How can the octet rule be used to explain why one magnesium (Mg) atom would bond with one oxygen (O) atom?
A. Oxygen has six valence electrons; it needs to lose these electrons to reach the octet rule with a full second energy orbital. Magnesium has two valance electrons; it would prefer to gain six valence electrons to reach the octet rule of a full second energy orbital. Therefore, one magnesium atom can satisfy the needs of the oxygen atom to form an ionic bond.
B. Magnesium has six valence electrons; it needs to gain two electrons to reach the octet rule with a full second energy orbital. Oxygen has two valance electrons; it would prefer to lose both valence electrons to reach the octet rule of a full second energy orbital. Therefore, one magnesium atom can satisfy the needs of the oxygen atom to form an ionic bond.
C. Oxygen has one valence electron; it needs to gain two electrons to reach the octet rule with a full first energy orbital. Magnesium has one valance electron; it would prefer to lose its valence electron to reach the octet rule of a full first energy orbital. Therefore, one magnesium atom can satisfy the needs of the oxygen atom to form an ionic bond.
D. Oxygen has six valence electrons; it needs to gain two electrons to reach the octet rule with a full second energy orbital. Magnesium has two valance electrons; it would prefer to lose both valence electrons to reach the octet rule of a full second energy orbital. Therefore, one magnesium atom can satisfy the needs of the oxygen atom to form an ionic bond.