QQuestionChemistry
QuestionChemistry
Determine the molecular geometry and bond angles for phosphorus trichloride, PCl^3.
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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, so it has 5 valence electrons - Chlorine (Cl) is in Group 17, so each Cl has 7 valence electrons
Step 3:: Electron Pair Arrangement
\text{Electron pairs: } 4 \text{ total (3 bonding, 1 lone pair)}
- Draw the Lewis structure with single bonds between P and Cl - Remaining electrons form lone pairs on the central phosphorus atom - Electron pair geometry: Tetrahedral
Step 4:: Molecular Geometry Determination
- Lone pair on central phosphorus affects molecular shape - Molecular geometry: Trigonal pyramidal - Number of electron domains: 4 - Number of bonding domains: 3 - Number of lone pair domains: 1
Step 5:: Bond Angle Calculation
- Actual bond angle will be approximately $$\approx 103^\circ
- Ideal trigonal pyramidal bond angle is slightly less than 109.5° - Lone pair repulsion causes slight compression of bond angles
Final Answer
- Molecular Geometry: Trigonal Pyramidal - Bond Angle: \approx 103^\circ
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