QQuestionChemistry
QuestionChemistry
Predict the molecular shape and give the approximate bond angle in the CO^2 molecule.
A. linear, 180°
B. trigonal planar, 120°
C. tetrahedral, 109.5°
D. trigonal pyramidal, 109.5°
E. bent, 120°
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Answer
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Step 1:Let's solve this step by step using VSEPR (Valence Shell Electron Pair Repulsion) theory:
Step 2:: Determine the number of valence electrons
- Total valence electrons: $$4 + 12 = 16$$ electrons
- Carbon (C): 4 valence electrons - Oxygen (O): 6 valence electrons × 2 = 12 valence electrons
Step 3:: Draw the Lewis structure
- Carbon is the central atom - Form double bonds between C and each O - Electron configuration shows 2 double bonds and no lone pairs on the central carbon
Step 4:: Count electron domains around the central atom
- 2 double bonds = 2 electron domains - No lone pairs on central carbon - Total electron domains: 2
Step 5:: Determine molecular geometry
- 2 electron domains arranged linearly to minimize electron repulsion - This results in a linear molecular shape
Step 6:: Calculate bond angle
- Linear molecular geometry means the bond angle is exactly $$180°
Step 7:: Verify electron domain arrangement
- Electron domains are maximally separated - This confirms the linear geometry
Final Answer
Key Reasoning: - CO^2 has a central carbon with two double bonds to oxygen - No lone pairs on the central atom - Electron domains are maximally separated - Results in a linear molecular shape with a 180° bond angle
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