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Chapter 23: Problem 16

How many electrons are in the valence \(d\) orbitals in these transition-metal ions? (a) \(\mathrm{Co}^{3+},(\mathbf{b}) \mathrm{Cu}^{+},(\mathbf{c}) \mathrm{Cd}^{2+},(\mathbf{d}) \mathrm{Os}^{3+}.\)

Short Answer

Expert verified
The number of electrons in the valence d orbitals in the transition-metal ions are: (a) Co^3+: 6 electrons, (b) Cu^+: 10 electrons, (c) Cd^2+: 10 electrons, and (d) Os^3+: 5 electrons.

Step by step solution

01

(a) Co^3+ ion electron configuration

To find the electron configuration of Co^3+, first determine the electron configuration of neutral cobalt (Co). Cobalt is element 27, so it has 27 electrons in its neutral state. The electron configuration for Co is \([Ar] 4s^2 3d^7\). When Co loses 3 electrons to form the Co^3+ ion, it loses two 4s electrons and one 3d electron, resulting in a final electron configuration of \([Ar] 3d^6\). Thus, there are 6 electrons in the valence d orbitals in Co^3+.
02

(b) Cu^+ ion electron configuration

To find the electron configuration of Cu^+, first determine the electron configuration of neutral copper (Cu). Copper is element 29, and a neutral copper atom has 29 electrons. The electron configuration for Cu is \([Ar] 4s^2 3d^9\). When Cu loses 1 electron to form the Cu^+ ion, it loses one 4s electron, resulting in a final electron configuration of \([Ar] 3d^{10}\). Thus, there are 10 electrons in the valence d orbitals in Cu^+.
03

(c) Cd^2+ ion electron configuration

To find the electron configuration of Cd^2+, first determine the electron configuration of neutral cadmium (Cd). Cadmium is element 48, and a neutral cadmium atom has 48 electrons. The electron configuration for Cd is \([Kr] 5s^2 4d^{10}\). When Cd loses 2 electrons to form the Cd^2+ ion, it loses both 5s electrons, resulting in a final electron configuration of \([Kr] 4d^{10}\). Thus, there are 10 electrons in the valence d orbitals in Cd^2+.
04

(d) Os^3+ ion electron configuration

To find the electron configuration of Os^3+, first determine the electron configuration of neutral osmium (Os). Osmium is element 76, so it has 76 electrons in its neutral state. The electron configuration for Os is \([Xe] 6s^2 4f^{14} 5d^6\). When Os loses 3 electrons to form the Os^3+ ion, it loses two 6s electrons and one 5d electron, resulting in a final electron configuration of \([Xe] 4f^{14} 5d^5\). Thus, there are 5 electrons in the valence d orbitals in Os^3+. To summarize, the number of electrons in the valence d orbitals in these transition-metal ions is: (a) Co^3+: 6 electrons (b) Cu^+: 10 electrons (c) Cd^2+: 10 electrons (d) Os^3+: 5 electrons

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Which type of magnetic material cannot be used to make permanent magnets, a ferromagnetic substance, an anti-ferromagnetic substance, or a ferrimagnetic substance?

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