QQuestionChemistry
QuestionChemistry
What is the molecular geometry, or shape, of phosphorus trichloride (PCl^3 )?
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Determine the Lewis Structure
- Total valence electrons: $$5 + (3 \times 7) = 22$$ electrons
- Phosphorus (P) is in Group 15 and has 5 valence electrons - Chlorine (Cl) is in Group 17 and has 7 valence electrons
Step 3:: Arrange Electron Domains
- Central phosphorus atom forms three single bonds with chlorine atoms - Electron domain geometry is determined by electron pairs around the central atom - Total electron domains: 4 (3 bonding, 1 lone pair on phosphorus)
Step 4:: Identify Molecular Geometry
- Using VSEPR (Valence Shell Electron Pair Repulsion) theory - 4 total electron domains with 3 bonding domains - This corresponds to a trigonal pyramidal shape - The lone pair on phosphorus causes slight distortion from perfect tetrahedral geometry
Step 5:: Confirm Structural Characteristics
- Bond angles will be slightly less than 109.5° due to lone pair repulsion - Approximate bond angle: around 103 - 107°
Final Answer
The molecular geometry of phosphorus trichloride (PCl₃) is trigonal pyramidal.
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