Final answer:
Magnesium (Mg) will easily create an ionic bond with elements from Group 16, which form -2 anions, as Mg2+ donates its two excess electrons to achieve a stable ionic compound like MgO.
Step-by-step explanation:
Magnesium (Mg), which is in Group 2 and has a charge of +2, will easily create an ionic bond with elements from Group 16, also known as the oxygen family. These elements, such as oxygen (O), sulfur (S), and selenium (Se), normally form anions with a charge of -2.
The reason why Mg2+ forms ionic bonds readily with Group 16 elements is that the Mg2+ ion needs to lose two electrons to achieve a stable octet configuration, while Group 16 elements need to gain two electrons to complete their octet. This complements perfectly as Mg2+ can donate its two excess electrons to a Group 16 element, which can accept two electrons, resulting in a stable ionic compound like magnesium oxide (MgO) or magnesium sulfide (MgS).
An example is the formation of MgO, where each oxygen atom gains two electrons to become O2- and each magnesium atom loses two electrons to become Mg2+. This transfer of electrons results in a strong electrostatic force of attraction between the oppositely charged ions, creating a stable ionic bond.