QQuestionChemistry
QuestionChemistry
Predict the molecular structure and give the approximate bond angles of the PCl^3 molecule.
A. Linear, 180°
B. Trigonal planar, 120°
C. Tetrahedral, 109.5°
D. Bent, around 107°
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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
- The central atom is phosphorus (P) - Chlorine (Cl) atoms are bonded to the phosphorus
Step 3:: Count valence electrons
- Total valence electrons: $$5 + (3 \times 7) = 22$$ electrons
- Phosphorus has 5 valence electrons - Each chlorine has 7 valence electrons
Step 4:: Draw the Lewis structure
- Three single bonds between P and Cl - One lone pair on the phosphorus atom - Electron configuration shows 3 bonding pairs and 1 lone pair
Step 5:: Apply VSEPR theory
- Total electron domains: 4 (3 bonding + 1 lone pair) - Electron domain geometry: Tetrahedral - Molecular geometry: Trigonal pyramidal due to lone pair
Step 6:: Determine bond angles
- Approximate bond angle: $$\approx 107°
- Lone pair causes slight compression of bond angles
Final Answer
Bent, around 107° Key Reasoning: - Lone pair repels bonding pairs - Causes slight deviation from perfect tetrahedral angle of 109.5° - Results in a bent molecular geometry with compressed bond angles
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