Question
Explain the anomalous behavior of copper and chromium.
✓
Answer
i. Copper:
- Copper (Cu) has atomic number 29.
- Its expected electronic configuration is $1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^2 3 d^9$.
- The 3d orbital is neither half-filled nor fully filled. Hence, it has less stability.
- Due to interelectronic repulsion forces, one 4 s electron enters into 3 d orbital. This makes 3 d orbital completely filled and 4 s orbital half-filled which gives extra stability and the electronic configuration of Cu becomes, $1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^1 3 d^{10}$.
- Chromium (Cr) has atomic number 24.
- Its expected electronic configuration is $1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^2 3 d^4$.
- The 3d orbital is less stable as it is not half-filled.
- Due to inter electronic repulsion forces, one 4 s electron enters into 3 d orbital. This makes 4 s and 3 d orbitals half-filled which gives extra stability and the electronic configuration of Cr becomes, $1 s^2 2 s^2 2 p^6 3 s^2 3 p^6 4 s^1$ $3 d^5$.
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