Ni2+, Goes from having 28 electrons to 30, giving it 10 electrons in its 3d subshell making that subshell full.
s subshell have energy more than d subshell
The 3s subshell is farther from the nucleus
Two electrons can occupy the 2s subshell, and 8 electrons can occupy the 3d subshell.
The 5p subshell is a p-subshell, and as such is filled by 6 electrons - three pairs spinning in opposite directions.The number of electrons in each subshell is as follows:Subshell s p d f theoretical next subshellsNo. of e- 2 6 10 14 18, 22, 26, etc.
silver
4f
This is because the D-Block in the Periodic Table is where the d-Subshell is being filled up. Chromium's d-Subshell is being filled up and is therefore in the D-Block.
Argon has completely filled M shell (or 3p orbital)
The period.
p-block elements have partially filled p-subshell. It is not completely filled.
According to definition, transition elements are those which have partially filled d-subshell in there elementary state or in one of the oxidation states. silver(z=47) can exhibit 2 oxidation state in which it has incompletely filled d-subshell (4d9). hence silver is regarded as trnsition element.
The 4f subshell is being filled for the rare earth series of elements.
Ni2+, Goes from having 28 electrons to 30, giving it 10 electrons in its 3d subshell making that subshell full.
noble gases.
they are similar due to the 2p subshell being one of the first to being added into an equation involving subshells. this is kin to getting on a bus as you and another person are one of the first to board the bus and thus they are similar.
d subshell = 2 p subshell = 6