Electron configuration og 32Ge is in short hand:
Ge => [Ar] 3d10 4s2 4p2
or complete: 1s2, 2s22p6, 3s2 3p6 3d10, 4s2 4p2
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The electron configuration of a neutral germanium atom is [Ar] 3d10 4s2 4p2. When germanium forms a +4 ion, it loses 4 electrons from its neutral configuration. Therefore, the electron configuration of Ge4+ is [Ar] 3d10.
By GE, I suspect you mean Ge (Germanium). If so, first you write out the electron configuration for Ge and then you deal with the +4 charge (if that is what you mean)
[Ar]4s23d104p2
and then for the +4 charge;
[Ar]3d10
The element with a valence electron configuration of 2s2 is beryllium. Beryllium has 4 electrons, with 2 in the 2s subshell, which makes it have a valence electron configuration of 2s2.
The longhand electron configuration of sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4.
The complete electron configuration of sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4.
The full electron configuration for sulfur is 1s^2 2s^2 2p^6 3s^2 3p^4.
The electron configuration of silicon is 1s2 2s2 2p6 3s2 3p2. You can represent this in shorthand notation by writing [Ne] 3s2 3p2, which indicates that silicon's configuration is the same as neon's configuration followed by the outermost electron sublevels of 3s2 3p2.