QQuestionChemistry
QuestionChemistry
Determine the molecular geometry of each of the following molecules.
SiO₂
A. bent
B. tetrahedral
C. trigonal planar
D. linear
E. trigonal pyramidal
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Determine the Lewis structure
- Total valence electrons: $$4 + (2 \times 6) = 16$$ electrons
- Silicon (Si) has 4 valence electrons - Oxygen (O) has 6 valence electrons
Step 3:: Electron Pair Geometry
- Silicon is the central atom - Two oxygen atoms are bonded to silicon - Electron configuration around silicon follows the octet rule - Total electron domains: 4 (2 bonding pairs, 0 lone pairs)
Step 4:: VSEPR Theory Analysis
- With 4 electron domains arranged symmetrically around the central atom - No lone pairs on the central atom - Bonds are equally distributed in three-dimensional space
Step 5:: Molecular Geometry Determination
- 4 electron domains with no lone pairs results in a tetrahedral geometry - All bonds are equivalent and point to the corners of a tetrahedron
Final Answer
Explanation: SiO₂ has a tetrahedral molecular geometry due to its symmetric arrangement of oxygen atoms around the central silicon atom, with no lone pairs present.
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