Multiple Choice
Which of the following best represents the Lewis dot structure for methane (CH_4)?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following correctly represents the Lewis dot structure for neutral magnesium phosphide (Mg3P2)?
A
Each Mg atom loses two electrons to form Mg2+ ions, and each P atom gains three electrons to form P3- ions; the structure shows Mg2+ ions and P3- ions with full octets.
B
Each Mg atom and P atom retain their valence electrons without any transfer or sharing.
C
Each Mg atom gains two electrons to form Mg2- ions, and each P atom loses three electrons to form P3+ ions.
D
Each Mg atom shares electrons with P atoms to form covalent bonds, with no ions present.
Verified step by step guidance1
Identify the elements involved: magnesium (Mg) and phosphorus (P). Magnesium is a metal, and phosphorus is a nonmetal.
Determine the typical ionic charges based on their positions in the periodic table: Mg commonly forms Mg^{2+} by losing two electrons, and P commonly forms P^{3-} by gaining three electrons.
Use the formula Mg_3P_2 to balance the charges: 3 Mg^{2+} ions contribute a total charge of +6, and 2 P^{3-} ions contribute a total charge of -6, resulting in a neutral compound.
Draw the Lewis dot structures showing Mg atoms losing their two valence electrons to become Mg^{2+} ions (no dots around Mg), and P atoms gaining three electrons to complete their octet, becoming P^{3-} ions with full octets represented by eight dots around P.
Confirm that the structure represents ionic bonding: Mg^{2+} and P^{3-} ions are held together by electrostatic attraction, not by sharing electrons, so the Lewis structure should show ions rather than covalent bonds.
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