QQuestionChemistry
QuestionChemistry
Determine the electron geometry, molecular geometry, and polarity of SF^6 .
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Answer
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Step 1:
First, let's determine the electron geometry of SF^6. The central atom, Sulfur (S), forms six bonds with Fluorine (F) atoms. In this case, we have a central atom surrounded by eight electron pairs (six bonding pairs and two lone pairs). The electron geometry for such a configuration is octahedral.
Step 2:: Electron geometry is octahedral.
Step 3:
Next, we'll determine the molecular geometry. In SF^6, all the electron pairs are bonding pairs, so the molecular geometry is the same as the electron geometry.
Step 4:: Molecular geometry is also octahedral.
Step 5:
Now, let's analyze the polarity of the molecule. Since Sulfur (S) is more electronegative than Fluorine (F), the S-F bonds are polar, and the dipoles point towards the Fluorine atoms. However, due to the symmetrical shape of the octahedron, these individual bond dipoles cancel each other out, resulting in a net dipole moment of zero.
Step 6:: Despite having polar bonds, the overall molecular polarity is nonpolar due to the symmetrical shape and cancellation of bond dipoles.
Final Answer
- Electron geometry: Octahedral - Molecular geometry: Octahedral - Polarity: Nonpolar
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