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Chapter 21: Problem 83

In which of the following is(are) the electron configuration(s) correct for the species indicated? a. Cu \(\quad[\mathrm{Ar}] 4 s^{2} 3 d^{9}\) b. \(\mathrm{Fe}^{3+} \quad[\mathrm{Ar}] 3 d^{5}\) c. Co \(\quad[\mathrm{Ar}] 4 s^{2} 3 d^{7}\) d. La \(\quad[\mathrm{Ar}] 6 s^{2} 4 f^{1}\) e. \(\mathrm{Pt}^{2+} \quad[\mathrm{Xe}] 4 f^{14} 5 d^{8}\)

Short Answer

Expert verified
The correct electron configurations for the given species are: b. \(\mathrm{Fe}^{3+}\) \([\mathrm{Ar}] 3d^{5}\) c. Co \([\mathrm{Ar}] 4s^{2} 3d^{7}\) d. La \([\mathrm{Ar}] 6s^{2} 4f^{1}\)

Step by step solution

01

1. Cu Electron Configuration

Cu (Copper) has 29 electrons in its neutral form. We can find its electron configuration by filling the orbitals following the Aufbau Principle. The electron configuration would be: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^9\). However, Copper is an exception to the aufbau principle because the half-filled d subshell provides extra stability. Therefore, one electron from the 4s orbital promotes to the 3d orbital, resulting in its correct electron configuration: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^1 3d^{10}\). The given electron configuration for Cu is incorrect.
02

2. Fe³⁺ Electron Configuration

Fe (Iron) has 26 electrons in its neutral form. We can find its electron configuration by filling the orbitals following the Aufbau principle: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^6\). When Fe loses 3 electrons to form Fe³⁺, the electron configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^5\) which is the same as the one given, [\(\mathrm{Ar}\) 3d⁵]. So the given electron configuration for \(\mathrm{Fe}^{3+}\) is correct.
03

3. Co Electron Configuration

Co (Cobalt) has 27 electrons in its neutral form. We can find its electron configuration by filling the orbitals following the Aufbau principle: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^7\). The given electron configuration for Co is the same, [\(\mathrm{Ar}\) 4s² 3d⁷], making it correct.
04

4. La Electron Configuration

La (Lanthanum) has 57 electrons in its neutral form. We can find its electron configuration by filling the orbitals following the Aufbau principle: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^1\). The given electron configuration for La is the same, [\(\mathrm{Ar}\) 6s² 4f¹], making it correct.
05

5. Pt²⁺ Electron Configuration

Pt (Platinum) has 78 electrons in its neutral form. We can find its electron configuration by filling the orbitals following the Aufbau principle: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 6s^2 4f^{14} 5d^9\). When Pt loses 2 electrons to form Pt²⁺, the electron configuration becomes: \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^7\). The given electron configuration for Pt²⁺ is [\(\mathrm{Xe}\) 4f¹⁴ 5d⁸], which is incorrect.

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Most popular questions from this chapter

Use standard reduction potentials to calculate \(\mathscr{E}^{\circ}, \Delta G^{\circ}\), and \(K\) (at \(298 \mathrm{~K}\) ) for the reaction that is used in production of gold: $$ 2 \mathrm{Au}(\mathrm{CN})_{2}^{-}(a q)+\mathrm{Zn}(s) \longrightarrow 2 \mathrm{Au}(s)+\mathrm{Zn}(\mathrm{CN})_{4}{ }^{2-}(a q) $$ The relevant half-reactions are $$ \begin{aligned} \mathrm{Au}(\mathrm{CN})_{2}^{-}+\mathrm{e}^{-} \longrightarrow \mathrm{Au}+2 \mathrm{CN}^{-} & \mathscr{E}^{\circ}=-0.60 \mathrm{~V} \\ \mathrm{Zn}(\mathrm{CN})_{4}^{2-}+2 \mathrm{e}^{-} \longrightarrow \mathrm{Zn}+4 \mathrm{CN}^{-} & \mathscr{E}^{\circ}=-1.26 \mathrm{~V} \end{aligned} $$

Name the following coordination compounds. a. \(\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{5} \mathrm{Br}\right] \mathrm{Br}_{2}\) b. \(\mathrm{Na}_{3}\left[\mathrm{Co}(\mathrm{CN})_{6}\right]\) c. \(\left[\mathrm{Fe}\left(\mathrm{NH}_{2} \mathrm{CH}_{2} \mathrm{CH}_{2} \mathrm{NH}_{2}\right)_{2}\left(\mathrm{NO}_{2}\right)_{2}\right] \mathrm{Cl}\) d. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{PtI}_{4}\right]\)

Both \(\mathrm{Ni}\left(\mathrm{NH}_{3}\right)_{4}{ }^{2+}\) and \(\mathrm{Ni}(\mathrm{SCN})_{4}{ }^{2-}\) have four ligands. The first is paramagnetic, and the second is diamagnetic. Are the complex ions tetrahedral or square planar? Explain.

When \(6 M\) ammonia is added gradually to aqueous copper(II) nitrate, a white precipitate forms. The precipitate dissolves as more \(6 M\) ammonia is added. Write balanced equations to explain these observations. [Hint: \(\mathrm{Cu}^{2+}\) reacts with \(\mathrm{NH}_{3}\) to form \(\left.\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}{ }^{2+} .\right]\)

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: $$ \mathrm{NH}_{2}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}-\mathrm{CH}_{2}-\mathrm{CH}_{2}-\mathrm{NH}_{2} $$ 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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