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Chapter 15: Problem 6

What is the coordination number of the metal in the following complexes? (a) \(\left[\mathrm{Mn}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{OH})_{\mathrm{A}}\right]^{2+}\) (b) \(\left[\mathrm{CuCl}_{4}\right]^{3-}\) (c) \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{ox})_{2}\right]^{2-}\) (d) \(\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{+}\)

Short Answer

Expert verified
Question: Determine the coordination number of the metal in the following complexes: (a) [Mn(NH3)2(OH)A]²⁺ (b) [CuCl4]³⁻ (c) [Cr(H2O)2(ox)2]²⁻ (d) [Au(CN)2]⁺ Answer: (a) Coordination number of Mn: 2 + A (b) Coordination number of Cu: 4 (c) Coordination number of Cr: 6 (d) Coordination number of Au: 2

Step by step solution

01

(a) Coordination number of Mn in \(\left[\mathrm{Mn}\left(\mathrm{NH}_{3}\right)_{2}(\mathrm{OH})_{\mathrm{A}}\right]^{2+}\)

In the given complex, Mn is the central metal ion, with ligands NH3 and OH. There are 2 NH3 ligands (indicated by the subscript 2) and A OH ligands. Thus, the coordination number of Mn in this complex is 2 + A.
02

(b) Coordination number of Cu in \(\left[\mathrm{CuCl}_{4}\right]^{3-}\)

In the given complex, Cu is the central metal ion with 4 Cl ligands (indicated by the subscript 4). Therefore, the coordination number of Cu in this complex is 4.
03

(c) Coordination number of Cr in $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}(\mathrm{ox})_{2}\right]^{2-}$

In the given complex, Cr is the central metal ion with H2O and ox ligands. There are 2 H2O ligands (indicated by the subscript 2) and 2 ox ligands (indicated by the subscript 2). Note that ox ligand (oxalate ion, C2O4^2-) is a bidentate ligand, which means it can donate two electron pairs to the central metal ion. Thus, the coordination number of Cr in this complex is 2 (from H2O ligands) + 2 * 2 (from 2 ox ligands) = 6.
04

(d) Coordination number of Au in \(\left[\mathrm{Au}(\mathrm{CN})_{2}\right]^{+}\)

In the given complex, Au is the central metal ion with 2 CN ligands (indicated by the subscript 2). Therefore, the coordination number of Au in this complex is 2.

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Most popular questions from this chapter

Consider the complex ion \(\left[\mathrm{Co}(\mathrm{en})_{2}(\mathrm{SCN}) \mathrm{Cl}\right]^{+} .\) (a) Identify the ligands and their charges. (b) What is the oxidation number of cobalt? (c) What is the formula for the sulfide salt of this ion?

[ \(\left[\mathrm{Cr}(\mathrm{CN})_{6}\right]^{4-}\) is less paramagnetic than \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{2+}\). Explain.

Consider the complex ion \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{2}(\mathrm{OH})_{2}\right]^{2-}\). (a) Identify the ligands and their charges. (b) What is the oxidation number of nickel? (c) What is the formula for the sodium salt of this ion?

Consider three complexes of \(\mathrm{Ag}^{+}\) and their formation constants, \(K_{\mathrm{f}}\) $$\begin{array}{ll}\hline \text { Complex lon } & K_{\mathrm{f}} \\\\\hline \mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}+ & 1.6 \times 10^{7} \\ \mathrm{Ag}(\mathrm{CN})_{2}^{-} & 5.6 \times 10^{18} \\\\\mathrm{AgBr}_{2}^{-} & 1.3 \times 10^{7} \\ \hline\end{array}$$ Which statements are true? (a) \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}{ }^{+}\) is more stable than \(\mathrm{Ag}(\mathrm{CN})_{2}^{-}\). (b) Adding a strong acid \(\left(\mathrm{HNO}_{3}\right)\) to a solution that is \(0.010 \mathrm{M}\) in \(\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}^{+}\) will tend to dissociate the complex ion into \(\mathrm{Ag}^{+}\) and \(\mathrm{NH}_{4}^{+} .\) (c) Adding a strong acid \(\left(\mathrm{HNO}_{3}\right)\) to a solution that is \(0.010 \mathrm{M}\) in \(\mathrm{AgBr}_{2}^{-}\) will tend to dissociate the complex ion into \(\mathrm{Ag}^{+}\) and \(\mathrm{Br}^{-} .\) (d) To dissolve AgI, one can add either \(\mathrm{NaCN}\) or \(\mathrm{HCN}\) as a source of the cyanide-complexing ligand. Fewer moles of NaCN would be required. (e) Solution \(A\) is \(0.10 M\) in \(B r^{-}\) and contains the complex ion \(\mathrm{AgBr}_{2}^{-}\). Solution B is \(0.10 M\) in \(\mathrm{CN}^{-}\) and contains the complex ion \(\mathrm{Ag}(\mathrm{CN})_{2}-\). Solution B will have more particles of complex ion per particle of \(\mathrm{Ag}^{+}\) than solution \(\mathrm{A}\).

In the \(\mathrm{Ti}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}{ }^{3+}\) ion, the splitting between the \(\mathrm{d}\) levels, \(\Delta_{\mathrm{o}}\) is \(55 \mathrm{kcal} / \mathrm{mol}\). What is the color of this ion? Assume that the color results from a transition between upper and lower d levels.
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