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Chapter 24: Problem 21

Predict: (a) which of the complex ions, \(\left[\mathrm{MoCl}_{6}\right]^{3-}\) and \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+},\) is diamagnetic and which is paramagnetic; (b) the number of unpaired electrons expected for the tetrahedral complex ion \(\left[\mathrm{CoCl}_{4}\right]^{2-}\).

Short Answer

Expert verified
\(\left[\mathrm{MoCl}_{6}\right]^{3-}\) and \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\) are both diamagnetic. \(\left[\mathrm{CoCl}_{4}\right]^{2-}\) has 3 unpaired electrons.

Step by step solution

01

Define magnetic property

First, remember the definitions for paramagnetic and diamagnetic substances. A diamagnetic substance is one that does not have any unpaired electrons and is not attracted to a magnetic field. On the other hand, paramagnetic substances do have unpaired electrons and are attracted to a magnetic field.
02

Find the Electron Configuration for each Complex

Find the electron configuration for the central atom in each complex. For \(\left[\mathrm{MoCl}_{6}\right]^{3-}\), Mo (molybdenum) has 42 electrons but the oxidation state here is +3, thus it has 36 valence electrons, which are all paired. For \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\), Co (cobalt) has 27 electrons and oxidation state of +3, thus left 24 electrons which are all paired as well.
03

Determine the Type of Magnetic Properties

Since both molybdenum and cobalt have all paired electrons, both \(\left[\mathrm{MoCl}_{6}\right]^{3-}\) and \(\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}\) are diamagnetic.
04

Electron Configuration for the Second Part

For the tetrahedral complex ion \(\left[\mathrm{CoCl}_{4}\right]^{2-}\), cobalt has 27 electrons with oxidation state of +2, which leaves us with 25 electrons. In the tetrahedral complex, cobalt doesn't pair its electrons.
05

Determining the Number of Unpaired Electrons

Since cobalt doesn't pair its electrons in the tetrahedral complex, it has 3 unpaired electrons after we fill up the electron orbitals.

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Most popular questions from this chapter

The following concentration cell is constructed. \(\mathrm{Ag} | \mathrm{Ag}^{+}\left(0.10 \mathrm{M}\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}, 0.10 \mathrm{M} \mathrm{CN}^{-}\right)\) $$\| \mathrm{Ag}^{+}(0.10 \mathrm{M}) | \mathrm{Ag}$$ If \(K_{f}\) for \(\left[\mathrm{Ag}(\mathrm{CN})_{2}\right]^{-}\) is \(5.6 \times 10^{18},\) what value would you expect for \(E_{\text {cell }}\) ? [Hint: Recall that the anode is on the left.]

What are the coordination number and the oxidation state of the central metal ion in each of the following complexes? Name each complex. (a) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{2+}\) (b) \(\left[\mathrm{AlF}_{6}\right]^{3-}\) (c) \(\left[\mathrm{Cu}(\mathrm{CN})_{4}\right]^{2-}\) (d) \(\left[\operatorname{CrBr}_{2}\left(\mathrm{NH}_{3}\right)_{4}\right]^{+}\) (e) \(\left[\operatorname{Co}(\text { ox })_{3}\right]^{4-}\) (f) \(\left[\mathrm{Ag}\left(\mathrm{S}_{2} \mathrm{O}_{3}\right)_{2}\right]^{3-}\)

Of the following complex ions, the one that exhibits isomerism is (a) \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right]^{+} ;\) (b) \(\left[\mathrm{CoNO}_{2}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+};\) \((\mathrm{c}) \quad\left[\mathrm{Pt}(\mathrm{en})\left(\mathrm{NH}_{3}\right)_{2}\right]^{2+};\) (d) \(\quad\left[\mathrm{CoCl}\left(\mathrm{NH}_{3}\right)_{5}\right]^{2+};\) (e) \(\left[\mathrm{PtCl}_{6}\right]^{2-}\).

Explain the following observations in terms of complex-ion formation. (a) \(\mathrm{CoCl}_{3}\) is unstable in aqueous solution, being reduced to \(\mathrm{CoCl}_{2}\) and liberating \(\mathrm{O}_{2}(\mathrm{g}) .\) Yet, \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right] \mathrm{Cl}_{3}\) can be easily maintained in aqueous solution. (b) AgI is insoluble in water and in dilute \(\mathrm{NH}_{3}(\mathrm{aq})\) but AgI will dissolve in an aqueous solution of sodium thiosulfate.

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