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Chapter 23: Problem 15

Write out the ground-state electron configurations of (a) \(\mathrm{Ti}^{3+},(\mathbf{b}) \mathrm{Ru}^{2+},(\mathbf{c}) \mathrm{Au}^{3+},(\mathbf{d}) \mathrm{Mn}^{4+} .\)

Short Answer

Expert verified
The ground-state electron configurations of the ions are: a) \(\mathrm{Ti}^{3+}\): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\) b) \(\mathrm{Ru}^{2+}\): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 4d^6\) c) \(\mathrm{Au}^{3+}\): \(1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^8\) d) \(\mathrm{Mn}^{4+}\): \(1s^2 2s^2 2p^6 3s^2 3p^6 3d^3\)

Step by step solution

01

(a) Titanium ion (\(\mathrm{Ti}^{3+}\)) electron configuration

1. Find the atomic number of Titanium (Ti). In the periodic table, it is 22. 2. Determine the electron configuration of the neutral atom: \[\mathrm{Ti}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^2\] 3. Remove three electrons from the atom to form the ion \(\mathrm{Ti}^{3+}\), starting from the outermost shell: \[\mathrm{Ti}^{3+}: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^1\]
02

(b) Ruthenium ion (\(\mathrm{Ru}^{2+}\)) electron configuration

1. Find the atomic number of Ruthenium (Ru). In the periodic table, it is 44. 2. Determine the electron configuration of the neutral atom: \[\mathrm{Ru}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^6\] 3. Remove two electrons from the atom to form the ion \(\mathrm{Ru}^{2+}\), starting from the outermost shell: \[\mathrm{Ru}^{2+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 4d^6\]
03

(c) Gold ion (\(\mathrm{Au}^{3+}\)) electron configuration

1. Find the atomic number of Gold (Au). In the periodic table, it is 79. 2. Determine the electron configuration of the neutral atom: \[\mathrm{Au}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^{10} 6s^1\] 3. Remove three electrons from the atom to form the ion \(\mathrm{Au}^{3+}\), starting from the outermost shell: \[\mathrm{Au}^{3+}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^{10} 4p^6 5s^2 4d^{10} 5p^6 4f^{14} 5d^8\]
04

(d) Manganese ion (\(\mathrm{Mn}^{4+}\)) electron configuration

1. Find the atomic number of Manganese (Mn). In the periodic table, it is 25. 2. Determine the electron configuration of the neutral atom: \[\mathrm{Mn}: 1s^2 2s^2 2p^6 3s^2 3p^6 4s^2 3d^5\] 3. Remove four electrons from the atom to form the ion \(\mathrm{Mn}^{4+}\), starting from the outermost shell: \[\mathrm{Mn}^{4+}: 1s^2 2s^2 2p^6 3s^2 3p^6 3d^3\]

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Most popular questions from this chapter

Write the formula for each of the following compounds, being sure to use brackets to indicate the coordination sphere: (a) hexamminechromium(III) nitrate (b) tetraamminecarbonatocobalt(III) sulfate (c) dichlorobis(ethylenediamine)platinum(IV) bromide (d) potassium diaquatetrabromovanadate(III) (e) bis(ethylenediamine) zinc(II) tetraiodomercurate(II)

Generally speaking, for a given metal and ligand, the stability of a coordination compound is greater for the metal in the \(+3\) rather than in the \(+2\) oxidation state (for metals that form stable \(+3\) ions in the first place). Suggest an explanation, keeping in mind the Lewis acid-base nature of the metal-ligand bond.

The coordination complex \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) forms colorless, diamagnetic crystals that melt at \(90^{\circ} \mathrm{C}\) . (a) What is the oxidation number of chromium in this compound? (b) Given that \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) is diamagnetic, what is the electron configuration of chromium in this compound? (c) Given that \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) is colorless, would you expect CO to be a weak-field or strong-field ligand? (d) Write the name for \(\left[\mathrm{Cr}(\mathrm{CO})_{6}\right]\) using the nomenclature rules for coordination compounds.

Carbon monoxide, CO, is an important ligand in coordination chemistry. When \(\mathrm{CO}\) is reacted with nickel metal, the product is \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right],\) which is a toxic, pale yellow liquid. (a) What is the oxidation number for nickel in thiscompound? (b) Given that \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) is a diamagnetic molecule with a tetrahedral geometry, what is the electron configuration of nickel in this compound? (c) Write the name for \(\left[\mathrm{Ni}(\mathrm{CO})_{4}\right]\) using the nomenclature rules for coordination compounds.

Indicate the coordination number and the oxidation number of the metal for each of the following complexes: (a) \(\mathrm{Na}_{2}\left[\mathrm{CdCl}_{4}\right]\) (b) \(\mathrm{K}_{2}\left[\mathrm{MoOCl}_{4}\right]\) (c) \(\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{4} \mathrm{Cl}_{2}\right] \mathrm{Cl}\) (d) \(\left[\mathrm{Ni}(\mathrm{CN})_{5}\right]^{3-}\) (e) \(\mathrm{K}_{3}\left[\mathrm{V}\left(\mathrm{C}_{2} \mathrm{O}_{4}\right)_{3}\right]\) (f) \(\left[\mathrm{Zn}(\mathrm{en})_{2}\right] \mathrm{Br}_{2}\)
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