QQuestionChemistry
QuestionChemistry
Look at the Lewis structure of the following molecule and predict its 3 -D shape according to the VSEPR theory:
Oxygen dichloride (OCl
2
)
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Answer
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Step 1:I'll solve this problem step by step using VSEPR theory and proper LaTeX notation:
Step 2:: Determine the central atom and valence electrons
- Total valence electrons: $$6 + (2 \times 7) = 20$$ electrons
- The central atom is oxygen (O) - Oxygen has 6 valence electrons - Chlorine (Cl) has 7 valence electrons
Step 3:: Draw the Lewis structure
- Arrange electrons to create a stable electron configuration - Oxygen is the central atom - Two chlorine atoms are bonded to oxygen - Typical Lewis structure shows single bonds and lone pairs
Step 4:: Count electron domains around the central atom
- Total electron domains: $$4$$ domains
- Two single bonds to chlorine atoms - Two lone pairs on the oxygen atom
Step 5:: Determine electron domain geometry
- $$AX_{2}E_{2}$$ type molecule (2 atoms, 2 lone pairs)
- With 4 electron domains, the electron domain geometry is tetrahedral
Step 6:: Determine molecular geometry
- Expected bond angle less than $$109.5^\circ$$, approximately $$110^\circ
- Lone pairs cause slight distortion from ideal tetrahedral angle - Molecular shape is bent (V-shaped)
Final Answer
The 3 -D shape of oxygen dichloride (OCl₂) is bent (V-shaped) with a bond angle slightly less than tetrahedral.
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