Question

Illustrate and describe the sequence in which ten electrons occupy the five orbitals related to an atoms d sublevel

Answer 1

Actually a d sublevel contains 5 orbitals. So in this case, the electrons would first fill each of the five orbitals so remaining electrons are 5. Now this remaining 5 electrons would pair with the filled orbital. That is, the 6th electron would pair its spin with the 1st orbital, the 7th electron would pair with the one in the 2nd orbital, and so on.

Answer 2

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 $d_{{z}^{2}},\, d_{xy},\, d_{yz},\, d_{xz},\, d_{{x}^{2}-{y}^{2}}$, 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

$d^{1}_{{z}^{2}},\, d^{1}_{xy},\, d^{1}_{yz},\, d^{1}_{xz},\, d^{1}_{{x}^{2}-{y}^{2}}$

Then the remaining five electrons, results in the pairing of electrons in each d-atomic orbital.

$d^{2}_{{z}^{2}},\, d^{2}_{xy},\, d^{2}_{yz},\, d^{2}_{xz},\, d^{2}_{{x}^{2}-{y}^{2}}$