QQuestionChemistry
QuestionChemistry
Using the VSEPR theory, predict the molecular structure of the following polyatomic ion:
PO^3−(4)
A. Linear
B. Bent (V-shaped)
C. Trigonal planar
D. Trigonal pyramid
E. Tetrahedral
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Answer
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Step 1:I'll solve this step by step using VSEPR theory:
Step 2:: Determine the central atom
- The central atom is phosphorus (P)
Step 3:: Count the total number of valence electrons
- Total valence electrons: $$5 + 24 + 3 = 32$$ electrons
- Phosphorus: 5 valence electrons - Oxygen: 6 valence electrons × 4 oxygens = 24 valence electrons - Negative charge: + 3 additional electrons
Step 4:: Draw the Lewis structure
- Phosphorus will be the central atom - Distribute electrons to create octets around oxygen atoms - Remaining electrons form bonds with the central phosphorus - Resulting structure shows 4 oxygen atoms bonded to phosphorus with one extra negative charge
Step 5:: Determine electron domain geometry
- Total electron domains around central atom: 4 - Bonding domains: 4 - Lone pair domains: 0
Step 6:: Apply VSEPR theory rules
- With 4 bonding domains and no lone pairs - This corresponds to a tetrahedral electron domain geometry - Molecular geometry will also be tetrahedral
Final Answer
Tetrahedral Explanation: The PO^{4 - 3} ion has a tetrahedral structure due to 4 bonding domains around the central phosphorus atom with no lone pairs, following VSEPR theory predictions.
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