QQuestionChemistry
QuestionChemistry
Of the three choices below, choose the best Lewis structure for OCl^2.
A. ⋯Cl−⋯O−⋯Cl
B. ⋯Cl−:O−⋯Cl
C. ⋯Cl−⋯O−⋯Cl
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Answer
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Step 1:I'll solve this Lewis structure problem step by step:
Step 2:: Determine the total number of valence electrons
- Total valence electrons: $$6 + (7 \times 2) = 20$$ electrons
- Oxygen (O): 6 valence electrons - Chlorine (Cl): 7 valence electrons × 2
Step 3:: Arrange atoms and connect with single bonds
- Initial electron distribution: $$\frac{20}{2} = 10$$ electron pairs
- Place O in the center - Connect two Cl atoms to O with single bonds
Step 4:: Complete octets for outer atoms (Cl)
- Each Cl needs 8 electrons - Place 3 electron pairs around each Cl atom
Step 5:: Distribute remaining electrons to central O
- Remaining electrons: $$20 - (3 \times 2 \times 2) = 14$$ electrons
- Place remaining electrons on O to complete its octet
Step 6:: Analyze the Lewis structures
- Option A and C are identical - Option B shows a different electron arrangement
Step 7:: Determine the most stable structure
- Option B (⋯Cl−:O−⋯Cl) provides the most stable electron configuration - Electrons are distributed to minimize formal charges - Central O has a complete octet - Cl atoms have complete octets
Final Answer
B (⋯Cl−:O−⋯Cl) is the best Lewis structure for OCl^2.
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