Multiple Choice
Which of the following statements correctly describes the Lewis dot structure of the neutral compound O2F2 (dioxygen difluoride)?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
Multiple Choice
Which of the following species has a valid Lewis dot structure as a neutral compound?
A
NO3-
B
NH4+
C
CO2
D
O2-
Verified step by step guidance1
Step 1: Understand that a valid Lewis dot structure for a neutral compound must have no overall charge, meaning the total number of valence electrons should match the sum of electrons contributed by all atoms without any extra or missing electrons.
Step 2: Analyze each species given: NO3⁻ (nitrate ion), NH4⁺ (ammonium ion), CO2 (carbon dioxide), and O2⁻ (superoxide ion). Note that NO3⁻ and NH4⁺ are ions with charges, so they are not neutral compounds.
Step 3: For CO2, count the total valence electrons: Carbon has 4 valence electrons, and each oxygen has 6 valence electrons, so total electrons = 4 + 2×6 = 16 electrons. This matches the electrons needed to form a stable neutral molecule with double bonds between carbon and oxygen atoms.
Step 4: For O2⁻, it is an ion with a negative charge, so it is not neutral. Its Lewis structure includes an extra electron compared to neutral O2, making it an ion rather than a neutral compound.
Step 5: Conclude that among the options, CO2 is the only species that can have a valid Lewis dot structure as a neutral compound because it has no charge and the correct number of valence electrons to form stable bonds.
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