Multiple Choice
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?
11. Bonding & Molecular Structure
Resonance Structures
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Determine which of the following drawings would be the best structure for the N2O molecule.
A
a
B
b
C
c
D
All are equally stable
Verified step by step guidance1
Step 1: Begin by counting the total number of valence electrons available for the N2O molecule. Nitrogen (N) has 5 valence electrons and oxygen (O) has 6 valence electrons. Therefore, the total number of valence electrons for N2O is 5 + 5 + 6 = 16 electrons.
Step 2: Evaluate each structure (a, b, c) to ensure that the total number of valence electrons used in the structure matches the calculated total of 16 electrons. Check that each atom satisfies the octet rule, where possible.
Step 3: Consider the formal charges for each atom in the structures. The formal charge is calculated using the formula: Formal Charge = (Valence Electrons) - (Non-bonding Electrons) - (Bonding Electrons/2). Calculate the formal charges for each atom in structures a, b, and c.
Step 4: Compare the formal charges calculated in Step 3. The most stable structure will have formal charges closest to zero, and any negative formal charge should ideally reside on the more electronegative atom, which is oxygen in this case.
Step 5: Analyze the resonance and bond order in each structure. The best structure will have a reasonable bond order and resonance stability, contributing to the overall stability of the molecule.
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