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Chapter 9: Problem 36

Write electron configurations consistent with the following data on numbers of unpaired electrons: \(\mathrm{Ni}^{2+}, 2 ; \mathrm{Cu}^{2+}, 1 ; \mathrm{Cr}^{3+}, 3.\)

Short Answer

Expert verified
The electron configurations for \(\mathrm{Ni}^{2+}\), \(\mathrm{Cu}^{2+}\), and \(\mathrm{Cr}^{3+}\) are \([Ar] 3d^8\), \([Ar] 3d^9\), and \([Ar] 3d^3\) respectively.

Step by step solution

01

Identify the atomic numbers

Identify the atomic numbers of Ni (Nickel), Cu (Copper), and Cr (Chromium), which are 28, 29, and 24 respectively.
02

Write electron configurations for neutral atoms

To write the electron configuration of neutral atoms, partially follow the Aufbau principle: - Ni: \([Ar] 4s^2 3d^8\) - Cu: \([Ar] 4s^2 3d^9\) - Cr: \([Ar] 4s^2 3d^4\)
03

Adjust the configurations based on the charge

For ions, subtract the charge from the total number of electrons. Following the Hund's rule, subtract first from the 4s orbital because its energy is higher than the 3d orbital. The configurations become: - \(\mathrm{Ni}^{2+}\): \([Ar] 3d^8\) - \(\mathrm{Cu}^{2+}\): \([Ar] 3d^9-2=3d^7\) - \(\mathrm{Cr}^{3+}\): \([Ar] 3d^4-3=3d^1\)
04

Adjust the configurations based on the number of unpaired electrons

Now adjust the configurations with the given unpaired electron data. Remember, filled (or half-filled) 3d-orbitals are more stable. The final configurations will be: - \(\mathrm{Ni}^{2+}\): \([Ar] 3d^8\) - \(\mathrm{Cu}^{2+}\): \([Ar] 3d^9\) - \(\mathrm{Cr}^{3+}\): \([Ar] 3d^3\)

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