Question
Asked By FrostBite26 at
Answered By Expert
Dwight
Expert · 3.7k answers · 3k people helped
To determine the most plausible resonance structure for the cyanate ion,
\mathrm{OCN}^{-}, we need to consider the distribution of electrons and the formal charges on each atom. Here’s a step-by-step guide to drawing the most plausible resonance structure:
Solution By Steps
Step 1: Identify the atoms and their electronegativities
Oxygen (O) is the most electronegative atom, followed by nitrogen (N), and carbon ©.
Step 2: Assign a central atom
Typically, the least electronegative atom is the central atom. In this case, carbon © is the least electronegative among the three.
Step 3: Draw the basic structure
Place C in the center, with O and N bonded to it.
Step 4: Determine the number of valence electrons
O: 6 valence electrons
C: 4 valence electrons
N: 5 valence electrons
An additional electron due to the negative charge: 1
Total valence electrons: 6 + 4 + 5 + 1 = 16
Step 5: Arrange the electrons to form bonds and lone pairs
Form a triple bond between C and N, and a single bond between C and O.
Assign the remaining electrons to satisfy the octet rule for each atom.
Step 6: Calculate formal charges
Formal charge = valence electrons - (lone pair electrons + 1/2 bonding electrons)
For O: 6 - (4 + 1/2 * 2) = 0
For C: 4 - (0 + 1/2 * 8) = 0
For N: 5 - (2 + 1/2 * 6) = 0
Step 7: Consider resonance structures
Move the electrons around to form different bonding patterns, ensuring that the formal charges are minimized.
Final Answer
The most plausible resonance structure for the cyanate ion,
\mathrm{OCN}^{-}, is one where carbon is the central atom, with a triple bond to nitrogen and a single bond to oxygen. All atoms have a formal charge of zero, and the structure is stable.
\begin{array}{ccc}
& :O^{\ominus} & \\
& | & \\
:N &\equiv &C: \\
\end{array}
🧑🏫 More Questions
👉 Interested in exploring further?
Chrome Extension
1. Search answers from our 90+ million questions database.
2. Get instantly AI Solutions powered by most advanced models like GPT-4, Bard, Math GPT, etc.
3. Enjoy one-stop access to millions of textbook solutions.
4. Chat with 50+ AI study mates to get personalized course studies.
5. Ask your questions simply with texts or screenshots everywhere.