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Chapter 21: Problem 27

What is the electron configuration for the transition metal ion in each of the following compounds? a. \(K_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\) b. \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{Cl}\) c. $\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right] \mathrm{Br}_{2}$ d. $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{NO}_{2}\right)_{2}\right] \mathrm{I}$

Short Answer

Expert verified
The electron configurations for the transition metal ions in the given compounds are: a. Fe^3+: \(1s^22s^22p^63s^23p^63d^5\) b. Ag^+: \(1s^22s^22p^63s^23p^64s^23d^{10}4p^64d^{10}\) c. Ni^2+: \(1s^22s^22p^63s^23p^63d^7\) d. Cr^+: \(1s^22s^22p^63s^23p^63d^5\)

Step by step solution

01

Compound a: \(K_{3}\left[\mathrm{Fe}(\mathrm{CN})_{6}\right]\)

1. The central transition metal ion is Fe. 2. Since there are three potassium ions (K) with a charge of +1 each, the complex must have a -3 charge. The charge on the Fe ion is +3. 3. Iron (Fe) has an atomic number of 26. Its electron configuration is \(1s^22s^22p^63s^23p^64s^23d^6\). 4. Adjust the electron configuration for a +3 charge on the Fe ion: remove 3 electrons from the 4s and 3d orbitals. The electron configuration for Fe^3+ is \(1s^22s^22p^63s^23p^63d^5\).
02

Compound b: \(\left[\mathrm{Ag}\left(\mathrm{NH}_{3}\right)_{2}\right] \mathrm{Cl}\)

1. The central transition metal ion is Ag. 2. Since there is one chloride ion (Cl) with a charge of -1, the complex must have a +1 charge. The charge on the Ag ion is +1. 3. Silver (Ag) has an atomic number of 47. Its electron configuration is \(1s^22s^22p^63s^23p^64s^23d^{10}4p^65s^24d^{10}\). 4. Adjust the electron configuration for a +1 charge on the Ag ion: remove 1 electron from the 5s orbital. The electron configuration for Ag^+ is \(1s^22s^22p^63s^23p^64s^23d^{10}4p^64d^{10}\).
03

Compound c: \(\left[\mathrm{Ni}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]\mathrm{Br}_{2}\)

1. The central transition metal ion is Ni. 2. Since there are two bromide ions (Br) with a charge of -1 each, the complex must have a +2 charge. The charge on the Ni ion is +2. 3. Nickel (Ni) has an atomic number of 28. Its electron configuration is \(1s^22s^22p^63s^23p^64s^23d^8\). 4. Adjust the electron configuration for a +2 charge on the Ni ion: remove 2 electrons from the 4s and 3d orbitals. The electron configuration for Ni^2+ is \(1s^22s^22p^63s^23p^63d^7\).
04

Compound d: $\left[\mathrm{Cr}\left(\mathrm{H}_{2} \mathrm{O}\right)_{4}\left(\mathrm{NO}_{2}\right)_{2}\right] \mathrm{I}$

1. The central transition metal ion is Cr. 2. Since there is one iodide ion (I) with a charge of -1, the complex must have a +1 charge. The charge on the Cr ion is +1. 3. Chromium (Cr) has an atomic number of 24. Its electron configuration is \(1s^22s^22p^63s^23p^64s^13d^5\). 4. Adjust the electron configuration for a +1 charge on the Cr ion: remove 1 electron from the 4s orbital. The electron configuration for Cr^+ is \(1s^22s^22p^63s^23p^63d^5\).

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Most popular questions from this chapter

The complex ion \(\mathrm{Cu}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}^{2+}\) has an absorption maximum at around 800 \(\mathrm{nm}\) . When four ammonias replace water, $\mathrm{Cu}\left(\mathrm{NH}_{3}\right)_{4}\left(\mathrm{H}_{2} \mathrm{O}\right)_{2}^{2+},$ the absorption maximum shifts to around 600 \(\mathrm{nm} .\) What do these results signify in terms of the relative field splittings of \(\mathrm{NH}_{3}\) and \(\mathrm{H}_{2} \mathrm{O}\) ? Explain.

a. In the absorption spectrum of the complex ion \(\mathrm{Cr}(\mathrm{NCS})_{6}^{3-}\) there is a band corresponding to the absorption of a photon of light with an energy of $1.75 \times 10^{4} \mathrm{cm}^{-1} .\( Given \)1 \mathrm{cm}^{-1}=1.986 \times 10^{-23} \mathrm{J},$ what is the wavelength of this photon? b. The \(\mathrm{Cr}-\mathrm{N}-\mathrm{C}\) bond angle in \(\mathrm{Cr}(\mathrm{NCS})_{6}^{3-}\) is predicted to be \(180^{\circ} .\) What is the hybridization of the N atom in the \(\mathrm{NCS}^{-}\) ligand when a Lewis acid-base reaction occurs between \(\mathrm{Cr}^{3+}\) and \(\mathrm{NCS}^{-}\) that would give a $180^{\circ} \mathrm{Cr}-\mathrm{N}-\mathrm{C}$ bond angle? \(\mathrm{Cr}(\mathrm{NCS})_{6}^{3-}\) undergoes substitution by ethylenediamine (en) according to the equation $$\mathrm{Cr}(\mathrm{NCS})_{6}^{3-}+2 \mathrm{en} \longrightarrow \mathrm{Cr}(\mathrm{NCS})_{2}(\mathrm{en})_{2}^{+}+4 \mathrm{NCS}^{-}$$ Does \(\mathrm{Cr}(\mathrm{NCS})_{2}(\mathrm{en})_{2}^{+}\) exhibit geometric isomerism? Does \(\mathrm{Cr}(\mathrm{NCS})_{2}(\mathrm{en})_{2}^{+}\) exhibit optical isomerism?

Which of the following ions is(are) expected to form colored octahedral aqueous complex ions? a. \(Z n^{2+}\) b. \(C u^{2+}\) c. \(M n^{3+}\) d. \(T i^{4+}\)

Figure 21.17 shows that the cis isomer of $\mathrm{Co}(\mathrm{en})_{2} \mathrm{Cl}_{2}^{+}$ is optically active while the trans isomer is not optically active. Is the same true for \(\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}+?\) Explain.

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