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Chapter 23: Problem 35

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) hexaamminechromium(III) nitrate (b) tetraamminecarbonatocobalt(III) sulfate (c) dichlorobis(ethylenediamine) platinum(IV) bromide (d) potassium diaquatetrabromovanadate(III) (e) bis(ethylenediamine) zinc(II) tetraiodomercurate(II)

Short Answer

Expert verified
\[[\text{Cr}(\text{NH}_3)_6] (\text{NO}_3)_3\], \[[\text{Co}(\text{NH}_3)_4 (\text{CO}_3)] (\text{SO}_4)_2\], \[[\text{Pt}(\text{en})_2 \text{Cl}_2] (\text{Br})_4\], \[\text{K}[\text{V}(\text{H}_2\text{O})_2 \text{Br}_4]\], \[[\text{Zn}(\text{en})_2] [\text{HgI}_4]\]

Step by step solution

01

(a) hexaamminechromium(III) nitrate

The compound has a chromium(III) ion in the coordination sphere, bound to six ammine ligands. The nitrate ion is the counter ion. The overall charge on the coordination sphere is +3 since chromium has a charge of +3. Thus, the formula is: \[ [\text{Cr}(\text{NH}_3)_6] (\text{NO}_3)_3 \]
02

(b) tetraamminecarbonatocobalt(III) sulfate

The compound has a cobalt(III) ion in the coordination sphere, bound to four ammine ligands and one carbonate ligand. The sulfate ion is the counter ion. The overall charge on the coordination sphere is +3 since cobalt has a charge of +3. Thus, the formula is: \[ [\text{Co}(\text{NH}_3)_4 (\text{CO}_3)] (\text{SO}_4)_2 \]
03

(c) dichlorobis(ethylenediamine) platinum(IV) bromide

The compound has a platinum(IV) ion in the coordination sphere, bound to two ethylenediamine ligands and two chloride ligands. The bromide ion is the counter ion. The overall charge on the coordination sphere is +4 since platinum has a charge of +4. Thus, the formula is: \[ [\text{Pt}(\text{en})_2 \text{Cl}_2] (\text{Br})_4 \]
04

(d) potassium diaquatetrabromovanadate(III)

The compound has a vanadate(III) ion in the coordination sphere, bound to two aqua (water) ligands and four bromide ligands. The overall charge on the coordination sphere is -1 since vanadate has a charge of +3 and there are four bromide ligands with a charge of -1 each. The counter ion is the potassium ion. Thus, the formula is: \[ \text{K}[\text{V}(\text{H}_2\text{O})_2 \text{Br}_4] \]
05

(e) bis(ethylenediamine) zinc(II) tetraiodomercurate(II)

The compound has a zinc(II) ion in the coordination sphere, bound to two ethylenediamine ligands. The overall charge on the coordination sphere is +2 since zinc has a charge of +2. The counter ion is the tetraiodomercurate(II) ion, which has a -2 charge since mercury has a charge of +2 and there are four iodide ligands with a charge of -1 each. Thus, the formula is: \[ [\text{Zn}(\text{en})_2] [\text{HgI}_4] \]

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Most popular questions from this chapter

Write the names of the following compounds, using the standard nomenclature rules for coordination complexes: (a) \(\left[\mathrm{Rh}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (b) \(\mathrm{K}_{2}\left[\mathrm{TiCl}_{6}\right]\) (c) \(\mathrm{MoOCl}_{4}\) (d) \(\left[\mathrm{Pt}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\right] \mathrm{Br}_{2}\)

Sketch a plot of atomic radius versus number of valence \(d\) electrons for the period 5 transition metals, and explain the trend.

Two Fe(II) complexes are both low spin but have different ligands. A solution of one is green and a solution of the other is red. Which solution is likely to contain the complex that has the stronger-field ligand? [Section 23.6\(]\)

A certain complex of metal \(\mathrm{M}\) is formulated as \(\mathrm{MCl}_{3} \cdot 3 \mathrm{H}_{2} \mathrm{O}\). The coordination number of the complex is not known but is expected to be 4 or 6. (a) Would conductivity measurements provide information about the coordination number? (b) In using conductivity measurements to test which ligands are bound to the metal ion, what assumption is made about the rate at which ligands enter or leave the coordination sphere of the metal? (c) Suppose you experimentally determine that this complex exists in aqueous solution as a single species. Suggest a likely coordination number and the number and type of each ligand.

Explain why the \(d_{x y}, d_{x z}\), and \(d_{y z}\) orbitals lie lower in energy than the \(d_{z}^{2}\) and \(d_{x^{2}-y^{2}}\) orbitals in the presence of an octahedral arrangement of ligands about the central metal ion.
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