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Chapter 21: Problem 22

What is the electron configuration for the transition metal ion(s) in each of the following compounds? a. \(\left(\mathrm{NH}_{4}\right)_{2}\left[\mathrm{Fe}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2} \mathrm{Cl}_{4}\right]\) b. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\right] \mathrm{I}_{2}\) c. \(\mathrm{Na}_{2}\left[\mathrm{TaF}_{7}\right]\) d. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right]\) Pt forms \(+2\) and \(+4\) oxidation states in compounds.

Short Answer

Expert verified
The electron configurations for the transition metal ions in the given compounds are: a. Fe: \(1s^22s^22p^63s^23p^63d^6\) b. Co: \(1s^22s^22p^63s^23p^63d^7\) c. This exercise contains an error in the composition of the substance. d. Pt(II): \(1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^8\) Pt(IV): \(1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^7\)

Step by step solution

01

Identify the transition metal

In this compound, the transition metal is iron (Fe).
02

Find the oxidation state

We can find the oxidation state of Fe by considering the charges of the other species within the compound: \[2 \cdot (\mathrm{NH}_{4})^{+} + [\mathrm{Fe}(H_2O)_{2}\mathrm{Cl}_{4}]^{x} = \mathrm{neutral}\] \[+2 + x = 0\] Solving for x, we find that the oxidation state of Fe is +2.
03

Determine the electron configuration

As a neutral atom, Fe has an electron configuration of: \[\mathrm{Fe}:\,\, 1s^22s^22p^63s^23p^63d^64s^2\] Now that we know the oxidation state of Fe is +2, we will remove two electrons from the configuration: \[\mathrm{Fe}^{2+}:\,\, 1s^22s^22p^63s^23p^63d^6\] So, the electron configuration for the iron ion in this compound is \(1s^22s^22p^63s^23p^63d^6\). #b. \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{2}\left(\mathrm{NH}_{2}\mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\right] \mathrm{I}_{2}\) #
04

Identify the transition metal

In this compound, the transition metal is cobalt (Co).
05

Find the oxidation state

We can find the oxidation state of Co by considering the charges of the other species within the compound: \[[\mathrm{Co}(NH_3)_{2}(NH_{2}CH_{2}CH_{2}NH_{2})_{2}]^{x} + 2 \cdot (\mathrm{I}^{-}) = \mathrm{neutral}\] \[x - 2 = 0\] Solving for x, we find that the oxidation state of Co is +2.
06

Determine the electron configuration

As a neutral atom, Co has an electron configuration of: \[\mathrm{Co}:\,\, 1s^22s^22p^63s^23p^63d^74s^2\] Now that we know the oxidation state of Co is +2, we will remove two electrons from the configuration: \[\mathrm{Co}^{2+}:\,\, 1s^22s^22p^63s^23p^63d^7\] So, the electron configuration for the cobalt ion in this compound is \(1s^22s^22p^63s^23p^63d^7\). #c. \(\mathrm{Na}_{2}\left[\mathrm{TaF}_{7}\right]\)#
07

Identify the transition metal

In this compound, the transition metal is tantalum (Ta).
08

Find the oxidation state

We can find the oxidation state of Ta by considering the charges of the other species within the compound: \[2 \cdot (\mathrm{Na}^{+}) + [\mathrm{TaF}_7]^{x} = \mathrm{neutral}\] \[+2 + x = 0\] Solving for x, we find that the oxidation state of Ta is -2.
09

Determine the electron configuration

As a neutral atom, Ta has an electron configuration of: \[\mathrm{Ta}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^36s^2\] Now that we know the oxidation state of Ta is -2, we will add two electrons to the configuration: \[\mathrm{Ta}^{-2}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^36s^2\] However, elements of group 5 do not form negative oxidation states in compounds; thus, this exercise contains an error in the composition of the substance. #d. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{Pt} \mathrm{I}_{4}\right]\) # In this compound, we have two different platinum ions, Pt(II) and Pt(IV).
10

Identify the transition metal.

In both parts of this compound, the transition metal is platinum (Pt).
11

Pt(II) Determine the electron configuration

As a neutral atom, Pt has an electron configuration of: \[\mathrm{Pt}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^96s^1\] Now that we know the oxidation state of the first Pt ion is +2, we will remove two electrons from the configuration: \[\mathrm{Pt}^{2+}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^8\] So, the electron configuration for the first platinum ion (Pt(II)) in this compound is \(1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^8\).
12

Pt(IV) Determine the electron configuration

In the neutral atom, Pt has an electron configuration of: \[\mathrm{Pt}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^96s^1\] Now that we know the oxidation state of the second Pt ion is +4, we will remove four electrons from the configuration: \[\mathrm{Pt}^{4+}:\,\, 1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^7\] So, the electron configuration for the second platinum ion (Pt(IV)) in this compound is \(1s^22s^22p^63s^23p^63d^{10}4s^24p^64d^{10}5s^25p^64f^{14}5d^7\).

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Most popular questions from this chapter

Write electron configurations for the following metals. a. \(\mathrm{Ni}\) b. \(\mathrm{Cd}\) c. \(\mathrm{Zr}\) d. \(\mathrm{Os}\)

Qualitatively draw the crystal field splitting of the \(d\) orbitals in a trigonal planar complex ion. (Let the \(z\) axis be perpendicular to the plane of the complex.)

Henry Taube, 1983 Nobel Prize winner in chemistry, has studied the mechanisms of the oxidation-reduction reactions of transition metal complexes. In one experiment he and his students studied the following reaction: \(\begin{aligned} \mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}(a q)+& \mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5} \mathrm{Cl}^{2+}(a q) \\\ \longrightarrow & \mathrm{Cr}(\mathrm{III}) \text { complexes }+\mathrm{Co}(\mathrm{II}) \text { complexes } \end{aligned}\) Chromium(III) and cobalt(III) complexes are substitutionally inert (no exchange of ligands) under conditions of the experiment. Chromium(II) and cobalt(II) complexes can exchange ligands very rapidly. One of the products of the reaction is \(\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cl}^{2+} .\) Is this consistent with the reaction proceeding through formation of \(\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Cr}-\mathrm{Cl}-\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{5}\) as an intermediate? Explain.

Write electron configurations for each of the following. a. \(\mathrm{Cr}, \mathrm{Cr}^{2+}, \mathrm{Cr}^{3+}\) b. \(\mathrm{Cu}, \mathrm{Cu}^{+}, \mathrm{Cu}^{2+}\) c. \(\mathrm{V}, \mathrm{V}^{2+}, \mathrm{V}^{3+}\)

How many bonds could each of the following chelating ligands form with a metal ion? a. acetylacetone (acacH), a common ligand in organometallic catalysts: b. diethylenetriamine, used in a variety of industrial processes: c. salen, a common ligand for chiral organometallic catalysts: d. porphine, often used in supermolecular chemistry as well as catalysis; biologically, porphine is the basis for many different types of porphyrin- containing proteins, including heme proteins:
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