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Chapter 24: Problem 7

Draw a plausible structure to represent: (a) \(\left[\mathrm{PtCl}_{4}\right]^{2-}\) (b) \(\operatorname{fac}-\left[\operatorname{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{2+}\) (c) \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}\right]^{2+}\)

Short Answer

Expert verified
The structures of the compounds are as follows: (a) \(\left[\mathrm{PtCl}_{4}\right]^{2-}\) is a square planar molecule with Pt at the center and four Cl atoms at the corners. (b) \(\operatorname{fac}-\left[\operatorname{Co}\left(\mathrm{H}_{2}\mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{2+}\) is an octahedral structure with Co at the center, the H2O ligands and the NH3 ligands arranged separately in two sets of adjacent corners. (c) \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2}\mathrm{O}\right)_{5}\right]^{2+}\) is also an octahedral structure with Cr at the center, surrounded by five H2O molecules and one Cl atom.

Step by step solution

01

Structure of \(\left[\mathrm{PtCl}_{4}\right]^{2-}\)

First, identify the coordination number of Pt in \(\left[\mathrm{PtCl}_{4}\right]^{2-}\). Here, 4 Cl atoms are bonded to Pt, which gives a coordination number of 4. This indicates that \(\left[\mathrm{PtCl}_{4}\right]^{2-}\) has a square planar geometry where Pt is at the center and is surrounded by four Cl atoms at the corners of the square.
02

Structure of \(\operatorname{fac}-\left[\operatorname{Co}\left(\mathrm{H}_{2}\mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{2+}\)

Next, examine the structure of \(\operatorname{fac}-\left[\operatorname{Co}\left(\mathrm{H}_{2}\mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{2+}\). With a total of six ligands - three H2O molecules and three NH3 molecules - bonded to the central metal ion Co, this complex has a coordination number of 6. The \(\operatorname{fac}\) prefix indicates that the same types of ligands are mutually adjacent, forming an octahedral geometry. Position Co at the center of the structure. Then, arrange the H2O ligands and NH3 ligands in two sets of adjacent corners of the octahedron.
03

Structure of \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2}\mathrm{O}\right)_{5}\right]^{2+}\)

Finally, look at the structure of \(\left[\mathrm{CrCl}\left(\mathrm{H}_{2}\mathrm{O}\right)_{5}\right]^{2+}\). Again, there is a coordination number of 6, indicating an octahedral geometry. In this case, with five water molecules and one Cl atom as the ligands bonded to the central metal ion Cr, position Cr in the center and surround it with the H2O molecules on five corners of the octahedron and the Cl atom on one corner.

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Most popular questions from this chapter

In Example \(24-5,\) we chose between a tetrahedral and a square-planar structure for \(\left[\mathrm{Ni}(\mathrm{CN})_{4}\right]^{2-}\) based on magnetic properties. Could we similarly use magnetic properties to establish whether the ammine complex of \(\mathrm{Ni}(\mathrm{II})\) is octahedral \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) or tetrahedral \(\left[\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}\right]^{2+} ?\) Explain.

How many different structures are possible for each of the following complex ions? (a) \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)\left(\mathrm{NH}_{3}\right)_{5}\right]^{3+}\) (b) \(\left[\operatorname{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{3+}\) (c) \(\left[\operatorname{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{3}\left(\mathrm{NH}_{3}\right)_{3}\right]^{3+}\) (d) \(\left[\operatorname{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{NH}_{3}\right)_{2}\right]^{3+}\)

Explain why aqueous solutions of \(\left[\operatorname{Sc}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}\) and \(\left.\mathrm{Zn}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right] \mathrm{Cl}_{2}\) are colorless, but an aqueous solution of \(\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Cl}_{3}\) is not.

Estimate the total \(\left[\mathrm{Cl}^{-}\right]\) required in a solution that is initially \(0.10 \mathrm{M} \mathrm{CuSO}_{4}\) to produce a visible yellow color. \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]^{2+}+4 \mathrm{Cl}^{-} \rightleftharpoons\left[\mathrm{CuCl}_{4}\right]^{2-}+4 \mathrm{H}_{2} \mathrm{O}\) \(K_{f}=4.2 \times 10^{5}\) Assume that \(99 \%\) conversion of \(\left[\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\right]^{2+}\) to \(\left[\mathrm{CuCl}_{4}\right]^{2-}\) is sufficient for this to happen, and ignore the presence of any mixed aqua- chloro complex ions.

Write simple chemical equations to show how the complex ion \(\left[\mathrm{CrOH}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5}\right]^{2+}\) acts as \((\mathrm{a})\) an acid; (b) a base.
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