Calculate the maximum number of unpaired electrons that can be placed in a 6d subshell

How many d sub-shells are there? 5? If those have only 1 electron then how many electrons can be there?

To calculate the maximum number of unpaired electrons that can be placed in a 6d subshell, we need to know the number of orbitals in the subshell and the electron filling order.

In general, the number of orbitals in a subshell is equal to (2l + 1), where "l" represents the azimuthal quantum number. For the 6d subshell, the azimuthal quantum number (l) is equal to 2, so there are (2 * 2 + 1) = 5 orbitals.

The electron filling order is determined by the Aufbau principle, which states that lower energy orbitals are filled before higher energy orbitals. In this case, since we are considering the 6d subshell, we need to determine the order in which the subshells are filled up until the 6d subshell.

The filling order for subshells is as follows:
1s, 2s, 2p, 3s, 3p, 4s, 3d, 4p, 5s, 4d, 5p, 6s, 4f, 5d, 6p, 7s, 5f, 6d

From this order, we can see that the 6d subshell comes after the 5f subshell.

The maximum number of electrons that can be accommodated in the 6d subshell is given by 2 * (number of orbitals) according to the Pauli exclusion principle, which states that each orbital can accommodate a maximum of 2 electrons with opposite spins.

Therefore, the maximum number of unpaired electrons that can be placed in a 6d subshell is equal to the number of orbitals, which is 5.