QQuestionChemistry
QuestionChemistry
What is the molecular geometry of the sulfate ion, SO^2−(4)?
A. trigonal planar
B. tetrahedral
C. trigonal pyramidal
D. bent
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Answer
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Step 1:Let's solve this step by step:
Step 2:: Determine the Lewis structure of the sulfate ion
- Sulfur (S) is the central atom - Oxygen (O) atoms are bonded to sulfur - The ion has a total charge of - 2 - Each oxygen atom will have a negative charge to balance the overall charge
Step 3:: Count the total number of valence electrons
- Total: $$6 + 24 + 2 = 32$$ valence electrons
- Sulfur: 6 valence electrons - Oxygen: 6 × 4 = 24 valence electrons - Charge of - 2 adds 2 more electrons
Step 4:: Analyze the electron arrangement
- 4 single bonds between S and O atoms - 2 oxygen atoms will have a double bond to S - Remaining electrons form lone pairs on oxygen atoms
Step 5:: Determine electron geometry and molecular geometry
- Central sulfur atom is surrounded by 4 electron domains - These 4 domains are arranged in a tetrahedral geometry - All 4 domains are bonding domains - No lone pairs on the central sulfur atom
Step 6:: Identify molecular geometry
- When all electron domains are bonding domains, the molecular geometry matches the electron geometry - Tetrahedral arrangement means 4 oxygen atoms are symmetrically positioned around the central sulfur atom
Final Answer
Tetrahedral
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