QQuestionChemistry
QuestionChemistry
What are the electron and molecular geometries, respectively, for iodine trifluoride, IF^3?
A. Electron geometry is trigonal bipyramidal. Molecular geometry is trigonal planar.
B. Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped.
C. Electron geometry is octahedral. Molecular geometry is T-shaped.
D. Electron geometry is trigonal planar. Molecular geometry is trigonal bipyramidal.
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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 and total valence electrons
- Total valence electrons: $$7 + (3 \times 7) = 28$$ electrons
- Central atom is Iodine (I) - Fluorine atoms (F) contribute 7 valence electrons each - Iodine contributes 7 valence electrons
Step 3:: Draw the Lewis structure
- Iodine forms single bonds with three fluorine atoms - Iodine will have two lone pairs - Total electron domains: 5 (3 bonding, 2 non-bonding)
Step 4:: Determine electron geometry
- 5 total electron domains - Electron geometry is trigonal bipyramidal - This means the electron domains are arranged to minimize repulsion
Step 5:: Determine molecular geometry
- 3 bonding domains, 2 lone pairs - Lone pairs occupy equatorial positions to minimize repulsion - Resulting molecular geometry is T-shaped
Step 6:: Analyze the options
- Option B matches our analysis: * Electron geometry is trigonal bipyramidal * Molecular geometry is T-shaped
Final Answer
Electron geometry is trigonal bipyramidal. Molecular geometry is T-shaped.
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