What is the Lewis Dot Structure for One Formula Unit of Magnesium Sulfide?

To understand the Lewis dot structure for magnesium sulfide (MgS), we first need to identify the valence electrons of the constituent atoms.

Magnesium (Mg) is in group 2 of the periodic table and has 2 valence electrons. Sulfur (S) is in group 16 and has 6 valence electrons. When magnesium and sulfur combine to form magnesium sulfide, magnesium donates its 2 electrons to sulfur, allowing both elements to achieve a stable electron configuration.

In the Lewis dot structure, magnesium is represented with no dots around it since it loses its 2 valence electrons, becoming a positively charged ion (Mg²⁺). Sulfur, on the other hand, gains those 2 electrons, leading to 8 valence electrons around it, which is depicted as having 8 dots (2 paired and 4 unpaired) around it, giving it a negatively charged ion (S^2-).

The Lewis dot structure can be illustrated as follows:

Mg⁺     :S: 

In summary, the Lewis dot structure for magnesium sulfide highlights the transfer of electrons from magnesium to sulfur, resulting in the formation of a stable ionic compound.