Easy
The electronic configuration of the valence shell of $Cu$ is $3d^{10}4s^{1}$ and not $3d^{9}4s^{2}$. How is this configuration explained?
- ADue to the stability of completely filled $d$-orbitals.
- BDue to the stability of half-filled $d$-orbitals.
- CDue to the exchange energy.
- DDue to the lower energy of $3d$ orbitals compared to $4s$.
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Quantum Number Information $(1)$ Principal quantum number $(A)$ Spatial orientation of the orbital $(2)$ Azimuthal quantum number $(B)$ Energy and size of the orbital $(3)$ Magnetic quantum number $(C)$ Electron spin $(4)$ Spin quantum number $(D)$ Shape of the orbital
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| $(1)$ Principal quantum number | $(A)$ Spatial orientation of the orbital |
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| $(3)$ Magnetic quantum number | $(C)$ Electron spin |
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