QQuestionChemistry
QuestionChemistry
Using the VSEPR theory, what is the shape of CH^2Cl^2?
A. Bent: The chlorine atoms will push the hydrogen and carbon atoms farther away from them and closer to each other due to their greater electronegativity.
B. Trigonal pyramidal: There are four shared pairs of electrons and no lone electron pairs in the molecule.
C. Tetrahedral: There are four shared pairs of electrons and no lone electron pairs in the molecule.
D. Linear: The atoms are all nonmetals with low electronegativity and will have equal repulsion forces on each other.
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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 central atom
- In CH₂Cl₂, carbon (C) is the central atom - Carbon has 4 valence electrons and forms 4 bonds
Step 3:: Count the total number of electron domains
- 4 single bonds (C-H and C-Cl bonds) - No lone pairs on the central carbon atom - Total electron domains = 4
Step 4:: Apply VSEPR theory rules
- With 4 electron domains and no lone pairs - The electron domains will arrange themselves to minimize repulsion - This results in a tetrahedral electron domain geometry
Step 5:: Analyze molecular geometry
- Bond angles will be approximately $$109.5^\circ
- All 4 domains are bonding domains (no lone pairs) - This means the molecular shape is also tetrahedral
Step 6:: Eliminate incorrect answers
- A (Bent): Incorrect - no lone pairs to cause bending - B (Trigonal pyramidal): Incorrect - requires a lone pair - D (Linear): Incorrect - does not match the electron domain arrangement
Final Answer
Tetrahedral The key is recognizing that the 4 electron domains around carbon arrange in a tetrahedral geometry with no lone pairs, resulting in a tetrahedral molecular shape.
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