3 and +2 oxidation states

In coordination compounds, a metal ion with a higher charge, such as +3 oxidation state, will have a stronger ability to accept electron pairs compared to a metal ion in the +2 oxidation state. As a result, the metal-ligand bond should be stronger when the metal is in the +3 oxidation state, leading to greater stability for the coordination compound.
05

Conclusion

Keeping in mind the Lewis acid-base nature of the metal-ligand bond, a possible explanation for the greater stability of coordination compounds for the metal in the +3 oxidation state rather than in the +2 oxidation state is that the increased charge of the metal ion leads to stronger metal-ligand bonds. This stronger bond results in a higher overall stability for the coordination compound.

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Most popular questions from this chapter

Determine if each of the following metal complexes is chiral and therefore has an optical isomer: (a) square planar \(\left[\mathrm{Pd}(\mathrm{en})(\mathrm{CN})_{2}\right],(\mathbf{b})\) octahedral \(\left[\mathrm{Ni}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+},(\mathbf{c})\) octahe- dral \(\operatorname{cis}-\left[\mathrm{V}(\mathrm{en})_{2} \mathrm{ClBr}\right]\)

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(a) A compound with formula \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) is dissolved in water, forming a solution that is approximately the same color as the solid. Immediately after forming the solution, the addition of excess AgNO \(_{3}(a q)\) forms 2 mol of solid AgCl per mole of complex. Write the formula for the compound, showing which ligands are likely to be present in the coordination sphere. (b) After a solution of \(\mathrm{RuCl}_{3}\) \(\cdot 5 \mathrm{H}_{2} \mathrm{O}\) has stood for about a year, addition of \(\mathrm{AgNO}_{3}(a q)\) precipitates 3 mol of AgCl per mole of complex. What has happened in the ensuing time?

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