Answer:
In an atom, subshell is defined as the set of states in a given shell that have the same azimuthal quantum number (ℓ).
For a d-subshell, the value of azimuthal quantum number (ℓ) is 3. Also, a d-subshell contains 5 atomic orbitals, namely [tex]d_{{z}^{2}},\, d_{xy},\, d_{yz},\, d_{xz},\, d_{{x}^{2}-{y}^{2}}[/tex], that can be occupied by 2 electrons each.
The filling of electrons in a subshell, such as the d-subshell, of a given shell is governed by the Hund's Rule of maximum multiplicity.
According to this rule, firstly all the 5 atomic orbitals of the d-subshell are singly filled and then the electrons are paired.
Since, a d-subshell can contain 10 electrons.
Therefore, firstly the 5 atomic orbitals are occupied with one electron each
[tex]d^{1}_{{z}^{2}},\, d^{1}_{xy},\, d^{1}_{yz},\, d^{1}_{xz},\, d^{1}_{{x}^{2}-{y}^{2}}[/tex]
Then the remaining five electrons, results in the pairing of electrons in each d-atomic orbital.
[tex]d^{2}_{{z}^{2}},\, d^{2}_{xy},\, d^{2}_{yz},\, d^{2}_{xz},\, d^{2}_{{x}^{2}-{y}^{2}}[/tex]
Ten electrons occupy the five orbitals related to an atom's d sub-level singly first before pairing takes place.
According to Hund's rule, electrons first occupy degenerate orbitals singly before they start pairing up.
The d sub-level consists of five degenerate orbitals; dxy, dyz, dxz, dx^2 - y^2 and dz^2. According to Hund's rule, electrons will be filled into these orbitals singly first before we start pairing.
If I have to fill ten electrons into the d sub-level, I will first fill in five electrons singly to occupy the five degenerate orbitals before I start adding a second electron to each of the degenerate orbital until all ten electrons are filled in.
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