Write the electron configuration of the copper atom and the...

Write the electron configuration of the copper atom and the $2+$ cation of copper. Remember that the electron configuration of copper atom is unusual. Does the fact that copper is an exception to the aufbau principle influence the electron configuration of $\mathrm{Cu}^{2+} ?$

Key Concepts

Ionization in Transition Metals

In transition metals, when forming cations, electrons are typically removed first from the outermost s orbital rather than the d orbitals, despite the d orbitals being lower in energy in the ionic state. This behavior is key to understanding the electron configuration of metal ions like Cu²?, as the process of ionization may result in configurations that differ from those of the neutral atoms.

Exceptions to the Aufbau Principle

Certain elements, particularly some transition metals like copper, deviate from the expected orbital filling predicted by the Aufbau principle in order to achieve a more stable electron configuration. In the case of copper, an electron is promoted from the s orbital to the d orbital, leading to a configuration that minimizes energy by achieving a half-filled or fully filled d sub-shell.

Aufbau Principle

The Aufbau principle is a guideline that electrons fill atomic orbitals starting from the lowest energy level to higher levels. This rule generally predicts the order in which electron orbitals are occupied, though it has exceptions, especially among elements with nearly degenerate orbitals.

Electron Configuration

Electron configuration is the distribution of electrons among the orbitals of an atom. This configuration dictates many aspects of an element's chemical behavior, including bonding, magnetism, and reactivity. In transition metals, electron configurations often involve electrons in both the s and d orbitals, which can be close in energy.

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