Sodium (Na) has 11 electrons and is located in Group 1 of the periodic table.
E. 2.8.6 - Sodium will lose one electron from its outermost shell, which has 6 electrons, to achieve the stable electron configuration of the previous noble gas, neon (2.8). This will result in the formation of a sodium ion with a +1 charge, written as Na+.
F. 2.8.2 - Sodium will lose two electrons from its outermost shell, which has 2 electrons, to achieve the stable electron configuration of the previous noble gas, neon (2.8). This will result in the formation of a sodium ion with a +2 charge, written as Na2+.
It's important to note that the formation of Na2+ is highly unlikely under normal conditions, as the ionization energy required to remove a second electron from a sodium atom is much higher than the energy required to remove the first electron.