Multiple Choice
Which of the following best describes the correct Lewis dot structure for the neutral compound CHF?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following correctly describes the Lewis dot structure for neutral magnesium phosphide (Mg3P2)?
A
Each Mg atom shares electrons with P atoms to form covalent bonds.
B
Each P atom loses three electrons to form P3+ ions, and each Mg atom gains electrons to form Mg− ions.
C
Each Mg atom loses two electrons to form Mg2+ ions, and each P atom gains three electrons to form P3− ions.
D
Each Mg atom gains two electrons from P atoms to form Mg2− ions.
Verified step by step guidance1
Identify the elements involved: magnesium (Mg) and phosphorus (P). Magnesium is a metal, and phosphorus is a nonmetal.
Recall that metals tend to lose electrons to form cations, while nonmetals tend to gain electrons to form anions. This is typical in ionic compounds.
Determine the common oxidation states: magnesium commonly forms Mg^{2+} ions by losing two electrons, and phosphorus commonly forms P^{3-} ions by gaining three electrons.
Use the charges to balance the formula: since Mg forms Mg^{2+} and P forms P^{3-}, the compound must have 3 Mg^{2+} ions and 2 P^{3-} ions to balance the total positive and negative charges, resulting in Mg_3P_2.
Understand that in the Lewis dot structure for Mg_3P_2, electrons are transferred from Mg atoms to P atoms, forming ionic bonds rather than shared electrons (covalent bonds). Therefore, Mg atoms lose electrons to become Mg^{2+} ions, and P atoms gain electrons to become P^{3-} ions.
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