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Chapter 20: Problem 4

Without referring to the text, write the ground-state electron configurations of the first-row transition metals. Explain any irregularities.

Short Answer

Expert verified
The electron configurations of first-row transition metals are: Sc: \([Ar] 4s^2 3d^1\), Ti: \([Ar] 4s^2 3d^2\), V: \([Ar] 4s^2 3d^3\), Cr: \([Ar] 4s^1 3d^5\), Mn: \([Ar] 4s^2 3d^5\), Fe: \([Ar] 4s^2 3d^6\), Co: \([Ar] 4s^2 3d^7\), Ni: \([Ar] 4s^2 3d^8\), Cu: \([Ar] 4s^1 3d^{10}\), Zn: \([Ar] 4s^2 3d^{10}\). The irregularities observed for Cr and Cu, where an electron is moved from the \(4s\) orbital to the \(3d\) orbital, occur because the energy of the \(4s\) and \(3d\) orbitals are quite close and configurations where the \(d\) shell is half-filled or fully-filled are more energetically favorable.

Step by step solution

01

Determine the ground-state electron configuration

The ground-state electron configurations are based on the order of filling of the atomic orbitals. The order can be determined using the periodic table. The electron configurations of these elements are: Sc: \([Ar] 4s^2 3d^1\), Ti: \([Ar] 4s^2 3d^2\), V: \([Ar] 4s^2 3d^3\), Cr: \([Ar] 4s^1 3d^5\), Mn: \([Ar] 4s^2 3d^5\), Fe: \([Ar] 4s^2 3d^6\), Co: \([Ar] 4s^2 3d^7\), Ni: \([Ar] 4s^2 3d^8\), Cu: \([Ar] 4s^1 3d^{10}\), Zn: \([Ar] 4s^2 3d^{10}\).
02

Explain the irregularities

Two irregularities can be observed. One occurs for Chromium (Cr) and the other for Copper (Cu). For Chromium, rather than following the expected configuration of \([Ar] 4s^2 3d^4\), it's actually \([Ar] 4s^1 3d^5\). This is because the energy of the \(4s\) and \(3d\) orbitals are quite close and a configuration with more electrons in the \(3d\) orbital is more stable, especially when it results in a half-full \(d\) shell. In the case of Copper, we might expect \([Ar] 4s^2 3d^9\), but instead it is \([Ar] 4s^1 3d^{10}\). Moving one of the \(4s\) electrons to the \(3d\) shell again results in a more stable configuration because it results in a completely filled \(d\) shell.

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Most popular questions from this chapter

The complex ion \(\left[\mathrm{Ni}(\mathrm{CN})_{2} \mathrm{Br}_{2}\right]^{2-}\) has a square planar geometry. Draw the structures of the geometric isomers of this complex.

Consider the following two ligand exchange reactions: \(\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+6 \mathrm{NH}_{3} \rightleftharpoons\left[\mathrm{Co}\left(\mathrm{NH}_{3}\right)_{6}\right]^{3+}+6 \mathrm{H}_{2} \mathrm{O}\) $$\left[\mathrm{Co}\left(\mathrm{H}_{2} \mathrm{O}\right)_{6}\right]^{3+}+3 \mathrm{en} \rightleftharpoons\left[\mathrm{Co}(\mathrm{en})_{3}\right]^{3+}+6 \mathrm{H}_{2} \mathrm{O}$$ (a) Which of the reactions should have a larger \(\Delta S^{\circ}\) ? (b) Given that the \(\mathrm{Co}-\mathrm{N}\) bond strength is approximately the same in both complexes, which reaction will have a larger equilibrium constant? Explain your choices.

Define the following terms: coordination compound, ligand, donor atom, coordination number, chelating agent.

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