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Chapter 20: Problem 22

Write electron configurations for the following ions. a. \(\mathrm{Ni}^{2+}\) b. \(\mathrm{Cd}^{2+}\) c. \(\mathrm{Zr}^{3+}\) and \(\mathrm{Zr}^{4+}\) d. \(\mathrm{Os}^{2+}\) and \(\mathrm{Os}^{3+}\)

Short Answer

Expert verified
The electron configurations of the ions are: a. \(\mathrm{Ni}^{2+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^8\) b. \(\mathrm{Cd}^{2+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\) c. \(\mathrm{Zr}^{3+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{7}\) and \(\mathrm{Zr}^{4+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{6}\) d. \(\mathrm{Os}^{2+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\, 5p^6\, 6s^2 \, 4f^{14} \, 5d^{6}\) and \(\mathrm{Os}^{3+}\): \(1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\, 5p^6\, 6s^2 \, 4f^{14} \, 5d^{5}\)

Step by step solution

01

a. Electron Configuration of \(\mathrm{Ni}^{2+}\)

The atomic number of nickel (Ni) is 28. In its neutral state, it has 28 electrons. As \(\mathrm{Ni}^{2+}\), it has lost 2 electrons, leaving it with 26 electrons. The electron configuration for 26 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^8\]
02

b. Electron Configuration of \(\mathrm{Cd}^{2+}\)

The atomic number of cadmium (Cd) is 48. In its neutral state, it has 48 electrons. As \(\mathrm{Cd}^{2+}\), it has lost 2 electrons, leaving it with 46 electrons. The electron configuration for 46 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\]
03

c. Electron Configuration of \(\mathrm{Zr}^{3+}\) and \(\mathrm{Zr}^{4+}\)

The atomic number of zirconium (Zr) is 40. In its neutral state, it has 40 electrons. For \(\mathrm{Zr}^{3+}\), it has lost 3 electrons, leaving it with 37 electrons. The electron configuration for 37 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{7}\] For \(\mathrm{Zr}^{4+}\), it has lost 4 electrons, leaving it with 36 electrons. The electron configuration for 36 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{6}\]
04

d. Electron Configuration of \(\mathrm{Os}^{2+}\) and \(\mathrm{Os}^{3+}\)

The atomic number of osmium (Os) is 76. In its neutral state, it has 76 electrons. For \(\mathrm{Os}^{2+}\), it has lost 2 electrons, leaving it with 74 electrons. The electron configuration for 74 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\, 5p^6\, 6s^2 \, 4f^{14} \, 5d^{6}\] For \(\mathrm{Os}^{3+}\), it has lost 3 electrons, leaving it with 73 electrons. The electron configuration for 73 electrons is: \[1s^2\, 2s^2\, 2p^6\, 3s^2\, 3p^6\, 4s^2\, 3d^{10}\, 4p^6\, 5s^2\, 4d^{10}\, 5p^6\, 6s^2 \, 4f^{14} \, 5d^{5}\]

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Most popular questions from this chapter

How many unpaired electrons are in the following complex ions? a. \(\mathrm{Ru}\left(\mathrm{NH}_{3}\right)_{6}^{2+}\) (low-spin case) b. \(\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) c. \(\mathrm{V}(\mathrm{en})_{3}^{3+}\)

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. \(\left[\mathrm{Pt}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{I}_{2}\right]\left[\mathrm{PtI}_{4}\right]\)

Consider the pseudo-octahedral complex ion of \(\mathrm{Cr}^{3+},\) where \(\mathrm{A}\) and B represent ligands. Ligand A produces a stronger crystal field than ligand B. Draw an appropriate crystal field diagram for this complex ion (assume the A ligands are on the \(z\) -axis).

How many bonds could each of the following chelating ligands form with a metal ion? a. acetylacetone (acacH), a common ligand in organometal:atalysts: 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:

The ferrate ion, \(\mathrm{FeO}_{4}^{2-},\) is such a powerful oxidizing agent that in acidic solution, aqueous ammonia is reduced to elemental nitrogen along with the formation of the iron(III) ion. a. What is the oxidation state of iron in \(\mathrm{FeO}_{4}^{2-},\) and what is the electron configuration of iron in this polyatomic ion? b. If \(25.0 \mathrm{mL}\) of a \(0.243 \mathrm{M} \mathrm{FeO}_{4}^{2-}\) solution is allowed to react with \(55.0 \mathrm{mL}\) of \(1.45 \mathrm{M}\) aqueous ammonia, what volume of nitrogen gas can form at \(25^{\circ} \mathrm{C}\) and 1.50 atm?
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