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Write a Lewis structure that obeys the octet rule for each molecule or ion. Include resonance structures if necessary and assign formal charges to each atom. b. CO32– c. ClO– d. NO2–
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11. Bonding & Molecular Structure
Resonance Structures
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Which of the following is a valid resonance structure for a molecule with nitrogen triple bonded to another nitrogen and single bonded to an oxygen with a lone pair of electrons?
A
N≡O-N
B
N≡N-O⁻
C
N-N=O
D
N=N=O
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Understand the concept of resonance structures: Resonance structures are different ways to draw the same molecule, showing the distribution of electrons. They are used to represent molecules where the electron distribution cannot be accurately depicted by a single Lewis structure.
Identify the given molecule: The molecule in question has nitrogen triple bonded to another nitrogen and single bonded to an oxygen with a lone pair of electrons. This is represented as N≡N-O⁻.
Analyze the electron distribution: In the given molecule, the nitrogen atoms are triple bonded, which means they share three pairs of electrons. The oxygen is single bonded to one of the nitrogen atoms and has a lone pair, indicating it carries a negative charge.
Consider the resonance possibilities: Resonance structures must have the same number of electrons and atoms, but the arrangement of electrons can differ. The valid resonance structure should maintain the overall charge and connectivity of the atoms.
Evaluate the options: The correct resonance structure should reflect the possibility of electron movement while maintaining the stability of the molecule. The structure N≡N-O⁻ is valid because it maintains the triple bond between the nitrogen atoms and the single bond to the oxygen, with the negative charge on the oxygen due to its lone pair.
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