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Chapter 7: Problem 76

Explain why the ground-state electron configurations of \(\mathrm{Cr}\) and \(\mathrm{Cu}\) are different from what we might expect.

Short Answer

Expert verified
The ground-state electron configurations of Chromium (Cr) and Copper (Cu) are different from what we would expect based onAufbau Principle because they achieve a more stable state by having half-filled (in case of Cr: \(4s^13d^5\)) or completely filled (in case of Cu: \(4s^13d^{10}\)) sub-levels.

Step by step solution

01

Expected Electron Configuration for Chromium

According to the Aufbau Principle, electrons fill the energies beginning from the lowest energy level. By this principle, Chromium (Cr) with atomic number 24 would have the electron configuration \(1s^22s^22p^63s^23p^64s^23d^4\).
02

Actual Electron Configuration for Chromium

However, the actual electron configuration is \(1s^22s^22p^63s^23p^64s^13d^5\). Chromium promotes one electron from the 4s orbital to the 3d orbital to achieve a half-filled sub-level, which offers more stability.
03

Expected Electron Configuration for Copper

For Copper (Cu) with atomic number 29, based on Aufbau Principle the expected electron configuration is \(1s^22s^22p^63s^23p^64s^23d^9\).
04

Actual Electron Configuration for Copper

On the contrary, the actual electron configuration is \(1s^22s^22p^63s^23p^64s^13d^{10}\). Similar to Chromium, Copper promotes one electron from the 4s orbital to the 3d orbital to get a fully filled sub-level, which increases the stability.

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Most popular questions from this chapter

Which orbital in each of the following pairs is lower in energy in a many- electron atom? (a) \(2 s, 2 p\) (b) \(3 p, 3 d ;\) (c) \(3 s, 4 s ;\) (d) \(4 d, 5 f\).

What is an atomic orbital? How does an atomic orbital differ from an orbit?

Describe the characteristics of an \(s\) orbital, a \(p\) orbital, and a \(d\) orbital. Which of the following orbitals do not exist: \(1 p, 2 s, 2 d, 3 p, 3 d, 3 f, 4 g ?\)

An electron in an atom is in the \(n=3\) quantum level. List the possible values of \(\ell\) and \(m_{\ell}\) that it can have.

Determine the maximum number of electrons that can be found in each of the following subshells: \(3 s\), \(3 d, 4 p, 4 f, 5 f\)
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