Magnesium (Mg) and sulfur (S) are both elements found in the periodic table, but they behave very differently when they form ions. Magnesium tends to lose two electrons to achieve a stable electron configuration, resulting in a +2 charge. In contrast, sulfur gains two electrons to fill its outer shell, resulting in a 2- charge.
Magnesium is located in group 2 of the periodic table, known as the alkaline earth metals. Elements in this group have two electrons in their outermost shell. To become stable, magnesium loses these two electrons, which gives it a +2 charge. The loss of these electrons allows magnesium to achieve a noble gas configuration similar to neon.
On the other hand, sulfur is located in group 16, where elements typically have six electrons in their outer shell. To reach stability, sulfur needs to gain two additional electrons to complete its octet. By gaining those two electrons, sulfur acquires a negative charge of 2-, resembling the electron configuration of the noble gas argon.
In summary, magnesium forms a +2 ion by losing two electrons, while sulfur forms a 2- ion by gaining two electrons. This behavior is driven by the desire of both elements to reach a stable electronic configuration.