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Chapter 23: Problem 25

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{Na}_{2}[\mathrm{Co}(\mathrm{EDTA})]\) (b) \(\mathrm{KMnO}_{4}\) (c) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}\) (d) \(\mathrm{K}_{3} \mathrm{Fe}(\mathrm{CN})_{6}\) (e) \(\mathrm{Rh}\left(\mathrm{PPh}_{3}\right)_{3} \mathrm{Cl}\) (f) $\mathrm{Zn}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}$

Short Answer

Expert verified
(a) Coordination number: 6, Oxidation number: +2 (b) Coordination number: 4, Oxidation number: +7 (c) Coordination number: 4, Oxidation number: +2 (d) Coordination number: 6, Oxidation number: +3 (e) Coordination number: 4, Oxidation number: +1 (f) Coordination number: 3, Oxidation number: +2

Step by step solution

01

a) \(\mathrm{Na}_{2}[\mathrm{Co}(\mathrm{EDTA})]\)

The metal in this complex is Co. The ligand is EDTA, which is a hexadentate ligand (it can bind to the metal through six donor sites). Therefore, the coordination number is 6. As for the oxidation number, the overall charge of the complex is -2 (due to the 2 sodium ions), and the charge of EDTA is -4. Therefore, the oxidation number of the Co is +2.
02

b) \(\mathrm{KMnO}_{4}\)

The metal in this compound is Mn. The ligands in this compound are four oxygen atoms. Therefore, the coordination number is 4. As for the oxidation number, K has a +1 charge and each oxygen atom has a -2 charge. Thus, \(1 + x + 4(-2) = 0\), where x is the oxidation number of Mn. Solving for x, we get the oxidation number of Mn as +7.
03

c) \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4}\right] \mathrm{Cl}_{2}\)

In this complex, the metal is Pt. The ligands are four ammonia molecules. Therefore, the coordination number is 4. As for the oxidation number, the overall charge of the complex is 0, and each NH3 molecule has a charge of 0. Therefore, the oxidation number of the Pt must be +2, as the overall charge of the chloride ions is -2.
04

d) \(\mathrm{K}_{3} \mathrm{Fe}(\mathrm{CN})_{6}\)

In this complex, the metal is Fe. The ligands are six CN- ions. Therefore, the coordination number is 6. As for the oxidation number, K has a +1 charge and each CN- ion has a -1 charge. So, \(3 + x - 6 = 0\), where x is the oxidation number of Fe. Solving for x, the oxidation number of Fe is +3.
05

e) \(\mathrm{Rh}\left(\mathrm{PPh}_{3}\right)_{3} \mathrm{Cl}\)

In this complex, the metal is Rh. There are three PPh3 ligands and one Cl- ligand. Therefore, the coordination number is 4. As for the oxidation number, since all PPh3 ligands have a charge of 0, we only need to consider the charge of Cl-, which is -1. The charge of the Rh must be +1 to balance this charge. So, the oxidation number of Rh is +1.
06

f) \(\mathrm{Zn}\left(\mathrm{C}_{2}\mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}\)

In this complex, the metal is Zn. There are one C2O4 ligand and two NH3 ligands. Therefore, the coordination number is 3. As for the oxidation number, since C2O4 has a charge of -2 and each NH3 has a charge of 0, the charge of the Zn must be +2 to balance the charge of the complex. Therefore, the oxidation number of Zn is +2.

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Most popular questions from this chapter

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) triamminetriaquachromium(III) nitrate (b) dichlorobis(ethylenediamine)platinum(II) (c) pentacarbonyliron(0) (d) ammonium diaquabis(oxalato)Co(II) (e) tris(bipyridyl)cobalt(III) sulfate

The molecule dimethylphosphinoethane $\left[\left(\mathrm{CH}_{3}\right)_{2} \mathrm{PCH}_{2} \mathrm{CH}_{2}\right.$ \(\mathrm{P}\left(\mathrm{CH}_{3}\right)_{2},\) which is abbreviated dmpe] is used as a ligand for some complexes that serve as catalysts. A complex that contains this ligand is \(\mathrm{Mo}(\mathrm{CO})_{4}(\) dmpe \()\). (a) Draw the Lewis structure for dmpe, and compare it with ethylenediamine as a coordinating ligand. (b) What is the oxidation state of Mo in \(\mathrm{Na}_{2}\left[\mathrm{Mo}(\mathrm{CN})_{2}(\mathrm{CO})_{2}(\) dmpe \()\right] ?(\mathbf{c})\) Sketch the structure of the $\left[\mathrm{Mo}(\mathrm{CN})_{2}(\mathrm{CO})_{2}(\text { dmpe })\right]^{2-}$ ion, including all the possible isomers.

For each of the following metals, write the electronic configuration of the atom and its \(2+\) ion: $(\mathbf{a}) \mathrm{Mn},(\mathbf{b}) \mathrm{Ru},(\mathbf{c}) \mathrm{Rh} .$ Draw the crystal-field energy-level diagram for the \(d\) orbitals of an octahedral complex, and show the placement of the \(d\) electrons for each \(2+\) ion, assuming a strong-field complex. How many unpaired electrons are there in each case?

The coordination complex \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) forms colorless, diamagnetic crystals that melt at \(90^{\circ} \mathrm{C}\). (a) What is the oxidation number of chromium in this compound? (b) Given that \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) is diamagnetic, what is the electron configuration of chromium in this compound? (c) Given that \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) is colorless, would you expect \(\mathrm{CO}\) to be a weak-field or strong-field ligand? (d) Write the name for \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) using the nomenclature rules for coordination compounds.

Draw the structure for $\mathrm{Pt}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)\left(\mathrm{NH}_{3}\right)_{2}$ and use it to answer the following questions: (a) What is the coordination number for platinum in this complex? (b) What is the coordination geometry? (c) What is the oxidation state of the platinum? (d) How many unpaired electrons are there? [Sections 23.2 and 23.6\(]\)
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