QQuestionChemistry
QuestionChemistry
Which of the following is the correct molecular geometry for the phosphate ion, PO^3 - 4?
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Answer
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Step 1:I'll solve this problem step by step, following the specified LaTeX formatting guidelines:
Step 2:: Identify the Central Atom
The central atom in the phosphate ion $$PO_{4}^{3-}$$ is phosphorus (P).
Step 3:: Determine the Number of Valence Electrons
- Total valence electrons: $$5 + 24 + 3 = 32$$ electrons
- Phosphorus: 5 valence electrons - Oxygen (4 atoms): 4 × 6 = 24 valence electrons - Charge of - 3: Add 3 electrons
Step 4:: Draw the Lewis Structure
- Phosphorus is the central atom - Four oxygen atoms bond to phosphorus - One oxygen will have a negative charge - Electrons are distributed to achieve octet for all atoms
Step 5:: Determine Electron Geometry
- Total electron domains around central atom: 4 - Electron geometry: Tetrahedral
Step 6:: Determine Molecular Geometry
- All 4 electron domains are bonding domains - No lone pairs on central phosphorus atom - Molecular geometry: Tetrahedral
Final Answer
The molecular geometry of the phosphate ion PO_{4}^{3 -} is tetrahedral.
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