Yes it is possible to write the noble gas configuration of all elements, though it is not possible to list all of them here.
Electron configuration of uranium is: [Rn]5f36d17s2
The electron configuration of fluorine is 1s2 2s2 2p5.
It is [Ar] 3d1 4s2
[Ne] 3s2 3p6
You think probably at Unbinilium (120Ubn) an element not still obtained. The supposed electron configuration of Ubn will be [Uuo]7s2.
Yes it is possible to write the noble gas configuration of all elements, though it is not possible to list all of them here.
Electron configuration of uranium is: [Rn]5f36d17s2
The electron configuration of fluorine is 1s2 2s2 2p5.
The first-row transition metal with the most unpaired electrons is manganese (Mn). Its expected ground-state electron configuration is [Ar] 3d5 4s2, meaning it has 5 unpaired electrons in the 3d subshell.
It is [Ar] 3d1 4s2
[Ne] 3s2 3p6
In noble gas notation, you don't have to write the electron configuration up to that noble gas. You simply put the noble gas in brackets [noble gas] and then continue to write the electron configuration from that point. It just makes it shorter and easier to write electron configurations for elements with a lot of electrons.
The electron configuration of aluminium is [Ne]3s2.3p1.
The electron configuration for zinc is 1s2 2s2 2p6 3s2 3p6 3d10 4s2 4p6 4d10.
The outer electron configuration for oxygen is 2s^2 2p^4. This means that oxygen has 6 outer electrons in its valence shell.
Because it is shorter and easier to write. Also saves time when compared to writing the complete electron configuration.