XeF6 Problem Help - Explaining Molecular Geometry & Hybridization

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SUMMARY

The XeF6 ion exhibits a distorted octagonal molecular geometry and a pentagonal bipyramidal electron pair geometry. The hybridization of xenon (Xe) in XeF6 is confirmed as d2sp3, with one lone pair present on the Xe atom. The total valence electron count for XeF6 is 50, accounting for six fluorine (F) atoms bonded to xenon, leaving one lone pair. The correct statements regarding XeF6 include the presence of an octahedral electron pair arrangement and the hybridization type.

PREREQUISITES
  • Understanding of molecular geometry and hybridization concepts
  • Familiarity with valence electron counting
  • Knowledge of the octahedral and pentagonal bipyramidal geometries
  • Basic principles of chemical bonding and lone pairs
NEXT STEPS
  • Study the principles of molecular geometry in VSEPR theory
  • Learn about hybridization types and their implications in molecular structures
  • Explore the characteristics of pentagonal bipyramidal geometries
  • Investigate the role of lone pairs in molecular shape determination
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Chemistry students, educators, and professionals interested in molecular geometry, hybridization, and the properties of xenon compounds.

Neurocscience
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This problem is giving me some trouble:
Check the statements that correctly apply to the XeF6 ion:

a. There is an octahedral electron pair arrangement around Xe
b. The hybridization of Xe is d2sp3
c. The molecular structure is octahedral
d. There is one lone pair on the Xe atom
e. There are no lone pairs on the Xe atom

Could someone please explain it to me?

I know its molecular geometry is distorted octagon and its electron pair geometry is pentagonal bipyramidal. It also has 2 lone electron pairs, right? The hybridization I'm no so sure about...
 
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I don't think it has two lone pair.
The total valence electron is 50. Because there are six F which already bond to the Xe, there is only two electrons left, that is only one lone pair.
 


It has one lone pair and hybridisation is SP3d3...
 

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