QQuestionChemistry
QuestionChemistry
What is the molecular geometry, or shape, of phosphorus trichloride (PCl₃)?
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX and formatting guidelines:
Step 2:: Identify the Central Atom
- The central atom in phosphorus trichloride ($$PCl_{3}$$) is phosphorus (P)
- Phosphorus is the central atom to which the chlorine atoms are bonded
Step 3:: Determine the Number of Valence Electrons
- Total valence electrons: $$5 + (3 \times 7) = 26$$ valence electrons
- Phosphorus: 5 valence electrons - Chlorine: 7 valence electrons
Step 4:: Draw the Lewis Structure
- Form single bonds between P and each Cl - Distribute remaining electrons as lone pairs - Phosphorus will have one lone pair of electrons
Step 5:: Apply VSEPR Theory
- Count electron domains around central atom: * 3 bonding domains (P-Cl bonds) * 1 non-bonding domain (lone pair) - Total electron domains: 4 - Electron domain geometry: Tetrahedral
Step 6:: Determine Molecular Geometry
- With 3 bonding domains and 1 lone pair - Molecular geometry is trigonal pyramidal
Final Answer
The molecular geometry of phosphorus trichloride (PCl_{3}) is trigonal pyramidal.
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