QQuestionChemistry
QuestionChemistry
The molecular geometry of the PF^4 + ion is
A. octahedral
B. tetrahedral
C. trigonal pyramidal
D. trigonal planar
E. trigonal bipyramidal
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Determine the central atom
- The central atom is phosphorus (P) - The ion is PF^4 +
Step 3:: Count the number of valence electrons
- Total valence electrons: $$5 + 28 - 1 = 32$$ electrons
- Phosphorus (P): 5 valence electrons - Fluorine (F): 7 valence electrons × 4 = 28 - Positive charge: Subtract 1 electron
Step 4:: Draw the Lewis structure
- Central P atom - 4 single bonds to F atoms - Remaining electrons as lone pairs
Step 5:: Determine electron domain geometry
- Total electron domains: 5 - Bonding domains: 4 - Lone pair domains: 1 - This corresponds to a trigonal bipyramidal electron domain geometry
Step 6:: Determine molecular geometry
- With 4 bonding domains and 1 lone pair - The lone pair will occupy an equatorial position - This results in a seesaw molecular geometry
Step 7:: Analyze the options
- Seesaw geometry is not among the given choices - Closest match is trigonal bipyramidal
Final Answer
E. trigonal bipyramidal
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