Which of the following diagrams best represents the transfer of electrons to form magnesium oxide (MgO)?

• A. A diagram showing Mg atom gaining two electrons from O atom, resulting in Mg^{2-} and O^{2+} ions.
• B. A diagram showing Mg atom sharing two electrons with O atom, forming a covalent bond.
• C. A diagram showing no electron transfer between Mg and O atoms.
• D. A diagram showing Mg atom losing two electrons to O atom, resulting in Mg^{2+} and O^{2-} ions.

Answer: (D)

Verified step by step guidance

1. Identify the types of elements involved: Magnesium (Mg) is a metal and Oxygen (O) is a nonmetal. Metals tend to lose electrons, and nonmetals tend to gain electrons to achieve stable electron configurations.
2. Determine the electron transfer based on their positions in the periodic table: Magnesium is in group 2 and has 2 valence electrons, while Oxygen is in group 16 and needs 2 electrons to complete its octet.
3. Understand ionic bond formation: Magnesium will lose its 2 valence electrons to achieve a stable electron configuration, becoming Mg^{2+}, and Oxygen will gain those 2 electrons to become O^{2-}.
4. Recognize that the transfer of electrons results in the formation of oppositely charged ions, which attract each other to form an ionic bond, creating magnesium oxide (MgO).
5. Conclude that the correct diagram must show Mg losing two electrons to O, resulting in Mg^{2+} and O^{2-} ions, representing the ionic nature of magnesium oxide.