Multiple Choice
Which of the following best represents the correct Lewis dot structure for a neutral N_2 molecule?
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11. Bonding & Molecular Structure
Lewis Dot Structures: Neutral Compounds
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Which of the following Lewis dot structures for CO$_2$ (carbon dioxide) represents the most stable arrangement based on formal charges?
A
O–C≡O, with one oxygen single-bonded and the other triple-bonded to carbon
B
O=C=O, with all atoms having a formal charge of 0
C
O=C–O, with one double bond and one single bond
D
O$^-$–C≡O$^+$, with oxygen having a -1 formal charge and carbon a +1 formal charge
Verified step by step guidance1
Recall that the stability of a Lewis structure is often determined by minimizing formal charges on atoms and placing negative formal charges on the more electronegative atoms.
Calculate the formal charge for each atom in the given Lewis structures using the formula: $\text{Formal Charge} = \text{Valence Electrons} - \text{Nonbonding Electrons} - \frac{1}{2} \times \text{Bonding Electrons}$.
For the structure O–C≡O, assign electrons to each atom and calculate formal charges, noting that one oxygen is single-bonded and the other is triple-bonded to carbon.
For the structure O=C=O, where carbon is double bonded to both oxygens, calculate formal charges and observe that all atoms have a formal charge of zero.
Compare the formal charges of all structures and identify the one with the smallest magnitude of formal charges (ideally zero on all atoms) as the most stable Lewis structure.
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