The noble gas configuration of magnesium is [Ne] 3s^2. This indicates that magnesium has the same electron configuration as the nearest noble gas, neon, with an outer shell containing 2 electrons in the 3s orbital.
[Ne] 3s2 3p6
The noble gas configuration of Mg2+ is [Ne] because the magnesium atom loses two electrons to form the Mg2+ ion. The electron configuration of Ne is 1s2 2s2 2p6, so when Mg loses its two valence electrons, it achieves a stable electron configuration similar to that of the noble gas Ne.
The noble gas configuration of silicon is [Ne] 3s^2 3p^2, where [Ne] represents the electron configuration of the noble gas neon. Silicon has 14 electrons, with two in the 3s orbital and two in the 3p orbital.
Sodium has the configuration Ne 3s2 . Sodium is group-1 element.
The noble gas configuration of magnesium is [Ne] 3s^2. This indicates that magnesium has the same electron configuration as the nearest noble gas, neon, with an outer shell containing 2 electrons in the 3s orbital.
The noble gas configuration of sulfur is [Ne]3s2 3p4. It represents the electron configuration of sulfur when it has achieved a stable electronic configuration similar to the nearest noble gas, neon.
[Ne] 3s2 3p6
The noble gas electron configuration of Phosphorus is [Ne] 3s2 3p3
[Ne]3s23p1
[Ne]3s23p2
[Ne]3s23p5
[Ne]3s2
[Ne] 3s2
[Ne]3s23p3
[Ne]3s23p2
[Ne] = [He]2s22p6